REESE LIBRARY 
 
 UNIVERSITY OF 
 CALIFORNIA 
 
 ERSITY OF CALIFORNI 
 
 SCIENCES Deceived MAR 13 1893 18 
 
 LIBRARY 
 
 No. Class 
 
MINERALOGY SIMPLIFIED. 
 
MINERALOGY SIMPLIFIED. 
 
 EASY METHODS OF IDENTIFYING MINERALS, 
 INCLUDING ORES, 
 
 BY MEANS OF THE BLOWPIPE, BY FLAME REACTIONS, 
 
 BY THE SPECTROSCOPE, AND BY HUMID 
 
 CHEMICAL ANALYSIS, 
 
 BASED ON PROF. VON KOBELL'S TABLES FOR THE 
 DETERMINATION OF MINERALS. 
 
 WITH AN INTRODUCTION TO MODERN CHEMISTRY, 
 
 BY 
 
 HENRI ERNI, A.M., M.D., 
 
 LATE PROFESSOR OF CHEMISTRY, SO^ME'TIME CHIEF CHEMIST OF THE UNITED STATES 
 DEPARTMENT OF AGRICULTURE. 
 
 SKCOND EDITION, REVISED AND ENLARGED. 
 
 ILLUSTRATED BY ONE HUNDRED AND TWENTY-ONE ENGRAVINGS 
 
 PHILADELPHIA : 
 CAREY BAIRD & CO., 
 
 INDUSTRIAL PUBLISHERS, BOOKSELLERS, AND IMPORTERS, 
 
 810 WALNUT STREET. 
 LONDON : E. & P. N. 8PON, 125 STRAND. 
 
 188o. 
 
EARTH 
 
 SCIENCES 
 
 LIBRARY 
 
 COPYRIGHT BY 
 
 HENRY CAREY BAIKD & CO. 
 1885. 
 
 COLLINS, PRINTER. 
 
PUBLISHERS' PREFACE. 
 
 THE favor with which the former edition of Dr. 
 Erni's Mineralogy Simplified was received induced the 
 publishers some time since to request the author to 
 prepare a new edition, which should bring the subject 
 down to the present time. This he has done with his 
 accustomed thoroughness. 
 
 He has retained, in the present edition, the admira- 
 ble system of classifying and determining the mineral 
 species established by von Kobell, which is universally 
 conceded by mineralogists to be the most trustworthy, 
 serviceable, and practical for the purposes of experi- 
 mental study. 
 
 Professor Erni introduces the subject of Determina- 
 tive Mineralogy with a series of chapters embracing 
 the principles of modern chemistry, descriptions of the 
 apparatus employed, with practical instructions as to 
 the mode of using it, with special reference as to the 
 proper use of the blowpipe, and an exhaustive and 
 lucid description of the reactions by which the various 
 chemical substances may be recognized. 
 
 1* 
 
VI PUBLISHERS PREFACE. 
 
 To the student, the amateur mineralogist, the civil 
 engineer, the miner, the prospector, and all others to 
 whom a knowledge of mineralogy may be serviceable, 
 the book can be recommended as a most valuable 
 guide. 
 
 The lamented death of Dr. Erni, which occurred 
 while the present edition was passing through the 
 press, necessitated the publishers to place the correc- 
 tion of the proof-sheet in other hands. They secured 
 for this important work the services of a competent 
 critic ; and they believe that he has performed the duty 
 in a thoroughly satisfactory manner. 
 
 PHILADELPHIA, October 1, 1885. 
 
CONTENTS. 
 
 PART I. 
 CHAPTER T. 
 
 CHEMICAL PHILOSOPHY. 
 
 PAGE 
 
 The New or Unitary System of Chemistry, or Substitution 
 Theory ; Berzelian Theory ; The older Berzelian or Electro- 
 Chemical Theory founded upon Dualism, and known as the 
 Binary Theory . . . . ... , . .25 
 
 The discovery of substitution by Dumas and others ; Gay- 
 Lussac's law of Combination by Volume .. . . .26 
 
 Avogadro's law 27 
 
 Changes of Notation in the New Chemical System ; Acids and 
 
 Halogens 28 
 
 Acids; Oxygen Acids; Sulphur Acids; Hydrogen Acids; 
 Oxacids ; Hydracids ; Hydroxyl Acids .... 29 
 
 The Hydrogen Acids ; Sulphur Acids ; Oxygen Bases ; Bases 30 
 Hydrates and Oxides of Metals ...... 31 
 
 Salts; Normal (Neutral) Salts; Acid Salts; Basic Salts 32 
 Acid Salts ; Basic Salts; Double Salts; Quantivalence ; Va- 
 lence, or Atomicity of Elements ..... 33 
 
 Indices of Valence, .Bonds of Attraction or Linking of Atoms; 
 
 Varying Valence in the same element ; Gerhardt's Residues 34 
 Tables of Atomic Weights of the elements according to the New 
 
 System 30 
 
 CHAPTER II. 
 
 AUXILIARY APPARATUS AND MANIPULATIONS IN THE 
 LABORATORY. 
 
 Pulverization 38 
 
 Solution and Carbon Dioxide (CO 2 ) Test .... 40 
 Precipitation and Decantation 41 
 
Vlll CONTENTS. 
 
 PAGE 
 
 Filtration . . . . . . . . .43 
 
 Washing Precipitates 45 
 
 Evaporation .......... 46 
 
 Porcelain Dishes and Crucibles ; Platinum Apparatus ; Cru- 
 cibles, Dishes, or Capsules ....... 48 
 
 Crucible Tongs . . . . . . . .49 
 
 Corks 50 
 
 Sand-bath; Wire Gauze; Triangular Supports for Crucibles . 51 
 
 Fletcher's Burners 53 
 
 Foot Blowers 55 
 
 Bending and Closing Glass Tubes ...... 56 
 
 CHAPTER III. 
 
 PREPARATION OF REAGENTS MOST FREQUENTLY REQUIRED FOR 
 ANALYSIS IN THE WET WAY. 
 
 Chemically Pure Water, H 2 O 59 
 
 Testing Water 62 
 
 Preparation of Test Papers ; Blue Litmus Paper ; Reddened 
 
 Litmus Paper ; Turmeric Paper ..... 63 
 Hydric Sulphide ; Sulphohydric Acid ; Sulphuretted Hydrogen, 
 
 H 2 S . . . . . . . 64 
 
 Sulphide of Ammonium (NH 4 ) 2 S ; Hydrofluoric Acid, HF1. 66 
 Wet Reagents generally. Water, H 2 O . . . .67 
 
 CHAPTER IV. 
 
 BLOWPIPE ANALYSIS AND APPARATUS. 
 
 The Mouth Blowpipe . . . . . . -'.. 69 
 
 Using the Blowpipe . . . . 71 
 
 The Blowpipe Flame . . . % .. . . . 72 
 
 Supports for the Assay. Charcoal ..... 75 
 
 Porcelain Supporters ; Aluminium Plate as a support in Blow- 
 pipe Analysis .... .... 76 
 
 Fuel Lamps, Stearine Candles, Olive Oil .... 78 
 
 Solid Fats ; Lamps filled with solid fats, such as Tallow, Paraf- 
 
 fine, etc. . . 80 
 
 Illuminating Gas ; Fixed Blowpipe and Blast Lamps . . 81 
 
 Automaton Blowpipes ; The Automaton Hand Blowpipe . 84 
 
 Fletcher's Improved Mouth Blowpipe . . ... 85 
 
CONTENTS. ix 
 
 PAGE 
 
 Fletcher's Hot-blast Blowpipe, 86 
 
 Platinum Apparatus and Appliances; Platinum Wire and 
 
 Spoons 87 
 
 Forceps with Platinum Points; Tubes of Hard Glass free from 
 
 Lead . . - 88 
 
 Closed Tubes and Glass Bulb Tubes or Matrasses, etc. ; Cut- 
 ting Pliers; Steel Magnet ; Magnetic Needle; Blowpipe Re- 
 agents 89 
 
 Preliminary Tests of Inorganic Solid Substances ... 91 
 
 CHAPTER V. 
 
 REACTION OF OXIDES WITH GENERAL REAGENTS. 
 
 Behavior of Metallic Oxides with Borax .... 94 
 Behavior of Metallic Oxides with Salt of Phosphorus . . 95 
 Examination of Minerals with Soda ..... 9G 
 Examination of Metals with Sodium Thiosulphate (hyposul- 
 phite of sodium), Na,S 2 O 3 98 
 
 Tabular Arrangement showing the behavior of Oxides when 
 treated before the Blowpipe with Sodium Thiosulphate, to- 
 gether with their Reactions with Borax ; Examination with 
 Acid Potassium Sulphate or Concentrated Sulphuric Acid . 99 
 A Colored Gas Evolved; A Colorless Odorous Gas Evolved . 100 
 A Colorless and Odorless Gas Evolved ; Examination with Zinc 
 and Hydrochloric Acid, after previous decomposition (fusion) 
 of the mineral ......... 101 
 
 Examination with Cobalt Solution . . . . .102 
 
 Table of the more definite Colorations caused by Cobalt solution 103 
 
 CHAPTER VI. 
 
 COLORED FLAMES, FLAME REACTIONS, AND SPECTRUM ANALYSIS. 
 
 Examination of the Assay in the Platinum Forceps for Flame 
 
 Coloration ......... 103 
 
 Table of the more definite Colorations ..... 104 
 
 Apparatus; Experiments ....... 105 
 
 Colors of the Flames produced with different absorptive media ; 
 
 A Blue, a Violet, a Red, and a Green Glass . . .106 
 Colors given by the Flame of Bunsen's Burner ; Testing Chemi- 
 cal Mixtures; Acids . 107 
 
 Alkalies 108 
 
X CONTENTS. 
 
 I' AGE 
 
 Alkaline Earths ; Copper 110 
 
 Bunsen's Flame Reactions ; Bunsen's Gas Lamp . . .111 
 Apparatus and Method employed for submitting Test substances 
 to the Flame ; Behavior of the Elements at High Tempera- 
 tures ... . . . . . . .112 
 
 Reagents .. . . . . . . . -. . .115 
 
 Methods of Examination ; Ignition of the Elements at High 
 Temperatures . . . . . . . . . .117 
 
 Oxidation and Reduction of substances ; Incrustations or Coat- 
 ings on Porcelain , . . . . .118 
 General Review of Flame Reactions '. . . . . . 120 
 
 Table of Volatile Elements which can be reduced as Films 
 or Coatings on Porcelain, arranged according to their Re- 
 actions ; Reducible to Metals, but yielding no Incrustations ; 
 Iron Compounds . . . . . . - . . 121 
 Nickel Compounds; Cobalt Compounds; Palladium Com- 
 pounds . . . . . .... .122 
 
 Platinum Compounds ; Iridium Compounds ; Rhodium Com- 
 pounds ; Osmium Compounds ; Gold Compounds ; Silver 
 Compounds . . . . . . .123 
 
 Copper Compounds ; Tin Compounds ; Elements which can 
 best be recognized from the Reactions of their Compounds ; 
 Molybdenum .- ... . . V . . 124 
 
 Tungsten (Wolfcamium) Compounds ; Titanium Compounds ; 
 Tantalum and Niobium Compounds ; Chromium Compounds ; 
 Vanadium Compounds . . . . . . ; . 125 
 
 Manganese Compounds ; Uranium Compounds ; Silicic Com- 
 pounds ; Phosphorus Compounds . . . . . 12G 
 
 Sulphur Compounds . . . . . . ... 127 
 
 Spectrum Analysis . . . . . . . .127 
 
 Spark Spectra ; Spectra of Permanent Gases *, 131 
 
 Spectrum Lines of the most important Flame-Coloring Elements 133 
 Solar and Stellar Chemistry . . . . . . .134 
 
 Stellar Chemistry . : . . 136 
 
 Spectroscope . . . . . . . " .' . 137 
 
 Measuring the Spectrum . . . . . . .138 
 
CONTKNTS. XI 
 
 CHAPTER VII. 
 
 SPECIAL METHODS FOR DETECTING CERTAIN ELEMENTS, OR SOME 
 OF THEIR COMBINATIONS WHEN PRESENT IN COMPLEX CHEMI- 
 CAL COMPOUNDS. 
 
 PAGE 
 
 Alumina . . . . . . . . 139 
 
 Ammonia .......... 140 
 
 Antimony . . .. . . . . . .141 
 
 Arsenic . . . . . . . . . . 144 
 
 Arsenic Spots ; Antimony Spots . . . . . . 145 
 
 Arsenic Mirror ; Antimony Mirror . . . . 146 
 
 Apparatus for Marsh's Tests . . . . . . .147 
 
 Test for Arsenic in Minerals containing no Sulphur, as Whit- 
 ney ite . 148 
 
 Baryta; Bismuth 150 
 
 Boric (Boracic) Acid 151 
 
 Cadmium . . . . . . . . . .153 
 
 Carbon 154 
 
 Cerium . . . . . . . . . .155 
 
 Chlorine 156 
 
 Chromium . . . . . . . . . .157 
 
 Cobalt '--'. . 150 
 
 Columbium or Niobium ; Copper . . . . . .160 
 
 Didymium 162 
 
 Erbium ; Fluorine . . . . . . . .163 
 
 (ilucina . . . . . . . . . .164 
 
 Gold H55 
 
 Iodine; Iridium . . . . . . . . .166 
 
 Iron 167 
 
 Lead 170 
 
 Lime . . . . . . . . . .171 
 
 Lithia 172 
 
 Magnesia . . . . . . . . . . 1 73 
 
 Deportment of the Alkaline Carbonates, with the Alkaline 
 
 Earths 174 
 
 Manganese 175 
 
 Mercury and Amalgams . . . . . . .177 
 
 Molybdenum 178 
 
 Nickel 180 
 
 Nitric Acid (Nitrates) ... .181 
 
XI 1 CONTENTS. 
 
 PAGE 
 
 Palladium ........ 132 
 
 Phosphoric Acid or Phosphates (Platinum) . . . .183 
 
 Potassium; Rhodium 184 
 
 Rubidium ; Ruthenium ; Selenium and Seleniurets ; Silicium, 
 
 Silicon, or the oxide, Silica . . . . . .185 
 
 Silver 186 
 
 Sodium ........ 188 
 
 Strontium; Sulphur . . 189 
 
 Tantalum; Tellurium ...... 191 
 
 Tin . 192 
 
 Separation of As, Sb, Sn 194 
 Titanium; Tungsten (Wolfram ram) . . , . .195 
 
 Uranium ' 197 
 
 Uranates ; Vanadium .... 199 
 
 Yttrium ...... 200 
 
 Zinc . 201 
 
 Zirconia ... . . . . 202 
 
 CHAPTER VIII. 
 
 FUSING AND FLUXING. 
 
 Deflagration. On the Use and Preservation of Platinum Vessels 205 
 
 PART II. 
 
 DETERMINATIVE MINERALOGY. 
 CHAPTER IX. 
 
 ON THE DETERMINATION OF MINERALS BY MEANS OF SIMPLE EX- 
 PERIMENTS WITH A BLOWPIPE AIDED BY HUMID ANALYSIS. 
 
 Introduction to the Tables 207 
 
 Lustre of the Mineral . . . . . . .208 
 
 Physical Properties of Minerals ; Lustre ; Fusibility . . 209 
 
 Hardness; Color 210 
 
 Streak; Specific gravity . 211 
 
 Professor Jolly's Spring Balance for determining the specific 
 gravity of Minerals . . . . . . .214 
 
CONTENTS. XI II 
 
 PAGE 
 
 Pyro-electricity 216 
 
 Optical Investigation of Minerals ; Crystallization . . .217 
 
 Systems of Crystallization ; Names used by different Authors . 218 
 Chemical Properties of Minerals ; Preliminary proceedings for 
 
 Testing and Properly Classifying them ; Example . . 219 
 
 Testing for Water . 220 
 
 Decomposition by Acids . . . . . . 221 
 
 Example ; Mineral species selected by von Kobell for the study 
 
 of Determinative Mineralogy ...... 222 
 
 French Weights and Measures ...... 223 
 
 Relations of the Scales of the Thermometers of Celsius (Centi- 
 grade), Reaumur, and Fahrenheit 224 
 
 KKY TO THE GENERAL CLASSIFICATION oil SYNOPSIS OF 
 
 THE TABLES ' .226 
 
 Group I. Minerals with Metallic Lustre .... 226 
 Group II. Minerals without Metallic Lustre . 227 
 
 Group I. Minerals with Metallic Lustre .... 230 
 
 Class I. Native Malleable Metals and Mercury . . . 230 
 Maldonite ; Native Silver ; Native Gold . . 230 
 
 Native Copper ; Native Lead ; Native Platinum ; Palla- 
 dium ; Native Iron ; Native Mercury . . .231 
 Class II. Fusibility from 1-5 or Easily Volatilized . . 232 
 Division 1 . B. B. on Coal Evolve the strong Odor of Arsenic 232 
 Native Arsenic ; Binnite ; Arsonomelane ; Jordanite ; 
 Dufienoysite ; Tennantite ; Polybasite ; Enargite ; 
 
 Rionite ; Domeykite 232 
 
 Rionite ; Enargite ; Dufrenoysite ; Tennantite ; Domey- 
 kite ; Algodonite ; Whitneyite ; Smaltite ; Skutteru- 
 
 dite; Cobaltite 233 
 
 Glaucodot ; Alloclasite ...... 234 
 
 Niccolite ; Cloanthite ; Gersdoiflite ; Corynite ; Wolf- 
 achite ; Arsenopyrite ...... 235 
 
 Division 2. B. B. on Coal, or in open Glass Tube, Evolve 
 
 the strong Horseradish Odor of Selenium . . 236 
 
 Guanajuatite (Frenzelite) ; Tiemannitc ; Lehrbachite ; 
 Guadalcazarite . . . . . . 236 
 
 C lausthalite ; Naumannite ; Berzelianitc (Seleniuret of 
 Copper) ; Raphanosmite (Seleniuret of Copper and 
 2 
 
XIV CONTENTS. 
 
 PAGE 
 
 Lead) ; Eucairite (Seleniuret of Silver and Copper) ; 
 
 Crookesite 237 
 
 Division 3. B. B. on Coal yield a whitish deposit, which 
 colors the reducing flame Greenish or Greenish-blue. 
 Impart to concentrated Sulphuric Acid, when gently 
 heated with it in a Test-tube, a Purple-red or Hya- 
 cinthine color, which, upon the addition of water, dis- 
 appears, while a Blackish-gray precipitate forms . 238 
 Native Tellurium ; Melonite ; Hessite ; Altaite . . 238 
 Muelleritc (aurotellurite) ; Tetradymite (Telluret of 
 Bismuth); Sylvanite ; Nagyagite .... 239 
 Division 4. B. B. on Charcoal evolve copious fumes of 
 
 Antimony 240 
 
 Native Antimony ; ' Stibnite ; Zinkenite ; Jamesonite ; 
 Bournonite ........ 240 
 
 Stylotypite ; -Zinkenite; Boulangerite ; Geocronite ; 
 Kilbrickenite ; Plagionite ; Meneghinite ; Dyscrasite; 
 Stephanite ; Tetrahedrite ; Antimonfahlerz . . 241 
 Miarygyrite ; Brogniardite ; Freieslebenite ; Diaphorite ; 
 
 Spaniolite; Chalcostibite . . . . . 242 
 
 Ullmannite ; Breithauptite ; Berthierite . . . 243 
 
 Division 5. Heated in an open Glass-tube give Sulphurous 
 
 Acid, which reddens a strip of moistened Blue Litmus 
 
 Paper placed in the end. B. B. with Soda give Hepar, 
 
 without presenting the general characters mentioned 
 
 in the preceding numbers 243 
 
 Argentite ; Jalpaite ; Acanthite 243 
 
 Alabandite ; Hauerite ; Cinnabar ; Galenite ; Cupro- 
 plumbite ; Huascolite ; Chalcocite ; Stromeyerite ; 
 Wittichenite ; Stannine ; Chalcopyrite ; Cuban ; Born- 
 
 ite 244 
 
 Belonite ; Saynite ; Cuproplumbite ; Pentlandite . 245 
 Chalcosite ; Carmenite; Digenite ; Cupreine ; Millerite; 
 
 Linneite; Pyrite . 246 
 
 Pyrrothite; Sternbergite 247 
 
 Bismuthinite . . . . . . . .248 
 
 Division 6. Not belonging to the preceding divisions . 248 
 Amalgam; Metacinnabarite ; Bismuth . . .248 
 
 Kabdionite; Haematite ; Cuprite; Magnetite; Horton- 
 olite ; Roepperite ; Fayalite ; Wolframite . . 249 
 
CONTENTS. XV 
 
 PAGE 
 
 Black Silicate ot Manganese ; Psilomelane ; Lievrite ; 
 
 Allanite; Plattnerite; Samarskite . . . .250 
 
 Class III. Infusible, or Fusibility above 5, and N on- volatile 251 
 Division 1. B. B. impart, in ever so small a quantity, to 
 the Borax Bead in the Oxidizing Flame an Amethys- 
 tine color of Manganese . . . 251 
 Lithiophorite ; Crednerite ; Braunite ; Hausmannite ; 
 Manganite . . . . . . '251 
 
 Psilomelane ; Pyrolusite . . . 252 
 
 Division 2. Are Magnetic, or B. B. when heated on Char- 
 coal perseveringly in the R. Fl. become so . . 252 
 Lolingite; Arsenopyrite ; Himnatite ; Franklinite ; Mag- 
 netite ; Jacobsite .... .252 
 
 Magnoferrite ; Menaccanite ; Limonite ; Sphalerite . 253 
 Division 3. Not included, but in some respects related to, 
 
 the preceding 254 
 
 ' Chromite ; Ferroilmenitc ; Molybdenite ; Graphite ; Per- 
 
 ofskite ... .254 
 
 Iridosimine ; Tantalite ; Columbite ; Yttrotantalite ; 
 
 Uranite ......... 255 
 
 Group II. Minerals without Metallic Lustre . . . . 256 
 
 Class I. Easily Volatile or Combustible .... 256 
 
 Native Sulphur ; Realgar ; Orpiment ; Arsenite ; 
 Valentinite ; Kermesite ; Senarmontite ; Sal Am- 
 moniac ; Mascagnite . . . . . 256 
 
 Cinnabar ; Calomel ; Cotunnite .... 257 
 
 Class II. Fuse easily between 1 and 5, and Volatilize only 
 
 partially or not at all ..... 258 
 
 Part A. B. B. Fused with Soda on Charcoal yield a metal- 
 lic globule, or, fused alone in the R. F., form a 
 mass which acts on the magnetic needle . . 258 
 Division 1. B. B. yield with Soda, or Soda and Borax 
 together, a silver globule. Those decomposable by 
 Nitric Acid yield, when this solution is treated 
 with Hydrochloric Acid, a white precipitate of 
 Chloride of Silver, which B. B. is easily reduced 
 on charcoal to metallic silver .... 258 
 
 Proustite ; Pyrargyrite ; Xanthoconite . . . 258 
 Cerargyritc ; lodyrite ; Embolite ; Selbite . . 259 
 
XVI CONTENTS. 
 
 PAGE 
 
 Division 2. B. B. with Soda yield a lead globule. The 
 compounds of this Group are soluble in Nitric 
 Acid ; Zinc precipitates metallic lead from the 
 solution ; Sulphuric Acid forms a heavy white 
 precipitate of Sulphate of Lead . . . 2GO 
 
 Bindheimite ; Nadorite ; Mimetite, Hedyphane ; 
 Pyromorphite ....... 260 
 
 Minium ; Crocoite ; Phoenicochroite, Pl.onicite ; I)e- 
 chenite ; Linarite ; Cerussite ; Lanarkite ; Phos- 
 genite 2G1 
 
 Leadhillite Susannite ; Anglesite ; Wulfenite ; 
 
 Stolzitc ; Vauquelinite ; Vanadinite ; Eusynchite 262 
 
 Descloizite ; Laxmannite ; Phosphochromite . 2G3 
 
 Division 3. Moistened with Hydrochloric Acid they 
 communicate to the Blowpipe Flame a transient 
 blue color; with Nitric Acid, form a sky-blue or 
 green solution, which becomes azure blue by the 
 addition of Ammonia in excess . . . 263 
 
 Section i. B. B. evolve a strong arsenical odor (and 
 generally give alone on coal a white, brittle me- 
 tallic globule of arsenical copper). Are of a green 
 color . . . . . . . . 2G4 
 
 Chenevixite ; Bayldonite ; Olivenite ; Abichite ; 
 Tyrolite ; Chalcophyllite ; Conichalcite ; Liro- 
 conite ........ 264 
 
 Euchroite ; Erinite ; Cornwallite . . .265 
 
 Section ii. B. B. evolve no arsenical odor, but gener- 
 ally give alone on coal a malleable globule of copper 265 
 
 Atacamite; Tallingite; Percylite; Nantokite; Chal- 
 canthite ; Brochantite 265 
 
 Langite ; Pisanite ; Cuprite ; Black Copper ore ; 
 Tcnosite ; Malachite; Azurite ; Mysorine ; Auri- 
 chalcite; Buratite 266 
 
 Libethenite ; Lunnite ; Ehlite ; Tagilite ; Torbern- 
 
 ite; Volborthite 267 
 
 Division 4. B. B. impart to a Borax Bead a fine sap- 
 phire blue color (Cobalt) 268 
 
 Erythrite ; Annabergite, Nickelbluethe ; Hetero- 
 genite ........ 268 
 
CONTENTS. XV11 
 
 PAGE 
 
 Division 5. Fused B. B. in the forceps or on coal in the 
 reduction flame, yield a black mass which acts 
 upon the magnetic needle (this includes none con- 
 tained in the preceding divisions) . 268 
 Section i. Evolve when fused upon coal strong arseni- 
 cal odor . . . 268 
 
 Pitticite; Pharmacosiderite ; Scorodite . 268 
 
 Arseniosiderite ; Morenosite 269 
 
 Section ii. Soluble in HC1 without perceptible resi- 
 due, and without gelatinizing. (Evolve B. B. no 
 arsenical odor when fused on Ch.) . . 269 
 
 Ludwigite ; Sussexite ; Rabdionite ; Pettkoite ; Me- 
 lanterite; Botryogen . 269 
 
 Melanterite; Coquimbite ; Roemerite; Jarosite ; 
 Fibroferrite ; Copiapite ; Raimondite ; Pastreite; 
 Carphosiderite ; Voltaite ; Siderite ; Hureaulite ; 
 Triplite ... 270 
 
 Sarcopside ; Triphylite ; Diadochite ; Vivianite ; 
 Dufrenite; Cacoxenite . .271 
 
 Beraunite; Hematite . .272 
 
 Section iii. With hydrochloric acid form a jelly, or are 
 
 decomposed with separation of silica . .272 
 
 Cronstedtite . . . .272 
 
 Chalcodite ; Voigtite ; Ekmannite ; Euralite ; Pa- 
 lagonite ; Lievrite ; Allanite ; Fayalite ; Horton- 
 olite ... .273 
 
 Knebelite; RSpperite; Pyrosmalite; Astrophyllite; 
 
 Lepidomelanc ; Allochroite ; Gillingite ; Xylotile 274 
 Section i v. Only slightly attacked by hydrochloric acid 2 75 
 
 Crocidolite; Arfvedsonite ; Glauconite ; Selado- 
 nite ; Acmite ; Babingtonite ; Almandite ; Wolf- 
 ramite ; Ferberite . . . . . .275 
 
 Mcgabasite ; Rhodonite; Lepidolite . .276 
 
 Division 6. Not included in the foregoing divisions . 276 
 
 Molybdite ; Eulytite ; Silicate of Bismuth ; Bis- 
 
 mutite ; Pucherite 276 
 
 Part B. B. B. Fused with Soda on coal yield no metallic 
 globule, or fused alone in the R. F. do not act on . 
 the magnetic needle . . . .277 
 
 2* 
 
CONTENTS. 
 
 PAGE 
 
 Division 1. After fusion and continued ignition on coal 
 in the forceps or the platinum spoon, give an alka- 
 line reaction, turning moistened red litmus paper 
 blue; and yellow turmeric paper brown. The 
 assay must be employed in splinters and not in 
 powder form . '.- . . . .277 
 Section i. In water easily and perfectly soluble . .277 
 
 Nitrate of Potassium ; Nitratine; Sodium Carbon- 
 ate ; Thermonatrite ; Trona or Sesquicarbonate of 
 Sodium . ; . . . .' . 277 
 
 Mirabilite ; Thenardite ; Aphthitalite ; Epsomite ; 
 Kalinite; Tachhydrite ...... 278 
 
 Carnallite; Halite; Borax' . . . 279 
 
 Section ii. Insoluble in water, or dissolving with dif- 
 ficulty . . > ..... 279 
 
 Ulexite . . . . I . ,. . . 279 
 
 Gay-lussite ; Witherite ; Staffelite ; Anhydrite ; 
 
 Gypsum; Polyhalite ; Brongniartine .' . 280 
 
 Anhydrite and Gypsum ; Syngenite ; Barite ; Celes- 
 tite ; Fluorite ; Cryolite ; Pharmaeolite . . 281 
 
 Chiolite ; ' Pachnolite ; Arksutite ; Chodneffite ; 
 
 Thomsenolitc ; Gearksutite ; Cancrinite . . 282 
 Division 2. Soluble in Hydrochloric Acid ; some also in 
 water without perceptible residue ; the solution 
 does not form a gelatinous mass -. . . 282 
 
 Durangite ; Chondroarsenite ; Trogerite ; Walpurg- 
 ite ; Adamite ; Fauserite ; Tschermigite ; Kera- 
 mohalite ; Goslarite ; Struvite . . . 283 
 
 Sassolite ; Boracite ; Stassfurthite ; Hydroboracitc ; 
 Larderellite; Sussexite . -.-.-. . 284 
 
 Liineburgite ; Alabandite ; Hauerite ; Wagnerite ; 
 Apatite ; Kjerulfine ; Brushite ; Isoclasite ; Am- 
 blygonite ....... 285 
 
 Hebronite ; Autunite 286 
 
 Division 3. Are entirely soluble in Muriatic Acid, form- 
 ing a thick jelly upon partial evaporation . . 286 
 Section i. B. B. in a matrass afford water .- . 286 
 
 Datolite ; Edingtonite ; Natrolite ; Scolecite . 286 
 
 Mesolite; Phillipsite ; Gismondite ; Ittnerite . 287 
 
CONTENTS. XIX 
 
 PAGE 
 
 Section ii. B. B. in a matrass give none, or only traces 
 
 of water . . . . . 287 
 
 Tephorite ; Helvite ; Danalite . . 287 
 
 Hauynite (Hauyne) ; Lapis- Lazuli ; Lasurstein; 
 Nosite ; Scolopsite ; Socialite ; Eudialyte ; Wollas- 
 tonite ; Nephelite . . 288 
 
 Meionite; Melilite ; Barsowite ; Tachylite . . 289 
 Division 4. Dissolve in Hydrochloric Acid, the Silicic 
 
 Acid separating without forming a perfect jelly . 289 
 
 Section i. B. B. in a matrass afford water . 289 
 
 Klipsteinite '. .289 
 
 Apophyllite; Pectolite ; Okenite; Analcite; Pyro- 
 
 sclerite ; Chonicrite ; Jollyte .... 290 
 
 Vermiculite ; Jefferisite ; Mosandrite ; Catapleiite ; 
 Brewstrite ; Stilbite ; Hipostilbite ; Chabazite ; 
 Prehnite ..... .291 
 
 Stilbite ; Mordenite ; Sepiolite ; Deweylite ; Sorda- 
 
 valite . . .292 
 
 Section ii. B. B. in a matrass yield no water, or only 
 
 a trace 292 
 
 Lapis- Lazuli ; Cryophyllite ; Tachylite . 292 
 
 Schorlomite ; Wernerite ; Porcellanite ; Wohlerite ; 
 
 Labradorite ; Anorthite 293 
 
 Grossularite ... .294 
 Division 5. Are only slightly attacked by Hydrochloric 
 Acid, and B. B. impart to borax glass the deep 
 amethystine color of manganese . . . 294 
 Carpholite ; Spessartite . . . . .294 
 Piedmontite ; Rhodonite; Richterite . . .295 
 Division 6. Not included in the preceding divisions. 
 The remaining minerals are all Silicates, except 
 Scheclite, which are not attacked, or are imper- 
 fectly decomposed by Hydrochloric Acid . . 295 
 Danburite; Howlite ; Scheelite . . . 295 
 Lepidolite ; Cookeite ; Thermophyllite ; Euphyllite ; 
 Margarite; Emerylite ; Muscovite; Biotite ; 
 Gumbelite ; Petalite ; Spodumene . . 296 
 Castor; Leucophanite ; Wilspnite ; Nohlite ; Dial- 
 lage 297 
 
XXM CONTENTS. 
 
 PAGE 
 
 Scheelite ; Cassiterite ; Octabedrite ; Brook ite ; ^Es- 
 
 chynitc 324 
 
 Euxenite ; Pyroehlore ; Opal; Xenotime . . 325 
 
 Section ii. Hardness 7, and above 7 .... 325 
 
 Quartz .325 
 
 Tridymite ; Cordierite ; Staurotite ; Beryl ; Euclase ; 
 
 Fhenacite; Zirconite 326 
 
 Topaz ; Uwarowite ; Spinel ; Pleonaste ; Gahnitc ; 
 
 Chlorospinel . . . ' . . .327 
 
 Dysulite ; Kreittonite > . . . . . .328 
 
 CARBON GROUP .... 328 
 
 Diamond . . . . . . . . . . 328 
 
 Mock diamonds 330 
 
 CHAPTER X. 
 
 CHARACTERISTIC BEHAVIOR OF THE MOST IMPORTANT ORES 
 BEFORE THE BLOWPIPE AND WITH SOLVENTS. 
 
 Ores of Antimony ........ 331 
 
 Native Antimony; Stibnite, Gray .Antimony, Antimony Sul- 
 phide; Berthierite ; Kermesite ...... 331 
 
 Ores of Arsenic ......... 332 
 
 Native Arsenic ; Orpiment, Yellow Arsenic Sulphide ; Realgar, 
 
 Red Arsenic Sulphide ; Arsenolite, White Arsenic . . 332 
 
 Ores of Bismuth 333 
 
 Native Bismuth ; Tetradymite ; Bismutite . . . . 333 
 
 Bismuthinite ; Bismite 334 
 
 Ores of Chromium ... . . . . . 334 
 
 Chromite (Chromic Iron) . . . . . . . 334 
 
 Daubreelite . . 335 
 
 Ores of Cobalt 335 
 
 Smaltite ; Cobaltite ........ 335 
 
 Linnaeite; Erythrite ; Asbolite 336 
 
 Ores of Copper 336 
 
 Native Copper .336 
 
 Chalcopyrite ; Bornite ; Chalcocite ; Tetrahedrite . . 337 
 
 Domeykite ; Atacamite ; Cuprite 338 
 
 Malachite ; Azurite ; Chalcanthite ; Olivenite . . . 339 
 
 Tyrolite ; Chrysocolla 340 
 
CONTENTS. XX111 
 
 PAGE 
 
 Ores of Gold, Platinum, Indium, and Palladium . . . 341 
 
 Native Gold ; Calaverite 341 
 
 Krennerite ; Sylvanite, or Graphic Tellurium; Nagyagite ; 
 
 Petzite ; Native Platinum 342 
 
 Platin-iridium ; Osmium ; Palladium ; Selenpalladite, or Allo- 
 
 palladium ; Torpezite . . . . . . . 343 
 
 Ores of Iron 343 
 
 Native Iron ; Meteoric Iron . . . . . . . 344 
 
 Limonite ; Brown Hematite ; Brown Ochre, Yellow Ochre ; 
 
 Brown and Yellow Clay Ironstone ; Bog Iron Ore; Gothite; 
 
 Turgite ; Hematite ........ 345 
 
 Specular Iron ; Micaceous Iron ; Red Hematite; Red Ochre ; 
 
 Red Chalk ; Jaspery Clay-iron ; Clay Ironstone ; Lenticular 
 
 Argillaceous Ore ; Martite ; Magnetite .... 346 
 
 Pyrite ; Marcasite ; Pyrrhotite . . . . . .347 
 
 Arsenopyrite ; Danaite ; Scorodite ; Iron Sinter; Menaccanite 348 
 
 Siderite; Melanterite 349 
 
 Vivianite ; Franklinite ....... 350 
 
 Ores of Lead . 350 
 
 Native Lead ; Galenite 350 
 
 Bournonite . . . . . . . . . 351 
 
 Cerussite ; Anglesite ; Minium ; Massicot . 352 
 Plumbogummite ; Crocoite ; Vauquelinite ; Stolzite, or Lead 
 
 Tungstate ; Wulfenite . . . . . . .353 
 
 Lanarkite ; Leadhillite ; Phosgenite ; Pyromorphite . .354 
 
 Ores of Manganese . . 354 
 
 Pyrolusite ; Hausmannite ; Braunite ..... 355 
 
 Manganite ; Psilomelane ; AVad ; Lampaditc ; Rhodochrosite 356 
 
 Rhodonite ; Franklinite . . . . . . . 357 
 
 Ores of Mercury 357 
 
 Native Mercury ; Native Amalgam . . . . .357 
 Cerargyrite ; Cinnabar ; Metacinnabarite ; Guadalcazarite ; 
 
 Mercury Iodide ; Tiemannite ; Coloradoite ; Magnolite . 358 
 
 Ores of Nickel . . 359 
 
 Nicolite (Copper Nickel ; Arsenical Nickel) ; Breithauptite or 
 
 Antimonial Nickel ; Gersdorffite ; Ullmannite . . .359 
 
 Grunanite ; Millerite ; Zaratite ; Annabergite . . . 360 
 Morenosite; Lindackerite ; Remingtonite ; Genthite; Rottisite; 
 
 Primetite ; Alipite 361 
 
XXIV CONTKNTS. 
 
 PAGE 
 
 Ores of Silver 3d 
 
 Native Silver * . . . . 3G1 
 
 Argentite ; Acanthite ; Stromeyerite ; Sternbergite ; Naunum- 
 
 nite ; Cerargyrite 362 
 
 Embolite ; Bromyrite ; lodyrite ; Hessite . . . .363 
 Petzite ; Tapaltite ; Sylvanite : Eucairite ; Dyscrasite ; Pyrar- 
 
 gyrite ; Proustite ........ 364 
 
 Stephanite ; Polybasite ; Miargyrite ; Brongniardite . . 365 
 
 Polyargyrite ; Freieslebenite ; Pyrostilpnite .... 366 
 
 Ores of Tin ......... 366 
 
 Cassiterite (Tin Ore, Tin Oxide) ; Stannite .... 366 
 
 Ores of Zinc' . 367 
 
 Zincite ; Red Zinc Ore ; Red Zinc Oxide ; Sphalerite . . 367 
 Smithsonite ; Calamine ; Willemite . . . . .068 
 
 APPENDIX. 
 
 Carbonaceous Compounds . . . . . . .369 
 
 Graphite (Plumbago) ; Anthracite; Bituminous Coal . . 36'J 
 Brown Coal ; Asphaltum ....... 370 
 
 Albertite ; Grahamite ; Amber . . . . . .371 
 
 Elaterite ; Retim'te or Retinasphalt ; Hatchettine ; Ozocerite 372 
 
 Petroleum 372 
 
 Petroleum Benzine ; Coal-tar Naphtha or Benzole . . 374 
 
 Detection of small quantities of Nitrogen in Organic Compounds 375 
 
 INDEX 377 
 
MINERALOGY SIMPLIFIED. 
 
 PART I. 
 
 CHAPTER I. 
 
 CHEMICAL PHILOSOPHY. 
 
 The New or Unitary System of Chemistry, or Substitution 
 Theory. 
 
 THIS term Gerhardt applied to his system of notation, 
 based on the reduction of all formulae to one common standard, 
 they being derived one from the other by substitution. 
 
 BERZELIAN THEORY. 
 
 The older Berzelian or electro-chemical theory being founded 
 upon dualism, whence it is also known as binary theory. Ac- 
 cording to this great chemist, each chemical combination, how- 
 ever complicated, contained two integrant parts either single 
 or compound both being as it were in opposition to one another. 
 Chemical affinity,* or attraction, would result from this oppo- 
 sition between two contrary forces always striving to neutralize 
 each other, and these opposing forces, controlling all chemical 
 
 * Not to be confounded with quantivalence. Affinity is the force 
 by which one atom attracts another. An element may have a strong 
 affinity for other elements and yet be univalent. Another may pos- 
 sess ;i weak affinity and yet be quadrivalent. Chlorine has a strong 
 affinity for hydrogen, yet they both are univalent elements. 
 
 a 
 
26 MINERALOGY SIMPLIFIED. 
 
 phenomena, were assumed to be of an electrical nature. 
 There are two electric fluids, a negative and a positive one, 
 hence every compound contained, according to Berzelius, an 
 electro-positive (basic, basylic), and an electro-negative (acid) 
 constituent. 
 
 Thus nitric acid was represented by the formula N 2 O 5 H 2 O ; 
 it was a combination of the second order, nitric acid anhydride 
 N 2 O 6 forming the electro-negative, water = H 2 0, the 
 electro-positive constituent. 
 
 In the nitrate salts we find this nitric acid united to an oxide, 
 e. g., KO,N 2 O 5 . Nitrate of potassa (saltpetre). To halve tire 
 formula N 2 O 6 ,H 2 0, as is done at present, viz., HNO 3 , would be 
 like attempting to destroy the very foundation of the old BER- 
 
 ZELIAN THEORY. 
 
 The discovery of substitution by Dumas and others struck 
 a death-blow at the electrical theory. It was found that the 
 most opposite elements, like chlorine and hydrogen, could 
 replace one another in a compound without altering its chemi- 
 cal nature, or its characteristic general properties. 
 
 Thus in the marsh gas= CH 4 , the four atoms of hydrogen 
 can gradually be substituted by chlorine, so that the following 
 substitution products were actually obtained : 
 
 C IV H 4 ; C IV H 3 C1; C IV H 2 C1 2 ; C IV HC1 3 ; C IV C1 4 . 
 
 Gay-Lussac's Law of Combination by Volume. 
 
 If Dalton succeeded in placing the laws of chemical com- 
 bination on a firm basis, to Gay-Lussac belongs the honor of 
 having discovered the law regulating the combination of gases 
 by volume. It was in 1805 that Gay-Lussac and A. Humboldt 
 found, by actual experiment, that 1 volume of oxygen gas 
 unites with exactly 2 volumes of hydrogen, to form 2 volumes 
 of water-gas or steam. 
 
 The molecules* of compound bodies in the gaseous state, 
 
 * A molecule is the smallest particle of a compound or element 
 that is capable of existence in a free state. Atoms are the indivisible 
 
CHEMICAL PHILOSOPHY. 27 
 
 both organic and inorganic, with a few exceptions, probably 
 only apparent, occupy twice the volume of an atom of hydro- 
 gen. No matter what may be the number of atoms, or volumes, 
 that enter into the compound, they all become condensed into 
 2 volumes, thus : 
 
 1 volume (1 atom) of hydrogen and 1 volume of chlorine 
 form 2 volumes of hydrochloric acid = HC1. 
 
 2 volumes (2 atoms) of hydrogen and 1 volume of oxygen 
 form 2 volumes of water-gas or steam = H 2 0. 
 
 3 volumes (3 atoms) of hydrogen and 1 volume of nitrogen 
 form 2 volumes of ammonia = H 3 N, etc. etc. 
 
 Another law, enunciated by Gay-Lussac, states that the 
 weights of the combining volumes of the gaseous elements bear 
 a simple ratio to their atomic weights. Thus, taking the unit 
 volume of hydrogen gas to weigh = 1, as the lightest sub- 
 stance known, we find that 
 
 The unit volume of nitrogen gas weighs, 14.01 
 " " oxygen " " 15. 9G 
 
 " " chlorine " " 35.37 
 
 " " bromine " " 79.70 
 
 " " iodine " " 126.54 
 
 and these numbers are identical with the atomic weights of 
 these elements. In other words, nitrogen is 14.01, and oxygen 
 15.96 times (nearly 16) as heavy as hydrogen, etc. etc. 
 
 Avogadro's Law. 
 
 From Gay-Lussac's fundamental law, and the great law of 
 Avogadro, that all substances in the condition of gases, under 
 like circumstances of temperature and pressure, contain in 
 equal volumes the same number of atoms, it follows that the 
 formula of water is not HO as formerly expressed, when the 
 
 constituents of molecules. They are the smallest particles that can 
 take part in chemical reactions, and most of them are incapable of 
 existence in the free state but are found in combination with other 
 atoms, either of the same kind or of different kinds. 
 
28 MINERALOGY SIMPLIFIED. 
 
 combining weight of oxygen was =8 (hydrogen taken as unit 
 = 1), but H 2 O, whence the atomic weight of oxygen (that of 
 1 atom = 1 volume of hydrogen taken as 1) must be 16. 
 
 Changes of Notation in the New Chemical System. 
 
 The following changes, induced by the new system of chem- 
 istry, must be remembered by the student. 
 
 1. The doubling of all the atomic weights, except those of 
 the monad or univalent elements (H, Cl, K, Na, etc.), and 
 also of Bi, As, Sb, N, P, and Bo, whose oxides are now written 
 Bi 2 O 3 , instead of Bi() 3 , etc. etc. Corresponding to this change 
 of binary compounds, involving the monad elements, as in the 
 case of water cited, are written H 2 O instead of HO, Na 2 O for 
 NaO, Na 2 S for NaS, etc.; also CaCl 2 instead of CaCl, SiF 4 
 instead of SiF 2 , etc. 
 
 2. The method of viewing the composition of ternary com- 
 pounds. (See Acids and Salts.) 
 
 The name " acid," in its former acceptation and significance, 
 is not necessary, if not absolutely wrong in teaching chemistry. 
 Modern chemistry gives the following definition of an acid. 
 
 ]. Acids and Halogens, viz., Chlorine, Bromine, Iodine, 
 and Fluorine. 
 
 The properties which characterize acids are the following : 
 
 1. They have an acid or sour taste. 
 
 2. They turn blue litmus red. 
 
 3." They act upon metals, hydrogen being evolved, and its 
 place being taken by the metals, the products obtained are 
 called SALTS. For instance : 
 
 2(HC1) + Zn = ZnCl 2 + 2H. 
 
 Hydrochloric Zinc. Zinc Hydrogen, 
 
 acid. chloride. 
 
 U 2 SO 4 -f Mn == MnSO 4 + 211. 
 
 Sulphuric Maiignne.se. Manganese Hydrogen, 
 
 acid. sulphate. 
 
 4. They act upon metallic hydroxides, forming neutral sub- 
 stances and water, as follows : 
 
HC1 + KOH 
 
 Hydrochloric Potassium 
 acid. hydroxide. 
 
 = KC1 + 
 
 Pofassium 
 chloride. 
 
 HN0 3 
 
 Nitric acid. 
 
 + NaOII 
 
 Sodium 
 hydroxide. 
 
 = NaNO 3 
 
 Sodium 
 nitrate. 
 
 H.SO, - 
 
 Sulphuric 
 acid. 
 
 h Ca(OH), 
 
 Calcium 
 hydroxide. 
 
 = CaS0 4 
 
 Calcium 
 
 sulphate. 
 
 CHEMICAL PHILOSOPHY. 29 
 
 H,0. 
 
 H,0. 
 
 2H 2 O. 
 
 ACIDS are divided into 
 
 a. OXYGEN ACIDS. 
 
 b. SULPHUR ACIDS, and 
 
 c. HYDROGEN ACTDS. 
 
 An acid may be looked upon as a salt of hydrogen. It con- 
 sists of an acid radical (either simple or compound) united 
 with hydrogen, which latter can be exchanged for a metal, 
 this being then the formation of a regular salt. The hydrogen 
 is the base of the acid, as the metal is the base of the salt. 
 Sulphuric acid, for instance, is sometimes written hydrogen 
 sulphate = H 2 SO 4 . 
 
 All acids contain hydrogen. 
 
 Oxacids are those whose radicals contain oxygen, as HNO 3 , 
 nitric acid. 
 
 Hydracids are those whose radicals contain no oxygen, as 
 HC1, hydrochloric acid, H 2 S, sulphydric acid, etc. The an- 
 hydride of an oxacid is what remains after removing from the 
 acid its basic hydrogen and enough oxygen to form water with 
 the hydrogen. The anhydride of H 2 SO 4 is SO 3 . That of car- 
 bonic acid = H 2 CO 3 is CO 2 . Acids that contain but 1 atom 
 of basic H are termed monobasic, as HNO 3 and HC1 ; those 
 with 2 atoms of replaceable hydrogen, dibasic, as H 2 8O 4 ; those 
 with 3 atoms H, tribasic, as II 3 PO 4 (phosphoric acid) ; those 
 with 4 atoms H, tetrabasic, as H 4 SiO 4 , silicic acid. 
 
 HYDROXYL ACIDS. In those acids which consist of hydro- 
 gen and an acid or negative radical of greater or less complexity, 
 e. y., HNO 3 , H 2 SO 4 , H 3 PO 4 (oxygen being nearly always a 
 
 3* 
 
30 MINERALOGY SIMPLIFIED. 
 
 constituent of said radical, sulphur only in few cases), it is be- 
 lieved that their radicals are united to hydrogen by means of 
 oxygen. In other words, the oxacids are compounds of nega- 
 tive radicals with hydroxyl (OH). They are acid hydroxides. 
 The above-mentioned acids would thus have the formulae : 
 
 (NO,)' (OH) ; (SO,)" (OH),; (PO)'" (OH) 3 ; 
 or still more definite, 
 
 H-CK / OH 
 
 H O NO,, \SO 2 ; PO OH 
 
 \OH 
 
 THE HYDROGEN ACIDS are formed by the combination of 
 tne halogens with hydrogen. They neutralize oxygen bases 
 with formation of haloid salts and water, e. </., 
 
 Na,O + 2HC1 = 2NaCl + H 2 O. 
 
 Sodium Hydrochloric Sodium Water. 
 
 monoxide. acid. chloride. 
 
 SULPHUR ACIDS, like sulphydric acid = H 2 S, etc,, are hydro- 
 gen acids of the same chemical constitution. They combine 
 with sulphur bases, forming sulphur salts. For instance, potas- 
 sium hydrosulphide = K S H, etc. 
 
 OXYGEN BASES are compounds of basic (positive) radicals 
 with hydroxyl. In its relation to other bodies hydroxyl is 
 analogous to the simple halogen radicals, Cl, Br, I, F. 
 
 In a majority of cases oxygen acids may be formed by the 
 reaction of an anhydride, i. e., an oxide of an electro-negative 
 element upon water, e. </., 
 
 N 2 O 5 + H 3 O = 2(NO 2 OH) 
 
 Nitric pentoxide. Water. Nitric acid. 
 
 /OH 
 SO S + H,0 = SO,(OH), or SO / 
 
 Sulphur teroxide. Water. Sulphuric acid. ^-OH. 
 
 2. BASES. 
 
 Bases have properties which are opposite to those possessed 
 by acids. Those soluble in water turn reddened litmus paper 
 blue, and yellow turmeric paper brown. They all contain 
 
HYDRATES AND OXIDES OF METALS. 
 
 31 
 
 oxygen and hydrogen, and these elements are combined as 
 hydroxyl. 
 
 The oxygen bases, or basic hydroxides, may also result from 
 the action of an oxide of an electro-positive body upon water. 
 K 2 O + H 2 O 2KOH 
 
 Potassium monoxide. Water. Potassium hydroxide. 
 
 When oxygen acids act upon metallic oxides, or hydroxides, 
 the metal of the latter takes the place of hydrogen, and an 
 oxygen salt is formed, while at the same time water is pro- 
 duced, e. g., 
 
 + KOH = 
 
 NO 2 (OH) 
 
 NO S OK 
 
 H O. 
 
 Nitric acid. 
 
 Potassium 
 
 Potassium 
 
 Water. 
 
 
 hydroxide. 
 
 nitrate. 
 
 
 S0 2 (OH) 2 
 
 + K,O = 
 
 SO,(OK) f + 
 
 H 2 O, and 
 
 Sulphuric 
 
 Potassium 
 
 Potassium 
 
 Water. 
 
 acid. 
 
 monoxide. 
 
 sulphate 
 
 
 
 
 (normal salt). 
 
 
 S0 2 (OH) 2 
 
 + KOH = 
 
 o n /OH 
 
 SO *\OK + 
 
 H! O 
 
 Sulphuric 
 
 Potassium 
 
 Hydrogen 
 
 Water. 
 
 acid. 
 
 hydroxide. 
 
 potassium 
 
 
 sulphate (acid salt). 
 
 S 2\OH + 
 
 7n /OH 
 n \OH : 
 
 S .<o/ Zft - 
 
 h 2H 2 
 
 Sulphuric 
 
 Zinc 
 
 Zinc sulphate 
 
 Water. 
 
 acid. 
 
 hydroxide. 
 
 (normal salt). 
 
 
 
 
 Zn/ OH 
 
 
 SO <OH + 
 
 2 < Zn \OH) 
 
 \ y~vv 
 \ \J \ o/^l 
 
 = Zn// ! 
 
 + 2H,0 
 
 
 
 \OH 
 
 
 Sulphuric acid. 
 
 Zinc hydroxide. 
 
 Zinc sulphate 
 
 Water. 
 
 
 
 (basic salt). 
 
 
 HYDRATES AND OXIDES OF METALS. 
 
 According to the quantivalence of the metals with which 
 hydroxyl is combined, we have bases with one, two, three, etc., 
 hydroxyl groups in a molecule, e. g., 
 
 Na(OII), sodium hydroxide. A1(OH) 3 , aluminium hydroxide. 
 Ca(OH) 2 , calcium hydroxide. Cr(OH) 3 , chromium hydroxide. 
 Ba (OH),, barium hydroxide. Fe(OH) 6 , ferric hydroxide. 
 
32 MINERALOGY SIMPLIFIED. 
 
 3. SALTS. 
 
 Compounds formed by the action of acids upon bases are 
 called salts. 
 
 According to the new system, ternary substances are no 
 longer regarded as compounds of an "oxide" and a so-called 
 ** acid" but as compounds, for the most part, of the several 
 elements concerned, and hence a metal in a salt is believed to 
 be replaceable by another metal, and not an oxide by another. 
 The discovery of salts which contained neither an acid nor a 
 basic oxide, but only two single radicals like the common salt 
 = NaCl, was sufficient to eventually dispose of the old dualistic 
 
 a. NORMAL (neutral) SALTS are those in which the acid 
 and base saturate one another, in which, therefore, all the 
 hydroxyls, whether of acid or base, are eliminated (in the form 
 of water), and the acid radical remains united to the metal by 
 means of oxygen, e. g., potassium, nitrate, etc. 
 
 b. ACID SALTS are those which retain a part of the acid 
 hydroxyl, e. g., hydrogen potassium sulphate. 
 
 c. BASIC SALTS are those in which a part of the hydroxyl 
 of the base, or of the oxygen of the positive oxide, remains in 
 combination, e. g.. basic zinc sulphate. 
 
 The common form of sulphuric acid is di-basic ; sulphates 
 may therefore be acid, normal, or double salts. Let M stand 
 for a monad metal, and they may be represented thus graphi- 
 cally : 
 
 II\ ~ M) so M| M| so 
 
 H | "* Hf MJ mj " 
 
 Acid. Acid salt. Normal salt. Double salt. 
 
 Examples : 
 
 a. Normal Salts. 
 
 Potassium chlorate, KC1O 3 . 
 Calcium sulphate, Ca"SO 4 . 
 Bismuth phosphate, Bi'"PO 4 . 
 Sodium silicate, Na 2 SiO 3 . 
 
SALTS. 33 
 
 b. Acid Salts. 
 
 Hydro-sodium sulphite, HNaSO 3 . 
 Hydro-caesium carbonate, HCsCO 3 . 
 Hydro-barium phosphate, HBaPO 4 . 
 Hydro-cupric silicate, H 2 CuSiO 4 . 
 
 c. Basic Salts. 
 
 Lead hydro-nitrate, H(NO 2 )'PbO 2 . 
 Copper hydro-acetate, H(Ac) / CuO 2 . 
 Mercuric hydro-iodite, H(JO)'HgO 2 . 
 Alumic hydro-silicate, H 2 Si IY Al 2 O 6 . 
 
 d. Double Salts. 
 
 Potassio-sodium selenate, KNaSe0 4 . 
 Sodio- calcium antimonate, NaCa /r SbO 4 . 
 Bario-zincic silicate, Ba /r Zn r/ SiO 4 . 
 Csesio-rubidic carbonate, Cs'Rb r CO 3 . 
 
 Quantivalence, Valence, or Atomicity of Elements. 
 
 Every atom of an element has an inherent power of holding 
 in combination a certain number of other atoms, this number 
 being dependent upon the combining power of the atoms held 
 in combination. The simplest atoms would represent the unit 
 of this power, and we must distinguish between these simplest 
 or unit-atomicity and such as have the power of holding in 
 combination two, three, four, five, or more unit-atoms. 
 
 Bodies whose atomic capacity is 
 
 One, are termed Monads, Monatomic, Monadic, or Univalents. 
 Two " Dyads, Diatomic, Dyadic, or Bivalent. 
 
 Three " Triads, Triatomic, Triadic, or Trivalent. 
 Four " Tetrads, Tetratomic, Tetradic, or Quadriva- 
 
 lents. 
 Five " Pentads, Pentatomic, Pendadic, or Quinqui- 
 
 valents. 
 
 Six " Hexads, Hexatomic, Hexadic, or Sexivalent. 
 
 Seven " Heptads, Heptatomic, Heptadic, or Septiva- 
 
 lent. 
 
34 MINERALOGY SIMPLIFIED. 
 
 Elements of even valency, viz., the dyads, tetrads, and hex- 
 ads, are also included under the general term artiads, and those 
 of uneven valency, viz., the monads, triads, tetrads, and hex- 
 ads are designated as perissads. 
 
 4. Indices of Valence, Bonds of Attraction, or Linking of 
 Atoms. 
 
 The quantivalence of elements maybe expressed in different 
 ways, as follows : 
 
 Monads. Diads. Triads. Tetrads. Pentads. Hexads. 
 
 H 1 O n N ra C 1V N v Fe VI 
 
 Instead of these Roman numbers the valency is expressed 
 by dashes, e. g., S", Bi'", 8b'", $n"". In chemical formulas 
 each dash, either horizontal, vertical, or inclined, indicates a 
 " bond" or unit of valence, and implies chemical combination 
 between the atoms or groupings whose symbols are thus con- 
 nected. 
 
 The -f sign and period are employed to express " molecular 
 combination," i. e., combination not amenable to the generally 
 received quantivalence, as in the case of crystal water. 
 
 Varying Valence in the same Element. 
 
 Many elements are not limited to one of valence ; thus 
 nitrogen may act either as a trivalent or quinquivalent body, 
 etc., e. g., 
 
 Trivalent. Quinquivalent. 
 
 TT TT 
 
 H H 
 
 \N_C1. 
 
 i 
 
 Ammonia gas. Aimnonic chloride. 
 
 5. GERHARDT'S RESIDUES. 
 
 Most chemical compounds are more complicated than those 
 we have been hitherto considering. If we take any of the 
 following formula?, as, for instance, 
 
SALTS. 35 
 
 /H /^ 
 
 H Cl, H 0--H, N_H, and C<! 
 
 \ TT \ -H- 
 
 \H 
 
 and divide them at any part, we obtain two residues of equal 
 valence, e. g., if we divide H Cl we obtain H arid Cl, both 
 univalent ; if we divide H O H (water) we obtain H, and 
 the univalent residue OH (hydroxyl), which requires an uni- 
 valent atom to saturate it. If we divide 
 
 /H 
 
 N H, we obtain H and NH 2 , or H a and NH ; 
 \H 
 
 by the former division there are left two univalent, by the latter 
 
 /H 
 
 two bivalent factors. If we divide the formula C<^TT, the fol- 
 
 \ L 
 \H 
 
 lowing cases are possible : H and CH 3 , H 2 and CH 2 , H 3 and CH ; 
 leaving in the first case two univalent, in the second two biva- 
 lent, and in the third two trivalent residues. If we abstract 
 from H 3 SO 4 two atoms of hydrogen, we obtain a residue SO 4 , 
 acting like a bivalent radical ; again by taking away from HNO 3 
 the hydrogen, the residue NO 3 will act as a univalent radical. 
 The residue then may be considered as a radical of equal 
 atomicity as the sum of the atoms of basic hydrogen, eliminated 
 from the original compound radicals, viz., 
 
 ' HN0 3 , H 2 S0 4 , H 3 P0 4 , etc. 
 
36 
 
 MINERALOGY SIMPLIFIED. 
 
 Table of Atomic Weights of the Elements according to the 
 New System* 
 
 Name. 
 
 HYDROGEN 
 
 Symbol of the atoms, 
 
 their vale nee or 
 
 atomicity. 
 
 II 
 
 Aluminium 
 
 A1 m,vi 
 
 Antimony (Stibium) 
 Arsenic .... 
 
 Sb 111 ' v 
 As" 1 - v 
 
 Barium . . . 
 
 Ba 11 
 
 Beryllium or . 
 Glucinum 
 
 Be 11 or m 
 Gl n or m 
 
 Bismuth .... 
 
 Bi 111 ' v 
 
 Boron .... 
 Bromine . 
 
 Bo 111 ' v 
 
 g r l, III, V, VII 
 
 Cadmium 
 
 Cd" 
 
 Caesium .... 
 
 Cs 1 
 
 Calcium . 
 
 Ca 11 
 
 Carbon .... 
 
 QIV, II 
 
 Cerium .... 
 
 Ce"- VI 
 
 Chlorine .... 
 
 QI, III, V, VII 
 
 Chromium . 
 
 Cr iv,vi 
 
 Cobalt .... 
 
 Co"' IV 
 
 Columbium 
 
 Cb v 
 
 (Niobium) . 
 Copper (Cuprum) 
 Didymium 
 Erbium .... 
 
 Nb v 
 Cu" 
 Di IV 
 E" 
 
 Fluorine .... 
 
 F 1 
 
 Gallium .... 
 
 Ga IV 
 
 Gold(Aurum). 
 Hydrogen 
 
 Au 1 - 111 . 
 H' 
 
 Atomic weights or 
 
 combining weights. 
 
 H = 1. 
 
 If 
 
 27. 
 120. 
 
 75. 
 137. 
 
 208. 
 
 11. 
 
 80. 
 112. 
 133. 
 
 40. 
 
 12. 
 141.2 
 
 35.4 
 
 52. 
 
 59. 
 
 94. 
 
 63.2 
 142.2 
 166.0 
 
 19. 
 
 69. 
 
 196. 
 
 1. 
 
 * According to the latest determinations. 
 
 f The lightest of the elements, or the unit of the series 
 
TABLE OF ATOMIC WEIGHTS. 
 
 37 
 
 Table of Atomic Weights Continued. 
 
 Name. 
 
 Symbol of the atoms, 
 their valence or 
 atomicity. 
 
 Atomic weights or 
 cotabiuing weights. 
 H = l. 
 
 Indium .... 
 
 In 111 
 
 113.4 
 
 Iodine .... 
 
 JI, III, V, VII 
 
 127. 
 
 Iridiura .... 
 
 Jj.II, IV, VI 
 
 193. 
 
 Iron (Ferrum). 
 Lanthanum 
 
 p e ii, iv, vi 
 La IV 
 
 56. 
 138. 
 
 Lead (Plumbum) 
 Lithium . . . . 
 
 Pb ii,iv 
 Li 1 
 
 207. 
 
 7. 
 
 Magnesium 
 Manganese 
 Mercury (Hydrargyrum) . 
 Molybdenum . 
 Nickel .... 
 
 Mg n 
 
 Mn II,IY,YI,VII 
 
 Hg 
 
 Mo VI 
 Ni n,iv 
 
 24. 
 55. 
 200. 
 96. 
 58. 
 
 Nitrogen. 
 Osmium .... 
 
 ^m,v 
 
 Q S II, IV, VI, VIII 
 
 14. 
 195. 
 
 Oxygen . . 
 Palladium 
 
 o 11 
 
 Pd. it, vi 
 
 16. 
 106. 
 
 Phosphorus 
 Platinum . 
 
 pin, v 
 
 Pfll, IV, VI 
 
 31. 
 195. 
 
 Potassium (Kalium) 
 Rhodium 
 
 K 1 
 
 Rh n,iv,vi 
 
 39. 
 104. 
 
 Rubidium 
 
 Rb 1 
 
 85.5 
 
 Ruthenium 
 
 R U H, IV, VI, VIII 
 
 103.5 
 
 Samarium 
 
 Sm 
 
 150. 
 
 Scandium 
 
 Sc 
 
 44. 
 
 Selenium 
 
 Se ii,iv,vi 
 
 79. 
 
 Silicon (Silicium) . 
 Silver (Argentum) . 
 Sodium (Natrium) . 
 Strontium 
 
 Si iy 
 Ag 1 
 Na 1 
 Sr 11 
 
 28. 
 108. 
 23. 
 
 87.5 
 
 Sulphur .... 
 Tantalum 
 
 gll, IV, VI 
 
 Ta v 
 
 32. 
 
 182. 
 
 Tellurium 
 
 Tgii, iv, vi 
 
 125. 
 
 Terbium 
 
 Tb? 
 
 p. 
 
 Thallium 
 
 Ti 1 - m 
 
 204. 
 
 Thorium 
 
 Th iv 
 
 232. 
 
 .Tin (Stannum) 
 Titanium 
 
 Sn IV 
 Ti iv 
 
 118. 
 48. 
 
38 
 
 MINERALOGY SIMPLIFIED. 
 
 Table of Atomic Weights Concluded. 
 
 Name. 
 
 Symbol of the atoms, 
 their valence or 
 atomicity. 
 
 Atomic weights or 
 combining weights. 
 II = 1. 
 
 Tungsten (Wolframium) . 
 
 W IT 
 
 184. 
 
 Uranium .... 
 
 XJVI, IV 
 
 239. 
 
 Vanadium 
 
 yni, v 
 
 51. 
 
 Ytterbium 
 
 Yb m 
 
 173. 
 
 Yttrium .... 
 
 ym 
 
 89. 
 
 Zinc . . . 
 
 Zn 11 
 
 65. 
 
 Zirconium 
 
 Zi IV 
 
 90. 
 
 CHAPTER II. 
 
 AUXILIARY APPARATUS AND MANIPULATIONS IN THE 
 LABORATORY. 
 
 1. PULVERIZATION. 
 
 Minerals usually require preparation for the blowpipe, as 
 for solution, by pulverization. They may be broken in small 
 
 'Fig. 1. 
 
 Fig. 2. 
 
 pieces with a hammer, and then crushed in a diamond steel 
 mortar (Fig. 1), in which A is a rim removable from bottom 
 
PULVERIZATION. 
 
 B. Pestle G fits the rim closely, and is driven by a heavy 
 hammer into the rim upon the mineral. If repetition of this 
 process does not soon prepare the mineral for the blowpipe^ 
 grinding in an agate mortar (Fig. 3) may be resorted to, as is 
 generally necessary for solution. 
 
 Fig. 3. Fig. 4. 
 
 Some minerals may be sufficiently reduced by wrapping 
 them in strong, clean paper, and giving them a blow with a 
 hammer, taking care not to contract any impurity. A small 
 jeweller's steel hammer will answer for blowpiping, but for 
 trimming minerals and for geological and mining purposes, 
 larger and variously shaped steel hammers have been adopted 
 and are sold. 
 
 Fig. 4, a, 6, c, G?, represent four different forms of hammers. 
 
 , Freiberg's pattern, one end flat, the other pointed. 
 
 6, Hutchinson's form, sharpened on both ends for trimming. 
 
 c, von Buch's form, one end flat the other sharpened. 
 
 c?, Hausmann's pattern, botli ends sharpened. 
 
 Fig. 5. 
 
 Fig. 6. 
 
 Anvil. A square, flat piece of hardened steel answers well 
 for an anvil. 
 
40 
 
 MINERALOGY SIMPLIFIED. 
 
 Cutting pliers or nippers are useful for cutting off small 
 fragments from a mineral specimen. 
 
 Magnets. A small steel bar magnet (Fig. 5), and a small 
 compass (Fig. 6), or a suspended magnetic needle are needed 
 for recognizing magnetic metals. 
 
 Fig. 7. 
 
 A good magnifying glass (Fig. 7) is useful in examining 
 metallic sublimations or deposits. 
 
 2. SOLUTION AND CARBONIC DIOXIDE (CO 2 ) TEST. 
 
 In qualitative analysis small quantities are usually employed, 
 therefore the solution of solids may be most conveniently con- 
 ducted in a test-tube which can be readily heated over an alco- 
 hol lamp or a gas-burner. Figs. 8 and 9 show two forms of 
 
 Fig. 8. 
 
 Fig. 9. 
 
 racks with test-tubes. The latter has an attachment for filtra- 
 tion. If, in dissolving a substance, a colorless and inodorous 
 gas is evolved, the latter may be carbonic dioxide (CO 2 ), and 
 can be tested in the following simple manner : During evolution 
 of gas in tube a (Fig. 10), the lip of the tube may be brought 
 upon that of tube 5, containing clear lime-water. As the gas 
 
PRECIPITATION AND DECANTATION. 
 
 41 
 
 from tube a flows into tube 6, the water will become milky 
 from formation of calcium carbonate CaCO 3 . 
 
 Fig. 10. 
 
 Fig. 11. 
 
 Fig. 12. 
 
 Fig. 11 shows a metallic test-tube stand with test-tube ; and 
 Fig. 12 a test-tube holder of brass with wooden handle, both 
 employed for heating purposes. 
 
 3. PRECIPITATION AND DECANTATION. 
 
 Many circumstances are to be considered in deciding whether 
 a precipitate will be produced with a given reagent, such as 
 temperature, concentration, or dilution ; the presence of some 
 disturbing agent, or absence of a substance which might favor 
 the action by the influence of some affinity. Therefore a single 
 
 Fig. 13. 
 
 trial should not satisfy the student ; the experiment should be 
 varied, especially if resort be had to heat, agitation, and time. 
 The beaker (Fig. 13), made of Bohemian glass of uniform 
 thickness, and a test-tube, serve best for precipitation, the 
 
 4* 
 
42 
 
 MINERALOGY SIMPLIFIED. 
 
 Fig 
 
 liquid in the former being agitated by a glass rod. When the 
 precipitation is complete, the subsidence of the precipitate often 
 allows the mother liquor to be removed by decantation. 
 
 Precipitation of baryta, for example, may be readily sepa- 
 rated and washed without filtration. To avoid spilling in 
 decanting, a portion of the lip of the vessel should be smeared 
 internally and externally with tallow, and 
 then this portion brought against a glass 
 rod held obliquely, when the liquid will 
 flow gently down the rod without danger 
 of waste. 
 
 Figs. 14 and 15 show how a stream of 
 liquid flowing from a beaker or basin (por- 
 celain dish) should be guided by a glass 
 rod placed against the point whence the 
 stream emerges. If the vessel be too large 
 or too full to handle with convenience, the 
 wash-water may be drawn off by a siphon, 
 as shown in miniature in Fig. 16. A siphon is a tube of glass, 
 metal, gutta-percha, or India-rubber, bent in the form of a V 
 
 Fig. 15. 
 
 Fig. 16. 
 
 or U, filled with water, and inverted ; one end immersed in 
 the wash-water and the other allowed to hang over the side of 
 the vessel ; so long as the outer orifice of the instrument is below 
 the level of the liquid in the vessel, so long will that liquid 
 flow from within outwards until the vessel be empty. 
 
FILTRATION. 
 
 43 
 
 Fig. 17 represents a set (nest) of beakers without spout, all 
 of uniformly thin glass, bearing well the heating of liquids 
 which they contain, in a sand-bath or over a free fire. 
 
 Fig. 18 shows a set of beakers with spout. 
 
 Fig. 17. 
 
 Fte. 18. 
 
 Fig. 19. 
 
 Fig. 19 exhibits German flasks of white glass with long 
 neck and flat bottom, in which liquids may be boiled, or mine- 
 rals dissolved in acids, over a free fire. 
 
 4. FILTRATION. 
 
 Precipitates are generally separated from the mother-liquor 
 by filtration, as shown in Fig. 20, through paper expressly 
 prepared for the purpose (Swedish is best, but a cheaper article 
 answers for qualitative analysis). The paper, as seen in Fig. 
 21, is cut in a circular form, , then folded in the shape of a 
 quadrant, b and c, the pointed part finally placed deep in a 
 
44 
 
 MINERALOGY SIMPLIFIED. 
 
 glass funnel, and one of the folds, </, spread back so that the paper 
 completely lines the glass, though it must not quite reach the 
 top. When fitted, the paper is moistened by a jet of water to 
 
 Fig. 20. 
 
 Fig. 21. 
 
 Fig. 25 
 
 cause it to adhere to the glass. If a precipitate subsides, the 
 supernatant liquid should first be run through the filter by itself 
 (to accelerate filtration). 
 
FILTRATION. 
 
 45 
 
 Figs. 22 and 23 show additional forms of filtering stands. 
 The latter, being made of iron, can also be used as a retort-stand 
 in distillations. 
 
 Fig. 23. 
 
 Fig. 24. 
 
 Fig. 25. 
 
 Washing Precipitates. 
 
 Fig. 24 represents the ordinary wash-bottle for washing pre- 
 cipitates from the side of a filter by a jet of water, by compres- 
 sion of the air in the bottle, caused by blowing (see Fig. 25). 
 To test whether the washing has been complete, a drop of the 
 filtrate coming from the funnel is evaporated on a platinum 
 spatula ; if no solid residue remains behind, the operation must 
 be discontinued. 
 
 In Fig. 26 a platinum spatula is shown in its natural size, 
 
40 
 
 MINERALOGY SIMPLIFIED. 
 
 and Fig. 27 shows a convenient wooden holder for spatula, 
 wire, and spoon for heating operations. 
 
 Fig. 26. 
 
 Fig. 27. 
 
 Fig. 28. 
 
 Fig. 28 is a holder for platinum spoon and wire, with screw 
 fastening. The handle is hollow to contain wire and spoon, 
 screw cap. 
 
 5. EVAPORATION. 
 
 After filtration the mother-liquor becomes so much in- 
 creased by washing as often to require concentration before 
 being treated for substances yet in solution. Evaporation may 
 be conducted in a porcelain dish, either over a lamp or on the 
 sand-bath. Boiling should be avoided, and for this purpose 
 the dish can be securely placed upon a water-bath of copper 
 (about five inches in diameter), shown in Fig. 29, which is 
 provided with rings to receive dishes of different sizes, and is 
 supported by a tripod or a retort-stand. Being partly filled 
 
EVAPORATION. 
 
 47 
 
 with water, it is heated by a small alcohol lamp or a gas-burner. 
 To prevent dust from falling into the dish, it may be covered 
 with filter-paper (supported by a glass rod, or closely bent over 
 the edge of the dish). When the dish is nearly full, the sub- 
 
 Fig. 29. 
 
 Fig. 30. 
 
 Fig. 31. 
 
 stance may often be prevented from running over the margin 
 by slightly touching the latter with tallow. In evaporating to 
 dryness, the process is facilitated by stirring. Fig. 30 shows 
 a simple tripod of iron, and Fig. 31 is a tripod with chimney, 
 by Bunsen, to be used in connection with his gas-burner. A 
 
 Fig. 32. 
 
 square piece of iron-wire gauze is frequently put under dishes, 
 beakers, or flasks, heated on these tripods, or iron retort-stands, 
 to moderate the effect of the direct flame of a gas-burner. 
 Figs. 32 (1 and 2) are tripods witli rings of different sizes. 
 
48 MINERALOGY SIMPLIFIED. 
 
 6. PORCELAIN DISHES AND CRUCIBLES. 
 
 Open dishes, which will bear heat without cracking, are 
 necessary implements in the laboratory for conducting the 
 evaporation of liquids. The best evaporating dishes are those 
 made of Berlin porcelain, glazed both inside and out, with a 
 small lip projecting beyond the rim. 
 
 The dishes of Meissen porcelain are not glazed on the outside, 
 and are not so durable, but much cheaper than those of Berlin 
 manufacture. Evaporating dishes are made of all diameters 
 from 3 cm. to 15 cm. 
 
 A deep porcelain dish, provided with a handle (called cassa- 
 rol), is seen in Fig. 33. 
 
 Fig. 33. Fig. 34. 
 
 Very thin, highly glazed porcelain crucibles, with glazed 
 covers (Fig. 34), are indispensable implements to the chemist. 
 For most purposes the best sizes are those between 3 cm. and 
 5 cm. in diameter. Porcelain crucibles are supported over a 
 lamp on an iron-wire triangle. They must always be gradually 
 heated, and never come suddenly in contact with any cold 
 substance while they are hot. 
 
 7. PLATINUM APPARATUS : CRUCIBLES, DISHES, OR 
 CAPSULES. 
 
 Platinum does riot oxidize in the air at any temperature, nor 
 is it attacked by any of the common acids used separately. 
 
CRUCIBLE TONGS. 
 
 49 
 
 This comparative inertness as a chemical agent, taken in con- 
 nection with its infusibility, renders platinum an extremely 
 useful metal to the chemist. 
 
 It is employed in the laboratory for crucibles, evaporating 
 dishes, stills, spatulas, forceps, wire, blowpipe-tips, etc., and 
 lately in the shape of perforated cones for filtering phosphate 
 precipitates over a layer of asbestos wool.* When a filter-pump 
 is on hand, other insoluble precipitates collected on an ordi- 
 nary paper-filter may be quickly washed when placed in such 
 a cone, and the latter in a glass funnel. 
 
 Fig. 35. 
 
 Fig. 36. 
 
 Fig. 35 represents a platinum crucible with a capsule-shaped 
 lid, convenient for the incineration of filters, etc. Fig. 36 
 shows a platinum evaporating dish with lip. 
 
 8. CRUCIBLE TONGS. 
 
 The following three convenient forms -for removing hot 
 crucibles from the fire are generally found in laboratories. 
 Fig. 37 represents plain tongs of malleable iron. Fig. 38 
 
 Fig. 38. 
 
 * See Fresenius's Quantitative Analysis (New System). Second 
 American edition, by Allen & Johnson. New York, 1883. Pages 
 100 and 101. 
 5 
 
50 
 
 MINERALOGY SIMPLIFIED. 
 
 shows tongs with a double curve. Fig. 39 exhibits somewhat 
 expensive, but durable, crucible tongs, made of German silver 
 with platinum points attached. 
 
 Fig. 39. 
 
 Fig. 40. 
 
 9. CORKS. 
 
 For chemical purposes these should be made of soft cork- 
 wood cut across the grain to prevent forming continuous chan- 
 nels for the passage of gases or liquids. Pierced corks are used 
 to form joints with retorts, gas-bottles, and other chemical 
 apparatus. Boring holes through corks to receive glass tubes, 
 necks of retorts, etc., may be done with 
 a round file (rat-tail), or better, by a 
 hollow cylinder of sheet brass sharpened 
 .at one end. Fig. 40 represents a set of 
 cylinders of graduated sizes, slipping one 
 within the other into a very compact 
 form. A stout wire of the same length 
 as the cylinders accompanies the set, 
 which serves a double purpose ; passed 
 transversely through two holes in the cap 
 which terminates each cylinder, it gives 
 the hand a better grasp of the tool while 
 
 penetrating the cork; and when the hole is made, the wire 
 thrust through the opening in the top of the cap expels the 
 little cylinder of cork which else would remain in the cutting 
 cylinder of brass. 
 
 Rubber stoppers of flexible unvulcanized caoutchouc, cast in 
 moulds of various sizes, and provided with 1, 2, and 3 holes, 
 are now employed in laboratories instead of cork stoppers. 
 Fig. 41 represents different samples. These will not harden, 
 and sell for $4 per pound. Caoutchouc stoppers of good quality 
 are much more durable than corks, and are in every respect to 
 
SAND-BATH, WIRE GAUZE, ETC. 
 
 51 
 
 be preferred. Caoutchouc stoppers can be bored like corks by 
 means of suitable cutters, and glass tubes can be fitted into the 
 holes thus made with a tightness unattainable with corks. 
 Stoppers can be bought provided with all the necessary holes 
 of various sizes. 
 
 Fig. 41. 
 
 In Fig. 42 is seen a gas-bottle, fitted with Fig. 42. 
 perforated stopper, funnel-tube, and jointed 
 delivery-tube. 
 
 10. SAND-BATH, WIRE GAUZE, TRIANGULAR 
 SUPPORTS FOR CRUCIBLES. 
 
 As a general rule it is not best to apply the 
 direct flame to glass or porcelain vessels; hence 
 a piece of wire gauze is stretched loosely over 
 the largest ring of an iron stand, and bent 
 downward a little for the reception of round- 
 bottomed vessels. On this gauze, flasks, retorts, and porce- 
 lain dishes are usually supported. In cases requiring a very 
 gradual and equable heat the wire gauze 
 is replaced by a small sand-bath, i. e., a Fig. 43. 
 
 shallow sheet-iron pan filled with dry 
 sand (Fig. 43). Crucibles or dishes of 
 porcelain or platinum, too small for the 
 smallest ring belonging to the stand, are 
 
MINERALOGY SIMPLIFIED. 
 
 conveniently supported on an equilateral triangle made of three 
 pieces of soft iron, copper, or platinum wire, twisted together 
 at the apexes ; this triangle is laid on one of the rings of the 
 stand. An iron tripod (Fig. 30) may be often used instead of 
 a stand, but it is not so generally useful because of the difficulty 
 of adjusting it to various heights ; with a sufficiency of wooden 
 blocks wherewith to raise the lamp or the tripod as occasion 
 may require, it may be made available. The whole apparatus 
 for ignition, in its various arrangements, is plainly shown in 
 the following illustrations. 
 
 Fig. 44 shows an ordinary iron stand with two rings ; on the 
 upper one is placed a wire triangle, and on the lower one a 
 piece of wire gauze. 
 
 Fig. 45 exhibits two such wire triangles, a and b ; the latter, 
 ft, is covered with tobacco-pipe stems. 
 
 Fig. 44. 
 
 Fig. 46 is a support of iron with fork for holding a Bunsen 
 burner, with rubber gas-tube attached. The burner with 
 chimney heats a crucible, resting on a wire triangle. 
 
 In Fig. 47 is seen the burner by itself with a star screwed 
 on for the support of a chimney and an arrangement to slide 
 on the fork of the iron stand. 
 
 Fig. 48 shows a burner with a support screwed on for hold- 
 ing small porcelain dishes. 
 
FLETCHER'S BURNERS. 53 
 
 An ordinary plain Bunsen gas-burner is seen in Fig. 40. 
 Fig. 46. Fig. 47. 
 
 Fig. 48. 
 
 Fig. 49, 
 
 11. FLETCHER'S BURNERS. 
 
 Fig. 50. Fletcher's Blast-Bunsen for high temperatures. 
 This is a Bunsen combined with a powerful blowpipe, and is 
 one of the most generally useful arrangements known in the 
 chemical laboratory. The blowpipe flame obtained with the 
 blast tube, when confined by the loose cap B, is compact and 
 extremely powerful, owing to the fact that the air mixture is 
 partially made before the blast begins to act. When the object 
 to be heated is fragile it can be warmed by the Bunsen flame 
 
 5* 
 
M IN E R ALOG Y S I M PL I F I K 1). 
 
 Fig. 50. 
 
 and the blast slowly turned on by the tap c. The convenience 
 
 of having a powerful flame at command under an ordinary re r 
 
 tort- stand without the necessity of readjusting the height or 
 
 position will.be fully appreciated. 
 
 Fig. 51. Fletcher-Plat tner Blowpipe Furnace, for Capsules, 
 
 or Crucibles, J in. diameter. This is made of Fletcher's patent 
 non-conductor, which does not require 
 renewing, and does not require the ob- 
 jectionable wire support of Plattner's 
 pattern, which generally fails at the 
 most critical moment. This pattern, 
 like that of Plattner, has the hole for 
 the blowpipe flame at the side ; but if 
 the hole is at the bottom, and an up- 
 right blowpipe is used, the improve- 
 ment is very great. With the blast Bun- 
 sen (as shown in Fig. 50) and a good 
 foot blower, 100 grains of cast iron can 
 
 be perfectly fused in two minutes ; the temperatures being, at 
 
 the same time, under the most perfect control. 
 
 Fig. 51. 
 
 Fig. 52. 
 
 In Fig. 52 is seen Erlenmeyer's Argand Burner for heating 
 purposes. It has met with much favor among chemists for the 
 intense, steady heat it gives. It may be used for simple fusions 
 of silicates nearly as well as a blast lamp. 
 
FOOT BLOWERS. 
 
 12. FOOT BLOWERS. 
 
 Fig. 53 is a simple, compact, and powerful arrangement. 
 The step for the foot 
 
 is very low, and en- Fig- 53. 
 
 ables the blower to be 
 used with ease whether 
 the operator is stand- 
 ing or seated. The 
 pressure is perfectly 
 steady and equal. If 
 the rubber disk is dis- 
 tended until forced 
 against the net, the 
 pressure can be in- 
 
 Fig. 54. 
 
 Fig. 55. 
 
 creased to almost any extent desired. It will give, if required 
 
 a heavy and continuous blast through a pipe of inch clear bore. 
 
 A great advantage is obtained in blowpipe work by attach- 
 
56 MINERALOGY SIMPLIFIED. 
 
 ing a stopcock to the air-pipe, thereby controlling the blast as 
 with the mouth. With the blast Bunsen lamp. connected with 
 such a blower, small quantities of cast iron can be perfectly 
 fused in a few minutes. 
 
 Fig. 55, reversing the position of the blower, does away 
 with the risk of mechanical injury to the disk, and obviates 
 the necessity for a wood casing or protection. Tt also prevents 
 the valve from picking up dirt from the floor, keeping the 
 whole arrangement cleaner, and the valves in more perfect 
 order. 
 
 13. BENDING AND CLOSING GLASS TUBES. 
 
 Small bore tubing can generally be worked in the flame of a 
 common gas or spirit-lamp, or over an ordinary gas-burner ; for 
 larger tubes the blast-lamp is necessary (see Figs. 50 and 51). 
 Glass tubing must not be introduced suddenly into the hottest 
 part of the flame, or laid at once upon a cold surface. Gradual 
 heating and gradual cooling are alike necessary, and more so, 
 the thicker the glass is. In heating a tube, whether for bend- 
 ing, drawing-out, or closing, the tube must be constantly turned 
 between the fingers, and also moved a little to the right and 
 left in order that it may be uniformly heated all around, and 
 that the temperature of the neighboring parts may be duly 
 raised. If a tube or rod is to be heated at any part except an 
 end, it should be held between the thumb and the first two 
 fingers of each hand in such a manner that the hands shall be 
 below the tube or rod, with the palms upward, while the lamp- 
 flame is between the hands. When the end of a tube or rod 
 is to be heated, it is best to begin by warming the tube or rod 
 about 2 cm. from the end, and from thence proceed slowly to 
 the end. 
 
 In bending tubing to make gas delivery-tubes and the like, 
 attention should be paid to the following points : 1st, the glass 
 should be equally hot on all sides ; 2d, it should not be twisted, 
 pulled out, or pushed together, during the heating ; 3d, the 
 bore of the tube at the bend should be kept round and not 
 altered in size ; 4th, if two or more bends be made in the same 
 
BENDING AND CLOSING GLASS TUBES. 57 
 
 piece of tubing (Fig. 56), c and rf, they should all be in the 
 same plane, so that the finished tube will lie flat upon the level 
 table. 
 
 Fig. 56. 
 
 - p rn 
 
 I \J 
 
 When a tube or rod is to be bent or drawn close at its ex- 
 tremity, a temporary handle may be attached to it by softening 
 the end of the tube or rod, and pressing against the soft glass 
 a fragment of a glass tube which will adhere strongly to the 
 softened end. The handle may subsequently be removed by a, 
 slight blow, or by the aid of a file. 
 
 If a considerable, bend is to be made, so that the angle be- 
 tween the arms will be very acute, as in a siphon, for example 
 at a, Fig. 56, the curvature cannot be well produced at one place 
 in the tube, but should be made by heating, progressively, several 
 centimetres of the tube, and bending continuously from one end 
 of the heated portion to the other. Small and thick tubes may 
 be bent more sharply than large or thin tubes. In order to 
 draw a glass tube down to a finer bore, it is simply necessary 
 to thoroughly soften, on all sides, one or two centimetres' 
 length of the tube, and then, taking the glass from the flame, 
 to pull the tube by a cautious movement of the hands. The 
 larger the heated portion of the glass, the longer will be the 
 tube thus formed. Its length and fineness also increase with 
 the rapidity of motion of the hands. 
 
 To obtain a tube closed at one end, it is best to take a piece 
 of tubing open at both ends, and long enough to make two 
 closed tubes. In the middle of the tube a ring of glass, as 
 narrow as possible, must be made thoroughly soft. The hands 
 
58 MINERALOGY SIMPLIFIED. 
 
 are then separated a little to cause a contraction in diameter at 
 the hot and soft part. The point of the flame must now be 
 directed, not upon the narrowest part of the tube, but upon 
 what is to be the bottom of the closed tube. This point is in- 
 dicated by the line a in Fig. 57. By drawing with the right 
 
 Fi>. 57. 
 
 hand, the narrow part of the tube is attenuated, and finally 
 melted off, leaving both halves of the original tube closed at 
 one end, but not of the same form ; the right-hand half is drawn 
 out into a long point, the other is more roundly closed. It is 
 not possible to close handsomely the two pieces at once. The 
 tube is seldom perfectly finished by the operation ; a superfluous 
 knob of glass generally remains upon the end. If small, it may 
 be got rid of by heating the whole end of the tube, and blowing 
 moderately with the mouth into the open end. The knob being 
 hotter, and therefore softer than any other part, yields to the 
 pressure from within, spreads out and disappears. If the knob 
 is large it may be drawn off by sticking to it a fragment of a tube, 
 and then softening the glass above the junction. The same 
 process may be applied to the too pointed end of the right- 
 hand half of the original tube, or to any misshapen result of an 
 unsuccessful attempt to close a tube, or to any bit of tube 
 which is too short to make two closed tubes. When the closed 
 end of a tube is too thin, it may be strengthened by keeping 
 the whole end at a red heat for two or three minutes, turning 
 the tube constantly between the fingers. It may be said in 
 general of all the preceding operations before the lamp, that 
 success depends on keeping the tube to be heated in constant 
 rotation in order to secure a uniform temperature on all sides 
 of the tube. 
 
CHEMICALLY TURK WATER. 
 
 59 
 
 CHAPTER III. 
 
 PREPARATION OF REAGENTS MOST FREQUENTLY REQUIRED 
 FOR ANALYSIS IN THE WET WAY. 
 
 1. CHEMICALLY PURE WATER H 2 O. 
 
 THE first reagent which the private chemical student must 
 prepare for himself is chemically pure water. Clean rain-water, 
 or some other very pure water, may be rendered suitable for 
 many laboratory purposes by simply boiling and filtering. But 
 it is usually better to distil water, rejecting the first eighth 
 which goes over, and leaving a yet larger quantity in the retort 
 at the close of the distillation. The retort should always be 
 well washed before refilling. Water thus purified should be 
 preserved in closely stoppered demijohns or stone jars. One of 
 
 Fig. 58. 
 
 the best and most convenient distilling apparatus, is that of 
 Beindorf, represented in Fig. 58, for the use of pharmaceutists 
 and chemists, for distilling, rectifying, evaporating, cooking, ex- 
 tracting, drying, and similar chemical operations, besides melt- 
 ing. It consists of the following parts : a furnace of wrought 
 iron ; water-bath of copper, 5 gallons capacity and tinned in- 
 side ; a still of block tin, 1^ gallons capacity, with head of 
 
GO 
 
 MINERALOGY SIMPLIFIED. 
 
 block-tin, and having all the contrivances necessary for steam 
 distillations, etc., all made of pure block tin ; two evaporating 
 
 dishes ; two infusion jars ; a complete condenser of the latest 
 construction, etc. 
 
 Fig. 59 represents a heavy copper still with movable head, 
 and lined inside with tin coating; connected with a block-tin 
 
 
CHEMICALLY PUKE WATER. 
 
 61 
 
 condensing worm, inclosed in a zinc vessel, with inlet for cold 
 and outlet for the warm water. 
 
 For most purposes a glass retort (3 quarts) may be employed, 
 or the distilling apparatus shown in Fig. 60, in which h is a 
 
 
 large glass retort resting on an iron stand or on a small coal fur- 
 nace ; a is Liehig's condenser, with an iron foot, y ; b is a flask 
 used us a receiver, which may be placed upon a stand or block, 
 or if necessary in a bowl of cold water. The condenser, a, 
 consists of a copper tube through which a glass tube passes, 
 6 
 
62 
 
 MINERALOGY SIMPLIFIED. 
 
 fitting water-tight at the ends. Both ends of the glass-tube 
 are usually provided with corks, except at the connection 
 with the flask. Now if cold water (put ice in the supply- 
 vessel, if necessary) be allowed to flow continuously into the 
 funnel tube, e, the copper tube will be filled with cold water, 
 and the warm water will flow out at the top by the tube,/ 
 (which may be connected again with a rubber-tube, and the 
 water thus conveyed to a sink), whilst the aqueous vapor from 
 retort, ^, in passing through the glass tube will be condensed 
 
 and retained in receiver, b. 
 
 Fig. 61. 
 
 When a Liebig's condenser is not on hand, the distillation 
 of water may be executed in an ordinary glass-retort, to which 
 a flask is joined as condenser, being surrounded with cold 
 water (Fig. 61). 
 
 2. TESTING OF WATER. 
 
 The common tests for water,* supposed to be pure, are : 
 1. Evaporation to dryness. (Salts.) 
 
 * Rain water collected in tlie open air may, in many cases, be sub- 
 stituted for distilled water. 
 
TESTING OF WATER. 63 
 
 2. Test-paper. (Red and blue litmus paper.) 
 
 3. Perfectly clear lime-water. (Carbonic dioxide.) 
 
 4. Solution of silver nitrate. (Chlorine.) 
 
 5. Solution of barium chloride. (Sulphuric acid.) 
 
 6. Solution of ammonia oxalate. (Lime.) 
 
 7. Nessler's test* for ammonia. 
 
 The first should leave no residue, and the others should show 
 no reaction. (A few drops of the reagent must be added to a 
 portion of water in a clean test-tube.) 
 
 Preparation of Test Papers. 
 
 1. Blue Litmus Paper. Digest 1 part of litmus of com- 
 merce with 6 parts of water, and filter the solution ; davide the 
 intensely blue filtrate into two equal parts ; saturate the free 
 alkali in the one part by repeatedly stirring with a glass rod 
 dipped in very dilute sulphuric acid, until the color of the fluid 
 just appears red ; add now the other part of the blue filtrate, 
 pour the whole fluid into a dish, and draw strips of filter paper 
 through it ; suspend these slips over threads, and leave them 
 to dry. The color of the litmus paper must be uniform, and 
 neither too light nor too dark. 
 
 2. Reddened Litmus Paper Stir blue solution of litmus 
 
 with a glass rod dipped into dilute sulphuric acid, and repeat 
 this process until the fluid has just turned directly red. Steep 
 slips of paper in the solution and dry them as in 1. 
 
 3. Turmeric Paper. Digest and heat 1 part of bruised 
 turmeric root (or turmeric powder) with 4 parts of alcohol and 
 2 of water, filter the tincture obtained, and steep slips of fine 
 paper in the filtrate. The dried slips must exhibit a fine yellow 
 tint. Test paper must be kept in closed boxes, or in black 
 bottles, away from light and fumes. 
 
 * Biniodide of mercury is dissolved in iodide of potassium, and the 
 colorless solution rendered powerfully alkaline by the addition of 
 soda or potassa hydrate. This reagent poured into water containing 
 mere traces of ammonia produces a yellow to brown color. 
 
64 
 
 MINERALOGY SIMPLIFIED. 
 
 3. HYDRIC SULPHIDE, SULPHOHYDRIC ACID, SULPHURETTED 
 HYDROGEN = SH 2 . 
 
 A colorless gas which should be evolved at the moment of 
 using it. For this purpose monosulphide of iron, or ferrous sul- 
 phide FeS, is prepared by mixing intimately 5 parts of flowers 
 
 Fig. 62. 
 
 of sulphur with 8 parts of iron filings, and bringing the mixture, 
 in small portions at a time, into a red-hot Hessian crucible 
 (around which, when supported on a brick in a furnace, a coal 
 fire is built) which is covered with a piece of fire-brick until 
 the whole mass glows. When cool, the sulphide of iron in 
 fragments of the size of a pea, is placed in a bottle, A, Fig. 62, 
 and covered with pure water. Through funnel tube, a, con- 
 centrated sulphuric acid is added by degrees, and the evolved 
 gas can escape only through b into flask B, which should con- 
 tain some water for washing the gas. From B the gas is forced 
 through tubes c and d (connected by India-rubber tubes, k) 
 into flask (7, which contains the solution to be treated. Gene- 
 rally obtained by the reaction, FeS + (H 2 SO 4 + Aq.) = 
 (FeS0 4 + Aq.) + H 2 S. 
 
 A very handy apparatus for generating H 2 S, in small quanti- 
 
ITYDRIC SULPHIDE, ETC. 
 
 ties, is Bubo's, mounted on a stand with rubber connection, as 
 shown in Fig. 63. 
 
 Fig. 64 represents a gas bulb for passing sulphide of hydrogen 
 (or chlorine gas) into liquids in test-tubes. After being charged 
 the orifice on the top is closed with a cork. 
 
 Fig. 63. Fig. 64. 
 
 Fig. 65. 
 
 The following simple contrivance has lately been devised by 
 Capanema* to saturate a solution with hydrosulphuric acid 
 without the annoyance of the bad odor of the excess of gas. 
 Fig. 65 represents the apparatus; a is 
 a bottle to which is fitted a doubly per- 
 forated stopper provided with a pipette, 
 6, with a large pear-shaped bulb, and a 
 bent tube, c, communicating by means 
 of rubber tube, rf, with the gas genera- 
 tor. The liquid to be saturated or pre- 
 cipitated is introduced in the bottle, a, 
 and the pipette at first drawn up, until 
 the lower end of its tube is above the 
 liquid. Hydrosulphuric acid is now 
 allowed to pass in until the atmospheric 
 air in the flask and pipette is displaced, 
 and the pipette then pushed down un- 
 til the lower end of its tube nearly 
 touches the bottom of the flask. The 
 pressure of the gas, will force some of 
 
 * In Fresenius, Zeitschr. f. anal. Cliemie, 1881, p. 519. 
 6* 
 
6G MINERALOGY SIMPLIFIED. 
 
 the liquid into the pipette. By cautious swinging of the appa- 
 ratus, new portions of the liquid are successively brought in 
 contact with the gas, and in consequence of its absorption, the 
 liquid in the pipette descends, sometimes with great rapidity. 
 The saturation or precipitation (of a metal) is completed when- 
 ever the -liquid no longer descends from the pipette. The cur- 
 rent of gas is then shut off, the whole briskly agitated, the 
 pipette drawn up, and, when all the liquid has run out, care- 
 fully washed with distilled water, ejected from a wash-bottle, 
 to free it from any particle of the precipitate which may adhere 
 to it. 
 
 If it is desired to prevent the escape of odor entirely, the 
 upper end of the pipette may be provided with an additional 
 tube, charged with a loose pellet of cotton and a quantity of 
 filter-paper saturated with a solution of acetate of lead (sugar 
 of lead), which greedily absorbs the gas. 
 
 4. SULPHIDE OF AMMONIUM (NH 4 ) 2 S. 
 
 Should be often freshly prepared, and preserved in well-stop- 
 pered bottles. It is obtained by conducting sulphydric acid 
 gas = H 2 S, into aqueous ammonia until the latter absorbs no 
 more of the gas. The apparatus, Fig. 62, will serve for the 
 purpose by the addition of a loose stopper to flask (7, in which 
 the aqueous ammonia is to be placed. 
 
 5. HYDROFLUORIC ACID HF1. 
 
 In experimenting with this acid, especially in a gaseous form, 
 great care is necessary, since the fumes, when inhaled, may 
 produce dangerous effects. 
 
 To obtain it in more or less concentrated liquid form, a 
 small retort of platinum or lead is used, on which, during the 
 operation, a helm is luted. The retort is previously charged 
 with 1 part of finely powdered fluor-spar and 2 parts of con- 
 centrated sulphuric acid. After the charge is thoroughly mixed 
 
WET REAGENTS GENERALLY. G7 
 
 by a platinum spatula, heat is applied. If a dilute acid is 
 desired, the receiver, consisting of a platinum dish, must con- 
 tain some water and be well cooled from without with ice or a 
 freezing mixture. 
 
 A glass plate may now be covered with etching-ground (con- 
 sisting of 6 parts of gum mastic, 1 part asphaltum, and 1 part 
 of wax), and parts of it removed with an etching needle (draw- 
 ing). The glass plate thus prepared may now be acted upon 
 (etched) either by the gaseous or liquid acid ; in the former 
 case the drawing is lustrous (like the original glass), while in 
 the latter the drawing appears dull or opaque. The etching- 
 ground can be removed with oil of turpentine. 
 
 For testing minerals for HF1 with sulphuric acid, it is well 
 to employ a platinum crucible, the cover of which has an open- 
 ing in the middle upon which a piece of glass is placed ; the 
 crucible and contents may then be heated over a lamp. Many 
 silicates containing fluorine, like topaz, give off no trace of 
 fluorine in this way. To prove its presence 2 grams of the 
 powdered mineral are mixed with caustic potash and a little 
 liquid silicate of potash (water glass), and the whole fused in 
 a silver crucible for a quarter of an hour. The cold mass is 
 then dissolved in water, the silica precipitated with a solution 
 of sal-ammoniac, and filtered off. To the filtrate, acidulated 
 with HC1, we add a solution of chloride of calcium, and preci- 
 pitate with ammonia the fluoride of calcium. This, after being 
 well dried, is further tested with sulphuric acid. 
 
 6. WET REAGENTS GENERALLY. WATER =H 2 O. 
 
 In all analytical operations for solutions of other reagents, 
 etc., pure distilled water ought to be used. 
 
 Hydrochloric or Muriatic ac/c? = HCl, both concentrated 
 and diluted. 
 
 Nitric acid = HNO 3 , both concentrated and diluted. 
 
 Aqua regia, nitro-muriatic acid, is a mixture of 2-4 parts of 
 concentrated hydrochloric and 1 part of nitric acid. 
 
68 MINERALOGY SIMPLIFIED. 
 
 Sulphuric acid (oil of vitriol) = H a SO 4 or S0 3 -f H 2 O, con- 
 centrated and diluted with water.* 
 
 Common phosphoric acid or (Ortho-phosphoric acid) = 
 P 2 O S +3H 2 O or (H 3 PO 4 ). It can easily be prepared from 
 phosphorus and (diluted) nitric acid. 
 
 Ammonia. Ammonic hydrate. Liquor ammonice, AmllO 
 =NH 3 HO -= NH 4 O. 
 
 Carbonate of Ammonia. Ammonic carbonate (NH t , CO S ). 
 
 Chloride of ammonia. Ammonic chloride. Sal~ammoniac=. 
 AmCl.(N 4 Ci). 
 
 Phosphate of soda. Sodic phosphate (Na 2 HP0 4 ,12H 2 O). 
 
 The commercial salt ought to be purified by solution in water 
 and recrystallized by evaporation. 
 
 Nitrate of baryta, Baric nitrate = Ba 2 N0 3 . 
 
 Nitrate of 'silver, Lunar caustic, Argentic nitrate AgNfK 
 
 Chloride of platinum = PtCl 4 . 
 
 Place a fragment of platinum in a little aqua regia and set 
 the vessel aside in a warm place, adding more acid from time 
 to time if necessary, a solution of perchloride of platinum = 
 PtCl 4 results. Evaporate the solution to remove excess of 
 acid, and complete the desiccation (drying) over a water-bath. 
 Dissolve the residue in 10 parts of water as a reagent for de- 
 tecting potassa in the presence of soda and lithia. It precipi- 
 tates, however, also salts of ammonia. 
 
 MoJybdate of Ammonia = (NH 4 ) 2 MoO 4 . It is obtained by 
 pulverizing and roasting the native sulphide of molybdenum 
 MoS 2 , whereby molybdic tri-oxide, or anhydride = MoO 3 , is 
 formed ; dissolve tlie latter in water, adding ammonia, filtering, 
 evaporating, and crystallizing. 
 
 To prepare the molybdenum solution used for precipitating 
 phosphoric and arsenic acids, 100 grams of molybdenum tri- 
 oxide are dissolved in 50 c.c. ordinary aqueous ammonia, and 
 80 c.c. water, and pouring the solution into a mixture of 500 
 
 * In diluting "oil of vitriol" the acid must gradually, and little at 
 a time, be pqured into water ; the reverse action may prove very dan- 
 gerous . 
 
THE MOUTH BLOWPIPE. 69 
 
 c.c. nitric acid and 300 c.c. water, and if a precipitate forms it 
 must be filtered off. 
 
 Oxalate of ammonia or Oxalate of ammonium = 2(NH 4 ) 2 
 C 2 O 4 , can be synthetically prepared according to the following 
 formula : 
 
 2H,C 2 4 + N 4 H 16 C 3 8 = 2(NH 4 )2C 2 4 + 3CO 2 + 2H 2 O 
 
 Oxalic Carbonate of Oxalate of Carbonic Water. 
 
 acid. ammonium. ammonium. di-oxide 
 
 set free. 
 
 To a nearly boiling solution of 1 part of oxalic acid in about 
 8 of water, add carbonate of ammonium uutil the liquid is neu- 
 tral to test-papers, filter while hot, and set aside for the forma- 
 tion of crystals. The mother liquors are further evaporated to 
 crystallization. To obtain the pure salt it ought to be re-crys- 
 tallized a second time. Dissolve 1 part of the pure salt in 30 
 parts of water. 
 
 Caustic potash or Potassic hydrate = KHO or K 2 O,H 2 O. 
 Dissolve some sticks of potassa in water, and separate the clear 
 solution from the sediment (Si0 2 ,Al 2 O 3 ) by decantation. 
 
 Chloride of barium. Baric chloride = BaCl 2 . 
 
 CHAPTER IV. 
 
 BLOWPIPE ANALYSIS AND APPARATUS. 
 1. THE MOUTH BLOWPIPE. 
 
 THIS simple instrument of' very ancient origin is a most 
 convenient apparatus for heating, melting, volatilizing, oxidiz- 
 ing, or reducing mineral substances on a small scale. By blow- 
 ing air into the interior of a flame, always a burning gas, 
 i. ., carbo-hydrogen, the combustion is of course rendered 
 more complete and rapid, and hence the intensity of heat in 
 creased. It is of the greatest service to the chemist, mine- 
 
70 MINERALOGY SIMPLIFIED. 
 
 ralogist, and practical miner, for the recognition of minerals 
 and ores, and the detection of certain chemical constituents, 
 such as metals and others. 
 
 The improved chemical blowpipe, Fig. 66, consists of a 
 chamber, c, near the extremity of the instrument, which col- 
 lects the condensed moisture ; this is connected with two tubes 
 
 Fig. 66. 
 
 Fig. 67. 
 
 Fig. 68. 
 
 with ground joints. To the longer one, a, is attached a mouth- 
 piece for blowing, of different shapes, and made of horn or 
 ivory. The shorter exit-tube is generally furnished with a 
 movable tip, e, made of solid platinum, which may be easily 
 cleansed from soot collecting upon it by simply heating it in 
 the flame of a spirit-lamp. 
 
 The best shape of the tip is that represented in its natural 
 size, Fig. 66, at e ; it always produces a well-defined and conical 
 flame. Fig. 67 represents Plattner's blowpipe,* with gas-blast 
 attachment, and marked regulating stopcock. The above 
 
 * This convenient blowpipe is used at Harvard College laboratory, 
 and is highly recommended. 
 
BLOWING WITH THE BLOWPIPE. 71 
 
 attachment is sold separate from the rest of the blowpipe, and 
 can be fastened to other blowpipes. 
 
 Fig. 68 is Fletcher's hot-blast chemical blowpipe a pattern 
 of the ordinary chemical blowpipe with the patent hot-blast 
 arrangement. 
 
 2. BLOWING WITH THE BLOWPIPE. 
 
 To keep up a continuous current of air through the blowpipe 
 is at first a difficult task. This, however, is easily overcome 
 by attending to the following directions: Closing the mouth, 
 keep the cheeks distended with air during a number of inspira- 
 tions and expirations performed through the nostrils. Next 
 attempt the same with the ivory mouth-piece of the blowpipe 
 between the lips. Now, as this provides an exit for the air in 
 the mouth, unless a fresh supply be kept up from the lungs, the 
 cheeks will soon collapse ; in order to prevent this, at the 
 moment of inspiration through the nose, a sufficient quantity of 
 air must be allowed to enter the mouth to preserve their dis- 
 tension. In this way the air in the mouth is constantly sub- 
 ject to the same compression, and flows in a uniform manner 
 from the little orifice. Having thus acquired the habit of 
 keeping up a continued stream of air from the blowpipe, the 
 beak with platinum cap is now brought within the border of 
 the flame. 
 
 A good way to acquire a practical knowledge of this instru- 
 ment, and of the effects of the different parts of the flame, is to 
 convert, for instance, a minute piece of lead, placed upon char- 
 coal, into oxide of lead, by exposing it to the outer flame, and 
 afterwards to reduce this oxide, i. e., to restore it to its original 
 metallic state by heating it in the inner flame. The reduction is 
 much facilitated by an admixture of soda or cyanide of potassium. 
 
 flaming, Flattern (Germ.); Flamber (French) In many 
 cases when a transparent bead is intermittingly heated in the 
 flame, or is repeatedly taken out oT the flame, peculiar effects 
 are obtained. This operation has obtained the name of " flam- 
 ing." Clear beads frequently become opaque, milk-white, or 
 
72 
 
 MINERALOGY SIMPLIFIED. 
 
 even colored. This depends upon the fact that certain com- 
 pounds which dissolve at a high temperature separate out on 
 being heated to a somewhat lower temperature, appearing as 
 peculiar crystals, which are sufficiently well formed in most 
 cases to be visible under the microscope when the bead has 
 been flattened whilst hot, or when it has been dissolved in 
 dilute acid so as to isolate the crystals. 
 
 3. THE BLOWPIPE FLAME. 
 
 The blowpipe serves to conduct a continuous fine current of uir 
 into a gas-flame, or into the flame of a candle or oil lamp. The' 
 flame of a candle (and equally so that of gas or of an oil lamp), 
 burning under ordinary circumstances, is seen to consist of 
 three distinct parts, as shown in Fig. 69, viz., 1st, a dark nu- 
 
 Fig. 69. 
 
 Atmospheric oxygeu. 
 
 JfoO 
 
 cleus in the centre, , a' ; 2d, a luminous cone surrounding this 
 nucleus, c, /, g; and 3d, a feebly luminous mantle encircling 
 the whole flame, />, c, d. The dark nucleus is formed by the 
 gases which the heat evolves from the tallow or oil, and whieli 
 
THE BLOWPIPE FLAME. 73 
 
 cannot burn here for want of oxygen. In the luminous cone 
 these gases come in contact with a certain amount of air, in- 
 sufficient for their complete combustion. In this part, there- 
 fore, it is principally the hydrogen of the carbides of hydrogen 
 evolved which burns, while the carbon separates in a state 
 of intense ignition, thus imparting to the flame the highly 
 luminous appearance observed. In the outer coat the access 
 of air is no longer limited, and all the gases not yet burned are 
 consumed here. This part of the flame is the hottest ; oxidiz- 
 able bodies oxidize therefore with the greatest possible rapidity 
 when placed in it, since all the conditions of oxidation are here 
 united, viz., high temperature and an unlimited supply of 
 oxygen. This outer part of the flame is therefore called the 
 oxidizing flame. 
 
 On the other hand, oxides having a tendency to yield up their 
 oxygen, suffer reduction when placed within the luminous part 
 of the flame, the oxygen being withdrawn from them by the 
 carbon and the still unconsumed carbide of hydrogen present 
 in this sphere. The luminous part of the flame is therefore 
 called the reducing flame. The effect of blowing a fine current 
 of air across the flame is, first, to alter the shape of the latter, 
 which, from tending upward, is now driven sideways in the 
 direction of the blast, and at the same time lengthened and 
 narrowed ; and, in t]ie second place, to extend the sphere of 
 combustion from the outer to the inner part. As the latter 
 circumstance causes an extraordinary increase of the heat of 
 the flame, and the former a concentration of that heat within 
 narrower limits," it is easy to understand the exceedingly ener- 
 getic action of the blowpipe flame. The way of holding the 
 blowpipe, and the nature of the current, will always depend 
 upon the precise object in view, viz., whether the operator wants 
 a reducing, or an oxidizing flame. The easiest way of pro- 
 ducing efficient flames of both kinds is by means of coal-gas 
 delivered from a tube. The task of keeping the blowpipe 
 steadily in the proper position may be greatly facilitated by 
 7 
 
74 
 
 MINERALOGY SIMPLIFIED. 
 
 resting that instrument firmly upon some movable metallic 
 support, such as, for instance, Bunsen's gas-lamp, Fig. 83. 
 
 Fig. 70 shows the flame for reducing, and Fig. 71 the flame 
 for oxidizing. 
 
 Fig. 70. 
 
 Fig. 71 
 
 The reducing flame is produced by keeping the tip of the 
 blowpipe just on the border of a. tolerably strong gas-flame, and 
 driving a moderate blast across it. The resulting mixture of 
 the air with the gas is imperfect, and there remains between 
 the inner bluish part of the flame, and the outer barely visible 
 part, a luminous and reducing zone, of which the hottest point 
 lies somewhat beyond the apex of the inner cone. 
 
SUPPORTS FOR THE ASSAY. 
 
 75 
 
 To produce the oxidizing flame, the gas is lowered, the tip 
 of the blowpipe pushed a little further into the flame, and the 
 strength of the current somewhat increased. This serves to 
 effect an intimate mixture of the air and gas, and an inner 
 pointed bluish cone, slightly luminous towards the apex, is 
 formed and surrounded by a thin, pointed, light bluish, barely 
 visible mantle. The hottest part of the flame is at the apex of 
 the inner cone. Difficultly fusible bodies are exppsed to this 
 part to effect their fusion ; but bodies to be oxidized are held a 
 little beyond the apex, that there may be no want of air for 
 their combustion. 
 
 
 
 4. SUPPORTS FOR THE ASSAY. 
 
 I. Charcoal, well burnt and of uniform texture, forms an 
 ordinary support for assays. The piece should be about six 
 inches long, one end wrapped in paper, and in the other a small 
 cavity must be cut, half the size of a pea, either with the point 
 
 Fi 
 
 Fi*. 73. 
 
 Fig. 74. 
 
 of a knife, or by means of charcoal borers, Figs. 72, 73, and 
 74. Fig. 75 represents two forms, after Plattner, with wooden 
 handles ; a is club shaped, b is four cornered. The heating of an 
 assay on charcoal in the blowpipe flame is illustrated in Fig. 76. 
 
76 
 
 MINERALOGY SIMPLIFIED. 
 
 Fig. 75. 
 
 Fig. 76. 
 
 II. Porcelain Supporters Foster and Fletcher in England 
 use pieces of glazed porcelain made of the size and shape of 
 charcoal supporters. On the end of these porcelain plates are 
 cavities into which small pieces of charcoal are fitted, upon 
 the surface of which the blowpipe assay is placed. The whole 
 surface of the porcelain is blackened over a lamp. This coat of 
 soot takes up and exhibits films or coatings as well as charcoal. 
 
 III. Aluminium Plate as a Support in Blowpipe Analysis. 
 The latest and best substitute for charcoal is aluminium foil, 
 first introduced by Colonel W. A. Ross.* A strip of such 
 foil should be 5 inches long, 1J inch wide, and about the thick- 
 ness of a ten cent piece ; one end should be turned up to form 
 a ledge, as directed by Ross, this ledge being between J to J 
 inch wide, and making rather less than a right angle with the 
 rest of the plate. Sheet aluminium, even of much greater 
 thickness than this, can be bent easily without any cracking, 
 by heating it in a Bunsen burner, and working it while hot.f 
 
 * Alphabetical Manual of Blowpipe Analysis by Lieut.-Colonel 
 W. A. Ross. London : Triibner & Co., 1880. 
 
 f Messrs. Johnson, Matthey & Co. in London are recommended as 
 dealers by Col. Ross. They furnish it of any thickness or dimensions 
 for 7s. 6d. per ounce. Some German aluminium plates of somewhat 
 lesser thickness the writer found impure, and fusing too easily over 
 a Bunsen burner. 
 
SUPPORTS FOR THE ASSAY. 77 
 
 After turning up the ledge, and rounding off the edges and 
 corners with a file, the plate should be well scoured with bone 
 ash and polished with leather and whiting, and may then be 
 used for a long time. 
 
 The test samples are either placed directly upon the metallic 
 edgfe, or are received on a small piece of charcoal half an inch 
 square, and of the thickness of a penny piece, which can 
 easily be cut and kept ready in large numbers. 
 
 When in use the plate is best held with spring forceps, 
 described by Ross, though other forceps can be made to serve 
 the purpose, the handles being covered with felt or flannel, as 
 they get very hot. It is held so as to be almost vertical, only 
 just enough inclined to prevent the assay and the slip of char- 
 coal from falling off the ledge. A little practice enables the 
 worker to hold it quite steadily with as much ease as he does 
 the ordinary piece of charcoal. The plate, it is said, is not 
 only a great gain as to portability, cleanliness, and economy, 
 but also gives, in most cases, much better indications of the 
 volatile substances sought for, which collect upon the larger 
 vertical portion of the plate. Such a plate will last any length 
 of time, as the hottest blowpipe flame, even one worked with a 
 small handblower, does it no injury, and there is scarcely any 
 substance (except melted gold) which may not be heated 
 directly upon it with perfect safety. The one side being kept 
 for sublimates, the other may be used for such purposes as 
 calcining sulphides, etc., before testing in beads, for which it 
 is far superior to charcoal, especially in the case of very fusible 
 minerals. A fragment of the substance about half the size of 
 a small pea, or if it decrepitates, a corresponding amount of 
 powder made to a paste with water, is laid upon the ledge close 
 up to the angle. 
 
 The following are the principal advantages of aluminium 
 over charcoal, according to W. M. Hutchings : 
 
 1. It enables us to get several sublimates in succession from 
 the same fragment of substance. Heated very gently on the 
 
 7* 
 
78 MINERALOGY SIMPLIFIED. 
 
 bare plate, only the most volatile constituents are given off.* 
 As the heat increases, more and more are given off, but a 
 limit is reached beyond which nothing is obtained, the less 
 volatile constituents not being given off at all, or only very 
 slightly, as long as the substance is cooled by lying directly on 
 the aluminium. The same fragment being then placed on a 
 slip of charcoal on the ledge, these less volatile constituents 
 are obtained in the separate sublimates. 
 
 2. The sublimates are generally much more concentrated on 
 the aluminium, as compared with ordinary charcoal, which, 
 when exposed to the flame for any length of time, gets red hot 
 some distance in front of the assay. The aluminium remains 
 comparatively cool; and the vertical surface prevents the subli- 
 mates being swept along by the blast as much as on the nearly 
 horizontal charcoal. 
 
 3. When the sublimate is once formed, the aluminium has 
 no further action upon it, and many very characteristic changes 
 may be observed by applying an oxidizing or reducing flame, 
 most of which cannot be obtained at all on charcoal, partly 
 because its being black would hide them, but chiefly because 
 it immediately begins to glow under the sublimates when the 
 flame is applied to them. 
 
 5. FUEL LAMPS. 
 
 1, Good stearine candles will answer for most purposes. 
 
 2. Olive Oil., A much better fuel is olive oil or rape-seed 
 oil, burnt in a brass lamp having a circular neck. This and 
 the .opening for filling the lamp are covered by screw caps, pre- 
 venting .all leakage. 
 
 Fig. 77 represents the form of blowpipe lamp invented by 
 Berzelius, and improved by Plattner. 
 
 Fig. 78 is the Freiburg pattern of the same style of lamp as 
 the preceding, but revolves on its axis, permitting the flame 
 from the blowpipe to be directed at any angle. 
 
 * When first applying heat, the point of the blowpipe flame ought 
 to be held at a distance of 1-2 cm. from the assay. 
 
FUEL LAMPS. 
 
 79 
 
 Another convenient lamp for using oil or petroleum is 
 Fletcher's improved blowpipe lamp, Fig. 79. 
 
 Fig. 77. 
 
 Fig. 78. 
 
 The wick holder will be found one of the best forms ever 
 made, in addition to the fact that the angle can be adjusted as 
 
 Fig. 79. 
 
 required by simply revolving it in the fixed collar. The wick 
 holder, J, lifts out for refilling. The lamp is engraved half size. 
 An ordinary alcohol lamp of glass, Fig. 80, may also be 
 used for blowpipe experiments, if the alcohol is mixed with 
 turpentine or benzol (1 part of turpentine or 3 parts of benzol 
 to 12 parts of strong alcohol of 80 to 90 per cent.). 
 
80 
 
 MINERALOGY SIMPLIFIED. 
 
 3. Solid Fats -Lamps filled with solid fats, such as tallow, 
 
 paraffine, etc., have lately been introduced, which are convenient 
 in traveling. Fig. 81 exhibits a modified form of the previously 
 described lamp of Fletcher. It is made for tallow or solid fats 
 for traveling. When tallow, etc., is used, the operation must 
 be commenced by first blowing the flame downwards to melt the 
 solid fat round the .wick. The heat of the flame will keep it 
 fused afterwards for any length of time. This pattern can be 
 used with solid or liquid fats of any kind, and is a perfect 
 traveler's lamp. Size, when closed, 2 in. by 2 in. Trim the 
 wick always while the lamp is hot, when hard fats are used. 
 
 Fig. 80. 
 
 Fig. 82. 
 
 The curved bottom of the lamp should stand on the open end 
 of the cover when in use. This makes a steady base, and 
 admits of adjustment of the angle of wick without reversing 
 or re-trimming. 
 
 In Foster's lamp, Fig. 82, solid fat is likewise used, e. g., 
 paraffine or tallow. It serves as a traveler's lamp, and consists 
 of a cylindrical vessel, A, to which the wick holder, B, is 
 soldered. When in use, the flame is at first directed down- 
 wards to melt the fat next to the wick, after which it yields a 
 steady flame for hours. The cover, C, forms also a support, 
 and is fastened by a bayonet-socket, D (d). 
 
FIXED BLOWPIPI^ AND BLAST-LAMPS. 
 
 81 
 
 Fig 
 
 G. ILLUMINATING GAS. 
 
 The most convenient combustible for blowpipe work is 
 illuminating gas. The burner used is the ordinary Bunsen 
 gas-burner, Fig. 83. For this 
 purpose it is provided with an 
 extra tube, g A, to slip over the 
 small gas jet at j, in the inte- 
 rior of the burner, e f, in such 
 a manner as to shut off all ex- 
 cess of air at a. The tube is 
 flattened at the top, see /, and 
 made a trifle lower at one side, 
 so that the blowpipe flame may 
 be directed downward when 
 necessary. The gas is then 
 lighted at the flattened end, h. A 
 cock, at the foot of the burner 
 for regulating the flow of the 
 gas is useful. 
 
 When testing substances for 
 sulphur, the gas flame should not 
 
 be employed, since the ordinary coal gas contains usually 
 enough of sulphur to vitiate the results. 
 
 7. FIXED BLOWPIPES AND BLAST-LAMPS. 
 
 For many experiments it is of great advantage to have the 
 blowpipe fixed to a support in order to leave the hands free for 
 manipulation. The following, Fig. 84, represents an improved 
 Herapath blowpipe for general use. This is a modification of 
 the well-known Herapath, from which it differs in its great 
 simplicity, and in its power of adjustment in any possible 
 position. The jet tube may be raised or lowered to any height, 
 and turned in any direction. A touch will direct the flame on 
 any point while the blowpipe stands in the same position on 
 
82 
 
 MINERALOGY SIMPLIFIED. 
 
 the table ; there being no necessity for raising, lowering, or 
 adjusting work before it. 
 
 Fig. 85, letter c, represents a blowing machine to be worked 
 either by the hand or the foot; it forces air into the expanding 
 regulator, &, and thence in a regular blast into the blowpipe, a. 
 The attachment on the stand permits motion in any direction. 
 
 Fig. 86 is a blast-lamp for gas; brass, small size. The blast 
 may be furnished from either the mouth or small bellows. The 
 flame can be turned in any direction. 
 
 Fig. 85. 
 
 Fig. 87, Fletcher's special Chemical Blowpipe with folding 
 stand, adjustable at any height or angle. It can be used either 
 
FIXED BLOWPIPES AND IJLAST-LAMPS. 
 
 83 
 
 with the mouth, or the small hand blower can be attached and 
 the blowing done by the lingers. With this blowpipe is supplied 
 one jet with, and one without the patent coil, to enable a larger 
 variety of flame to be obtained. The lamp or a weight should 
 be placed on the stand when in use. The blower when not in 
 use shuts up flat for the pocket. The pressure of air is ad- 
 justed by a delicate lever tap on the air tube. 
 
 Fig. 87. 
 
 Fig. 88 represents double bellows for hand use ; two rubber 
 bulbs for use with the blowpipe or other small blasts. 
 
 Fig. 88. 
 
 Fig. 89 is Bunsen's improved gas-blowpipe and blast-lamp 
 united. The nozzle of the blowpipe, a, is surrounded with a 
 brass casing, b. The blast from a double bellows is thrown 
 through a flame of illuminating gas, giving sufficient heat to 
 ignite a crucible, and can also be used as a glass-blower's lamp 
 or blowpipe. The flame can be turned in any direction. Three 
 different brass nozzles, adapted for different purposes, accom- 
 pany each. 
 
84 
 
 MINERALOGY SIMPLIFIED. 
 
 The following devices, invented and patented by Thomas 
 Fletcher, are very excellent patterns of blowpipes : 
 
 Fig. 89. 
 
 Air. 
 
 Gas. 
 
 1st. The Automaton Blowpipe This blowpipe (Fig. 90) is 
 mounted on a stand, with a universal ball-joint, so as to enable 
 it to be used at any angle or in any position. The ball-joint 
 can be secured fast in position. 
 
 It is simple, self-adjusting for both gas and air, requiring 
 only a slight motion of a small lever to obtain instantly any 
 flame, from the smallest to the largest. 
 
 It has all the delicacy of the best mouth blowpipe used with 
 the utmost skill, with the power and advantages obtained with 
 a mechanical blower. 
 
 A slight motion from side to side of the pin A changes the 
 power and character of the flame instantly as required, or stops 
 the power without extinguishing the flame, the blowpipe being 
 both self-lighting and self-adjusting. 
 
 2d. The Automaton Hand Blowpipe Fig. 91 shows the 
 
 hand blowpipe, with both tubes underneath, and will be found 
 
FIXED BLOWPIPES AND BLAST-LAMPS. 
 
 85 
 
 the most convenient pattern for small work, brazing, anneal- 
 ing, etc. 
 
 The power of a blowpipe depends not only on the size of the 
 air-jet and gas supply, but on the pressure of the air supplied 
 
 Fig. 91. 
 
 by the blower. The foot-blowers are so perfect for all blow- 
 pipe work as to leave nothing to be desired. After ten years 
 they remain beyond the possibility of improvement in the 
 slightest detail, unapproached by any other form. 
 
 Fig. 02. 
 
 3^7. Fletcher's New Patent Month Blowpipe. Fig. 92 re- 
 presents this blowpipe. The improved nickel-plated mouth- 
 piece, c, is said to cause no strain on the lips, while the tongue 
 has the necessary control over the opening. 
 
86 MINERALOGY SIMPLIFIED. 
 
 The blowpipe proper is held as a pencil, the chamber, A, on 
 the stem stops all condensed moisture, and prevents the heat 
 traveling up the end ; it is sold with two tips, A, for cold, and 
 J5, hot blast. It might easily be fastened to an immovable 
 stand, and connected with a hand- or foot-blower. 
 
 4th. Fletcher's Hot-Blast Blowpipe Figs. 93 and 94 
 
 represent this blowpipe for temperatures above the power of 
 ordinary gas and air blowpipes. As will be seen from the 
 
 Fig. 93. Fig. 94. 
 
 engraving, the air-pipe is coiled round the gas-pipe in a spiral 
 form, and both are heated by three small Bunsen burners 
 underneath, which are controlled by a separate stopcock. 
 The power of this arrangement is about double that of an 
 ordinary blowpipe; and when the jet is turned down to a small 
 point of flame it will readily fuse a moderately thick platinum 
 wire. In power it is nearly equal to the oxy-hydrogen jet, 
 and it is a good arrangement, both for chemical purposes and 
 also for soldering and general use. They are made with three 
 sizes of jet : small, for chemical purposes ; medium and large, 
 for soldering, etc.; and the size of jet or the purpose for which 
 it is required should be specified in ordering. 
 
PLATINUM APPARATUS AND APPLIANCES. 
 
 87 
 
 8. PLATINUM APPARATUS AND APPLIANCES. 
 
 Platinum wire is used as a support when an assay is to 
 be fused with borax or salt of phosphorus (Ex., S. Ph.), etc., to 
 
 Fig. 95. 
 
 n -P 
 
 Fig. 96. 
 
 ascertain the color of the beads produced. One extremity of 
 the wire, about three inches long and of the thickness of horse- 
 hair, is bent into a hook or is coiled. This wire may be fused 
 into a small glass-tube for a handle (Fig. 95). Before being 
 used, it Should be thoroughly cleaned, by placing it in dilute 
 sulphuric acid and rinsing with water. 
 
 Platinum spoons (Fig. 96, natural size) are very useful for 
 melting assays and other operations. A glass, wooden or cork- 
 handle should be adapted to it. A piece of platinum foil, 
 properly bent, may answer for the same purpose as a spoon. 
 
88 
 
 MINERALOGY SIMPLIFIED. 
 
 Forceps with platinum points (Fig. 97) to hold small laminre 
 of minerals in the flame to ascertain their fusibility. 
 
 Fig. 97. 
 
 9. TUBES OF HARD GLASS, FREE FROM LEAD. 
 
 They are one-twelfth to one-fourth incli in diameter, and four 
 to six inches long, and are absolutely necessary. They serve 
 for the ignition of mineral fragments in a current of air. The 
 substance is placed near the end, and the tube is then held 
 
 Fig. 98. 
 
 somewhat inclined, either in the flame of a Bunsen burner or 
 of the blowpipe. To prevent the falling out of the substance 
 
 Fig. 99, 
 
 Fig. 100. 
 
 the tube may be slightly bent as represented in Fig. 98. For 
 each new operation a clean tube must be employed. 
 
BLOWPIPE REAGENTS. 89 
 
 
 
 Closed tabes and glass bulb-tubes, or matrasses (Fig. 99), 
 are used for heating bodies out of contact with air. They are 
 easily made of hard glass tubing before a. glass-blower's lamp, 
 or a Bunsen-burner connected with a blast, as previously 
 described. For chemical experiments a variety of soft glass 
 tubing ought to be on hand ; which, in the flame of a blast- 
 lamp, can be readily bent or drawn out and sealed at one end. 
 
 A triangular file is used for cutting glass. A notch is cut 
 in one side of the tube, when it is .easily broken in two. 
 
 Watch-glasses are used for keeping powdered minerals and 
 for various other purposes. 
 
 For other accessory apparatus mortars, flasks, test-tubes, 
 etc see Laboratory Apparatus and Manipulations, page 
 38-58 ; and for acids and other chemicals, see Wet Reagents, 
 page 59-G9. 
 
 10. CUTTING PLIERS ; STEEL MAGNET ; MAGNETIC 
 NEEDLE. 
 
 Cutting pliers (Fig. 100) are useful for detaching fragments 
 from mineral specimens. 
 
 A common steel magnet (Fig. 5, page 39) serves to recognize 
 magnetic bodies. 
 
 A magnetic needle (compass, Fig. 6, page 39) is useful for 
 delicate determinations. 
 
 11. BLOWPIPE REAGENTS. 
 
 The quantities used are small and'thei'e are but few, which, 
 however, have to be scrupulously pure. The dry preparations 
 are generally purchased from dealers. 
 
 Carbonate of soda, called simply soda, Na 2 CO 3 . Biborate 
 of soda or borax with water of crystallization = Na 2 O, 
 2B 2 O 3 + 10H 3 O or Na a B 4 O 7 + 10H 2 O, and fused boric acid, 
 = B 2 O 3 , for the detection of copper in lead. Phosphate of soda 
 and ammonia, or salt of phosphorus or microcosmic salt = 
 (Na 2 O, NH 4 O, H 2 O) P 2 O 5 + 4H 2 O or Na(NH 4 )HPO 4 + 
 4H 2 O). Cyanide of potassium = KCN or KCy (a dangerous 
 
 8*. 
 
90 MINERALOGY SIMPLIFIED. 
 
 poison). Bisulpliate of potash or acid potassium sulphate 
 HKSO 4 , or strong H 2 SO 4 . Nitrate of potash saltpetre 
 K 2 0, N 8 O 6 , or KNO 3 . Iodide of potassium, KI. Sulphur, S. 
 Flowers of sulphur. Nitrate of cobalt, Co(NO 3 ) 2 + 6H 2 O 
 in solution. The crystals of the nitrate are dissolved in ten 
 parts of water. For use the cobalt solution is most conveni- 
 ently kept in dropping glasses. 
 
 Fig. 101, a, &, c, show different forms of this apparatus. 
 a, according to Bunsen ; b and c, according to Schuster, with 
 and without a ground glass-stopper. 
 
 Oxalate of nickel, or nitrate of nickel, Ni(NO 3 ) 2 -f 6H 2 O. 
 Black oxide of copper, or cupric oxide = CuO. Fluoride of 
 calcium (Fluor spar) = CaF 2 . The powder must be deprived 
 of water by ignition. Nitroprusside of sodium for detecting 
 sulphur. 
 
 Iron : Fine sifted iron filings. Ferrum pulveratum, or 
 alcoholisatum of the druggists. 
 
 Lead : Pure lead or proof lead. 
 
 Tin : Strips or tin-foil. 
 
 Zinc : Strips of common sheet zinc. 
 
 Magnesium : Bits of foil or wire are useful in detecting 
 phosphoric acid. . 
 
 Silver-foil for the detection of sulphur. A smooth bright 
 silver coin, however, will answer every purpose. 
 
 Bone-ash : A little cup of bone ashes, called a cupel, is 
 used for the cupellation of gold and silver. 
 
 Test-papers: Blue litmus paper, red litmus paper, turmeric 
 paper, and Brazil wood paper. 
 
 Charcoal. 
 
TESTS OF INORGANIC SOLID SUBSTANCES 
 
 Aluminium plate. 
 
 A small alcohol lamp. 
 
 Bottle for hydrochloric acid to test for carbon- 
 ates, with a ground, tight glass stopper, reaching 
 nearly to the bottom, thus enabling one 'to with- 
 draw and use a single drop of acid. It may also 
 be used for cobalt solution, Fig. 102. 
 
 12. PRELIMINARY TESTS OF INORGANIC SOLID 
 SUBSTANCES. 
 
 The substances must be dry and in the form of fine powders. 
 In most of the following experiments, the blowpipe may be 
 replaced by a Bunsen burner. The beads must be examined 
 both hot and cold. 
 
 1. Easily volatilized 
 when heated upon 
 charcoal (or upon 
 platinum foil or in 
 a dry test-tube). 
 
 Water ; compounds of ammonia, mercury, and 
 some of arsenic. Sulphur and its acids. 
 Carbon burns by ignition in the air ; all 
 organic compounds are decomposed when 
 heated, most of them with separation of carbon 
 (blackening). 
 
 2. Deflagrate when 
 heated upon char- 
 coal platinum. 
 
 Nitrates, chlorates, iodates, bromates, etc. ; 
 common salt, and other salts, as likewise 
 many minerals, decrepitate. 
 
 3. Fusible without 
 volatilizing ami 
 without changing 
 color. 
 
 Most salts of the alkalies and some of those of 
 the alkaline earths. After intense ignition in 
 the R. F. they color moist tutneric paper 
 brown. 
 
 4. B. li. infusible, or 
 difficultly fusible, 
 without changing 
 color. 
 
 The earths and their salts ; most of the alkaline, 
 earths and their salts. When heated they glow 
 with white light. The earths proper show no 
 alkaline reaction after ignition. Silica and 
 many of its compounds. Metals : Fe, Ni, Co, 
 PI, Mo, W, Pd, Ir, Klff 
 
92 
 
 MINERALOGY SIMPLIFIED. 
 
 5. Give when ignited 
 with soda or soda 
 and cyanide of 
 potassium in the 
 R. F. upon char- 
 coal, or the lumin- 
 ous flame of a 
 Eunsen burner. 
 
 a. Garlic odor: Most compounds of arsenic. 
 
 b. Hepar: All compounds of sulphur. The 
 
 mass when moistened blackens silver, and 
 with acids develops sulphide of hydrogen. 
 
 c. Metallic grains: Sn, Ag, Cu, Au. Gray 
 
 magnetic powder: Fe, Ni. Co. Non- 
 magnetic: Mo, W, PI, Ir. Brittle: Sb, Bi. 
 Malleable : Pb. Incrustation : Zn (white), 
 Cd (brown). 
 
 6. Give, when heated 
 in a glass open at 
 both ends, and 
 held obliquely. 
 
 a. Odorous gases : Metallic sulphides, of burning 
 
 sulphur. Selenides, of decaying radishes. 
 Arsenides, of garlic. Some ammoniacal salts 
 yield NH 3 turning moistened red litmus 
 paper blue. 
 
 b. Metallic coating : Mercury and arsenic com- 
 
 pounds. 
 
 c. White coating: Metallic arsenides, antimo- 
 
 nides, sulphide, of lead, some salts of am- 
 monia, such as sal-ammoniac. 
 
 7. Color the non-lu- 
 minous flame of a 
 Bunseii gas-lamp 
 (O.F.). 
 
 a. Yellow: Na. 
 
 b. Violet: K, Cs, Rb. 
 
 c. Crimson: Li, Sr. 
 
 d. Blue: As, Sb, Pb, Se. 
 
 e. Green : Boracic acid ; borates after moisten- 
 
 ing with sulphuric acid. 
 
 L With phosphorus 
 salt or borax upon 
 platinum wire in 
 O. F. and R. F. 
 
 o. Colorless bead: Silica. 
 
 b. Yellowish brown or reddish : Iron. 
 
 c. Amethyst color: in O. F. (not in R. F.) man- 
 
 ganese. 
 
 d. Blue: copper (in the 0. F. only), cobalt. 
 
 e. Yellowish- green: Chromium. 
 
REACTIONS OF OXIDES WITH GENERAL REAGENTS. 93 
 
 CHAPTER V. 
 
 REACTIONS OF OXIDES WITH GENERAL REAGENTS. 
 
 THE. folio wing reactions of oxides with borax and salt of 
 phosphorus are taken from Wurtz's Dictionnaire de Chemie, 
 vol. i., art. Chalumeau ; the others from Landauer's Lothrohr- 
 analyse, 2d edit., Berlin, 1881. 
 
MINERALOGY SIMPLIFIED. 
 
 1. BEHAVIOR OF METALLIC OXIDES WITH BORAX. 
 
 Color of 
 the bead. 
 
 In the oxidizing flame. 
 
 In the reduction flame. 
 
 Hot. 
 
 Cold. 
 
 Hot. 
 
 Cold. 
 
 Colorless. 
 
 Si, Al,Su,Ba,Sr 
 
 SLAl,Sn,Ba,Sr, 
 
 Si, Al, Sn, Ba,Sr, 
 
 Si.Al.Sn, Di, Mn, 
 
 
 Ca, Mg, Gl, Y, 
 
 Ca, Mg, 61, Y, 
 
 Ca, Mg, Gl, Y, 
 
 Ba, Sr, Ca, Mg, 
 
 
 Zr, Th, La, Tef 
 
 Zr, Th, La, Te, 
 
 Zr, Th, La, De, 
 
 Gl, Y, Zr, Th, 
 
 
 Ta,Nb,W, Mo, 
 
 Ta, Kb, Ti, W, 
 
 Mn, Nb, only 
 
 ( saturated ), 
 
 
 Ti, Zn, Cd, Pb, 
 
 Mo,Zn,Cd, Pb, 
 
 in s. q., or else 
 
 La, Ce, Ta, 
 
 
 Bi. Sb, only in 
 s. q. or yellow. 
 
 Mo, Zn, Ag, 
 white by fl., 
 Fe in s. q. 
 
 gray and op., 
 Ag,Zn,Cd. Pb, 
 Bi, Sb Ni, Te 
 
 white and op. 
 by fl., Nb, in s. 
 q., or else gray 
 
 
 
 
 by c. b. or else 
 
 and op., Ag, 
 
 
 
 
 gray and op. 
 
 Zn, Cd, Pb, Bi, 
 
 
 
 
 
 Sb, Ni, Te, by 
 
 
 
 
 
 c. b., or else 
 
 
 
 
 
 fray and op., 
 
 
 
 
 
 e, in s. q. 
 
 Giay and 
 
 o] aque. 
 
 " 
 
 11 
 
 Air, Zn, Cd, Pb, Ag, Zn, Cd, Pb, 
 'Bi, Si), Ni, Te,| Bi . Sb, Ni, Te, 
 
 
 
 
 especially cold by blowing l:t- 
 
 
 
 
 and by little! tie, or else co- 
 
 
 
 
 blowing, or lorless ; Nb, in 
 
 
 
 
 -else colorless, 
 
 s. q. 
 
 
 
 
 Nb, ins. q. 
 
 
 Very pale 
 
 Ag, in s. q. 
 
 Ag, in 1. q. by fl. 
 
 
 
 " 
 
 yellow. 
 
 
 
 
 
 Pale yel- 
 
 Ag, Cd, Zn, in 
 
 < 
 
 
 
 
 
 low. 
 
 1. q. 
 
 
 
 
 Yellow. 
 
 Ti,W,Pb,Sb, Mo, 
 
 Va,Fe,Ce, white 
 
 Ti,in s. q. orel.se 
 
 Mo in 1. q. op., 
 
 
 in 1. q., U, in 
 
 op. by fl., U, 
 
 bluish- violet, 
 
 and brown, W. 
 
 
 s. q. 
 
 yellow, op. by 
 
 Mo, in s. q., in 
 
 in .1. q. brown. 
 
 
 
 fl. 
 
 1. q. brown, W, 
 
 
 
 
 
 Va. 
 
 
 Orange. 
 
 Or, Fe, in 1. q., 
 Bi, in 1. q. 
 
 ii 
 
 U. 
 
 " 
 
 Red. 
 
 Ce 
 
 " 
 
 " 
 
 a 
 
 Deep red. 
 
 Fe, in 1. q. 
 
 Mn (violet-red). 
 
 " 
 
 " 
 
 Brownish- 
 
 Cr,U 
 
 Ni 
 
 Cu by blowing 
 
 Cu, by blowing 
 
 red. 
 
 
 
 little (muddy). 
 
 little (muddy). 
 
 Violet. 
 
 Mn, Ni, Di 
 
 Di 
 
 " 
 
 Ti, op. by fl. 
 
 Blue. 
 
 Co 
 
 Co, Cu green 
 
 Co 
 
 Co, Cu, nearly 
 
 
 
 when getting 
 
 
 colorless by 
 
 
 
 cold. 
 
 
 c. b. 
 
 Green. 
 
 Ca 
 
 Cr, yellowish 
 
 Fe,Cr, brownish. 
 
 Fe, U, bottle- 
 
 
 
 when getting 
 
 Cu, nearly col- 
 
 green, Cr, Va, 
 
 
 
 cold. 
 
 orless by c. b. 
 
 emerald-green. 
 
 NOTE. Abbreviations employed: s. q., small quantity; 1. q., large quantity; 
 fl., by flaming; c. b., continued blowing; op., opaque. 
 
METALLIC OXIDES WITH SALT OF PHOSPHORUS. 
 
 95 
 
 2. BEHAVIOR OF METALLIC OXIDES AVITH SALT OF 
 PHOSPHORUS. 
 
 Color of 
 the bead. 
 
 In the oxidizing flame. 
 
 In the reduction flame. 
 
 Hot. 
 
 Cold. 
 
 Hot. 
 
 Cold. 
 
 Colorless, a 
 portion of 
 tin- sub- 
 stance un- 
 dissolved 
 (silica 
 skeleton). 
 
 Si 
 
 Si 
 
 Si 
 
 Si 
 
 Colorless. 
 
 Al, Sn, Ba, Ca, 
 Mg, Gl, Y, Zr, 
 Th,La,Nb,Te, 
 in all propor- 
 tions : Tsi, Ti, 
 W, Zn, Cd,Pb, 
 Bi, Sb, in s. q. 
 or else trove or 
 less yellow. 
 
 Al, Sn, Ba, Sr, 
 Ca, Mi;, 01, Y, 
 Zr, Th, La, Te, 
 W, Zn, Cd, Pb, 
 Bi, Sb, Fe, in 
 s. q. 
 
 Al, Sn, Ba, Sr, 
 Ca, M, Gl, Y, 
 Zr, Th, La, Ce, 
 Di, Mn,Ta,Ag, 
 Zu, Cd, Pb, Bi, 
 Sb, Ni, Te, by 
 very c. b., or 
 else gray and 
 op. 
 
 Al, Sn, Ba, Sr, 
 Co, Mg, Gl, Y, 
 Zr, Th (satura- 
 ted),!^, op. by 
 fl. Ce, 1)1, Mn, 
 Ta, Ag, Zn,Cd, 
 Pb, Bi, Sb, Ni, 
 Te, by c. b. or 
 else gray and 
 op. Fe in s. q. 
 
 Gray and 
 opaque. 
 
 it 
 
 - 
 
 Ag, Zn, Cd, Pb, 
 Bi, Sb, especi- 
 ally when cold. 
 Te, Ni. 
 
 Ag, Zn, Cd, Pb, 
 Bi, Sb, Te, Ni. 
 
 Pale yel- 
 low. 
 
 Sb, Zu, in 1. q. 
 
 Ag, Fe 
 
 " 
 
 Fe (greenish in 
 l.q.). 
 
 Yellow. 
 
 Pb, vervl.q.,Bi, 
 Cd, T'a, Ti, W, 
 iu l.q., Ag,Ca, 
 Ni, U, Va, Cr, 
 Fe, in s. q. 
 
 Fe.in l.q ; Ni, in 
 s. q., U (green- 
 ish), Va. 
 
 Ti 
 
 Fe (greenish in 
 l.q.). 
 
 Orange. 
 
 Cr, Fe, in 1. q. 
 
 Ni, in 1. q. 
 
 Fe in s. q. Va. 
 
 Fe while getting 
 cold. 
 
 Red. 
 
 " 
 
 " 
 
 Fe (browu) 
 
 (i 
 
 De.-p red. 
 
 (i 
 
 " 
 
 " 
 
 Cu, op. 
 
 R<'ddish- 
 bruwn. 
 
 Fe, Cr, in very 
 l.q. 
 
 " 
 
 Cr 
 
 Cu, op. 
 
 Violet. 
 
 Mn, Di 
 
 Mn, Di 
 
 Nb in 1. q. 
 
 Nb, Ti 
 
 Blue. 
 
 Co 
 
 Co, Cu (greenish 
 when getting 
 cold). 
 
 Co, W, Nb, in 
 very 1. q. 
 
 Co, W, Nb, iu 
 very 1. q. 
 
 Green. 
 
 Ca, Mo. (yellow- 
 ish) 
 
 Mo, U, (yellow- 
 ish), Cr, emer- 
 ald green. 
 
 U, Mo, Cn 
 
 Cr. U, Mo. Va. 
 
 NOTK. Abbreviations employed: s. q., srnajl quantity; 1. q., large quantity; 
 fl , by flaming; c. b , continued blowing ; op., <>p;iqm.!. 
 
96 MINERALOGY SIMPLIFIED. 
 
 3. EXAMINATION OF MINERALS WITH SODA (Sodium Car- 
 bonate), Na. 2 CO 3 . 
 
 The examination with soda is generally performed on char- 
 coal in the reduction flame, and, as a general rule, the flux is 
 added successively in small portions. It is sometimes better 
 to form the finely pulverized assay into a paste with moistened 
 soda before placing it upon the charcoal. This is particularly 
 necessary when the assay is to be tested for its fusibility with 
 soda, since a great many minerals and ores behave quite dif- 
 ferently with different quantities of flux. 
 
 Instead of sodium carbonate, the neutral potassium oxalate or 
 potassium cyanide may advantageously be used for all experi- 
 ments of reduction, since these reagents exercise even a more 
 powerful reducing action than soda. They are for this reason 
 frequently employed when the presence of such metallic oxides 
 is suspected, whose conversion into metals requires a high tem- 
 perature and the aid of a very efficient deoxidizing agent. 
 
 In subjecting a body to the treatment of soda, we must di- 
 rect our attention to two points. Some substances unite with 
 soda to fusible compounds, others form infusible compounds, 
 and others again are not fused at all ; in the last case the soda 
 is simply absorbed by the charcoal, and the assay is left com- 
 pletely unchanged. 
 
 With soda, the following substances produce fusible com- 
 pounds with effervescence of carbon dioxide (CO 3 ) : 
 
 Silicic oxide Silica (SiO 2 )* fuses to a transparent glassy 
 bead which, after cooling, remains transparent if the soda has 
 not been added in too great excess. 
 
 Titanium dioxide (TiO 2 ) fuses to a transparent glassy bead, 
 
 * Silica belongs to the class of acid-forming oxides, and the silicic 
 acid corresponding to the oxide Si0 2 must have the formula H 4 Si0 4 or 
 Si(OH) 4 =rSi0 2 -f 2H 2 = H 4 Si0 4 . Silicic acid is just as little known 
 as is sulphurous acid = H 2 S0 2 , or carbonic acid = H 2 C0 3 , and, like 
 these acids, it has a great tendency to split up into water and the acid- 
 forming oxide. 
 
EXAMINATION OF MINERALS WITH SODA. 97 
 
 which is dark-yellow while hot, but on cooling becomes turbid 
 and crystalline. 
 
 Tungsten trioxide (WO 3 )* and Molybdenum trioxide (MoO 3 )t> 
 after the carbon dioxide is driven off, are absorbed by the char- 
 coal. 
 
 Tantalum pentoxide (Ta 2 O 5 ), Vanadium pentoxide (V 2 O 5 ), 
 and Columbiutn (niobium) pentoxide (Cb 2 O 5 ) or (Nb 2 O 5 ) also 
 yield fusible compounds and sink into the charcoal. 
 
 Lime, magnesia, zirconia, thoria, yttria, and glucina (beryl- 
 lium oxjde), as well as cerium and uranium oxides, are not 
 attacked: they remain. unchanged, while the soda sinks into 
 the charcoal. 
 
 The salts of barium and strontium form, with soda, fusible 
 compounds, which are absorbed by the charcoal. 
 
 Sodium carbonate is also used for the detection of 
 
 a. Sulphur, selenium, and tellurium compounds, which give 
 with it a fused mass,]: yielding a black, or brown, stain when 
 laid upon a piece of silver and moistened with water. 
 
 b. Manganese and chromium, with the soda alone, or, better, 
 with addition of sodium nitrate, yield colored masses; the for- 
 mer a green mass of inanganate, and the latter a yellow mass 
 of chromate. 
 
 The second point to be observed is the elimination of metal- 
 lic matter. 
 
 When treated with soda on charcoal in the R. FL, the follow- 
 ing metallic oxides are reduced: the oxides of the noble metals 
 and the oxides of arsenic, antimony, bismuth, indium, cadmium, 
 copper, cobalt, iron, lead, mercury, nickel, tin, zinc, molyb- 
 denum, tungsten, arid tellurium. Of these, arsenic and mercury 
 vaporize so rapidly that frequently not even a coating is left on 
 the charcoal. Antimony, bismuth, cadmium, lead, zinc, and 
 tellurium are partially volatilized, and form distinct coatings on 
 the charcoal. 
 
 * Tungstic acid (wolframic acid) = H a WO 
 f Molybdic acid = Il,MoO 4 -f- 1I,O. 
 J Ilepar sulplmris (liver of sulphur), 
 i) 
 
98 MINERALOGY SIMPLIFIED. 
 
 The non-volatile reduced metals are found mixed with the 
 soda. To separate them from the adhering soda and charcoal 
 powder, we proceed in the following manner: The fused mass 
 of soda and metal, and the portion of the charcoal immediately 
 below and around the assay, are placed in a small mortar, ground 
 to powder, then mixed with a little water and stirred up. The 
 heavy metallic particles settle to the bottom, a portion of the 
 soda dissolves, and the charcoal powder remains suspended in 
 the water. The liquid is carefully poured off, and the residue 
 treated repeatedly in the same manner until all foreign matter 
 is removed. The metal remains behind as a dark heavy pow- 
 der; or, when the metal is ductile or easily fusible, in the shape 
 of small flattened scales with metallic lustre. These may be ex- 
 amined with the magnifying glass and also with the magnet. 
 If the substance under examination contains several metallic 
 oxides, the metallic mass obtained is usually an alloy, in which 
 the several metals may be detected by processes to be described 
 hereafter. It is only in some exceptional cases that separate 
 metallic globules are obtained, as, for example, in substances 
 containing iron and copper. 
 
 4. EXAMINATIONS OF METALS WITH SODIUM THIOSULPHATE 
 (HYPOSULPHITE OF SODIUM), Na 2 S 2 O 3 . 
 
 With all the metals which can be precipitated in the wet way 
 by hydrogen sulphide, the same reaction may be obtained in 
 the dry way by heating the powdered substance with powdered 
 thio sulphate of sodium in a reagent tube. After the decompo- 
 sition has taken place recognized by the evolution of hydrogen 
 sulphide the melted mass exhibits very clearly the peculiar 
 coloration of the metallic sulphides produced. In many cases 
 this reaction is enhanced by a small addition of oxalic acid. 
 
 Since the thiosnlphate of sodium contains considerable water 
 of crystallization, the greater portion of this must be removed 
 from this reagent before experimenting, or the glass-tube must 
 be held horizontally to prevent its cracking, in which case the 
 open end had better be closed with cotton-wool. 
 
EXAMINATION WITH ACID POTASSIUM SULPHATE. 09 
 
 The sulphide reactions of the metals are demonstrated in the 
 following table, in which their behavior with borax on platinum 
 wire is shown by way of comparison. These methods supple- 
 ment each other very instructively. 
 
 5. TABULAR ARRANGEMENT SHOWING THE BEHAVIOR OF 
 OXIDES, WHEN TREATED BEFORE THE BLOWPIPE, WITH 
 SODIUM THIOSULPHATE, TOGETHER WITH THEIR REAC- 
 TIONS WITH BORAX. 
 
 Metallic oxides. 
 
 Behavior with 
 
 Na 2 So0 3 . 
 
 Behavior with borax on platinum wire 
 (the bead cold). 
 
 Oxidizing flamo. 
 
 Reducing flame. 
 
 Antimony oxide 
 
 Orange-red, 
 
 Colorless, 
 
 Gray to colorless. 
 
 Arsenic 
 
 Lemon yellow, 
 
 (Vaporizes), 
 
 (Vaporizes). 
 
 Bismuth 
 
 Black, 
 
 Colorless, 
 
 Gray to colorless. 
 
 Cadmium 
 
 Yellow, 
 
 t I 
 
 a n u 
 
 Chromium 
 
 Green, 
 
 Grass-green, 
 
 Emerald-green. 
 
 Cobalt 
 
 Black, 
 
 Blue, 
 
 Blue. 
 
 Copper 
 
 " Bluish-green, 
 
 Brown. 
 
 Gold 
 
 K 
 
 Reduced to metal 
 
 without dissolv'g. 
 
 Iron 
 
 a 
 
 Yellow, 
 
 Bottle-green. 
 
 Lead 
 
 tl 
 
 Colorless, 
 
 Gray to colorless. 
 
 Manganese 
 
 Light-green, ; Violet (amethyst) 
 
 Colorless. 
 
 Mercury 
 
 Black, 
 
 Vaporizes, 
 
 Vaporizes. 
 
 Molybdenum 
 
 Brown, 
 
 Colorless, 
 
 Brown. 
 
 Nickel 
 
 Black, 
 
 Reddish-brown, 
 
 Gray to colorless. 
 
 Platinum 
 
 i t 
 
 Reduced to metal 
 
 without dissolv'g. 
 
 Silver 
 
 " 
 
 Colorless, 
 
 Gray to colorless. 
 
 Thallium 
 
 a 
 
 < i 
 
 Colorless. 
 
 Tin 
 
 Brown, 
 
 a 
 
 u 
 
 Uranium 
 
 Black, 
 
 Yellow, 
 
 Bottle-green. 
 
 Zinc 
 
 White, 
 
 Colorless, 
 
 Gray to colorless . 
 
 G. EXAMINATION WITH ACID POTASSIUM SULPHATE OR 
 CONCENTRATED SULPHURIC ACID. 
 
 To determine the presence of volatile acids, a small quantity 
 of the substance is heated with acid potassium sulphate, or with 
 concentrated sulphuric acid (in the latter case, however, not 
 to the boiling-point of the acid), and the following appearances 
 noticed : 
 
100 MINERALOGY SIMPLIFIED. 
 
 1. A COLORED GAS is EVOLVED. 
 
 a. Nitrogen tetroxide (N0 2 ) fumes are recognized by their 
 reddish-brown color and characteristic odor ; evolved from 
 nitrates and nitrites. With nitrates the reaction is promoted 
 by the addition of copper filings. 
 
 b. Chlorine tetroxide (hypochloric acid), C1 2 O 4 , yellowish- 
 green, odor like chlorine, bleaches litmus paper. The evolution 
 of this gas by this treatment indicates the presence of chlorates.* 
 
 c. Iodine, from iodides, may be recognized by its violet 
 vapors, which color starched paper blue. lodates* give this 
 reaction after the addition of ferrous sulphate (copperas). 
 
 d. Bromine ; reddish-brown vapors, with pungent, unpleasant 
 odor, which turn starch-paste yellow. Yielded by bromides and 
 bromates. The color of the vapor is best seen on looking down 
 the tube. 
 
 2. A COLORLESS, ODOROUS GAS IS-EVOLVED. 
 
 a. Sulphur dioxide (sulphurous acid), evolved from sulphites 
 and polythionates, is easily recognized by its suffocating odor 
 and bleaching properties (litmus, etc.). 
 
 b. Hydrochloric acid, from chlorides, recognized by its odor 
 and by the clouds of ammonium chloride (sal-ammoniac) which 
 are formed, when a glass-rod, moistened with ammonia-solution, 
 is held over the tube. 
 
 c. Hydrofluoric acid, from fluorides, smokes, has a very suf- 
 focating odor, and strongly etches glass. 
 
 d. Hydric sulphide (sulphydric acid, sulphide of hydro- 
 gen, sulphuretted hydrogen), H 2 S, from sulphides, of a repul- 
 sive odor, blackens paper moistened with lead acetate (sugar of 
 lead) solution. 
 
 e. Cyanic acid, from cyanates, has a characteristic pungent 
 odor ; it brings tears to the eyes, and renders lime-water turbid. 
 
 f. Acetic acid, from acetates, is known by its pungent, 
 " vinegar" odor, and also by yielding fragrant acetic ether on 
 heating with sulphuric acid and alcohol. 
 
 * The chlorates, iodates, and bromates deflagrate when heated on 
 charcoal. 
 
EXAMINATION WITH ZINC AND HYDROCHLORIC ACID. 101 
 
 3. A COLORLESS AND ODORLESS GAS is EVOLVED. 
 
 a. Carbon dioxide (carbonic acid gas) = CO 2 , is expelled 
 from carbonates with effervescence ; it renders lime-water turbid. 
 
 b. Carbon monoxide (carbonic oxide), CO, which burns 
 with a bluish flame, may arise from oxalates, formates, cyan- 
 ides, ferrocyanides, and ferricyanides, 
 
 c. Chromic acid evolves oxygen, and the liquid turns brown 
 or green. 
 
 d. Organic acids are recognized by the blackening due to 
 the separation of carbon (except oxalic acid, which yields CO 
 and C0 2 ). 
 
 The acids which cannot be detected by the above methods, 
 though easily detected in other ways, are : sulphuric, phos- 
 phoric, arsenic, boric, silicic, tungstic, molybdic, and titanic. 
 
 7. EXAMINATION WITH ZINC AND HYDROCHLORIC ACID 
 AFTER PREVIOUS DECOMPOSITION (FUSION) OF THE MlN- 
 
 ERAL. 
 
 A mixture of sodium carbonate and nitre is added to the finely- 
 powdered assay, the mass is moistened slightly, and placed in a 
 small spiral of platinum wire, of about 2 to 3 mm. diameter. 
 After fusing for a short time, the glowing mass in the spiral is 
 thrown off into a porcelain dish and digested with a little water 
 in a test-tube. Afterwards, a little hydrochloric or sulphuric 
 acid is added, and a strip of zinc is brought into the solution. 
 By the reducing agency of the nascent hydrogen thus formed 
 various colors are produced, as shown in the following table : 
 
 Molybdic trioxide (molybdic acid) : blue, then green, finally 
 blackish-brown. 
 
 Tungsten trioxide (Wolframic acid) : blue, then copper-rejj. 
 
 Columbium (niobium) pentoxide (niobic acid) ; blue, often 
 also brown (with strongly acid solution). 
 
 Vanadium pentoxide (vanadic acid) : blue, then green, 
 finally violet. 
 
 Chromium trioxide (chromic acid) : green. 
 
 Titanium dioxide (titanic acid) : violet. 
 
 9* 
 
102 MINERALOGY SIMPLIFIED. 
 
 8. EXAMINATION WITH COBALT SOLUTION. 
 
 A few substances, when moistened witli a solution of cobalt 
 nitrate and exposed to the action of the 0. Fl. assume a pecu- 
 liar color. The use of this test is, however, very limited, since 
 the reaction can only be clearly seen in those bodies which, 
 after having been acted upon by the O. FL, present a white 
 appearance or nearly so. 
 
 Substances which are sufficiently porous to absorb a liquid 
 are merely moistened with a drop of cobalt solution, held with 
 the platinum -forceps; and submitted to the O. Fl. Other sub- 
 stances must be powdered, the powder placed on charcoal, 
 moistened with a drop of cobalt solution, and treated as above. 
 The color can only be distinguished after cooling. A bluish 
 color of more or less purity, but rather dull, indicates the pre- 
 sence of alumina, and a flesh-color (pale-reddish color) that of 
 magnesia. It must, however, be borne in mind that the alka- 
 line and some other silicates, when heated with cobalt solution 
 to a temperature above their fusing point, also assume a blue 
 color, owing to the formation of cobalt silicate. In testing for 
 alumina, therefore, the heat must not be raised so high as to 
 cause fusion of the assay. In testing for magnesia this precau- 
 tion is not necessary ; as, on the contrary, the color will appear 
 the brighter and the more distinct the higher the temperature 
 to which the assay is exposed. The alumina and magnesia 
 reactions are prevented by the presence of colored metallic 
 oxides, which generally produce a gray or black mass, unless 
 present in too minute quantity. 
 
 Among the oxides of the heavy metals, those of zinc and tin 
 assume characteristic colors with solution of cobalt. The re- 
 action is best seen when the assay, alone or mixed with soda, 
 is exposed to the R. Fl. on charcoal. The ring of oxide which 
 is deposited around the assay is then moistened with solution 
 of cobalt and treated with the O. Fl. Zinc takes a fine yel- 
 lowish-green, and tin oxide a bluish-green color. 
 
 Besides the compounds above mentioned, there are some 
 
EXAMINATION FOR FLAME COLORATIONS. 103 
 
 others which, when exposed to the action of cobalt solution and 
 heat, experience a change of color, but still this reagent does 
 not justify its employment for their recognition. In fact, only 
 the colorations of alumina, magnesia, zinc, and tin are of real 
 use in the determination of these substances. 
 
 The following table gives the more definite colorations caused 
 by cobalt solution : 
 
 Blue: Alumina; deep color ; infusible. 
 
 Silica and silicates; pale blue; with much solution, black or 
 
 dark gray. Thin edges of assay fuse to a reddish-blue glass 
 
 at a high temperature. 
 Phosphates, borates, and silicates of the alkalies yield a blue glass. 
 
 Green : Zinc oxide ^yellowish-green. 
 
 Titanium dioxide * > 
 
 Tin oxide ; bluish-green. 
 
 Antimony oxide ; impure-green. 
 Flesh-red : Magnesia ; pale flesh-red or pink. 
 
 Tantalum pentoxide ; hot, light gray ; cold, flesh-red. 
 Violet : Zirconia ; impure violet. 
 
 Magnesium arseuate and phosphate fuse and become violet-red. 
 Brown: Baryta ; hot, reddish-brown or brick-red ; cold, colorless. 
 Gray: Strontia ; dark-gray to black. 
 
 Lime ; gray. 
 
 Glucina : bluish-gray. 
 
 Columbium (niobium) pentoxide ; brownish-gray. 
 
 CHAPTER VI. 
 
 COLORED FLAMES, FLAME REACTIONS, AND SPECTRUM 
 ANALYSIS. 
 
 1. EXAMINATION OF THE ASSAY IN THE PLATINTM 
 FORCEPS FOR FLAME COLORATIONS. 
 
 MANY substances, especially the alkalies and alkaline earths, 
 wnen brought into a non-luminous flame, impart to it distinct 
 colorations, affording in many cases characteristic means for 
 detecting them even in the minutest quantities, e. g., sodium 
 
1 Barium salts obscure the reaction. 
 
 104 MINERALOGY SIMPLIFIED. 
 
 salts tinge the flame yellow ; potassium compounds, violet ; 
 strontium salts, scarlet red ; lithium salts, carmine-red ; etc. 
 
 The Bunsen burner, previously described (Fig. 49), is especi- 
 ally well adapted to such observations. The coloring substance 
 may be brought on a platinum wire loop into the zone of fusion 
 of the flame. When mixtures of different flame-coloring sub- 
 stances are examined, indecisive tests are usually produced ; 
 thus, in a mixture of sodium and potassium salts, only the yellow 
 sodium flame is evident, but by viewing the flame, according 
 to Bunsen and Merz, through colored glasses or fluids, the 
 mixed colors may be dissected. 
 
 The following table gives the more (iefinite colorations : 
 
 Red Flames. 
 
 Lithium : carmine-re^. 
 Strontiums scarlet-red.* 
 Calcium : yellowish-red.* 
 
 Violet Flames. 
 
 Potassium : violet-red. Sodium and lithium salts obscure the 
 
 reaction. 
 
 Caesium: ) Like potassilim . 
 Rubidium : > 
 
 Yellow Flames. 
 Sodium salts. 
 
 Green Flames. 
 
 Copper oxide : emerald-green; when mois-tened with HC1, blue. 
 
 Thallium: grass-green. 
 
 Phosphoric acid : bluish-green. > After their salts are moistened 
 
 Boric acid : yellowish-green. > with sulphuric acid. 
 
 Barium salts : yellowish-green.* 
 
 Molybdic acid : faint yellowish-green. 
 
 Tellurious acid : green, giving off fumes. 
 
 Nitric and nitrous acid : bronze-green, disappearing quickly. 
 
 Zinc : whitish-green. 
 
 Slue Flames. 
 
 Copper chloride : a7,ure-blue, afterwards green. 
 Iridium : indigo-blue (in both flames). 
 
 * Especially after moistening with HC1. 
 
EXPERIMENTS. 
 
 105 
 
 Selenium : cornflower blue, accompanied by the odor of rotten 
 bone-radish. 
 
 Arsenic : bluish. 
 
 Antimony : faint greenish-blue. 
 
 Lead : blue. 
 
 2. APPARATUS. 
 
 The apparatus for these observations is simple, viz., a blue, 
 a violet, a red, and a green glass. The stained glasses found 
 
 Fig. 103. 
 
 in commerce possess generally the proper shades of color. 
 Indigo solution may be substituted for blue glass. A hollow 
 prism (Figs. 103 and 104), made of plate glass, whose 
 principal section forms a triangle 150 millimetres in Fig. 104." 
 length, and 35 millimetres in diameter at the thick 
 end. The solution with which it is filled is pre- 
 pared by dissolving 1 part of indigo powder in 8 
 parts of strong sulphuric acid, heating the mixture 
 on the sand-bath, and stirring it frequently with a 
 glass rod. The syrupy solution thus obtained is 
 diluted with '1500 to 2000 parts of water,* and 
 filtered through felt or thick blotting paper. 
 
 3. EXPERIMENTS. 
 
 In the following experiments the prism is moved horizontally 
 before the eye, so that the rays of the flame always pass through 
 gradually thicker layers of the fluid medium. The alkaline 
 
 * The cold indigo solution must be gradually poured into the proper 
 amount of water, the reverse operation might prove dangerous. 
 
10G MINERALOGY SIMPLIFIED. 
 
 substances, brought singly into the flame, exhibit the following 
 changes : 
 
 a. Chemically pure calcium chloride,* CaCl 2 , produces a 
 yellow flame, which, even with very thin layers of the indigo 
 solution, passes through a tinge of violet into the original blue- 
 lamp flame. 
 
 b. Chemically pure sodium chloride, NaCl, the same. 
 
 c. Chemically pure potassium carbonate, K 2 C0 3 , or potas- 
 sium chloride, KC1, appears of a sky-blue, then violet, and at 
 last of an intense crimson color, even when seen through the 
 thickest layer of the solution. Admixtures of sodium or cal- 
 cium do not hinder the reaction. 
 
 d. Chemically p~ure lithium carbonate, Li 2 CO 3 , or lithium 
 chloride, LiCl, gives a violet-red flame, which, with increas- 
 ing thickness of the medium, becomes gradually feebler, and 
 disappears before the thickest layers pass before the eye. Cal- 
 cium and sodium are without influence on this reaction. 
 
 A Blue, a Violet, a Red, and a Green Glass. 
 
 The stained glasses found in commerce possess generally the 
 proper shades of color. The blue is colored by cobalt pro- 
 toxide ; the violet by manganese sesquioxide ; the red (partly 
 colored and partly uncolored) by cuprous oxide ; and the green 
 by iron sesquioxide and cupric oxide. Merz,j" who has made 
 a complete study of this subject, employs with these glasses 
 Bunsen's burner, and also a flame of pure hydrogen. The 
 substances which he describes as giving characteristic colors 
 to the flame of a Bunsen burner, in addition to those previously 
 known, are nitric and chromic acids, while phosphoric and sul- 
 
 * Chlorides, on account of their volatility, yield generally the best 
 coloration, and for this reason the substance under examination is 
 moistened with hydrochloric acid, or is treated with silver chloride 
 and again heated. The substance is held in the one hand and the 
 colored glass in the other. 
 
 f Gr. Merz, Plammenfiirbungen, Journ. f. pract. Chemie, Bd. 80, p. 
 487. 
 
TESTING CHEMICAL MIXTURES. 107 
 
 phuric acids give a peculiar coloration to the dark core of the 
 flame of hydrogen. 
 
 The flame of Bunsen's burner, which is preferred for these 
 reactions, gives three sorts of colors. 
 
 1. Border colors. These are of course peculiar only to the 
 most volatile substances. To produce them, the loop of plati- 
 num wire is held outside of the flame about one or two milli- 
 metres from the lower portion of the outer limit. 
 
 2. Mantle colors. Those which are seen when the substance 
 is held in the bright blue-colored mantle which forms the outer 
 portion of the flame. 
 
 3. Flame colors. To produce these, the loop is to be held 
 horizontally and in the hottest part of the mantle. The hydro- 
 yen flame yields another fourth species of color, viz., the 
 
 4. Core colors. These are produced only by sulphuric and 
 phosphoric acids, which communicate respectively a blue and 
 green tinge to the cold core of the hydrogen flame. 
 
 4. TESTING CHEMICAL MIXTURES. 
 
 In order to detect several flame-coloring elements when occur- 
 ring together it is best to use the spectroscope (Figs. Ill, 112), 
 the theory, construction, and use of which will be found fully 
 described on page 127 and following pages, to which the reader 
 is referred for information. The direct-vision pocket spectro- 
 scope, such as that of Browning and others, is well adapted for 
 blowpipe investigations. 
 
 All flame-coloring substances may, according to their vola- 
 tility, be arranged in three classes: 1, certain acids; 2, alka- 
 lies ; and 3, alkaline earths, to which may be added the heavy 
 metal copper. If the substances are brought into the flame of 
 the Bunsen burner mentioned on page 111, we may detect 
 
 Acids. 
 
 a. Nitric and nitrous acids give a bronze-green border color, 
 usually with an orange-colored margin. The assay is to be 
 previously dried in the flame, and then either moistened with 
 
108 MINERALOGY SIMPLIFIED. 
 
 HC1, or dipped into a solution of acid potassium sulphate, 
 according as we wish to test for nitrous or nitric acid. Am- 
 monium and cyanogen compounds give the same reaction but 
 more faintly. 
 
 b. Phosphoric acid gives a gray yellowish-green border color, 
 after moistening with sulphuric acid. In the presence of boric 
 acid, phosphoric acid can only be discovered by the intense 
 green flame produced by heating the assay in a hydrogen flame 
 after moistening with a solution of hydrofluosilicic acid. For 
 this purpose the hydrogen is delivered from a platinum jet, for 
 instance, the side tube of a blowpipe. 
 
 c. Boric acid gives a beautiful green mantle color, which is 
 so intense that this acid may be recognized in the presence of 
 considerable quantities of phosphoric acid. Borates require to 
 be first decomposed with sulphuric acid. 
 
 d. Molybdic acid yields a yellowish-green flame similar to 
 that shown by barium salts. 
 
 e. Hydrochloric acid gives a very weak greenish-blue border 
 color which lasts but an instant, and hence frequently escapes 
 detection. 
 
 f. Sulphuric acid produces a fine blue core color, being re- 
 duced to sulphur dioxide. The free acid gives the color when 
 the platinum wire loop is held in the border of the flame, but 
 a sulphate must be held in the middle of the flame. In the 
 latter case it is best to first dip the assay into concentrated 
 hydrochloric or hydrofluosilicic acid. 
 
 Chromic acid gives a dark brownish-red border color and a 
 rose-red mantle color. The dry assay is to be moistened with 
 concentrated sulphuric acid, and held in the border. Chromic 
 oxide gives no color, and should be first oxidized to chromic acid 
 by moistening with a solution of sodium hypochlorite and dry- 
 ing. 
 
 Alkalies. 
 
 a. Potassium gives a grayish-blue mantle color and a rose- 
 violet flame color. The color appears reddish-violet through 
 
TESTING CHEMICAL MIXTURES. 109 
 
 a blue glass* (detection in presence of sodium), violet through 
 violet-colored glass, and bluish-green through green glass. 
 The assay is to be moistened with sulphuric acid, and re- 
 peatedly exposed to the flame for a short time. 
 
 b. Sodium gives an orange-yellow flame color, which in 
 quantity appears blue through blue glass, but which is invisi-. 
 ble when present in small amounts. Seen through green glass 
 the flame has an orange color, characteristic of all sodium 
 compounds. If a crystal of potassium-bichromate is held near 
 to the sodium flame, the former becomes quite colorless, and a 
 red spot of mercuric iodide on paper becomes white with a 
 faint tinge of fawn color. The assay is moistened with sul- 
 phuric acid, dried, and then held in the hottest part of the 
 flame. 
 
 c. Lithium yields a carmine-red flame color, which appears 
 violet-red through blue glass, and carmine-red through violet 
 glass. In the presence of sodium, lithium is detected by the 
 blue glass. In the presence of potassium, Bunsen's method is 
 employed. The assay is brought into the zone of fusion of a 
 Bunsen gas-lamp, and this flame is compared simultaneously, 
 through an indigo prism, with one obtained from a pure potas- 
 sium salt held in the corresponding part of the flame opposite 
 to the assay. Through the thinnest layer of 'the solution the 
 lithium flame appears redder than the pure potassium flame ; 
 through thicker layers the flames appear equally red, when the 
 proportion of lithium to potassium is very small. If, however, 
 lithium predominates in the assay, the intensity of the red 
 flame diminishes rapidly as the prism is moved ; whilst the 
 pure potassium flame is scarcely any feebler. Sodium, when 
 not present in large excess, modifies these effects but slightly. 
 
 Potassium and lithium are not likely to be confounded with 
 strontium if the assay be treated as described under potassium, 
 since strontium compounds are not volatilized at the low tem- 
 perature thus obtained. 
 
 * Cartmell, Phil. Mag., May, 1858, p. 328. 
 10 
 
110 MINERALOGY SIMPLIFIED. 
 
 Alkaline Earths. 
 
 The assay is repeatedly moistened with sulphuric acid, dried 
 and placed in the hottest part of the mantle. After all the 
 alkalies are volatilized the following reactions appear : 
 
 a. Barium gives a yellowish-green flame color, which appears 
 bluish-green through green glass. If the green disappears, 
 and a red color makes its appearance, the assay is to be re- 
 peatedly moistened with hydrochloric acid, and immediately 
 introduced while wet into the hottest part of the flame. When 
 the bluish-green color is no longer seen we proceed to test for 
 calcium. 
 
 b. Calcium is present when the red-flame color, on evapo- 
 rating the last portion of hydrochloric acid (spitting of the 
 assay), appears finch-green through the green glass. 
 
 c. Strontium is known by the purple to rose color, which 
 appears through blue glass, as the assay spits in the flame after 
 being moistened with HC1. Under identical conditions calcium 
 gives a faint greenish-gray color. 
 
 Copper. 
 
 Copper chloride yields a sky-blue flame color ; the nitrate 
 gives a pure green one. By the combined observations of 
 both colors, copper may readily be distinguished from all other 
 metals which give similar colors. 
 
 The remaining flame-coloring metals, such as arsenic, anti- 
 mony, tin, lead, mercury, and zinc, exhibit, especially in the 
 form of chlorides, more or less intense bluish or greenish mantle 
 colors, which, however, are of no great value in analysis. As 
 a rule the appearance of these colors can be prevented by 
 moistening with sulphuric acid. It is best, however, to expel 
 on charcoal the metals which give an incrustation, before 
 testing for alkalies or alkaline earths by flame coloration. 
 
 In order to detect the alkalies in silicates it is sufficient to 
 decompose the assay on platinum wire with some pure gypsum 
 (sulphate of lime). If, on the contrary, the alkaline earths 
 
To face p. 111. 
 
 Fig. 105. 
 
 ft.,, a, a, ft,, the dark nucleus 
 a,, c, a,, b, the flame mantle, 
 a, fc, a, the luminous point not in 
 the normal flame, but formed, 
 when needed, by partially turn- 
 ing the collar. 
 
BUNSEN'S FLAME REACTIONS. Ill 
 
 are looked for, the decomposition must be effected by means 
 of sodium carbonate. The substance is fused with the reagent 
 in a platinum spoon, the fused mass extracted with water, and 
 the residue treated with HC1, when. silicic acid separates out, 
 and the solution is then examined in the flame. 
 
 5. BUNSEN'S FLAME REACTIONS. BUNSEN'S GAS-LAMP. 
 
 According to Bunsen,* most of the tests obtainable with a 
 blowpipe can be produced by means of the non-luminous flame 
 of a Bunsen burner, Fig. 105, provided with a movable collar, 
 m (by turning of which the access of air may be regulated), 
 and a conical chimney, d, d, d 1 , d f , of such dimensions, that 
 the flame burns perfectly steady. The flame should have the 
 dimensions shown in Fig. 105. 
 
 The six portions of the flame, which serve for conducting 
 the different reactions, are distinguished as follows : 
 
 I. The base of the flame at A, having the lowest tempera- 
 ture, is especially adapted for separating from a mixture of 
 flame-coloring substances the most volatile ones first. 
 
 II. The zone of fusion at B, having the highest temperature, 
 is therefore particularly suited for testing the fusibility, vola- 
 tility, etc., of an assay. 
 
 III. The lower oxidizing flame at G, is especially employed 
 for the higher oxidation of oxides dissolved in fused beads. 
 
 IV. The upper oxidizing flame at E, acts with the greatest 
 power when the draft holes, A, are completely opened. All 
 the roastings and oxidations are here executed, provided that 
 not too high a temperature is required. 
 
 V. The lower reducing flame at D, less energetic than the 
 
 * Annal. der Chem. u. Pharm., Bd. 138, p. 257 ; also, J. Landauer, 
 "Liithrohr Analyse," 2te Anil. Berlin, 1881, p. 62. 
 
 A new edition of R. Bnnsen's flame reactions has lately appeared, 
 entitled : Flammen Reactionen, Heidelberg, 1880, which the author 
 AV.-IS unable to consult, however, but made free nse of many descrip- 
 tions given by J. Landauer, in his " Lothrohr Analyse," Berlin, 1881. 
 
 Extracts are also found in Annal. Chem. und Pharm. cxxxviii. p. 
 257, and Philog. Mag. [4] xxxii. p. 81 (translated by Prof. Roscoe). 
 
112 
 
 MINERALOGY SIMPLIFIED. 
 
 following, gives for that very reason peculiar reactions ; it 
 serves especially for reductions on charcoal, and of beads of 
 fused salts. 
 
 VI. The upper reducing flame at C. The point aba, 
 above the dark cone of the flame, is not visible when the draft 
 holes, h, are entirely o'pen ; but if this luminous point is made 
 too large, soot is deposited, which is not admissible. This part 
 of the flame is particularly suitable for the reduction of metals 
 which it is desired to collect as metallic incrustations or coatings. 
 
 The following apparatus serves as a support for bringing test 
 specimens into the flame : 
 
 6. APPARATUS AND METHOD EMPLOYED FOR SUBMITTING 
 
 TEST SUBSTANCES TO THE FLAME. 
 
 Behavior of the Elements at High Temperatures This is 
 
 one of the most important reactions which can be employed 
 for the detection and separation of substances. To produce 
 with the flame alone a temperature as high or higher than that 
 of the ordinary blowpipe, the radiating surfaces of the heated 
 body must be as limited as possible, and therefore be on a very 
 small scale. 
 
 By bringing the moistened loop of the platinum wire (of the 
 thickness of a horsehair) in contact with the powdered sub- 
 stance that is to be examined, a portion of it adheres ; and 
 
 when the loop is held for some 
 time near the flame, and finally 
 within it, the substance sinters 
 or fuses firmly upon the wire. 
 When the substances act upon 
 platinum, a thread of asbestos 
 is used. Salts that decrepitate 
 are ground to the finest powder 
 on the porcelain lamp plate, 
 Fig. 106, with the elastic blade 
 of the knife, Fig. 107, and 
 
 Fig. 105. 
 
SUBMITTING TEST SUBSTANCES TO THE FLAME. 
 
 113 
 
 drawn up on to a moistened strip of one square centimetre 
 of Swedish filter paper. If the paper is then burnt, being 
 held with the platinum forceps, or better, between two rings 
 of fine platinum wire, the sample remains as a coherent crust, 
 which may now, without difficulty, be heated in the flame. 
 
 Fig. 106. Fig. 107. 
 
 Fig. 108. 
 
 Q 
 
 The substance under examination may be kept for any length 
 of time in a given part of the flame by means of a Bunsen 
 , Fig. 108. The arm, a, is fastened to the carrier, A 
 10* 
 
114 MINERALOGY SIMPLIFIED. 
 
 so fixed on the stand by a self-clamping spring slide, that it 
 can be moved both horizontally and vertically. The glass 
 tube, c?, is fastened on this arm, a, and the fine platinum wire 
 (fused into the glass tube) thus held in the flame. Splinters 
 (fibres) of asbestos are inserted in the glass tube, &, which 
 slips into the holder, and may be moved with the carrier, A. 
 The carrier, B, is provided with a spring-clamp for holding 
 test-tubes, which have to be heated for a considerable time in 
 a particular part of the flame. The little turn-table, c, con- 
 tains nine upright supports for storing the wire tubes employed 
 in the experiments* 
 
 For testing liquids, the wire of the loop is flattened by a 
 few taps with a hammer; then, if dipped into the substance, 
 it lifts up a drop, which, by holding it near the flame, slowly 
 evaporates, and the residue, if any, may be brought into the 
 zone of fusion. By means of these arrangements, a small 
 particle of the substance may be brought into the flame, and 
 its behavior in the coldest and hottest parts of the flame 
 ascertained, the substance being examined with a lens after 
 each change of temperature. 
 
 Platinum wire, no thicker than a horsehair (i. e., a piece 
 1 decimetre long, must not exceed 0.034 grrns. in weight), is 
 used in experiments for examining the fusibility, volatility, 
 flame coloring, and also for reactions with borax, salt of phos- 
 phorus, and soda. 
 
 Fibres of asbestos, about one-fourth as thick as an ordinary 
 match, serve instead of platinum (where this metal is attacked), 
 and are moistened before receiving the test substance. 
 
 Charcoal rods as a substitute for ordinary charcoal. They 
 are prepared from ordinary friction matches ; the head is broken 
 off and three-quarters of its length coated with fused, crystal- 
 lized sodic carbonate, and charred in the flame with a rotary 
 motion. The rods when thus glazed are partially protected 
 against combustion. 
 
 Tubes of thin glass 3 cm. long, 2 to 3 mm. wide, and closed 
 at one end. 
 
REAGENTS. 115 
 
 7. REAGENTS. 
 
 The following chemical reagents are specially employed for 
 Bunsen's flame reactions : 
 
 Stannous chloride (SnCl 2 ). The solution must be kept in a 
 glass-stoppered bottle. In order to prevent its transformation 
 to stannic chloride (SnCl 4 ) g, few small grains or pieces of 
 metallic tin are -placed in the bottle. The salt is a powerful 
 reducing agent, and serves to distinguish metallic coatings, 
 and for the recognition of Gold, Molybdenum, Tungsten 
 ( Wolfram), etc. 
 
 Caustic soda solution (NaOH) is likewise employed for 
 recognition of metallic coatings, as alsp for the recognition of 
 Cobalt, Nickel, Tin, etc. 
 
 Nitrate of silver solution (AgNO 3 ), quite neutral, is used to 
 distinguish coatings and for detecting Chromium and Vana- 
 dium. 
 
 Faming hydriodic acid (IH), obtained by the action of 
 moist air on phosphorus tri -iodide. To prepare the latter, 1 
 part of phosphorus is dissolved in carbon di-sulphide, and 
 gradually 12.3 parts of iodine added. This solution is now 
 gently heated to expel most of the di-sulphide of carbon, and 
 next placed in some cooling mixture, whence crystalline lamina; 
 of phosphoric tri-iodide separate, which fuse at 55 C. These 
 are put into a wide-necked, flat-bottomed glass flask, which can 
 be tightly closed with a glass stopper. The small porcelain 
 dishes with the adhering coatings on their surfaces may thus 
 be placed over the flask and readily exposed to'the fumes of the 
 hydriodic acid, converting these deposits into iodine compounds. 
 When the fuming of this reagent ceases, it is rendered active 
 again upon the addition of some anhydrous phosphoric acid. 
 These coatings may likewise be turned into iodides by saturat- 
 ing an asbestos-rod with an alcoholic solution of iodine, firing 
 it, and moving the flame to and fro, beneath the coated porce- 
 lain dish. Should a brown-colored product, resulting from the 
 
116 MINERALOGY SIMPLIFIED. 
 
 separation of free iodine, condense on the porcelain dish, it may 
 be removed by careful heating. 
 
 Ammonia (NH 3 ) and ammonium sulphide (or ammonium 
 sulphydrate), NH 4 HS, are employed for determining such 
 coatings. 
 
 Bromine (Br), kept in a wide-necked, well-closed flask, is 
 used for exposing substances to its vapor, which, in the presence 
 of water, acts as an oxidizing agent. 
 
 Ferrocyanide of potassium (yellow prussiate of potash), 
 K 4 Fe"Cy 6 , or 4KCyFe /; Cy 2 , serves in solution for the recogni- 
 tion of Iron, Copper, and Molybdenum. 
 
 Plumbic acetate (Pb 2 C 2 H 3 O 2 ) is used for tracing Chromium. 
 
 Bismuthous nitrate, Bi'" (NO S ) 3 , 5H 2 O, or Bi 2 O 3 , 3N 2 O 5 
 10H 2 O, as reagent for Tin. 
 
 Acetic acid (C 2 H 4 O 2 ) is employed in investigations of Chro- 
 mium,, Vanadium, Manganese, and Uranium. 
 
 Mercuric cyanide, Hg r/ (CN) 2 , or Hg^Cy.,. Its solution is 
 sometimes used for the detection of Palladium. 
 
 Hydrochloric and nitric acid, as well as a mixture of the 
 two, or aqua regia, are quite frequently employed the latter 
 in testing for gold, platinum, etc. 
 
 For test operations, only very minute quantities of the sub- 
 stances are used. Decrepitating bodies, as already stated, are 
 ground into very fine powder, and absorbed by a moistened 
 strip of filter paper (1 centimetre square). If this is placed 
 between two rings (coil) made of hair-fine platinum wire and 
 then burnt, a cohering crust remains which may be tested in 
 the flame withotit any difficulty. 
 
 When substances require to be held in the flame for a long 
 time, it is very convenient to use a Bunsen stand, which is 
 provided with horizontal clips and arms, movable horizontally 
 and vertically on the vertical support. The arms carry small 
 glass tubes supporting platinum wire or asbestos fibres, and the 
 clips are used for holding the test tubes. 
 
MKTIIODS OF EXAMINATION. 117 
 
 8. METHODS OF EXAMINATION. 
 A. Ignition of the Elements at High Temperatures. 
 
 When heating small assays the following phenomena must 
 be considered : 
 
 1. The emission of light, which is ascertained by holding 
 the substance on platinum wire in the hottest part of the zone 
 of fusion. The emissive power is estimated as low, medium, or 
 high, according as the luminosity of the specimen falls below, 
 equals, or exceeds that of the platinum wire, introduced at the 
 same time. 
 
 2. The fusibility, or melting point, is expressed by a scale 
 of temperature of the following six grades, distinguishable by 
 the appearance of a thin platinum wire in different portions of 
 the flame, viz : 
 
 a. Below red heat. 
 
 b. Incipient red heat. 
 
 c. Red heat. 
 
 d. Incipient white heat. '. 
 
 e. White heat. 
 
 f. Intense white heat. 
 
 3. The volatility is determined by the time required to vola- 
 tilize a weighed bead (0.01 grm.) in the zone of fusion, and 
 comparing it with the time required to volatilize an equal 
 weight of sodic choride, the volatility of which is taken as a 
 unit of comparison. The odor evolved, if any, must be 
 observed. 
 
 4. Flame coloration. Many volatile substances may be 
 detected by placing the test specimen in the upper reducing 
 
 flame at C, when the colorations appear in the upper oxidizing 
 flame at E. Mixtures of flame-coloring bodies may first be 
 tested in the coolest part of the flame base at A, to obtain 
 (for a moment only) the coloration produced by the most 
 volatile bodies, unmixed with the less volatile ones. 
 
118 MINERALOGY SIMPLIFIED. 
 
 B. Oxidation and Reduction of Substances. 
 
 1. Fused Glass Beads The oxidation and reduction of 
 fused substances are executed on platinum wire. The beads 
 adhering to the ends of the wires are oxidized in the lower 
 oxidizing flame at G, and reduced in the lower reducing 
 flame at D. 
 
 2. Reductions in Closed-glass Tubes The completely dried 
 test specimen is heated together with soda and carbon (soot 
 of turpentine is the best) or with metallic sodium, or metallic 
 magnesium wire-clippings. The tubes made of thin glass are 
 3 mm. wide, and 3 cm. long. The sodium is freed from the 
 naphtha, in which it was preserved, with blotting paper, next 
 rolled between the fingers into a small cylinder which is placed 
 in the tube, and surrounded by the test specimen. The tube 
 is now heated to its own melting point (whereby usually a 
 combustion takes place in the interior). The cold tube is then 
 crushed, and the reduced material carefully collected on glazed 
 paper for further investigation. 
 
 3. Reduction on the Charcoal Rod On the point of the 
 
 small charcoal rod, already described, we place the test speci- 
 men, of about the size of a mustard seed and previously 
 mixed with a drop of fused sodic carbonate, into the lower 
 oxidizing flame at G, for the purpose of fusion, and next pass 
 it into the hotter portion of the lower reducing flame opposite 
 at D. After the reduction has taken place, recognizable by the 
 violent boiling up and frothing of the soda, the specimen is 
 allowed to cool in the dark interior of the flame. The end of 
 the charcoal rod is then nipped off, placed in an agate mortar, 
 and ground with a few drops of water. After lixiviating the 
 charcoal, the products of reduction are kept for further inves- 
 tigation. 
 
 C. Incrustations or Coatings on Porcelain. 
 
 The volatile elements reducible by hydrogen or carbon may 
 either be separated as such from compounds, or as oxides, and 
 
METHODS OF EXAMINATION. 119 
 
 collected upon glazed porcelain. Such deposits may next be 
 converted into iodides, sulphides, or other combinations having 
 characteristic qualities, by means of which they can be recog- 
 nized. The incrustations or films consist in the centre of a 
 thick layer surrounded on all sides by a thinner coating pass- 
 ing to the merest tinge. These reactions are so sensitive, that 
 in many cases 0.1 or 0.001 grm. of. material suffice to produce 
 them, surpassing in delicacy Marsh's arsenic test. 
 The incrustations produced are as follow : 
 
 a. Metallic Films or Incrustations are prepared by heating 
 a very small particle of the substance placed on an asbestos 
 fibre, in the upper reduc.iny flame at C (not too large, and per- 
 fectly free from smoke), with one hand, whilst holding at the 
 same time in the other a thin and glazed porcelain capsule (0.1 
 metre in diameter), filled with cold water, and placing it closely 
 over the asbestos fibre into the upper reducing flame. The 
 volatile metals, if present, will be deposited as a dark incrus- 
 tation, either dull or lustrous. This deposit is then further 
 examined as to its solubility in dilute nitric acid (containing 
 20 per cent, of anhydrous acid). 
 
 b. Oxide Incrustations These are formed by holding the 
 porcelain capsule in the preceding experiment, at some dis- 
 tance from the test-specimens, into the upper oxidizing flame 
 at E. It may then be tested 
 
 1st, by a drop of stannous chloride; if no reduction is effected 
 we add : 
 
 2. Caustic soda solution until the precipitated hydride of 4in 
 oxide is redissolved, and observe whether a reduction is the 
 result. 
 
 3. The incrustation is touched with some drops of neutral 
 argentic nitrate solution by means of a glass rod spread out, 
 and ammonia vapor blown upon it.* If a precipitate is formed, 
 the color is observed, etc. 
 
 * The latter is best accomplished by using a small sized ordinary 
 wasli bottle, in which the blowing-tube extends under the ammonia 
 solution, and the pointed ejection-tube only to the lower end of the 
 perforated cork. 
 
120 MINERALOGY SIMPLIFIED. 
 
 c. Iodide Films These are formed by placing the oxide 
 incrustation on the cold capsule over the wide-mouthed glass 
 flask containing hydriodic acid and phosphorous acid (derived 
 from the gradual deliquescence of phosphoric tri-iodide). The 
 iodide coating may be further tested by the moist breath (solu- 
 bility), and by having ammonia vapor blown upon it. 
 
 d. Sulphide Incrustations are produced from the iodide 
 incrustation by blowing a current of sulphide of ammonium 
 vapor upon it, and expelling the superfluous ammonium sul- 
 phide by gently heating the porcelain capsule. The sulphide 
 incrustation left is then further tested to examine its solubility 
 in water by blowing the warm breath upon it, or by adding a 
 drop of water, and for its solubility in ammonium sulphite, 
 either by blowing or dropping the reagent upon it. 
 
 9. GENERAL REVIEW OF FLAME REACTIONS. 
 
 The elements which may be recognized by the flame-reactions 
 may be divided into three groups, according to their behavior 
 during their oxidation and reduction. 
 
 A. Volatile elements, separable by reduction as incrustations 
 (see the table of volatile elements appended hereto). 
 
 B. Reducible metals furnishing no incrustations. 
 
 C. Elements which may best be recognized from the deport- 
 ment (reactions) of their compounds. 
 
 By considering, in addition, those substances recognizable by 
 their flame coloration, the following general schedule of flame- 
 reactions may be given, and their further chemical behavior, 
 elsewhere described, may be considered and compared with it. 
 
A. Table of Volatile Elements which can be reduce( 
 
 to thei 
 
 
 Metallic In- 
 crustation and 
 Coating, 
 
 Oxide In- 
 crustation 
 and Coat- 
 ing. 
 
 Oxide In- 
 crustation 
 with SnCla, 
 
 Oxide Incrus- 
 tation with 
 SnClo and 
 NaHO. 
 
 Oxide Incrusta- 
 tion with 
 AgN0 3 and 
 NH 4 HO 
 
 TELLURIUM, 
 
 Black; with 
 brown coating. 
 
 White. 
 
 Black. 
 
 Black. 
 
 White, tinged 
 yellowish. 
 
 SELENIUM, 
 
 Cherry-red ; 
 with brick red 
 
 coating. 
 
 White. 
 
 Brick-red. 
 
 Black. 
 
 White. 
 
 ANTIMONY, 
 
 Black; with 
 brown coating. 
 
 White. 
 
 White. 
 
 White. 
 
 Black ; insolu- 
 ble in JMH 3 . 
 
 ARSENIC, 
 
 Black; with 
 bi'own coating. 
 
 White. 
 
 White. 
 
 White. 
 
 Lemon-yellow 
 or brownish- 
 red ; soluble iu 
 NH 3 . 
 
 BISMUTH, 
 
 Black ; with 
 soot-brown 
 coating. 
 
 Yellowish- 
 white. 
 
 White. 
 
 Black 
 
 White. 
 
 MERCURY, 
 
 Gray; non-cohe- 
 rent coating. 
 
 
 
 
 
 THALLIUM, 
 
 Black ; with 
 brown coaling. 
 
 White. 
 
 White. 
 
 White. 
 
 White. 
 
 LEAD, 
 
 Black ; with 
 brown coating. 
 
 Light ochre- 
 yellow. 
 
 White. 
 
 White. 
 
 White. 
 
 CADMIUM, 
 
 Black ; with 
 brown coating. 
 
 Brownish- 
 black ; with 
 white coat- 
 ing. 
 
 White. 
 
 White 
 
 White coating 
 becomes blue- 
 black. 
 
 ZINC, 
 
 Black; with 
 brown coating. 
 
 White. 
 
 White. 
 
 White. 
 
 White. 
 
 INDIUM, 
 
 Black ; with 
 brown coating. 
 
 Yellowish- 
 white. 
 
 White. 
 
 White. 
 
 White. 
 
To J ace jtage 121. 
 
 ? Films or Coatings oil Porcelain, arranged according 
 Reactions. 
 
 e Incrustation 
 id Coating, 
 
 Iodide Incrus- 
 tation with 
 NH 3 (blown 
 upon it), 
 
 Sulphide In- 
 crustation and 
 Coating, 
 
 Sulphide In- 
 rustaiion with 
 H(NH 4 )S, 
 
 Color of flame 
 and odor, 
 
 Ution of dilute 
 nitric acid 
 HN0 3 +^2. 
 
 n ; breathed 
 i disappears 
 i time. 
 
 Msapp^ars per- 
 manently. 
 
 Black to black- 
 ish-brown. 
 
 Disappears for 
 a time. 
 
 Jpper reduc- 
 tion zone fa- 
 ded blue ; up- 
 per oxidizing 
 flame green ; 
 no odor. 
 
 Substances 
 whose metal- 
 lic incrusta- 
 . tions are 
 scarcely af- 
 fected by di- 
 lute nitric 
 acid. 
 
 Substances 
 whose metal- 
 lic incrusta- 
 . tions are 
 with diffi- 
 cnltydissolv- 
 ed by dilate 
 nitric acid. 
 
 J 
 
 Substances 
 whose metal- 
 lic incru.sta- 
 . tions are in- 
 stantly dis- 
 solved by di- 
 lute nitric 
 acid. 
 
 n ; breathed 
 i does not 
 lly disappear. 
 
 Does not dis- 
 appear. 
 
 Yellow to 
 orange. 
 
 Orange, then 
 disappears for 
 a time. 
 
 fine blue ; odor 
 ot rotten horse- 
 radish. 
 
 ?e-red ; breath- 
 pon disappears 
 i time. 
 
 Disappears per- 
 manently. 
 
 Orange. 
 
 Disappears for 
 a time. 
 
 Jpper reduc- 
 tion-zone faded 
 green. 
 
 /ellow;breath- 
 pon disappears 
 i time. 
 
 Msappears per- 
 manently. 
 
 Lemon-yellow. 
 
 Disappears for 
 a time. 
 
 Tpper reduc- 
 tion-zone laded 
 blue ; odor of 
 garlic. 
 
 h-brown; with 
 .-red to crim- 
 red coating ; 
 thed upon dis- 
 ir for a time. 
 
 Crimson-red to 
 egg-yellow ; 
 chestnut-brown 
 when dry. 
 
 Umber-brown ; 
 with coffee- 
 brown coating. 
 
 Does not dis- 
 APpear. 
 
 Bluish, not cha- 
 racteristic. 
 
 ine andlemon- 
 w ; breathed 
 i does not dis- 
 :ar. 
 
 Disappears for 
 a time. 
 
 Black. 
 
 Does not dis- 
 appear. 
 
 
 n-yellow ; 
 hed upon does 
 Lisappear. 
 
 Does not dis- 
 appear. 
 
 Black ; with 
 bluish-gray 
 coating. 
 
 Does not dis- 
 appear. 
 
 Light grass- 
 green. 
 
 yellow to le 
 -yellow; 
 thed upon does 
 Lisappear. 
 
 Disappears for 
 a time. 
 
 Brownish-red 
 to black. 
 
 Does not dis- 
 appear. 
 
 Faded blue. 
 
 White. 
 
 White. 
 
 
 
 Lemon-yellow. 
 
 Does not dis- 
 appear. 
 
 
 White. 
 
 White. 
 
 White. 
 
 Does not dis- 
 appear. 
 
 
 owish-white. 
 
 Yellowish- 
 white 
 
 White. 
 
 Does not dis- 
 appear. 
 
 Intense indigo- 
 blue. 
 
METHODS OF EXAMINATION. 
 
 121 
 
 Method employed. 
 
 Reactions obtained 
 
 Indications of: 
 
 I. We endeavor 
 to obtain a itie- 
 tallic incrusta- 
 tion in a por- 
 celain capsule. 
 
 All incrustation 
 which is to be 
 tested in regard 
 to its solubility 
 in dilute nitric 
 acid, thus : 
 
 Scarcely attacked : Te, Se, Sb, As. 
 With difficulty dissolved : Bi, Hg, 
 T (Thallium). 
 Instantly dissolved : Pb, Cd, Zn, 
 I (Indium). 
 
 II. The sub- 
 stance is heat- 
 ed with addi- 
 
 a. A gray pow- -| 
 der: j 
 
 magnetic: Fe, Ni, Co. 
 Nou -magnetic : Pd, Pt, Rh, Ir. 
 
 tion of sodic 
 carbonate on a 
 charcoal rod. 
 
 6. A metallic ] 
 globule : \ 
 
 . Cu, Sn, Ag, Au. 
 
 III. The mass, 
 mixed with 
 
 a. A white or ] 
 colorless fusion : J 
 
 . Mo, W (tungsten), Ti, Ta, Nb, Si. 
 
 Na 2 C0 3 and K 
 N0 3 is heated 
 on a platinum 
 wire. 
 
 b. A yellow ' 
 fusion : \ 
 c. A green , 
 fusion : '. 
 
 . Cr, V. 
 . Mn. 
 
 IV. Special proceedings for finding : U, P, S (described in our special 
 
 methods of detection). 
 
 V. Flame-coloration : K, Na, Li, Sr, Ba, Ca. 
 
 Besides the characteristic flame coloring by which certain 
 substances may be recognized, there is a large series of general 
 flame-reactions, which may be systematized as follows : (See 
 Table A.) 
 
 B. Reducible to Metals, but yielding no incrustations. 
 
 IRON COMPOUNDS. Reduction on the charcoal rod furnishes 
 neither metallic globules nor lustrous scales ; ground fine in an 
 11 
 
122 MINERALOGY SIMPLIFIED. 
 
 agate mortar the reduced mass is attracted by a magnet in the 
 form of a black, dull brush, which, when rubbed upon paper, 
 then touched with a drop of aqua regia and gently warmed, 
 produces a yellow spot that turns deep blue by the addition of 
 a drop of ferrocyanide of potassium solution. The paper ought 
 previously be tested for iron. 
 
 Borax Bead Ignited in oxidizing flame with some oxide 
 furnishes whilst hot, according to the quantity, a yellowish-red 
 to brownish dark-red glass, which, on cooling, turns yellow to 
 brownish-yellow. In reduction flame the bead is red whilst 
 hot, and bottle-green when cold. 
 
 NICKEL COMPOUNDS Reduction on the charcoal rod fur- 
 nishes white, lustrous, ductile, metallic spangles, which are 
 attracted by the magnet. Rubbed on paper the metal yields, 
 with a drop of nitric acid, a green solution which, when 
 touched with a drop of caustic soda, on a glass .rod, thence ex- 
 posed to bromine vapor, and again touched with caustic soda, 
 furnishes a black spot of peroxide of nickel. 
 
 Borax Bead Oxidizing flame dirty violet ; upper reducing 
 flame gray from metallic nickel, which at times unites to a 
 silver-white nickel sponge, whilst the bead turns colorless. 
 
 COBALT COMPOUNDS Reduction on the charcoal rod yields 
 white, shiny, ductile, metallic spangles, which are attracted by 
 the magnet. Rubbed on paper the metal furnishes, in contact 
 with nitric acid, a red solution which, when touched with a 
 drop of hydrochloric acid and then dried, yields a green spot 
 which, when moistened with water, again disappears. By 
 means of caustic soda and bromine vapor we obtain, as with 
 nickel, a brownish-black spot of peroxide of cobalt. 
 
 Borax Bead Oxidizing flame and reducing flame deep blue. 
 
 PALLADIUM COMPOUNDS. With Soda on Platinum Wire. 
 In the upper oxidation flame we obtain a gray mass similar to 
 platinum sponge which, when rubbed in an agate mortar, forms 
 silver-white, lustrous, ductile, metallic spangles, which form a 
 red solution with nitric acid. Adding a drop of mercury cya- 
 nide and blowing a current of ammonia vapor over the liquid, 
 
METHODS OF EXAMINATION. 123 
 
 a white flaky precipitate is produced, which is redissolved by 
 an excess of the reagent. 
 
 PLATINUM COMPOUNDS. With Soda on Platinum Wire. 
 In the upper oxidizing flame they are reduced to a spongy mass 
 which, ground in an agate mortar, yields silver-white, shiny, 
 ductile spangles, insoluble in nitric or hydrochloric acid, but 
 easily soluble in aqua regia (a mixture of both), with a light 
 yellow color when the platinum is pure ; with a brownish- 
 yellow color, if palladium, rhodium, or iridium is present. 
 
 Mercury cyanide with a current of ammonia vapor gives no 
 white precipitate, but a yellow crystalline one of ammonium 
 platinum chloride. 
 
 IRIDIUM COMPOUNDS. With Soda on Platinum Wire In 
 the upper oxidizing flame a metallic reduction takes place ; the 
 mass ground in an agate mortar is not shining nor ductile, and 
 is insoluble in acids, including aqua regia. 
 
 RHODIUM COMPOUNDS Distinguished from iridiurn com- 
 pounds, only that the metallic powder, when fused with potas- 
 sium sulphate, is partly oxidized, and forms a rose-red solution. 
 
 OSMIUM COMPOUNDS. In the oxidizing flame osmium acid 
 is produced, possessing a chlorine-like, pungent odor, attacking 
 the eyes. 
 
 GOLD COMPOUNDS. With Soda on a Charcoal Rod. A yel- 
 low, lustrous granule is obtained, which, in a mortar, yields 
 golden yellow spangles. Insoluble in nitric and hydrochloric 
 acids, but soluble in aqua regia. The light yellow solution 
 imbibed by white blotting (filter) paper, and touched with a 
 drop of stannous chloride (SnClJ produces a splendid purple 
 color (purple of Cassius), used in the arts for imparting to 
 glass a ruby color. 
 
 SILVER COMPOUNDS. With Soda on a Charcoal Rod. A 
 white, ductile globule is produced which, when heated, is dis- 
 solved in nitric acid. Hydrochloric acid throws down from the 
 solution a white, curdy precipitate, soluble in ammonia, but 
 insoluble in nitric acid. 
 
124 MINERALOGY SIMPLIFIED. 
 
 COPPER COMPOUNDS. With Soda on a Charcoal Rod A 
 
 copper-red, ductile globule is obtained, soluble in nitric acid 
 with a blue color. If some of the solution is imbibed by white 
 blotting paper, and a drop of ferrocyanide of potassium added, 
 a brown spot is produced. 
 
 Borax Bead. The oxidizing flame furnishes a blue bead 
 which, in the lower reduction flame, upon the addition of a 
 little stannic oxide yields a brownish-red color of cuprous 
 oxide (Cu 2 O). By alternating the oxidizing and reducing pro- 
 cess a ruby red, transparent bead is obtained ; which is best 
 obtained when the reduced bead is allowed to oxidize slowly. 
 
 TIN COMPOUNDS. On a Charcoal Rod White, bright, duc- 
 tile globule, dissolving slowly in hydrochloric acid ; by nitric 
 acid it is not dissolved, but is converted into insoluble, white, 
 stannic oxide. In tin solutions bismuthic nitrate and an 
 excess of caustic soda, furnishes a bla.ck precipitate. 
 
 C. Elements which can best be recognized from the reactions 
 of their compounds. 
 
 MOLYBDENUM COMPOUNDS. With Soda on the Charcoal 
 Rod. Reducible with difficulty to a gray powder. 
 
 Borax Bead (not very characteristic) The bead in the 
 
 oxidizing flame is at first colorless, but when completely satu- 
 rated, forms a bluish enamel. 
 
 Special Reactions The finely powdered substance is mixed 
 with soda (best obtained by fusion of a fragment of a soda 
 crystal), and this mixture fused within a platinum spiral of 
 2-3 mm. diameter exposed to the flame of a Bunsen lamp. 
 The mass, when heated to a white heat, is knocked off and 
 dissolved in a few drops of warm water. The clear liquid, 
 above the sediment, is imbibed by a strip of blotting paper, 
 and submitted to the following tests : After being acidulated 
 with hydrochloric acid, the addition of ferrocyanide of potas- 
 sium produces a red brown spot. Stannous chloride, added 
 gradually, forms at once, or after gentle heating, a blue color. 
 Ammonium sulphide produces a brown color, and upon the 
 
METHODS OF EXAMINATION. 125 
 
 addition of hydrochloric acid, a brown precipitate, whereby 
 the paper often turns blue. 
 
 TUNGSTEN (WOLFRAMIUM) COMPOUNDS A fusion is pro- 
 duced like that described by molybdenum. The aqueous solu- 
 tion is absorbed by blotting paper. Hydrochloric acid and 
 ferrocyanide of potassium give no reactions. Stannous chloride 
 furnishes at once a blue color, or after slight warming. 
 Ammonium sulphide causes neither alone nor with hydro- 
 chloric acid a precipitate, but turns (especially after slight 
 heating) the paper blue or greenish. 
 
 TITANIUM COMPOUNDS. With Salt of Phosphorus In 
 oxidizing flame, colorless ; in reduction flame of a feeble 
 amethystine color ; adding to the bead some ferrous sulphate, 
 it assumes in the lower reduction flame a red color. 
 
 With Soda on Platinum Wire. Fuses to a colorless trans- 
 parent mass turning turbid when cold. If the bead while hot 
 is touched with stannous chloride, and heated in the lower 
 reduction zone, a gray mass is obtained which, with hydro- 
 chloric acid, and slightly heated, gives a pale amethyst color. 
 
 TANTALUM AND NIOBIUM COMPOUNDS exhibit the same 
 deportment as titanium compounds. 
 
 CHROMIUM COMPOUNDS. With Soda in the Platinum 
 
 Spiral Such compounds fused with repeated additions of 
 
 saltpetre assume a light yellow color, soluble in water with the 
 same color. The liquid removed from the sediment, then 
 acidulated with acetic acid and imbibed by blotting-paper, 
 yields with solution of lead acetate, a yellow ; with silver salts, 
 a reddish-brown precipitate. Ammonium sulphide, stannous 
 chloride, or the evaporation with aqua regia turn the yellow 
 colored solution green. 
 
 Borax Bead In both flames emerald green. 
 
 VANADIUM COMPOUNDS. . Fusion with Soda and Saltpetre 
 in the Platinum Spiral. A yellow fusion is obtained. The 
 solution when acidulated with acetic acid, is colored yellow by 
 silver solution. When the solution is mixed with aqua regia 
 and evaporated, we obtain not a green, but a yellow or 
 
 11* 
 
12G MINERALOGY SIMPLIFIED. 
 
 yellowish-brown liquid which is turned blue by stannous 
 chloride. . 
 
 Borax Bead Oxidizing flame, greenish-yellow; reduction 
 flame, green. 
 
 MANGANESE COMPOUNDS. Borax Bead Oxidizing flame, 
 amethyst color ; reduction flarne, colorless. 
 
 With Soda and Saltpetre in the Platinum Spiral The 
 
 fused mass obtained is green, and the aqueous solution like- 
 wise. Upon the addition of acetic acid the liquid turns red ; 
 later, colorless with separation of brown flakes. 
 
 URANIUM COMPOUNDS. Borax Bead Oxidizing flame, 
 
 yellow; reduction flame, green. From the similar iron re- 
 action, the hot uranium bead is distinguished by emitting a 
 bluish-green light. 
 
 Phosphorus Salt Bead Reduction flame, fine green ; 
 while 'iron yields, when cold, a reddish or colorless bead. 
 
 With Acid Potassic Sulphate in the Platinum Spiral The 
 
 fused mass is ground together with a few granules of crystal- 
 lized soda, moistened with water, and absorbed by blotting- 
 paper. When acidulated with acetic acid, ferrocyanide of 
 potassium produces a brown spot. 
 
 SILICIC COMPOUNDS. Phosphorus Salt Small splinters 
 
 of silicates yield a gelatinous, infusible, silica mass, suspended 
 or swimming in the bead. 
 
 With Soda on Platinum Wire In oxidizing flame a clear 
 bead is produced with strong effervescence. When this bead 
 is treated with water and acetic acid, and the solution carefully 
 evaporated, a gelatinous mass of hydrous silicic acid separates. 
 
 PHOSPHORUS COMPOUNDS The completely dried sample 
 is put into a glass tube together with a few cuttings of magne- 
 sium wire, or a small piece of metallic sodium, and heated over 
 the burner until the whole mass glows and fuses. The tube is 
 now broken and the contents moistened with water, when 
 the characteristic odor of phosphide of hydrogen is evolved, 
 resembling that of rotten fish. 
 
SPECTRUM ANALYSIS. 127 
 
 SULPHUR COMPOUNDS. With Soda on the Charcoal Rod. 
 In the lower reduction zone a fused mass is obtained which, 
 when placed upon silver-foil, or a silver coin, and then 
 moistened with a drop of water, produces a black spot. How- 
 ever, this reaction is only reliable, when the* coal gas, used in 
 the burner, is free from sulphur, and after the absence of sele- 
 nium and tellurium has been ascertained, since these elements 
 yield the same reaction. 
 
 Metallic sulphides show their contents of sulphur by the 
 evolution of sulphorous acid gas (SO 2 ), bleaching vegetable 
 colors, such as litmus, and having the well-known suffocating 
 odor of burning sulphur. 
 
 10. SPECTRUM ANALYSIS.* 
 
 An entirely new branch of chemical analysis of great deli- 
 cacy and importance, was developed in 1859, chiefly by the 
 researches of R. Bunsen and G. Kirchhoff, the principles of 
 which may here be briefly stated. 
 
 It had long been known that certain chemical substances, 
 especially the salts of the alkalies and alkaline earths, when 
 strongly heated in the blowpipe, or other nearly colorless flame, 
 impart to that flame a peculiar color by the occurrence of 
 which the presence of the substance may be detected. If 
 many of these substances are present together, the detection of 
 each by the naked eye becomes impossible, owing to the colors 
 being blended and interfering with each other. Thus a small 
 trace of soda giving to the flame an intense yellow color prevents 
 the eye from recognizing the purple tint of potassium salts, 
 even if large quantities of these are present. This difficulty 
 is completely overcome, and this method of observation 
 rendered extremely sensitive, if, instead of regarding the flame 
 
 * Prof. Roscoe's " Lessons in Elementary Chemistry, Inorganic and 
 Organic." London. Same author : Spectrum Analysis with Engrav- 
 ings, etc. Prof. Lockyer's Three Manchester Science Lectures. 
 London. Same author: "Studies in Spectrum Analysis." Young 
 on " The Sun." The two last named volumes in the " International 
 Scientific Series." 
 
128 MINERALOGY SIMPLIFIED. 
 
 with the naked eye, it is examined through a prism. This 
 consists of a triangular piece of glass, in passing through 
 which the light is refracted or bent out of its course each differ- 
 ently colored ray being differently refracted, so that if a source 
 of white light, such as the flame of a candle, is thus regarded, 
 a continuous band of differently colored rays is observed the. 
 compound white light being resolved into all its single, vari- 
 ously colored constituents. The colored band is called spectrum, 
 and each source of pure white light gives the same continuous 
 spectrum, stretching from red (the least refrangible) to violet 
 (the most refrangible) color, identical in fact with the colors of 
 the rainbow. 
 
 The light of the sun and of celestial bodies in general, as well 
 as that of the electric spark and of all ordinary flames, is of a 
 compound nature. If a ray of light from any of the sources 
 mentioned be admitted into a dark room by a small hole in a 
 shutter, or otherwise, and suffered to fall upon a glass prism in 
 the manner described below, it will not only be refracted from 
 
 Fig. 109. 
 
 its straight course, but will be decomposed into a number of 
 colored rays, which may be received upon a white screen 
 placed behind the prism. When solar light is employed, the 
 colors are extremely brilliant, and spread into an oblong space 
 of considerable length. The upper part of this image or spec- 
 trum will be violet and the lower red, the intermediate portion, 
 commencing from the violet, being indigo, blue, green, yellow, 
 and orange, all graduating imperceptibly into each other. 
 This is the celebrated experiment of Sir Isaac Newton ; and 
 from it he drew the inference that white light is composed of 
 
SPECTRUM ANALYSIS. 129 
 
 % 
 
 seven primitive colors, the rays of which are differently refran- 
 gible by the same medium, and hence capable of being thus 
 separated. The violet rays are most refrangible, and the red 
 rays least. 
 
 If these colored flames are examined by means of a prism, 
 the light being allowed to fall through a narrow slit upon the 
 prism, it is at once seen that the light thus refracted differs 
 essentially from white light, inasmuch as it consists of only a 
 particular set of rays, each flame giving a spectrum containing 
 a few bright lines. Thus the spectrum of the yellow soda 
 flame contains only one tine bright yellow line, while the 
 purple potash flame exhibits a, spectrum in which there are two 
 bright lines, of a poppy-red color, one lying at the extreme red, 
 and the other of a bluish-purple color at the extreme violet end. 
 These peculiar lines are always produced by the same chemical 
 element, and by no other known substance, and the position of 
 these lines always remains unaltered. When the spectrum of 
 a flame tinted by a mixture of sodium and potassium salts is 
 examined, the yellow ray of sodium is found to be confined to 
 its own position, while the potassium-red and bluish-purple 
 lines are as plainly seen as they would have been had no 
 sodium been present. 
 
 The colored flames which are exhibited by the salts of 
 lithium, barium, strontium, and calcium, all give rise, like- 
 wise, to a peculiar spectrum by which the presence or absence 
 of very small quantities of these substances can be ascertained 
 with certainty when mixed together, simply by observing the 
 presence or absence of the peculiar bright lines characteristic 
 of the particular body. The advantage which this new method 
 of analysis possesses over the older processes lies in the ex- 
 treme delicacy, as well as in the great facility with which the 
 presence of particular elements can be detected with certainty.* 
 
 * A little of the substance under examination is put upon the loop 
 of a clean platinum wire, and inserted in the flame of the Bunsen 
 gas burner.' Then, almost at a glance, whatever spectra may be 
 present can be recognized. 
 
130 MINERALOGY SIMPLIFIED. 
 
 Thus a portion of sodium salt less than 55^55$ part of a grain 
 can be detected ; and compounds are found to be most widely 
 disseminated throughout the earth, which were supposed to occur 
 very rarely. The extreme delicacy of the method is seen 
 when we learn that every substance which has ever been ex- 
 posed to the air for a moment gives the soda line, when placed 
 in a colorless flame ; and when we find that the lithium com- 
 pounds, which were formerly supposed to be contained in only 
 four minerals, by aid of spectrum analysis, are found to be 
 substances of most common occurrence, being observed in 
 almost all spring waters, in tea, tobacco, milk, and blood, but 
 existing in such minute quantities as to have altogether 
 eluded recognition by the older and less delicate analytical 
 methods ; for example, SMOMOO f a grain of sodium, or 67000,000 
 of a grain of lithium, will reveal its presence immediately. 
 Thus, in a drop of native spring water, Li can be detected 
 if a platinum wire is dipped into it and held in the flame. A 
 most striking proof of the high value of spectrum analysis lies 
 in the fact of the recent discovery of four new elements by its 
 means. Two new alkaline metals, c&sium and rubidium, 
 having been found together with soda and potash in certain 
 mineral springs, and two new metals, thallium and indium, 
 having been respectively discovered in iron pyrites and zinc 
 ores. The new alkaline metals resemble potassium so closely 
 in their properties, that it would be nearly impossible to have 
 detected them by the ordinary analytical methods, although 
 their spectra exhibit very distinct bright bands not seen in the 
 potassium or any other known spectrum. The metal thallium 
 was discovered by observing a splendid green line which did 
 not belong to any known substance ; whilst indium was recog- 
 nized by the presence of the two lines, In a in the indigo and 
 In j3 in the violet portion of the solar spectrum. 
 
 It is not only those bodies which have the power of impart- 
 ing color to the flame which yield characteristic spectra, for 
 this property belongs to every elementary substance, whether 
 metallic, non-metallic, solid, liquid, or gaseous, and it is always 
 
SPECTRUM ANALYSIS. 131 
 
 observed when such element is heated to the point at which its 
 vapor becomes luminous ; for then each element emits the 
 peculiar light given off by it alone, and the characteristic 
 bright lights become apparent when its spectrum is observed. 
 
 Spark Spectra. 
 
 Most metals require a much higher temperature than that 
 of the non-luminous flame, in order that their vapor should 
 become luminous ; but they may be easily heated up to the 
 requisite temperature by means of the electric spark, which, 
 in passing between two points of the metal in question, vola- 
 tilizes a small portion, and heats it so intensely as to enable it 
 to give off its peculiar light. Thus all the metals, among 
 others iron, platinum, silver, and gold, may each be recognized 
 by the peculiar bright lines which their spectra exhibit. It is 
 to be remembered, however, that the bright lines of the gases 
 through which the spark passes (the air lines) will likewise 
 be observed. 
 
 Spectra of Permanent Gases. 
 
 The permanent gases also yield characteristic spectra when 
 they are strongly heated by the passage of an electric spark. 
 Thus if the spark be passed through an atmosphere of hydro- 
 gen gas, the light emitted is one bright red, one green, and 
 one blue line ; whilst in nitrogen gas the spark has a purple 
 color, and the peculiar and complicated spectrum of nitrogen 
 is observed when this spark is examined with a prism. 
 
 Tn order to detect several flame-coloring elements when 
 occurring together, it is easiest and best to use the spectro- 
 scope. If a colored flame be observed by means of the spectro- 
 scope, bright colored lines upon a dark ground are perceived. 
 This arises from the fact that each element gives out a light 
 peculiar to itself, which is resolved into single rays by the 
 prism of the spectroscope, and these rays form the lines seen in 
 the apparatus. The lines vary in color, position, and manner 
 of grouping with each element : these characteristic differ- 
 
132 MINERALOGY SIMPLIFIED. 
 
 ences form the basis of the most sensitive and exact method 
 of analysis, the so-called spectrum analysis. 
 
 The spectrum lines of the most important elements are given 
 in the following table. The numbers in this table indicate the 
 divisions of a scale on which the various lines fall when the 
 sodium line coincides with the fiftieth division. The heavy 
 figures represent the prominent characteristic lines, which 
 only appear at high temperatures and then soon disappear. 
 
SPECTRUM ANALYSIS. 
 
 133 
 
 1 
 
 
 
 s 2 
 
 o CD 
 ^ ^H 
 
 i 
 
 
 1 
 
 : 
 
 i 
 
 
 
 00 00 
 
 IT3 
 
 O 
 
 00 
 rH 
 
 V^-v-^ 
 
 i 
 
 I 8 
 
 i 5 
 
 rH 
 rH 
 rH 
 
 o 
 
 S iH 
 
 l ~ l 
 
 1 I I 1 
 
 : 
 
 
 
 rH 
 
 . ^~ . 
 
 : : 
 
 
 
 : : 
 
 g : : 
 
 s O 
 a 00 
 
 
 
 S 
 
 CO GO 
 
 t* 
 
 rH ' 
 
 
 
 g 
 
 CO co Ir- 
 co CO -^ er^ 
 i - i T ?* rl 
 
 CO CO CO 
 
 CO . N I> . 
 
 g : CD CD ^: 
 
 Is o 
 
 5 d QO 
 
 CO t- 
 
 ^ 
 
 csf * <^ * ' 
 
 T5 lO 
 
 I g 
 
 ^5 lO '^ 
 
 ro lO , lO ( ~ c> 
 
 "^l^lfl ^ ^--05 : : 
 
 1 o 
 
 o ^r 
 
 Z I CO . ; 
 
 Oi co co IT- ; ; 
 
 CO CO CO CO 
 
 
 5 i 8 S 5 
 
 S : ^^ : i 
 
 1 8 
 
 15 =r^ = 
 
 : co : : : 
 
 1 s 
 
 to 
 : t* : : ""* 
 
 : rH : (g 
 
 rH 
 
 : : : : : 
 
 
 
 rH 
 
 i : : i : 
 
 : : : : : 
 
 .2 
 
 1 o 
 
 
 5 
 
 s s 
 
 a - a g .2 
 1 S .2 I 5 
 
 1 1 3 8 - 
 
 02 PH h^ O ' 
 
 S a 
 
 1 1 1 1 | 
 
 d loll 
 
 12 
 
134 MINERALOGY SIMPLIFIED. 
 
 Solar and Stellar Chemistry. 
 
 If sunlight be allowed to fall upon the slit of the spectro- 
 scope, it is observed that the solar spectrum thus obtained 
 differs essentially from the spectra which we have hitherto 
 considered, inasmuch as it consists of a band of bright light 
 passing from red to violet, but intersected by a very large num- 
 ber of fine dark lines, of different degrees of breadth and 
 shade, which are always present, and always occupy exactly 
 the same relative positions in the solar spectrum. The student 
 is recommended to consult the colored charts which are pub- 
 lished, giving the general appearance of the solar spectrum and 
 the position of some of the most important of these dark lines, 
 marked with the letters of the alphabet. These lines indicate 
 the absence in sunlight of particular rays, and they may be con- 
 sidered as shadows, or spaces where there is no light; they 
 are called " Frauenhofer" lines,* after a German optician 
 who first satisfactorily mapped and described them. 
 
 In the last few years the existence of these lines has become 
 a matter of great importance and interest, as it is by their 
 help that the determination of the chemical constitution of the 
 sun and far-distant stars has become possible. The spectra of 
 the moon and planets (reflected sunlight) are found to exhibit 
 these same lines in unaltered position, while in the spectra of 
 the fixed stars, dark lines also occur, but these stellar lines are 
 different from those seen in direct and reflected sunlight. 
 Hence the conclusion has been drawn that the Frauenhofer 
 lines are in some way produced in the body of the sun itself; 
 but it is only recently that the cause of their production has 
 been discovered by the joint labors of Bunsen and Kirchhoff, 
 and thus the foundation laid for the science of solar and stellar 
 chemistry. 
 
 If the position of these "dark lines in the solar spectrum be 
 carefully compared in a powerful spectroscope with those of the 
 
 * Dark lines running lengthwise of the spectrum often confuse the 
 beginner. They are due to dust-specks on the slit of the spectroscope. 
 
SPECTRUM ANALYSIS. 135 
 
 bright lines in the spectra of certain metals, such as sodium, 
 iron, and magnesium, etc., it is seen that each of the bright 
 lines of the particular metal coincides not only in position- but 
 also in breadth and intensity with a dark solar line ; so that, 
 if the apparatus be so arranged that a solar and metallic spec- 
 trum be both allowed to fall, one below the other, in the field 
 of the telescope, the bright lines of the metal are all seen to be 
 continued in dark solar lines. In the case of metallic iron 
 alone, more than sixty such coincidences have been observed, 
 and the higher the magnifying power employed, the more strik- 
 ing and exact does this coincidence appear. 
 
 With other metals, such for instance as gold, antimony, 
 lithium, no single coincidence can be noticed, while all the 
 lines of certain other metals have their dark representatives in 
 the sun. From these facts it is clear that there must be some 
 kind of connection between the bright lines of these metals and 
 the coincident dark solar lines. Are such coincidences of the 
 dark solar lines with the bright iron lines caused by the pre- 
 sence of iron in the sun ? And if so, how do these lines come 
 to appear dark in the solar spectrum ? 
 
 The explanation of this is given by an experiment in which 
 the bright metallic lines are reversed or changed into dark lines. 
 Thus the bright yellow soda lines (coincident with Frauenho- 
 fer's line " D'') can be made to appear as a dark line, by allow- 
 ing the rays from a strong source of white light, such as the 
 oxyhydrogen light, to pass through a flame colored by soda, 
 and then fall upon the slit of thespectroscope.* Instead of 
 then seeing the usual soda spectrum of a bright yellow double 
 line upon a dark ground, a double dark line, identical in posi- 
 
 * The experiment may be made thus : Between the strong light, 
 capable of giving a continuous spectrum, and the slit in the spectro- 
 scope, a layer of sodium vapor is interposed, produced by heating a 
 little metallic sodium in an iron spoon. This sodium vapor absorbs 
 the yellow ray which the more intensely heated sodium vapor of the 
 oxyhydrogen light emits, and a dark line will be seen in its place, 
 i. e., the sodium line has been reversed. 
 
136 MINERALOGY SIMPLIFIED. 
 
 tion and breadth -with the soda line, will be seen to intersect 
 the continuous spectrum of the white light. Here then the 
 yellow flame has absorbed the same kind of light as it emitted, 
 a consequent diminution of intensity in that part of the spec- 
 trum occurred, and a dark line made its appearance. In like 
 manner the spectra of many other substances have been re- 
 versed, each substance in the state of vapor having the power 
 of absorbing the same rays it emits, or being opaque to such 
 rays.* 
 
 The explanation of the existence of dark lines in the solar 
 spectrum, coincident with bright metallic lines, now becomes 
 evident. These dark lines are caused by the passage of white 
 light through the glowing vapor of the metals in question, 
 present in the sun's atmosphere, and these vapors absorb ex- 
 actly the same kind of light which they are able to emit. The 
 sun's atmosphere, therefore, contains these metals in the condi- 
 tion of glowing gases ; the white light proceeding from the solid 
 or liquid strongly heated mass of the sun which lies in the 
 interior. 
 
 By observing the coincidences of these dark lines with the 
 bright lines of terrestrial metals, we arrive at a knowledge of 
 the presence of such metals in the solar atmosphere with as 
 great a degree of certainty as we are able to attain in any 
 question of physical science. The metals hitherto detected in 
 the sun's atmosphere are nine in number, viz., iron, sodium, 
 magnesium, calcium, chromium, nickel, barium, copper, and 
 zinc. Hydrogen and oxygen are also known to exist in the sun. 
 
 Stellar Chemistry. 
 
 The same methods of observation and reasoning apply to the 
 determination of the chemical constitution of the atmospheres 
 of the fixed stars, as these are self-luminous suns ; but the ex- 
 perimental difficulties are greater, and the results, therefore, 
 
 * This is in accordance with the physical law that substances when 
 cold absorb the same rays which they give out when hot. 
 
SPECTRUM ANALYSIS. 
 
 137 
 
 are as yet less complete, though not less conclusive, than is the 
 case with our sun. 
 
 The spectra of the stars contain dark lines, but these are for 
 the most part different from the solar lines, and differ from one 
 another ; hence we conclude that the chemical constitutions of 
 the solar and stellar atmospheres are different. Many of the 
 substances known on the earth have been detected in the 
 atmosphere of the stars by Mr. Huggins and Prof. W. A. Miller, 
 to whom we owe this most important discovery. 
 
 The bright star Aldebarcm, for instance, contains hydrogen, 
 sodium, magnesium, calcium, iron, antimony, mercury, bis- 
 muth, and tellurium. 
 
 Spectroscope. 
 
 The instrument used in these experiments is termed a spec- 
 troscope. It consists of a prism, a (Fig. 110), fixed upon a 
 firm iron stand, and a tube, b (collimator), carrying the slit, rf, 
 through which the rays from the colored. flames, e f and e* fall 
 
 Fig. 110. 
 
 upon the prism, being rendered parallel by passing through a 
 lens. The light having passed through the prism, and having 
 been refracted or split up into its constituents, the differently 
 colored rays are received by the telescope,/, and the image 
 
 12* 
 
138 
 
 MINERALOGY SIMPLIFIED. 
 
 magnified before reaching the eye. The rays from each flame 
 are made to pass into the telescope,/, one set through the un- 
 covered half of the slit, the other by total reflection through 
 a small prism through the lower half; thus bringing the two 
 spectra into the field of view at once, so as to be able to make 
 any desired comparison of the lines. 
 
 Measuring the Spectrum. But for scientific purposes the 
 instrument requires the most accurate means for measuring the 
 spaces of the spectrum. For this purpose a third tube, g, has 
 been added. At its outer end there is a glass plate upon which 
 is engraved or photographed a scale of minute divisions. A 
 lamp, ^, placed in front of this tube, #, throws the image of 
 this scale through the tube and lens at the end nearest to the 
 prism, so that it falls upon the face of the prism, a, at such an 
 angle as to be reflected through the telescope,/, to the eye. 
 The scale is permanent, and parallel with it the observer sees 
 the spectrum of whatever light is employed, and can thus fix 
 arid compare the position of the lines with exactness. 
 
 Fig. 112. 
 
 c / , 
 
 In Fig. Ill is seen the tube, g, containing the photographed 
 scale, illuminated by a gas jet, c, and the manner in which 
 both are fastened to the brass case, having a cover to keep off 
 foreign light as well as dust, from the prism. The Bunsen 
 
DETECTING CERTAIN ELEMENTS. 139 
 
 burners, /, A, together with the two supporters, i, and &, serve 
 for volatilizing the substances to be investigated. If the 
 flames, e and e', are brought in proper position relative to the 
 slit of tube, #, the brass case, together with prism and tubes, 
 is then turned until the intensity of the spectrum light" has 
 attained its maximum value. As the illuminating lamp, e, 
 and the scale, g, are likewise fastened to the brass case, all 
 must turn together, and the illumination of the scale will 
 remain the same. 
 
 CHAPTER VII. 
 
 SPECIAL METHODS FOR DETECTING CERTAIN ELEMENTS, OR 
 SOME OF THEIR COMBINATIONS WHEN PRESENT IN COM- 
 PLEX CHEMICAL COMPOUNDS. 
 
 1. ALUMINA, A1 2 O 3 . This may be traced in most of the 
 infusible minerals by the blue color which the assay assumes 
 when, after being strongly heated, it is moistened with cobalt 
 solution and reheated. Very hard minerals, such as corundum, 
 must previously be very finely pulverized. 
 
 Native crystallized alumina, such as corundum, ruby, sap- 
 phire, emery, are, like strongly ignited amorphous alumina, 
 almost entirely insoluble in acids, but when fused with bisul- 
 phate of potassium, caustic or carbonate of potassium pass into 
 a soluble condition. The colorless alumina salts are either 
 insoluble or soluble in water, losing the acid upon ignition. 
 Caustic alkalies precipitate from solutions a gelatinous basic 
 salt, soluble in an excess of the precipitant. From this solution 
 alumina is thrown down by sal-ammoniac (or better, after the 
 neutralization with HC1, by ammoniaor carbonate ofammonium). 
 Ammonia, carbonate of ammonium, and sulphide ofammonium, 
 
140 MINERALOGY SIMPLIFIED. 
 
 precipitate gelatinous hydroxide = A1 2 (OH) 6 , soluble somewhat 
 
 in the first, insoluble in the other reagents mentioned, e. g., 
 
 (S0 4 ) 4 A1 2 K 2 + 6NH.+ 6H 2 = 3[SO 4 (NH 4 ) J+ SO 4 K S 
 
 + A1,(OH) 6 . 
 
 In the presence of magnesia the precipitate, resulting from 
 alkalies, contains magnesia, readily separated by repeated solu- 
 tions in HC1, and reprecipitation by ammonia, or preferably by 
 boiling with sal-ammoniac solution until no ammoniacal odor 
 can be perceived, when the magnesia passes into solution as 
 an ammoniacal double salt. 
 
 Phosphate of soda precipitates from alumina salts gelatinous 
 phosphate of alumina, soluble in potassa, but insoluble in acetic 
 acid (distinctive from lime phosphate). Chloride of barium, 
 or aqueous baryta solution, removes from a solution of phosphate 
 of alumina in potassa, all the phosphoric acid in the form of 
 phosphate of baryta. From an alkaline solution of alumina 
 the addition of silicate of potassa (soluble glass) produces a 
 precipitate of silicate of alumina, leaving in solution all the 
 phosphoric acid. 
 
 2. AMMONIA. The substance is mixed with some caustic 
 soda, potash or lime in the closed tube (a common reagent tube 
 will answer), arid the mixture heated, when ammonia gas is 
 evolved, recognizable 1st, by its pungent odor (hartshorn) ; 
 2d, by turning moistened red litmus paper blue ; 3d, by its 
 producing dense white fumes with the vapor of concentrated 
 hydrochloric acid, when the latter, suspended on a glass-rod, 
 is brought near it ; 4th, by Nessler's test. The fact must not 
 be overlooked, however, that organic nitrogenous bodies evolve 
 ammonia as a product of decomposition, when these are 
 heated to redness with a sufficient excess of powdered caustic 
 potash or soda, or a mixture of caustic (burnt) lime and 
 soda. 
 
 Ammonia jnay be obtained even from a nitrate salt by igni- 
 tion with potash-lime, provided that a non-azotized body, like 
 sugar, be added to the mixture, but only when the latter is in 
 
DETECTING CERTAIN ELEMENTS. 141 
 
 great excess, e. g., 1 part nitre and 40 parts sugar, has been 
 found to be the best proportion. 
 
 Platinic chloride precipitates from ammonia solutions a yel- 
 low precipitate, insoluble in alcohol or ether. It leaves upon 
 ignition pure, spongy platinum. 
 
 3. ANTIMONY. The ores of antimony afford usually white 
 fumes or charcoal when heated on aluminium foil, which are 
 inodorous. In the open tube antimony gives a white sublimate, 
 coating the glass. Antimony sulphides give at a strong heat in 
 the closed tube a sublimate which is black while hot, brownish- 
 red when cold. Treated with nitric acid, compounds of antimony 
 deposit white antimonic oxide (Sb 2 O 5 ). 
 
 In order to trace antimony when combined with other volatile 
 metals, the white coating on coal is touched with a drop of 
 hydriodic acid,* and once more heated. When its coating con- 
 sists of antimony it turns to a fine red ; if bismuth, to brown ; if 
 lead, to a light yellow ; if cadmium, to white. Since these 
 colored coatings are very distinct and different, all the metals 
 quoted may be recognized when present together (Haanel). 
 
 When antimony is combined with lead and bismuth it is best 
 detected by treating the substance with fused boric acid on the 
 O. F. When the oxides of lead and bismuth are aborbed by 
 the boric acid, and the charcoal becomes coated with a subli- 
 mate which, when the blowing has not been too strong, consists 
 of oxide of antimony, only free from the oxides of lead and 
 bismuth. 
 
 When antimony is combined with copper it is separated from 
 it with difficulty, and the coating of antimony is scarcely re- 
 cognizable on the charcoal. Under these circumstances the 
 alloy is heated in the O. F. with a bead of S. Ph. until the 
 latter has dissolved a portion of the antimony, the glass is then 
 removed from the remaining metallic granule, placed on char- 
 coal and heated with tin in the R. F. If the bead turns turbid 
 
 * HI is obtained when pulverized iodine is suspended in water and 
 a current of sulphide of hydrogen gas passed through it. 
 
142 MINERALOGY SIMPLIFIED. 
 
 and black, antimony is indicated. However, as bismuth gives 
 the same reaction, it is best to separate and distinguisli them 
 in the wet way. 
 
 When the oxides of antimony, tin, and copper are combined 
 together, we treat the mineral powder with a mixture of soda 
 and borax in the R. F. on coal. The metallic globules are re- 
 moved from the glassy mass and fused with 3-4 parts (by 
 volume) of pure test-lead and fused boric acid, when metallic 
 copper remains behind, while tin goes into the slag, and anti- 
 mony coats the coal white. 
 
 Sulphides of lead and antimony are mixed with soda and 
 treated in the R. F. on charcoal ; when near the assay the yellow 
 lead coating appears, and beyond this the white sublimate of 
 antimony. 
 
 Compounds of antimony are, according to Plattner, heated 
 for a short time in the open tube, when they yield a mixture 
 of crystals (compare arsenic) and amorphous antimonious acid. 
 A small amount of antimony mixed with sulphide of arsenic is 
 detected by heating the dry mixture gently in a closed tube ; 
 the sulphide of arsenic volatilizes, while the dark colored sul- 
 phide of antimony remains where the assay was originally 
 placed. The tube is then cut off between the two sulphides, 
 and the dark sulphide of antimony transferred to an open tube. 
 By applying heat the characteristic antimony reaction will 
 appear. When the quantity is extremely small, the tube is 
 crushed, and the fragments, with the adhering sulphides, are 
 introduced into the open tube. 
 
 Antimony fuses at 425 C. (797 F.), and volatilizes slowly 
 at a white heat. By fusing it in the air it takes fire, forming 
 a dense white, inodorous vapor, consisting of antimonious oxide, 
 Sb 2 O 3 . Antimony is very nearly insoluble fn HC1, and H 2 SO 3 ; 
 in aqua regia easily soluble to antimonious or antimonic chlo- 
 ride, SbCl 3 and SbCl 5 . With nitric acid it forms a mixture of 
 white antimonious and white antimonic oxide, insoluble in the 
 acid. Hot sulphuric acid dissolves it, forming antimonious 
 sulphate with evolution of SO 2 . All the sulphur compounds of 
 
DETECTING CERTAIN ELEMENTS. 143 
 
 antimony are soluble in hot concentrated HC1, forming SbCl 3 
 with evolution of H 2 S. 
 
 Sb 2 O 3 is volatile at red heat, easily soluble in hydrochloric 
 and tartaric acids, insoluble in nitric acid. Its unstable salts 
 are decomposed with much water, a white basic salt separates, 
 while the acid solution contains yet Sb 2 O 3 , viz., 4SbCl 3 -f5H 2 
 rr=2SbOCl-fSb 2 O 3 +10HCl. Tartaric acid prevents this re- 
 action. Zinc separates from solutions of Sb. 2 O 3 , in the absence 
 of nitric acid, a black powder of metallic Sb. When a few 
 drops of a compound of antimony, previously acidulated with 
 HC1 (nitric acid is injurious) is brought together with a little 
 zjnc upon platinum foil, the latter becomes covered with a black 
 or brown deposit. This reaction is very sensitive, and takes 
 place even with a dilute solution, a brown spot being formed 
 at once,* soluble in warm nitric acid, antimonic acid being 
 produced. 
 
 H 2 S produces in acid solutions of antimonious acid salts, 
 orange-red Sb 2 S 3 , easily soluble in (NH 4 ) 2 S, or in caustic alkali, 
 but very little soluble in ammonia, and insoluble in bicarbonate 
 of ammonium and dilute acids. Warm HC1 dissolves it to SbCl 3 , 
 while H 2 S escapes. A dilute solution of tartar emetic is colored 
 orange by H 2 S, but is precipitated by the addition of acid. 
 Caustic alkalies, alkaline carbonates, as well as ammonia, and 
 carbonate of ammonia, throw down white amorphous antimo- 
 nious hydroxide, Sb(OH) 3 , soluble in caustic alkali, insoluble 
 in ammonia. 
 
 There are two hydrogen antimoniates or acids : antimonic 
 acid, H 2 OSb 2 O 5 , or HSbO 3 (monobasic) and metantimonic acid 
 (H 2 0) 2 Sb 2 O 7 (dibasic), or isomeric with antimonic acid, and 
 monobasic. 
 
 The normal antimoniates, as KSbO 3 , are all insoluble in 
 water, except a hydrated potassium antimoniate, and this is 
 made anhydrous and insoluble by boiling the solution. 
 
 The super-antimoniates, as (K 2 O) 2 Sb 2 O 5 , are all insoluble in 
 water. 
 
 * A characteristic difference from arsenic and tin compounds. 
 
144 MINERALOGY SIMPLIFIED. 
 
 The monobasic potassium meta-antimoniate, KSb0 3 , is used 
 as a precipitant for sodium (with all other acids soda forms 
 soluble salts], and is prepared by fusing antimonic acid with a 
 large excess of potassium hydrate; then dissolving, filtering, 
 evaporating, and digesting hot the syrupy solution, with large 
 excess of potassium hydrate, best in a silver dish, decanting 
 the alkaline liquor, and stirring the residue, to granulate dry ; 
 this reagent must be kept dry, and only dissolved when re- 
 quired for use to precipitate soda. The reagent is of course 
 not applicable to acid solutions. 
 
 On the insolubility of meta-antimoniate of soda rests one of 
 the best methods for the separation of antimony from other 
 metals, and particularly from arsenic. Any compound of an- 
 timony (except the sulphide) being intimately mixed in a porce- 
 lain crucible with four parts of nitrate of soda and two parts of 
 anhydrous carbonate of soda, and heated until the mass becomes 
 entirely white, then treated, when cold, with water (or still 
 better with very dilute alcohol), all the antimony remains as 
 meta-antimoniate of soda, the arsenic as an arseniate of the 
 alkali is found in the solution. 
 
 For the formation of and reaction of antimonious hydride, 
 SbH 3 , compare arsenic. 
 
 4. ARSENIC (Arsenicum). A steel-gray, lustrous, brittle, 
 and easily pulverizable non-metallic element, vaporizing directly 
 from the solid state at 356 C. (673 F.) in closed vessels; 
 the vapor being colorless, with a strong garlic odor. 
 
 Arsenious and arsenic acids are reduced to the elementary 
 metallic state by several methods of great analytical importance. 
 By the action of hydrogen gas, generated from an acid solution 
 (Marsh's test), it is reduced from all its soluble compounds 
 when it enters into a combination with the hydrogen, to arseni- 
 ous hydride, AsH 3 , which is gaseous and extremely poisonous. 
 The latter can be identified by numerous reactions, and from 
 it the arsenic can again readily be obtained in its free elemen 
 tary state. The hydrogen is generated by sulphuric acid 
 
DETECTING CERTAIN ELEMENTS. 145 
 
 diluted with 6 to 8 parts of water and zinc (both free from 
 arsenic). 
 
 Zn + H 2 Sb 4 =ZnSb 4 + 2H. 
 
 The hydrogen removes the oxygen from either oxide of 
 arsenic,* forming water, and then combines with the arsenic, 
 two atoms of hydrogen taking the place of one atom of oxygen. 
 H 3 AsO 3 + 3(Zn -f H 2 SO 4 ) = 3ZnSO 4 + 3H 2 + AsH 3 . 
 
 Arsenious hydride gas (arsine) burns with a somewhat lumi- 
 nous and slightly bluish flame (distinct from pure hydrogen). 
 
 If a piece of cold porcelain is held in the flame the reduction 
 of temperature prevents the oxidation of As, which is at once 
 deposited in dark, steel-gray spots. 
 
 Arsenious hydride is decomposed by heat alone. In passing 
 through glass tubes, heated to incipient redness, the gas is de- 
 composed, the arsenic adhering to the inner surface of the tube 
 beyond the heated part, as a steel-gray mirror coating. The 
 following reactions exhibited by these deposits will serve to 
 distinguish arsenic from antimony. 
 
 ARSENIC SPOTS. ANTIMONY SPOTS. 
 
 Dissolve in liypochlorite of soda, Do not dissolve in hypochlorite. 
 (NaCIO). 
 
 Warmed with a drop of ammo- Warmed with sulphide of ammo- 
 nium sulphide form yellow ilium form orange spots, insoluble 
 spots soluble in ammonium in ammonium carbonate, soluble 
 carbonate, insoluble in HC1. in HC1. 
 
 A drop of hot nitric acid dis- A drop of hot dilute nitric acid 
 
 solves them. turns them white. 
 
 This clear solution mixed with a These white spots, treated with 
 
 drop of solution of silver ni- silver nitrate and vapor of am- 
 
 trate, gives when treated with monia, give no color, but when 
 
 vapor of ammonia (evolved warmed with a drop of ammo- 
 
 from a glass rod, moistened mum hydrate they assume a 
 
 with ammonium hydrate) a black color, 
 brick-red or a yellow color. 
 
 * Free arsenic and arsenious sulphides are not acted upon by the 
 nascent hydrogen. 
 13 
 
146 
 
 MINERALOGY SIMPLIFIED. 
 
 With vapor of iodine the color 
 turns yellow, by formation of 
 arsenious iodide readily volatile 
 when heated. 
 
 With vapor of iodine color more 
 or less carmine-red, by formation 
 of antimonious iodide not readily 
 volatile by heating. 
 
 ARSENIC MIRROR. 
 
 Deposited beyond the flame, the 
 gas being decomposed at a red 
 heat. 
 
 By vaporization in the stream of 
 gas arsenic escapes with a gar- 
 lic odor. 
 
 By the slow vaporization of arsenic 
 in a current of air, established 
 in an open glass tube, contain- 
 ing the assay, which should 
 be held obliquely over a lamp, 
 a deposit of octahedral crys- 
 tals (see Fig. 113) is obtained 
 beyond the source of heat. 
 Should enough As be present, 
 a dense, white coating is de- 
 posited which, when examined 
 with a magnifying glass, may 
 exhibit crystalline forms. This 
 white sublimate of As 2 3 is so- 
 luble in water, and the solu- 
 tion can be tested in the wet 
 way. 
 
 ANTIMONY MIRROR. 
 
 Deposited before or on both sides ; 
 the gas being decomposed con- 
 siderably below a red heat. 
 
 The vapor has no odor. 
 
 By vaporization in a current of air 
 a white amorphous coating is 
 obtained, insoluble in water, so- 
 luble in HC1, and giving reactions 
 for antimony. 
 
DETECTING CERTAIN ELEMENTS. 
 
 147 
 
 Apparatus for "Marsh's" Tests above mentioned. 
 
 In Marsh's apparatus, Fig. 114, A is the gas evolving bottle, 
 provided with funnel tube a, and escape tube b. B is a chloride 
 
 Fig. 114. 
 
 Fig. 115. 
 
 of calcium tube supported by stand O. Tube b is connected to 
 c by India-rubber joint d. The gas issues at point of tube /, 
 where it may be inflamed.* A simple apparatus, consisting of 
 a test-tube provided with a cork and deliv- 
 ery tube, may serve in many experiments. 
 A convenient form of Marsh's instrument 
 is that shown in the drawing (Fig. 115); 
 it consists of a bent tube having two bulbs 
 blown upon it, fitted with a stopcock and 
 narrow jet. Slips of zinc are put into the 
 lower bulb, which is afterwards filled with 
 the liquid to be examined. On replacing 
 the stopcock, closed, the gas collects and 
 forces the fluid into the upper bulb, which 
 then acts by its hydrostatic pressure, and 
 expels the gas through the jet as soon as 
 the stopcock is opened. It must be borne 
 
 * The inexperienced experimenter is cautioned not to light the gas 
 before all the air has escaped, otherwise an explosion, and destruction 
 of the apparatus may take place. 
 
118 MINERALOGY SIMPLIFIED. 
 
 in mind that both common zinc and sulphuric acid often contain 
 traces of arsenic.* 
 
 Test, for Arsenic in Minerals containing no Sulphur, as 
 Whitneyite (Cu g As). 
 
 Having lately had occasion to examine a mineral new to me, 
 and of unknown composition, made up of small, angular gra- 
 nules, having a submetallic lustre, and a yellowish-brown color, 
 soluble in nitric acid, and free from sulphur, but containing 
 copper, I proceeded to test for arsenic in the usual way, includ- 
 ing Marsh's test, but without success. I found the following 
 simple process the most accurate and delicate :| The mineral 
 powder is placed in a large test-tube or small flask, treated 
 with pure zinc and diluted sulphuric acid, and a piece of filter- 
 ing paper, moistened with nitrate of silver solution, tied over 
 the mouth. If arsenic be present, arsenious hydride (AsH 3 ) is 
 evolved which, acting upon the nitrate of silver, will in a short 
 time blacken it, more especially after some standing. 
 
 Should sulphur be present in a mineral the interference of 
 H 2 S thus formed may be avoided by causing the gas to pass 
 through cotton-wool moistened with a solution of lead acetate, 
 and carefully placed within so as to fill the neck of the flask, 
 then left standing for several hours. This operation may be 
 perfectly relied upon for negative results, and is well suited for 
 testing preliminarily the purity of the reagents employed, viz., 
 zinc and sulphuric acid. 
 
 * Where the amount of arsenic present is small, it becomes neces- 
 sary to take advantage of the effects of heat, and cause the gas to 
 pass slowly through a red-hot tube, until all the zinc is dissolved. 
 The reduced arsenic will be deposited on the cool part of the tube just 
 beyond the heated portion. In all cases in using the above test, it is 
 necessary to ascertain the purity of the zinc and acid by trial, previ- 
 ous to the addition of the suspected liquid. 
 
 f Qualitative Chemical Analysis, by Drs. S. H. Douglas and A. B. 
 Prescott. New York, D. Van Nostrand, 1880, p. 117. 
 
DETECTING CERTAIN ELEMENTS. 
 
 149 
 
 Arsenious and arsenic acids, and their salts, as well as the 
 sulphides of arsenic, are examined by pulverizing and placing 
 them in a glass bulb, covering them with six times their weight 
 of a dry mixture of equal parts of cyanide of potassium and 
 carbonate of soda. The mass is next gently heated, and the 
 moisture, if any be present, removed by inserting a piece of 
 bibulous paper. The operation is repeated until the mixture 
 is perfectly dry. Finally, the bulb is strongly heated over an 
 alcohol lamp, or by the blowpipe flame, when a mirror metallic 
 arsenic deposits in the cool part of the above tube. 
 
 Very small traces of arsenious acid can also be detected 
 according to Berzelius by introducing the assay into a closed 
 glass tube, drawn out to a small diameter (Fijj;. 116), and in- 
 serting a splinter of charcoal above it from a to b. The char- 
 
 Fig. 116. 
 
 Fig. 117. 
 
 coal is first heated, and then the assay ; the arsenious acid is 
 reduced as it passes over the hot charcoal, and As is deposited 
 in the form of a metallic mirror at c. If the tube be cut off 
 between the mirror, c, and the sealed end, a, the mirror, upon 
 heating, gives off the arsenical odor of garlic. 
 
 Arsenic tubes, for the reduction of arsenical compounds and 
 sublimation of arsenic, should all be made of hard German or 
 Bohemian glass, free from reducible metals. 
 
 13* 
 
150 MINERALOGY SIMPLIFIED. 
 
 They are usually about three inches long. Fig. 117 repre- 
 sents the forms mostly used for this purpose, and which the 
 student may readily prepare for himself from glass tubing of 
 suitable width with the aid of the Bunsen blast-burner. 
 
 Reinsch's test is founded upon the fact that metallic copper 
 reduces arsenious acid from a hot hydrochloric acid solution. 
 
 A bright slip of copper foil is boiled in the liquid previously 
 acidulated with hydrochloric acid, the copper withdraws the 
 arsenic and becomes covered with a white alloy. By heating 
 the metal in a glass tube the arsenic is expelled and oxidized 
 to arsenious acid. 
 
 5. BARYTA All salts of baryta, except silicates and phos- 
 phates, yield the characteristic yellowish-green coloration of 
 the flame, especially after moistening with HC1. Even the 
 insoluble sulphate BaS0 4 (heavy spar), obtained when any 
 soluble mineral containing baryta is .dissolved in HC1, and the 
 solution precipitated by dilute sulphuric acid, causes the same 
 coloration. When observed through green glass (colored with 
 oxide of copper) the baryta flame appears bluish-green. See 
 flame coloration, page 104. 
 
 Strontia may interfere with the baryta reaction. The pre- 
 sence of sulphate of baryta with the sulphate of strontia can be 
 detected by fusing the mixture with 3 or 4 parts of chloride of 
 calcium in a platinum spoon, and boiling the fused mass with 
 water. If a cloudiness is produced by adding to the clear dilute 
 solution a few drops of chromate of potassa, the presence of 
 baryta is indicated. Strontia is only precipitated from the 
 concentrated solution (Chapman). 
 
 Sulphate of baryta (heavy spar) fuses B. B.; the fused mass 
 reacts alkaline with test-paper ; on charcoal it is reduced to 
 sulphide. With soda by continued blowing it yields hepar, 
 which placed on a clear silver surface, and moistened with a 
 drop of water, yields black sulphide of silver. 
 
 6. BISMUTH. Fuses and gives off inodorous fumes. When 
 treated alone or with soda in the R. F. on charcoal, it pro- 
 
DETECTING CERTAIN ELEMENTS. 151 
 
 duces a dark-brown oxide, which turns pale-yellow on cooling. 
 The presence of other metals renders this reaction sometimes 
 unsafe, and the wet way for its detection is preferable. If a com- 
 pound of bismuth be treated with a mixture of equal parts of 
 iodide of potassium and flowers of sulphur, and fused B. B. on 
 charcoal, a beautiful red sublimate of iodide of bismuth will be 
 deposited (von Kobell). Compounds containing lead treated 
 in the same manner yield a yellow coating ; their presence does 
 not interfere with the reaction for bismuth. 
 
 Bismuth is insoluble in HC1, but easily soluble in nitric acid 
 or aqua regia, forming a nitrate (NO 3 ) 3 Bi, or a chloride BiCl 3 
 also soluble in hot sulphuric acid, producing a sulphate (SO 4 ) 3 Bi 2 . 
 
 The teroxide of bismuth, Bi 2 O 3 , is formed by a strong igni- 
 tion of the metal in the air, or by heating the nitrate salt. The 
 salts are colorless ; their solutions, if there is not too much acid 
 present, are decomposed by water, and a white basic salt is 
 precipitated. The acid which has been set free always holds 
 some teroxide in solution, 
 
 (N0 3 ) 3 Bi + H 2 O = NO 3 Bi(OH) 2 -f 2NO 3 H. 
 The decomposition of the chloride is more complete, 
 BiCl a + H 2 O = BiOCl + 2HC1. 
 
 In examining small quantities of a substance for minute 
 amounts of bismuth, the HC1 solution is evaporated to a few 
 drops, and these thrown in water. The white precipitate is 
 insoluble in tartaric acid or tartrate of potassa, which dis- 
 tinguishes it from the oxide of antimony, which is soluble. 
 H 2 S and (NH 4 ) 2 S precipitate brown sulphide, (B5 2 S 3 ), insoluble 
 in an excess of sulphide of ammonium. Ammonia and caustic 
 alkali throw down white hydroxide, BiO.(OH), insoluble in an 
 excess. Chromate of potassium throws down yellow chromate 
 of bismuth. If into a clear solution of stannous chloride in an 
 excess of potassa we drop a solution of a bismuth salt, a black 
 precipitate falls which is bismuth monoxide, BiO. 
 
 7. BORIC (boracic) ACID is recognized by the intense green 
 color it or its compounds, especially silicates, impart to the 
 
152 MINERALOGY SIMPLIFIED. 
 
 flame at the instant of fusion, when melted with three parts of 
 the flux, called " Turner's reagent" (a mixture of two parts of 
 fluor-spar and one of bisulphate of potassium). The trial should 
 be made in a dark place. 
 
 Borate of sodium alone tinges the flame pure yellow, but if it 
 be moistened with H 2 SO 4 , boric acid is set free, tinging its mix- 
 ture with alcohol, when ignited, lively green. 
 
 Another very delicate and reliable reaction is that of lies. 
 The finely pulverized mineral is moistened with H 2 S0 4 on 
 platinum foil, the excess of acid evaporated at a gentle heat, 
 and the residue worked into a paste with glycerine, which, 
 when brought on a platinum wire into the flame colors it yellow- 
 ish-green. Compounds of boric acid with an alkali, or an 
 alkaline earth, are tested with turmeric paper as follows : The 
 compound is dissolved in dilute HC1 (till blue litmus is reddened 
 by it); a strip of turmeric paper is then half immersed in the 
 solution for some time, and then dried in a watch-glass at a 
 gentle heat (not over 100 C. or 212 F.). If boric acid is 
 present, the immersed portion of the paper assumes a brown- 
 ish-red color* (Rose). 
 
 If this brownish-red turmeric paper is treated with some 
 alkali or alkaline carbonate, it turns to a bluish or greenish- 
 black ; hydrochloric acid restores the original color. 
 
 If alcohol is poured over a borate with the addition of a suf- 
 ficient quantity of concentrated sulphuric acid to liberate the 
 boric acid, and the alcohol be kindled, the flame appears dis- 
 tinctly green, especially upon stirring with a glass rod and after 
 heating the alcoholic mixture. 
 
 Bromine When bromides are added to a bead of S. Ph., 
 which has previously been saturated with oxide of copper, and 
 is exposed, B. B., to the point of the blue flame, the bead is 
 surrounded with a beautiful greenish-blue color on the edges. 
 (Chlorine acts, however, similarly.) 
 
 * This color must not be mistaken for the blackish-brown shade 
 produced by concentrated HC1. 
 
DETECTING CERTAIN ELEMENTS. 153 
 
 If a bromide is fused in a mattrass with bisulpliate of potas- 
 sium, red bromine vapor is set free, which may also be recog- 
 nized by its characteristic odor. (Berzelius.) If moistened 
 starch-paper is exposed to this vapor yellow bromide of starch 
 is formed. 
 
 The method proposed by Goldschmidt for the detection of a 
 bromine compound alone, or in the presence of iodine and 
 chlorine, is as follows : If a bromine compound is fused in mi 
 open glass tube with pulverized bismuth sulphide (made by 
 fusing metallic bismuth with sulphur), a yellow sublimate is 
 formed. An iodine compound treated in the same way forms 
 a red sublimate and a chlorine compound a white one. With 
 a little care these elements can be readily recognized in the 
 presence of one another. 
 
 8. CADMIUM The pulverized substance for examination is 
 
 heated B. B. in the R. F. on charcoal whereby the metal is 
 oxidized to a reddish-yellow oxide, which being volatile coats 
 the coal reddish -yellow. 
 
 To detect a minute quantity of cadmium (one per cent, or 
 even less, found in zinc or its ores), the assay powder is mixed 
 with soda and heated B. B. in the R. F. on charcoal for a 
 short time, when the latter is coated near the assay with red- 
 dish-brown oxide of cadmium. The zinc being less volatile 
 forms a white coating only after continued blowing. 
 
 Caustic potash throws down from solutions of cadmium salts 
 a white precipitate of hydrated oxide, Cd(HO) 2 , insoluble in 
 an excess. 
 
 Alkaline carbonates, also carbonate of ammonium, throw down 
 the white carbonate of cadmium CO 3 Cd, not soluble in excess. 
 In the presence of free ammonia no precipitate takes place. 
 Cyanide of potassium dissolves the precipitate and gives with 
 salts of cadmium a white' precipitate soluble in an excess, 
 whereby a double salt (K 2 CdCy 4 ) is formed, from which sul- 
 phydric acid precipitates yellow sulphide of cadmium. 
 
 Sulphydricacid and sulphide of ammonium precipitate yellow 
 sulphide of cadmium from saline solutions, easily soluble in 
 
154 MINERALOGY SIMPLIFIED. 
 
 acids. An acid solution, therefore, must be strongly diluted 
 before it is acted upon by H 2 S. Sulphide of cadmium is inso- 
 luble in cyanide of potassium, while sulphide of copper is solu- 
 ble. Hence, in order to separate these two metals, qualitatively 
 as well as quantitatively, their solution is precipitated by KCy, 
 and redissolved in an excess of the reagent. By conducting 
 a current of H 2 S into their joint solution yellow sulphide of 
 cadmium falls while the copper remains in solution, and can 
 only be recovered by decomposition of the cyanide of copper 
 by means of concentrated sulphuric acid added until no longer 
 any hydrocyanic acid escapes. From the resulting solution of 
 sulphate of copper, black oxide of copper is precipitated by 
 caustic potash at a boiling heat. 
 
 9. CARBON It is found in a free state and crystallized in 
 the form of diamond and graphite. In the ordinary stonecoal, 
 in anthracite, soot, etc., the carbon is amorphous; with oxygen 
 it forms mainly two compounds which we shall briefly consider. 
 
 1. Carbon monoxide (Carbonic Oxide), CO A colorless 
 gas, burning in the air with a blue characteristic flame to car- 
 bonic acid, CO 2 . It is a poisonous gas resulting from incom- 
 plete combustion. We obtain it by conducting carbonic acid 
 (CO 2 ) over ignited coal, and by the ignition of many organic 
 compounds, e. g. : 1, oxalic acid ; 2, ferrocyanide of potassium, 
 with concentrated sulphuric acid 
 
 1. C 2 H 2 4 + S0 4 H 2 = S0 4 H 2 -f H f O + m CO, + CO. 
 
 2. Fe(CN) 2 + K 4 (CN) 4 + 6SO 4 H 2 + 6H 2 O = 2SO 4 K 2 + 
 
 S0 4 Fe + 3[S0 4 (NH 4 )J + 6CO. 
 
 It combines in direct sunlight with chlorine at a common 
 temperature to a compound, COC1 2 , having a characteristic 
 suffocating odor. 
 
 Most organic acids, except oxalic and formic acids, leave, 
 after ignition, carbon behind. 
 
 CO gas is very slightly soluble in water, but is readily ab- 
 sorbed in a solution of cuprous chloride in hydrochloric acid. 
 A loose compound, Cu 2 Cl 2 , CO-p2H 2 O, is formed, which by 
 
DETECTING CERTAIN ELEMENTS. 155 
 
 boiling, indeed by mere dilution with water, is decomposed, 
 and CO set free. 
 
 Carbonic Dioxide (Carbonic Acid) CO 2 It is soluble in 
 water, the solution turning blue litmus paper to a dark red. 
 
 Carbonic dioxide renders a solution of caustic lime turbid, 
 forming insoluble carbonate of lime, and yields no hydrate. It is 
 a feeble acid, and many metals like aluminium, etc., form mono- 
 carbonates. Only the carbonates of the alkalies are soluble in 
 water. 
 
 Fused with saltpetre carbon detonates, carbonate of potassium 
 being thereby produced. Carbonates effervesce when treated 
 with a drop or two of dilute hydrochloric acid, etc. ; a few 
 kinds require previous pulverization, and in some cases even 
 heat must be applied before effervescence takes place. 
 
 Some carbonates (lime, etc.) lose their carbonic acid by 
 simple heating in the closed tube. 
 
 10. CERIUM is found in the mineral cerite (Ce,LaDi) 2 SiO 4 
 -|-Ag. The mineral may be decomposed by hydrochloric acid, 
 aqua regia, and sulphuric acid, but more completely by fusion 
 with carbonate of soda. If the finely-powdered mineral be 
 heated along with sulphuric acid, a few drops of nitric acid 
 being added, and then cold water be poured on it, the sulphate 
 of the above oxides of cerite will be dissolved out and the 
 silicic acid be left behind. A hot saturated solution of sulphate 
 of potassium in a moderately dilute solution of cerite precipitates 
 the three oxides as double salts, which, after being washed 
 with a saturated solution of sulphate of potassium, and dissolved 
 in boiling water containing some Hydrochloric acid, are precipi- 
 tated while warm by excess of potassa. Cold and very dilute 
 nitric acid extracts the oxide of lanthanium as the nitrate from 
 the brown mixture of. these oxides (freed from sulphuric acid), 
 which, after its precipitation by carbonate of ammonium and 
 its ignition, is white. 
 
 By repeated treatment of the mixture of these oxides with 
 strong potassa lye and chlorine gas the cerium passes into 
 yellow insoluble proto-sesquioxide, Ce 3 O 4 , while lanthanium 
 
156 MINERALOGY SIMPLIFIED. 
 
 and didymium remain in solution as chlorides. Metallic Ce,La, 
 and Di are obtained by reducing the chlorides with sodium in 
 the form of gray powders, which decomposes water at a common 
 temperature, dissolve in dilute acids with evolution of hydrogen. 
 
 The protoxide of cerium (CeO) is bluish-gray, the hydroxide, 
 Ce(OH) a , colorless. The former quickly passes, on ignition, 
 into Ce 3 O 4 , which is yellowish- white, and when heated orange- 
 yellow. It is soluble in sulphuric (but not in hydrochloric and 
 nitric acid) with a yellow color. Ceroxide, Ce 2 3 , is reddish- 
 yellow, soluble in hot concentrated sulphuric acid with a yellow 
 color ; decomposable by concentrated HC1, with addition of 
 alcohol with production of chloride. 
 
 11. CHLORINE Chlorides like bromides may be detected, 
 B. B., by adding a small portion of them to a bead of S. Ph., 
 which has previously been saturated with oxide of copper; the 
 bead is at once surrounded with an intensely blue flame without 
 the green tinge observed with bromides. The presence of 
 chlorine may also be detected by the blue color which it causes 
 on a paper moistened with a solution of potassium iodide and 
 starch paste. An excess of chlorine removes the color again. 
 Bromine, ozone, nitrous fumes, etc., produce, however, the 
 same effect. 
 
 If a metallic chloride is mixed with solid potassium dichro- 
 mate and concentrated sulphuric acid in a small glass vial a 
 bright brownish-red gas of chloro-chrornic acid is given off, 
 condensing to drops of a like color. Ammonia turns them 
 yellow. 
 
 Soluble chlorides placed upon a piece of clean silver, along 
 with a fragment of sulphate of copper or sulphate of iron, pro- 
 duce at once a black stain on the silver. Insoluble chlorides 
 must previously be melted, together with soda, on a platinum 
 wire to produce this reaction. Bromides yield the same re- 
 action. 
 
 Nitrate of silver produces, even in very dilute solutions of 
 hydrochloric acid or metallic chlorides, a white curdy precipi- 
 
DETECTING CERTAIN ELEMENTS. 1;>7 
 
 tate of 'chloride of silver, turning dark when exposed to sun- 
 light. 
 
 12. CHROMIUM (B. B.). Chromic oxide and chromic salts 
 dissolve in beads of S. Ph. and of Bx., in both the O. F. and 
 R. F., with a yellowish-green tint while hot, becoming emerald- 
 green when cold. Chromium must not be confounded with 
 vanadium, which gives the same reactions in the R. F., but 
 differs by yielding a yellow bead with S. Ph. in the O. F. 
 
 Minerals containing but little oxide of chromium, associated 
 with other metals (Fe, Cu, etc.) which color the fluxes, are 
 best treated by fusing on platinum wire, or in a platinum spoon, 
 with a mixture of equal parts of soda and nitre in the O. F., 
 whereby red chromic acid is formed. The fused mass is dis- 
 solved in water, and the solution poured off from the residue ; 
 to this solution a few drops of acetic acid, and, afterwards, a 
 crystal of acetate of lead (sugar of lead), are added, when an 
 orange-colored precipitate of chromate of lead is formed. This 
 may be collected on a filter, washed, and tested with Bx. and 
 S. Ph. A silicate which contains a small trace of chromium 
 besides iron, and is not decomposed by nitre, is fused upon 
 charcoal in the O. F. with one part of soda and one-half part 
 of borax to a clear bead; this is pulverized, dissolved in HC1, 
 evaporated to dryness, and dissolved in water, and the resi- 
 due of SiO 2 filtered off; the protochloride of iron is changed 
 to sesquichloride by boiling with a few drops of nitric acid, 
 and the chromium, alumina, iron, etc., precipitated with am- 
 monia. The precipitate is filtered off, washed, and tested as 
 above. 
 
 The sesquioxide of chromium, Cr 2 O 3 , is a green powder in 
 water, and, after ignition, insoluble in acids. The chromates 
 are green or violet, partly soluble in water, partly only in acids. 
 Ammonia produces a bluisli-green or greenish-gray hydrate 
 (chrornhydroxide), Cr 2 (OII) 6 , which is partly soluble in excess 
 of the reagent, giving a reddish solution. 
 
 Caustic potassa or soda likewise precipitates the hydrated 
 sesquioxide, readily soluble in an excess, furnishing a green 
 14 
 
o MINERALOGY SIMPLIFIED. 
 
 color. If this alkaline solution is boiled for some time the 
 sesquioxide is reprecipitated, and the supernatant liquid be- 
 comes colorless. 
 
 Alkaline carbonates as well as sulphide of ammonium throw 
 down also hydroxide or a basic salt. In the presence of mag- 
 nesia, zinc, or lead salts, the precipitate with alkalies has the 
 formula MO,O 2 O 3 . 
 
 If the green solution of Cr 2 O 3 in caustic alkali is boiled with 
 some peroxide of lead, chromic acid, Cr0 3 , is formed and turns 
 yellow, and the filtrate when acidulated with acetic acid or 
 neutralized with nitric acid separates yellow chromate of lead. 
 
 The Cr 2 O 3 , insoluble in acid, becomes soluble by fusion with 
 bisulphate of potassium ; by fusion with carbonate and nitrate of 
 an alkali mixed together it becomes converted into a soluble 
 chromate of alkali. This deportment is made use of in search- 
 ing for the Cr 2 O 3 in insoluble compounds, and for its separation 
 from oxides like magnesia, alumina, and sesquioxide of iron, 
 which, undergoing no further oxidation, remain undissolved in 
 the alkaline liquid. 
 
 Chromic acid, CrO 3 , is known only as an anhydride, forming 
 scarlet-red, deliquescent crystals. Its salts are red, like, for 
 instance, the acid potassium salt, Cr 2 O 7 K 2 , or yellow, like the 
 neutral potassium salt, CrO 4 K 2 . The alkaline salts and those of 
 the alkaline earths are both soluble in water ; nearly all the 
 other salts are either insoluble, or with difficulty soluble, in 
 water. 
 
 Chloride of barium precipitates from soluble chromates yel- 
 low CrO 4 Ba ; lead salts throw down a yellow precipitate, 
 CrO 4 Pb ; salts of bismuth produce a yellow, nitrate of silver a 
 purple-red, and mercurous salts a brick-red precipitate. All 
 these precipitates are soluble in nitric acid except chromate of 
 lead, which is soluble in potassa, and can be thrown again by 
 acids. 
 
 Chromic acid is reduced to green sesquioxide by H 2 S,SO. 2 , 
 by alcohol and sugar (in the presence of a free acid), by oxalic 
 
DETECTING CERTAIN ELEMENTS. 159 
 
 and tartaric acid, and by any metal which (like zinc) disen- 
 gages hydrogen. 
 
 13. COBALT may generally be recognized B. B. by the blue 
 bead it affords with Bx. and S. Ph. in both flames. This color 
 will, however, be modified by the presence of other metals. 
 Thus, if iron be present the bead will appear green while 
 hot, and blue when cold. The sulphurets should be roasted on 
 Ch. before testing for cobalt with Bx. on Ch. 
 
 Cobalt forms two well-marked oxides, both 'of which repre- 
 sent bases in corresponding classes of salts : cobaltous and 
 cobaltic salts. 
 
 Cobaltus oxide (protoxide), CoO, is an olive-green powder, or, 
 when in the condition of a hydrate, Co(HO) 2 , rose-red ; its 
 salts are generally blue when anhydrous, or in solutions con- 
 taining free concentrated acids, through their aqueous solutions 
 are pink. 
 
 H 2 S and (NH 4 ) 2 S precipitate black CoS, quite insoluble in 
 (NH 4 ) 2 S ; once formed it is with great difficulty soluble in 
 dilute nitric, sulphuric, and acetic acid. A solution of a salt 
 of cobalt when previously mixed with some acetate of sodium 
 and warmed, is more readily and completely precipitated by 
 H 2 S than a salt of nickel under like circumstances (separation 
 of Co and nickel from manganese). 
 
 Ammonia produces, in acid solutions of cobaltous salts, or in 
 solutions containing ammonia salts, only a red color, which' 
 soon passes into brown. Caustic potash throws down all the 
 cobalt as a blue basic salt, which, by exclusion of air (and 
 quickly by heating), passes into rose-red cobaltous hydroxide, 
 Co(()H) 2 , and this in the air turns to olive-green cobaltous 
 cobaltic hydrate. 
 
 Alkaline carbonates precipitate peach-blossom red basic car- 
 bonate, which is readily soluble in excess of carbonate of am- 
 monium, retaining the same color, but only slightly soluble in 
 the carbonate of sodium and potassa. Ferrocyanide of potas- 
 sium produces a green ; ferricyanide of potassium a brownish- 
 red precipitate. If to a neutral solution of a cobaltous salt, we 
 
100 MINERALOGY SIMPLIFIED.' 
 
 add nitrite of potassium in excess; and next, acetic or dilute 
 nitric acid, a yellow, crystalline precipitate, (N0 2 ) 3 Co-f 3NO 2 K, 
 is thrown down, containing nearly all the cobalt. The precipi- 
 tate is with difficulty soluble in cold water ; insoluble in potas- 
 sium salts and in alcohol of 80 per cent. 
 
 Cobaltic oxide, peroxide of cobalt, Co 2 O 3 . It yields salts, 
 while the corresponding NiO 3 cannot form any, and attempts 
 to produce them yield protoxide salts. 
 
 To detect nickel together with cobalt we proceed thus : The 
 solution, which must only contain these two metals (and be 
 free from manganese for instance) is feebly acidulated with 
 IIC1, cyanide of potassium added in excess, and heated to boil- 
 ing; if now, upon addition of dilute II Cl or H 2 S0 4 , a precipitate 
 follows, nickel is present. 
 
 14. COLUMBIUM, Cb, or NIOBIUM, Nb Marignac has 
 
 shown that nearly all tantalites and .colurnbites contain both 
 tantalum and columbium. To obtain free columbic acid, 
 Cb 2 O 5 , and tantalic acid, Ta 2 O 5 , the powdered minerals are 
 fused with six parts of bisulphate of potassium until completely 
 dissolved. The fused mass is treated with hot water, when 
 both acids remain behind, while the bases and titanic acid, 
 if present, will be dissolved, and can thus be separated. The 
 residue is washed with ammonia and sulphide of ammonium 
 to remove tungstic acid and oxide of tin, while hydrochloric 
 acid dissolves iron. The filtered and thoroughly washed resi- 
 due is now treated with either HC1 or H 2 SO 4 in a porcelain 
 dish, and metallic zinc added. If a tantalate alone be present, 
 no coloration or but a slight one ensues. A columbate thus 
 treated assumes a blue color, which gradually fades and finally 
 turns brown. 
 
 15. COPPER It is easily detected by the green color which 
 most copper compounds impart to the B. B. flame. The pro- 
 duction of a red bead with salt of phosphorus in R. F. is 
 rendered more certain by the treatment of the bead on charcoal 
 with a small amount of tinfoil. 
 
 Copper may also be detected by saturating a salt of phosphor- 
 
DETECTING CERTAIN ELEMENTS. 161 
 
 ous bead with the substance containing it, and adding common 
 kitchen salt (NaCl), when the bead will color the flame beauti- 
 fully blue, owing to the formation of chloride of copper. 
 
 Many minerals give this reaction by simply moistening with 
 HC1, and exposing them in the platinum forceps to the flame. 
 Silicates should first be pulverized, moistened with HC1, and 
 evaporated to dryness in a porcelain capsule, then made into a 
 paste with water, and heated on platinum wire, when the green 
 color is imparted to the R. F. Sulphurets of copper are first 
 roasted on coal and then examined with salt of phosphorus. 
 Hot sulphuric acid dissolves copper with evolution of SO 3 ; 
 nitric acid with evolution of NO. 
 
 1. Cu + 2SO 4 H 3 =zSO 4 Cu + 2H 2 O + S0 3 . 
 
 2. Cu 3 + 8N0 3 H = :3(N0 3 )2Cu + 4H 2 O + 2NO. 
 Cuprous oxide, Cu 2 O, is red when anhydrous, orange as 
 
 hydroxide, Cu 2 (OH) 2 . It is formed by ignition of cupric 
 Oxide, CuO, with metallic copper, or from the cupric oxide 
 salts, by the reducing action of sugar, arsenious acid, etc., in the 
 presence of free alkali. With sulphuric acid it is decomposed 
 into metallic copper and cupric sulphate. HC1 forms white cu- 
 prous chloride, Cu 2 Cl 2 , little soluble in water, but readily soluble 
 in HC1. Its nearly colorless solutions, in acids and in ammo- 
 nia, turn, in the air, rapidly into blue or green cupric compounds. 
 
 Cupric oxide, CuO, is black when anhydrous, greenish- blue 
 as hydroxide, Cu(OH) 2 , insoluble in water, soluble in nearly 
 all acids. Its anhydrous salts are nearly white, the hydrates 
 green or blue. H 2 S and (NHJ2S precipitate from solutions 
 black sulphide of copper, soluble in cyanide of potassium. 
 Caustic potassa in the cold throws down greenish-blue hydroxide, 
 at a boiling heat, black oxide. Ammonia precipitates at first 
 a green basic salt, next blue hydroxide, which, with an excess 
 of the precipitant, form a beautiful azure blue solution. Iodide 
 of potassium precipitates, in the presence of SO 3 , or ferrous 
 oxide, salts, all the copper as white Cu 2 I 3 , soluble in hyposul- 
 phite of soda, and in ammonia in the air. 
 
 Ferrocyanide of potassium precipitates brownish-red ferro- 
 
 14* 
 
162 MINERALOGY SIMPLIFIED. 
 
 cyanide of copper, FeCy 2 -f 2CuCy 2 , insoluble in HC1, soluble 
 in NH 3 . Iron and zinc precipitate in solutions, acidulated 
 with HC1, metallic 'copper. If a solution of copper is put into 
 a platinum dish, a little HC1 and a piece of zinc added, red 
 metallic copper is thrown down, visible even in a state of great 
 dilution. Nitric acid is the best solvent of the metal or its 
 compounds, a cupric nitrate, (NO 3 ) 2 Cu, being formed. The 
 solution in hot sulphuric acid contains SO 4 Cu, that in aqua 
 regia CuCl 2 . Oxide of copper, CuO, is black when anhydrous, 
 as a hydroxide, Cu(OH) 2 , greenish-blue, both insoluble in 
 water, but soluble in nearly all acids. The anhydrous salts 
 are almost all white, as hydrates, green or blue. Hydrosul- 
 phuric acid and sulphide of ammonium precipitate from solu- 
 tions black sulphide of copper, CuS, easily oxidizing in the 
 air, soluble in KCy, insoluble in HC1. Caustic potash throws 
 down in the cold a greenish-blue hydroxide, Cu(OH) 2 , and at 
 a boiling heat black oxide (CuO) ; ammonia throws down at 
 first a greenish basic salt, then the blue hydrate, which is 
 soluble in excess of the reagent, giving a beautiful azure blue, 
 perceptible even in highly diluted solutions. Carbonate of 
 ammonium acts similarly. Ferrocyanide of potassium pre- 
 cipitates in very dilute solutions brownish-red ferrocyanide of 
 copper, FeCy 2 + 2CuCy 2 , insoluble in HC1, soluble in NH 3 . 
 Iron and zinc precipitate from solutions containing some free 
 HC1, metallic copper. 
 
 16. DIDYMIUM, Di It is trivalent. Sesquioxide of didy- 
 mium, Di 2 O 3 . Didymium chloride, DiCl 3 . Didymium hy- 
 droxide, Di(OH) 3 or Di 2 (OH) 6 . Potassium hydrate, or sodium 
 hydrate, throws down, from solution of the salts, a white bulky 
 precipitate of Di(OH) 3 , not soluble in an excess. Ammonia 
 shows the same behavior, but the precipitate is soluble in a 
 hot solution of sal ammoniac, B. B. With borax the sesqui- 
 oxide yields in both flames a colorless, in large quantities an 
 amethyst colored glass. Phosphorus salt dissolves it in the 
 R. Fl. to an amethystine colored rather violet bead. Carbon- 
 ate of sodium yields in the O. Fl. a grayish colored mass (dis- 
 
DETECTING CERTAIN ELEMENTS. 163 
 
 tinction from manganese). Didymium is found in the minerals 
 cerite, monazite, gadolinite, fluocerite, orthite, euxenite, etc. 
 
 Solutions of didymium salts exhibit a well-marked absorption' 
 spectrum, containing two black lines, inclosing a very bright 
 space. One of these black lines is in the yellow, immediately 
 following Frauenhofer's line " D," the other is situated between 
 " E" and b. These characters can be distinctly recognized in 
 a solution half an inch deep, containing only 0.01 per cent, of 
 didymium salt. Lanthanium salts do not exhibit an absorption- 
 spectrum. 
 
 17. ERBIUM Its oxide, EbO, obtained by ignition of 
 erbium nitrate or oxalate, has a faint rose color. It does not 
 melt at the strongest white heat, but aggregates to a spongy 
 mass glowing with an intense green light, which, when ex- 
 amined by the spectroscope, exhibits a continuous spectrum 
 intersected by a number of bright bands. Solutions of erbium 
 salts, on the other hand, give an absorption-spectrum, exhibit- 
 ing dark bands, and the points of maximum intensity of the 
 light bands in the emission-spectrum coincide exactly in posi- 
 tion with the lines of greatest darkness in the absorption-spec- 
 trum. The position of these bands is totally different from 
 those in the emission and absorption-spectra of didymium 
 (Bahr and Bunsen). 
 
 18. FLUORINE When fluorides are heated in a glass tube 
 with 4 parts of bisulphate of potassium, hydrofluoric acid is given 
 off. This imparts to red Brazil-wood paper a straw-yellow 
 color, and etches the tube immediately above the assay, espe- 
 cially visible after the cleansing and drying of the tnbe. 
 
 The best method for the detection of fluorine, even when 
 present in minute quantities, is to heat the assay with previ- 
 ously fused salt of phosphorus (both finely pulverized) in an 
 open glass tube in such a manner that the flame passes into the 
 end of the tube. This latter is thereby rendered opaque where 
 the hydrofluoric acid formed is condensed. This acid is further 
 recognized by its pungent odor and its action on Brazil-wood 
 paper, ?". ?., coloring it straw-yellow. 
 
164 MINERALOGY SIMPLIFIED. 
 
 19. FLUORINE.* Hydrofluoric acid, HF1, and fluorides. 
 Cone. HF1 gives off fumes in the air which are greedily ab- 
 sorbed by water. The aqueous solution dissolves many metals 
 and metallic oxides, forming fluorides. Gold and platinum are 
 not attacked, lead with difficulty. HF1 has the distinguishing 
 property of dissolving silica or silicates -not affected by otheracids 
 with great facility, forming SiFl 4 . Upon this property depends 
 the decomposition of silicates, the etching of glass, and its de- 
 tection. All metallic fluorides are decomposed by cone, sul- 
 phuric acid with evolution of hydrofluoric acid, e. g., CaFl a -f- 
 SO 4 H 2 = SO 4 Ca + 2HF1. Hydrofluoric acid imparts to Brazil- 
 wood paper a straw-yellow color. Silicates containing even a 
 small quantity of fluorine, when heated in the closed tube, give 
 off hydrofluosilicic acid ; this is decomposed into silicic acid, 
 which is separated near the assay, and hydrofluoric acid, which 
 passes off'; but the latter may be detected by inserting a strip 
 of moistened Brazil-wood paper as just mentioned. 
 
 When fluorides are heated in a glass tube with bisulphate of 
 potash, hydrofluoric acid is given off. This etches the tube 
 immediately above the assay, and gives the reaction with Brazil- 
 wood paper. 
 
 20. GLUCINA (Beryllia, oxide of beryllium), BeO, is found 
 in a few minerals, viz., phenakite, beryl, euclase. It gives no 
 characteristic reaction B. B. With borax on platinum wire it 
 is soluble in large quantities in a clear glass, that becomes 
 milk-white by flaming, or when saturated by simple cooling. 
 With salt of phosphorus it behaves as with borax. With solu- 
 tion of cobalt in O. F. it acquires a pale bluish-green color. 
 
 The wet reactions bear a close resemblance to those of 
 alumina ; it differs, however, from the latter by its solubility 
 in carbonated alkalies and in boiling sal-ammoniac solution 
 with evolution of ammonia ; by its salts affording no precipitate 
 of glucinaalum with sulphate of potassium, and by the fact that 
 
 * Free fluorine gas is affirmed to have been found by Oscar Low, at 
 Munich, in fluor-spar from Wolsendorf. See Berichte d'er Deutscheii 
 
DETECTING CERTAIN ELEMENTS. 165 
 
 its dilute solution in the caustic alkalies is decomposed by long 
 boiling, the earth being precipitated. Alkaline carbonates 
 throw down in solutions of its salts BeCO 3 , soluble only in 
 considerable excess of the precipitant. A concentrated solution 
 of carbonate of ammonia dissolves the precipitate more readily 
 than either the carbonate of sodium or potassium; but by boil- 
 ing the earth is again precipitated in such a solution. Native 
 minerals containing glucina are fused with 4 parts of carbon- 
 ated alkali. The mass is evaporated with a slight excess 
 of sulphuric acid to dryness, and the SiO 2 separated by the 
 addition of water. From the concentrated filtrate nearly the 
 whole amount of alumina may be removed in the form of alum, 
 while the BeO remains all dissolved in the mother-liquor. 
 This solution is poured into a warm concentrated solution of 
 carbonate of ammonium. After remaining in contact for several 
 days the solution, containing BeCO 3 , is filtered off and boiled 
 for a long time to precipitate the BeCO 3 ; or it may, after being 
 acidulated with HC1, be thrown down by ammonia as glucinum 
 hydroxide Be(OH) 2 . 
 
 Glucina occurs usually in combination with silica and 
 alumina in minerals. 
 
 21. GOLD may generally be recognized by its physical char- 
 acters : color, lustre, malleability, spec. grav. When a gold 
 compound is heated on a carbonized match in R. F. ? a yellow 
 malleable bead is obtained, which dissolves in aqua regia. If 
 this solution be dropped on to filter paper and one drop of stan- 
 nous cliloride added, a purple-red color is observed. Gold can 
 be readily detected in its solutions, inasmuch as it is obtained 
 in the metallic state by reducing agents*, the well- washed pre- 
 cipitate being dissolved and tested with stannous chloride. It 
 is separated from the easily volatile metals by simple heating 
 on charcoal in O. F. If associated with copper or silver, it 
 must be fused with a large excess of pure metallic lead and 
 subjected to cupellation. The copper is absorbed into the 
 cupel with the lead, while the silver remains alloyed with 
 
166 MINERALOGY SIMPLIFIED. 
 
 the gold. If the globule is quite yellow, it is a proof that but 
 little silver is present, it is then to be tested with salt of phos- 
 phorus, to prove the presence of silver, which, after fusion 
 on charcoal in 0. F., will impart an opaline character to the 
 cool bead. If it be more of a silver-white color, the amount 
 of gold will be small, and in order to prove its presence and 
 approximate quantity the globule must be digested in a por- 
 celain capsule with nitric acid, by application of heat. The 
 silver is thus dissolved, and the gold remains as a dark powder, 
 or as a spongy mass. If this powder be washed and fused 
 with borax on charcoal, it will yield a globule of metallic gold. 
 
 22. IODINE Iodides added to a bead of salt of phospho- 
 rus previously saturated with oxide of copper, tinge the O. F. 
 intensely emerald-green. Compare chlorine and bromine, 
 pages 152 and 156. 
 
 Iodides, like bromfdes, are decomposed and yield, by fusion 
 with bisulphate of potassium, free iodine, which may be recog- 
 nized by its purple-colored vapor and disagreeable odor. 
 
 When an emulsion of starch-paste is mixed with a little 
 iodide of potassium, and some HC1 is added, iodine is libe- 
 rated, which colors the starch blue. 
 
 The iodide of silver, and the iodides of the alkalies, are dis- 
 tinguished, in the presence of other halogen compounds, by 
 the fine scarlet coating they produce, B. B., on coal, when 
 fused with sulphide of bismuth (obtained by heating flowers of 
 sulphur and bismuth). 
 
 23. IRIDIUM, Ir -The metal itself is easily distinguished 
 from all others, excepting rhodium and ruthenium, by its in- 
 solubility in acids, not being attacked in the compact state by 
 any acid whatever, and in a state of fine division, only very 
 slowly by nitro-muriatic acid. Its infusibility, even in an ordi- 
 nary oxyhydrogen blowpipe flame, serves also to distinguish it 
 from all other metals, except rhodium, ruthenium, and osmium. 
 It may be distinguished from rhodium by fusing it, in the finely 
 divided state, with acid (bi) sulphate of potassium. The 
 
DETECTING CERTAIN ELEMENTS. 167 
 
 iridium is then converted into sesquioxide, but does not dis- 
 solve in the acid sulphate or color it pink-red as rhodium does. 
 
 Another method of distinguishing iridium from rhodium, 
 and likewise from ruthenium, is to mix it intimately with 
 potassium or sodium chloride, heat the mixture in a stream of 
 chlorine, and dissolve the resulting double chlorides in water. 
 Iridium thus treated yields a blackish-brown solution, rhodium 
 a rose-red, and ruthenium an orange-yellow solution. All 
 compounds of Ir are easily reduced to the metallic state by 
 ignition in an atmosphere of hydrogen ; the reduced metal may 
 then be tested in the manner just described. 
 
 24. IRON The oxides of iron impart a brownish or yellow- 
 ish-red color to Bx. or S. Ph. in the O. F., and a green one in 
 the R. F., which color nearly disappears on cooling. 
 
 In order to ascertain whether a substance contains protoxide 
 or sesquioxide of iron, some of it is dissolved B. B. in a bead 
 of Bx. previously saturated with some black oxide of copper. 
 If sesquioxide be present the bead turns bluish-green ; if pro- 
 toxide, red opaque spots and streaks are visible on the bead 
 from separated cuprous oxide (Cu 2 O). 
 
 Ferrous oxide, FeO. The salts of this oxide are formed by 
 dissolving iron in dilute HC1 or H 2 SO 4 , with evolution of hydro- 
 gen gas. In warm HN0 3 iron is oxidized to a ferric salt. 
 The ferrous salts are white when anhydrous ; bluish-green as 
 hydrates. T.hey oxidize gradually on exposure to the air, 
 forming a yellow basic ferric oxide, which is deposited in a 
 neutral solution. They give up their acids at a red heat, when 
 red sesquioxide is left behind. 
 
 Caustic alkalies and ammonia precipitate from ferrous salts 
 white hydrated ferrous oxide, Fe(OH) 2 , which turns green, 
 and finally brown in the air. In the presence of ammonia- 
 salts, or organic acids, the precipitation is incomplete. 
 
 Sulphydric acid gives no precipitate in acid solutions of 
 ferrous salts.* 
 
 * Except the ferrous acetate, which is partially precipitated, even 
 in the presence of free acetic acid. 
 
1C8 MINERALOGY SIMPLIFIED. 
 
 Sulphide of ammonium throws down the iron completely as 
 'black sulphide, FeS, slightly soluble in an excess only, when 
 much carbonate of soda is present. FeS is easily soluble in 
 HC1, being converted into FeCl 2 with evolution of SH 2 . 
 
 Ferrocyanide of potassium gives with ferrous salts a white 
 precipitate, or with solutions containing small quantities of 
 ferric oxide a bluish-white one, FeCy 2 -{- KCy, which, on ex- 
 posure to the air, changes quickly into Prussian blue. 
 
 Ferricyanide of potassium gives at once a fine blue precipi- 
 tate (TurnbulPs blue), 3FeCy ? -f FeCy 6 (characteristic distinc- 
 tion of the two oxides). 
 
 Tincture of galls produces no change unless the ferrous salts 
 contain some sesquioxide. 
 
 Ferrous salts reduce chloride of gold and nitrate of silver to 
 the metallic condition. 
 
 Ferric oxide (sesquioxide) of iron, Fe 2 O 3 . This reddish- 
 brown powder remains unchanged when ignited by itself. In 
 this form iron is always determined quantitatively. Fe 2 O 3 is 
 completely soluble in HC1. The native oxide, or that which 
 has been previously ignited, being only slowly soluble. The 
 salts of the sesquioxide in dilute, and as nearly as possible 
 neutral solution, or when the solution is previously treated with 
 acetate of sodium, are decomposed at a boiling heat, sesquioxide 
 of iron being precipitated ; if phosphoric or arsenic acid be 
 present these acids will be contained in the precipitate. By 
 warming a solution of ferric salts with metallic iron, zinc, or 
 with sulphurous acid, or by passing H 2 S through it, they are 
 reduced to ferrous salts. On the contrary, solutions of ferrous 
 salts are converted into ferric salts if at a boiling heat some 
 nitric acid is added. The presence of another free acid 
 (e. g., HC1 or H 2 SO 4 ) is advantageous. The nitric acid is 
 thereby decomposed, and nitric oxide gas, NO (turning to red 
 nitrous acid fumes in the air) is given off, viz.: 
 
 6FeCl 2 + 6HC1 + 2NHO 3 = 3(Fe 2 )Cl 6 + 2NO -f 4H 2 O. 
 
 If no free acid is present, there are partly basic and usually 
 insoluble ferric salts produced. Chlorine gas likewise causes 
 
DETECTING CERTAIN ELEMENTS. 169 
 
 an analogous oxidation of ferrous salts. Thus, if one of the 
 latter, after being acidulated with HC1, is warmed and some 
 chlorate of potassium, KC1O 3 , is added (not more than 2 or 3 
 crystals), the HC1 is decomposed into water and chlorine, which 
 latter, indicated by its odor, accomplishes the oxidation thus: 
 2FeCl 2 -fCI 2 ^(Fe 2 )Cl 6 . 
 
 The following equation expresses the action of chlorate of 
 potassium : 
 
 6FeCl 2 +' 6HC1 + KC1O, = 3(Fe 2 ) C1 6 + 3H 2 O + KC1. 
 
 Free chlorine gas, or chlorine water, may be thus employed, 
 or chlorides, such as the perchloride of tin, SnCl 4 (which yields 
 chlorine). In the separation of Fe 2 O 3 from FeO, MnO, etc., 
 we precipitate the Fe 2 O 3 with carbonate of barium, which pre- 
 cipitates the Fe 2 O 3 completely, even in the cold, while ferrous 
 oxide remains unaltered in the solution (if free from access of 
 air). 
 
 The two oxides, when both are present at the same time, are 
 found by two experiments: 1st, with ferricyanide of potassium 
 (red prussiate of potassium) we test for ferrous oxide (blue 
 precipitate) ; and 2d, with ferrocyanide of potassium "(yellow 
 prussiate of potassium) we test for ferric oxide (blue precipi- 
 tate). From the alkalies sesquioxide of iron is separated by 
 ammonia ; from the alkaline earths and magnesia, by precipi- 
 tating with ammonia, in the presence of sal ammoniac, and 
 boiling until the odor of ammonia disappears. Oxides of the 
 formula MO, that were likewise partially thrown down, pass 
 thus again in solution. From manganese, nickel, Ni(HO) 2 , 
 cobalt, Co(HO) a , it is more readily separated if the dilute 
 solution, containing ferric oxide, is heated with carbonate of 
 sodium until it turns brownish-red, then acetate of sodium 
 added and heated to boiling, when only Fe 2 O 3 is thrown down. 
 
 Tincture of galls precipitates the sesqui salts of iron bluish- 
 black (ink). 
 
 Sulphocyanide of potassium (CNKS) produces a blood-red 
 15* 
 
170 MINERALOGY SIMPLIFIED. 
 
 color, which is not destroyed by HC1, but disappears in the 
 presence of acetate of sodium. 
 
 Ferric acid, FeO 3 , i only known in combination with alka- 
 lies, forming fine, amethystine-red solutions. 
 
 25. LEAD B. B. with Sd. on Ch, a malleable globule of me- 
 tallic lead is obtained from lead compounds ; the coating has 
 a yellow color near the assay, and further oft' a white color 
 (carbonate) ; on being touched with the R. F. both of these 
 disappear, tinging the flame azure-blue. In solutions, dilute 
 sulphuric acid gives a white precipitate of lead sulphate, nearly 
 insoluble in water and in dilute acids. The acid mixture is then 
 best evaporated on a water-bath, water added to the residue^ 
 when the lead sulphate, if present, may further be experimented 
 with. This precipitate, SO 4 Pb, is decomposable by hot con- 
 centrated HC1, is soluble in caustic potassa, also in tartrate of 
 ammonium, containing an excess of ammonia, from which 
 latter solutions it can be precipitated by svlphide of ammonium 
 (black) or chromate of potassium (yellow) ; by being boiled with 
 carbonate of sodium, SO 4 Pb is completely converted into car- 
 bonate of lead. Salts of lead are precipitated both by sulphide 
 of hydrogen and sulphide of ammonium, the black precipitate, 
 PbS, being insoluble in dilute acids, potassa, and sulphide of 
 ammonium. In the presence of much free HC1, the precipi- 
 tated sulphide of lead looks brown or almost red. When in 
 thick masses, such as the common sheets and pipes of commerce, 
 lead is scarcely at all acted upon by cold sulphuric acid, and is 
 but slowly corroded by hydrochloric acid. Both these acids 
 form, by their action on the lead, nearly insoluble salts, and as 
 soon as a layer of the salt has once been deposited upon the 
 surface of the metal, the latter is thereby protected from further 
 corrosion. On exposure to the air lead soon tarnishes, owing 
 to the formation of a thin coating of lead suboxide. By the 
 simultaneous or alternate action of water and air, lead is very 
 rapidly corroded in consequence of the formation of a lead 
 hydrate, which is converted by the carbonic acid in the air into 
 lead carbonate. All natural waters act more or less on lead. 
 
DETECTING CERTAIN ELEMENTS. 171 
 
 In some cases the action is so slight that lead pipes are used 
 with safety for conveying the water ; in other cases, the use 
 of lead pipes is very dangerous on account of the poisonous 
 character of the salts of lead. The author of this book has 
 had frequently occasion to test water, which passed through 
 lead pipes, for this injurious ingredient. Even very minute 
 quantities of lead may be traced thus : A measured quantity 
 of suspected water is evaporated nearly to dryness, and the 
 thus concentrated liquid placed in a small, bright, new porcelain 
 dish, where it is first acidulated with pure acetic acid, and next 
 sulphide of hydrogen passed into it, when, if lead is present, 
 either a black or brown precipitate of PbS is thrown down. 
 Owing to the presence of free acetic acid, ordinary metals like 
 iron do not interfere with the reaction. 
 
 26. LIME, B. B. It imparts a yellowish-red color to the 
 flame. When observed through copper-green glass the lime- 
 flame appears siskin-green ; with cobalt-blue glass it is pale 
 greenish-gray. 
 
 Many calcium salts give an alkaline reaction with test papers 
 after ignition (caustic lime). 
 
 Calcium hydroxide Ca(HO) 2 is soluble in 600-700 parts 
 of cold water (lime-water), which reacts alkaline and becomes 
 turbid in the air (CaCO 3 ). Sulphate of calcium, CaSO 4 -f 2H 2 O, 
 is soluble in 500 parts of water, more readily in acids, but in- 
 soluble in alcohol. " When sulphate of calcium is digested, even 
 in the cold, with carbonate of potassa or carbonate of ammonium, 
 it is entirely converted into carbonate of calcium. Oxalic acid, 
 or soluble oxalates, precipitate lime completely, even from very 
 dilute solutions, as calcium oxalate, C 2 O 4 Ca + H 2 O. Ammo- 
 nia promotes the formation of the precipitate, which is insol- 
 uble in water, acetic, and oxalic acid, but easily soluble in 
 mineral acids, and in neutral magnesia salts. From solutions 
 previously warmed, we precipitate lime generally by oxalate of 
 ammonium and free ammonium (the liquid must smell of free 
 ammonia), and let it rest for twelve hours in a covered glass 
 beaker, decant the clear supernatant liquid, and bring the rest 
 
172 MINERALOGY SIMPLIFIED. 
 
 upon a filter and wash with hot water. For quantitative deter- 
 minations the dried precipitate, with filter, is brought into a 
 platinum crucible and heated, at first gently, and then for ten 
 minutes to a light red heat. The crucible is brought into a 
 drier, and, when cold, weighed. The oxalate has thus been 
 converted into carbonate of calcium. If the heat be too great, 
 some caustic lime may be formed (indicated by moist turmeric 
 paper) ; in that case, a piece of carbonate of ammonium is thrown 
 into the crucible and heat again applied with great care. It is 
 simpler and safer to convert all into caustic lime by heating 
 the crucible over a blast-lamp for twenty minutes. Lime- 
 stones are tested for strontia by calcining, then adding water 
 and boiling, when all the strontia and some little lime will be 
 found in the filtrate. Compare the whole group of alkaline 
 earths (Ba, Sr, Ca, Mg) and note the distinctive reactions. 
 
 27. LITHIA (LiO). Lithia is found in small quantities in 
 petalite, spodumene, amblygonite, lepidolite, tryphylite, and 
 also in the waters of mineral springs. 
 
 B. B. Salts of lithium impart a carmine color to the gas flame 
 or to that of alcohol, which is not prevented by the presence 
 of potassa but is concealed by the intensely yellow color of the 
 salts of sodium. Silicates containing but little lithium scarcely 
 tinge the flame, but if the fine mineral powder is mixed with 
 one part of finely pulverized fluor-spar, and one and a half part 
 of bisulphate of potassium, the whole kneaded with some water 
 into a paste, and this exposed on platinum wire to the point of 
 the blue cone of the flame, the outer flame will be colored dis- 
 tinctly red ; if no lithium be present, the mixture gives a faint 
 violet flame. Chapman has shown that the lithium flame, unlike 
 strontium, is not obscured by the presence of barium. He sug- 
 gests fusing lithium minerals with chloride of barium. Thus, if 
 tryphylite (an iron-manganese-lithium phosphate) is treated in 
 this manner, it yields a beautiful crimson color. (^See flame 
 reactions. ) 
 
 The salts of lithium are all soluble in water, but the oxide, 
 carbonate, and phosphate of lithium are nearly insoluble in 
 
DETECTING CERTAIN ELEMENTS. 173 
 
 watef, hence salts of lithium, in concentrated solution, will 
 give precipitates with carbonate or phosphate of sodium, 
 especially when they are heated and somewhat evaporated. 
 Lithium-platinic chloride is soluble in water, alcohol, and ether. 
 
 28. MAGNESIA, B. B. -^-Magnesia, and many magnesian 
 silicates, afford a clear rose-red color with cobalt solution after 
 a long heating. A fragment after heating should be moistened 
 with the solution and then heated again, the color deepens on 
 cooling. It is distinguished from baryta and strontia in the 
 wet way, by the fact that sulphuric acid gives no precipitate 
 in dilute HC1 solutions, but gives a precipitate in concentrated 
 solutions of calcium salts, which fact again distinguishes lime 
 from magnesia, the sulphate of which (Epsom salts) is soluble 
 in water. The calcium sulphate differs from barium and 
 strontium sulphates by being soluble in a concentrated solution 
 of ammonium sulphate. 
 
 The whole group of the metals of the alkaline earths, like 
 that of the alkalies, occurs only in the form of salts. Their 
 oxides, the alkaline earths (BaO, SrO, CaO), are soluble in 
 water, taking up first a portion thereof and forming, with evo- 
 lution of heat, oxyhydrates (hydroxides) of the general for- 
 mula MO, H 2 O = M(OH) 2 . Magnesia, MgO, is insoluble in 
 water, though with difficulty soluble as a hydrate. Their car- 
 bonates, CO 8 M, and phosphates, (PO 4 ).,M 8 , are insoluble in 
 water but soluble in acids, the soluble salts of the alkaline 
 earths are hence precipitated by soluble and neutral carbonate 
 and phosphate salts. 
 
 Owing to the possibility that the precipitated carbonates of 
 Ba, Sr, and Ca may be partly retained (dissolved), by the 
 free carbonic acid, the precipitation with carbonate of ammo- 
 nium should take place with the slightly warmed liquid and in 
 the presence of free ammonia. The precipitation is somewhat 
 slow, but complete in the absence of ammonium salts, especi- 
 ally chloride. of ammonium. 
 
 For qualitative analysis the following reactions are not with- 
 out some importance. The phosphates of the alkaline earths, 
 
 15* 
 
174 MINERALOGY SIMPLIFIED. 
 
 viz., Ba 3 (PO 4 ) 2 , Sr s (PO 4 ) 2 , Ca 3 (PO 4 ) 2 , are obtained by pre- 
 cipitating the earthy salt solution with a soluble phosphate. 
 The precipitates are white, amorphous, soluble in mineral and 
 acetic acids, but insoluble in water. Consult Magnesia, p. 173. 
 Solubility of the chlorides and nitrates of the alkaline earths 
 in alcohol 
 
 BaCl 2 ). in SrCl 2 | soluble. CaCl 2 ) solu- 
 Ba(NO 3 ) 2 j !1 ' Sr(NO 8 ),j insoluble. Ca(NO 3 ) 2 j ble. 
 
 These reactions can be used for the separation of the group 
 mentioned (also quantitative) in the absence of water, i. e., the 
 salt must be completely dry, and the alcohol must be anhy- 
 drous (100 p. c.)- 
 
 Deportment of the Alkaline Carbonates with the Alkaline 
 Earths. 
 
 When the sulphates of barium, strontium, and calcium are 
 fused in a crucible with carbonate of potassium or sodium, they 
 are quickly and completely converted into carbonates. By 
 merely boiling these earthy salts with a concentrated solution of 
 carbonate of sodium, the sulphates of strontium and of calcium 
 pass readily into carbonates, whilst the sulphate of barium 
 decomposes very slowly, and the solution of the carbonate of 
 sodium must be repeatedly poured off, and be replaced by a 
 new portion and heat applied. 
 
 Separation of sulphate of strontium from sulphate of calcium 
 by sulphate of ammonium. 
 
 A solution of sulphate of ammonium in large excess (1 part 
 of dry salt and 4 parts of water) after boiling for one hour, or 
 in contact for twelve hours at a common temperature, dissolves 
 sulphate of calcium completely, whilst sulphate of strontium 
 (and sulphate of barium) are not altered. From the solution of 
 the sulphate of ammonium the lime is precipitated as oxalateof 
 calcium, which, on ignition, forms carbonate of calcium. 
 
 Sulphuric acid and soluble sulphates produce no precipitate 
 in a solution of a magnesium salt, but the fixed caustic alkalies, 
 
DETECTING CERTAIN ELEMENTS. 175 
 
 and also baryta, and lime-water, especially at a slightly elevated 
 temperature, throw down all the magnesium in form of a hydrate, 
 Mg(OH) 2 , which, however, upon addition of an ammonium salt, 
 in sufficient quantity, disappears again, or when ammonium salts 
 are present, is not precipited at all.* An excess of neutral car- 
 bonate of ammonium precipitates from neutral magnesium salts, 
 when the solution is not too diluted, all the magnesium in the 
 form of an insoluble double salt, e. g., CO 3 MgCO 3 (NH 4 ) 2 + 
 4H 2 O, by which process magnesium may be separated from the 
 fixed alkalies. The fixed carbonates of the alkalies throw down 
 at a boiling heat all the magnesia in the form of gelatinous 
 basic carbonate of magnesium (magnesia alba), 3CO 3 Mg + 
 Mg(OH) 8 -f 4H 2 O, but only in the absence of ammonium salts. 
 
 Phosphate of sodium, (PO 4 HNa 2 ), produces even in dilute solu- 
 tions of magnesium salts, in the presence of sal-ammoniac and 
 free ammonia, a white crystalline precipitate (PO 4 HNa(NH 4 ) 
 -f GH 2 O), soluble in acids, even acetic acid, but entirely in- 
 soluble in dilute ammonia, with which it is washed when filtered 
 off. When ignited it passes into pyrophosphate of magnesium 
 (P 2 0,,M? 3 ). 
 
 29. MANGANESE The oxide (Mn 2 O 3 ) gives with borax 
 
 in the O. F. an amethystine bead (very dark with excess), 
 which becomes colorless in the R. F. (protoxide). The soda 
 test when executed on platinum foil is the most sensitive. 
 The deep green color is more quickly obtained when a small 
 fragment of nitre or chlorate of potassium be added to the assay 
 before fusion. When testing substances which do not dissolve 
 readily in soda, it is well to add a little borax to the bead, and 
 this also makes the test much more delicate (Chapman). By 
 this operation the manganese is oxidized to manganic acid, 
 which forms with soda green manganate of sodium, MnO t Na 2 . 
 
 Manganese forms with oxygen a series of compounds, viz., 
 Manganous oxide, MnO, Manganic oxide (sesquioxide) Mn 2 O 3 
 
 * For 1 mol. of magnesium salt at least 4 mol. of carbonate of am- 
 monium are required. 
 
176 MINERALOGY SIMPLIFIED. 
 
 Manganese dioxide (pyrolusite), MnO 2 . Manganic acid, MnO 3 
 forming manganates, but not used as an acid. Permanganic 
 acid, Mn 2 O 7 , only known arid in use as permanganate salt, as 
 a powerful oxidizing agent. The manganous salts are either 
 of a rose color or colorless, mostly soluble in water, the solution 
 undergoing no higher oxidation in the air; the sulphate is 
 permanent even when ignited. All the oxygen compounds of 
 manganese (and carbonates) form, when ignited, manganous- 
 manganic oxide (Mn 3 O 4 ). All the higher oxides, on being 
 heated with HC1, pass into the condition of manganous chloride 
 (MnCl 2 ), corresponding with manganous oxide (MnO), e. g., 
 MnO 2 + 4HC1 = MnCl 2 + 2C1 + 2H 2 O. 
 
 Manganic oxide is not decomposed by HC1 in the cold. 
 Heated with cone, sulphuric acid all the higher oxides evolve 
 oxygen with formation of SO 4 Mn. 
 
 Sulphydric acid occasions no precipitate in solutions of 
 manganous salts, not even with the acetate. 
 
 Sulphide of ammonium gives a flesh-colored precipitate of 
 manganous sulphide, MnS. Acetic acid acting on the preci- 
 pitated sulphides, separates manganese from cobalt and nickel 
 and from a part of zinc (separation of zinc from manganese 
 and other metals). 
 
 We may also proceed thus : To the examining solution we 
 add acetate of sodium, and precipitate with H 2 S, which throws 
 down sulphide of zinc, and leaves in solution manganese and 
 iron. Acid solutions must previously be neutralized with car- 
 bonate of sodium until they become slightly turbid, and next 
 be acidulated with acetic acid. 
 
 MnS when dissolved in acetic acid in the air gives off H 2 S, 
 takes up oxygen, and turns brownish-black. 
 
 Caustic potash or soda precipitates white manganous hydrate, 
 Mn(OH) 2 , insoluble in excess, and becoming quickly brown in 
 the air, and is then no longer completely soluble in chloride of 
 ammonium. 
 
 Ammonia gives in acid solutions of the manganous salts, or 
 
DETECTING CERTAIN ELEMENTS. 177 
 
 in those which contain ammoniacal salts, no precipitate at first, 
 but the solution becomes turbid on exposure to the air, and 
 deposits (if sufficient ammonia be used) all the metal as brown 
 hydroxide of manganese, Mn 2 (OH) 6 . 
 
 Alkaline carbonates, phosphates, arseniates, and oxalates 
 occasion white precipitates. 
 
 Ferrocyanide of potassium gives a white precipitate with 
 manganous salt, and ferricyanide of potassium a brownish-yel- 
 low one. If lead dioxide or superoxide (PbO 2 ), or minium 
 (2PbO, PbO 2 ) be heated with an excess of nitric acid, and a 
 trace of a manganous salt be added (or the solution to be tested 
 for manganese free from sal-ammoniac), the fluid assumes the 
 intense purple color of permanganic acid, which is very per- 
 ceptible after the separation of the excess of dioxide of lead 
 (a delicate test for manganese). 
 
 Manganic oxide (sesquioxide), Mn 2 O 3 , as well as the corre- 
 sponding hydroxide, Mn 2 (OH) 6 , form brownish-black powders. 
 The solution in cold sulphuric acid is cherry-red or crimson, 
 and passes, like other manganic salts, into manganous salts, 
 with a loss of color when in contact with reducing agents 
 (hydrochloric, sulphurous, and nitrous acid, organic matters, 
 etc.), or when heated by themselves. Dioxide of manganese 
 (peroxide), MnO 2 , is the most important native mineral (pyro- 
 lusite). 
 
 By ignition it yields one-third part of oxygen gas, and when 
 treated with cone, sulphuric acid half its contents of oxygen. 
 
 Permanganic acid. Its salt dissolves in water with an in- 
 tense purple color, which is immediately decolorized by organic 
 materials (analysis of water), and all the following reducing 
 agents (HC1,SO 2 , As 2 O 3 , H 2 S, ferrous salts, etc.). 
 
 30. MERCURY and AMALGAMS yield a sublimate of finely 
 divided metallic mercury, when heated in the closed tube. 
 Compounds of mercury heated in the closed tube together with 
 soda, yield also metallic mercury which condenses above the 
 assay. When a gray sublimate is obtained, without exhibiting 
 distinct metallic globules, these may be made to coalesce by 
 
178 MINERALOGY SIMPLIFIED. 
 
 means of a feather, or the part of the tube containing the sub- 
 limate is cut off' with a file, brought into a test-tube, and boiled 
 with some dilute HC1, by which treatment the mercury unites 
 in shining globules. In cases where mercury is present in 
 such small quantities that no distinct sublimate is formed, it 
 may be detected by inserting into the tube a piece of gold-leaf 
 wrapped around the end of an iron wire and held just above 
 the assay. On heating, the mercury is volatilized, and com- 
 bining with the gold forms a grayish-white amalgam. 
 
 Mercurous compounds of ordinary occurrence are insoluble 
 in water, except the normal nitrate, the sulphate, and the ace- 
 tate, which are sparingly soluble (300 to 600 parts of water). 
 All these require acidulated water for their solution, becoming 
 decomposed by water at a certain degree of dilution, and yield- 
 ing precipitation of basic salts. 
 
 Solutions of mer citrons salts are precipitated by HC1 and 
 by soluble chlorides, the precipitate being white mercurous 
 chlorides or calomel, Hg 2 Cl a , which turns black with caustic 
 potash or ammonia. 
 
 Solutions of mercuric oxide, Hg 2 O 2 are not precipitated by 
 HC1, since the mercuric chloride (corrosive sublimate) is solu- 
 ble in about twelve parts of cold, or two to three parts of boil- 
 ing water, and freely soluble in alcohol and ether. 
 . Stannous chloride (SnCl 2 ) throws down calomel from mer- 
 curic chloride (HgCI 2 ) solutions. A clean strip of copper, 
 placed in a slightly acid solution of a salt of mercury, become 
 coated with metallic mercury, and when gently rubbed with 
 cloth or paper, presents the tin-white lustre of the metal, the 
 coating being driven off by heat. 
 
 31. MOLYBDENUM B. B., on charcoal, gives a copper-red 
 stain in the O. F. on cooling, which becomes azure blue when 
 touched for a moment with the R. F. 
 
 When it is present in small quantity, particularly when as- 
 sociated with copper or tin, as in some furnace products, it is 
 necessary to have recourse to the wet way. The silver-white 
 molybdenum is not oxidized in the air at an ordinary tempe- 
 
DETECTING CERTAIN ELEMENTS. 179 
 
 rature, but when slowly heated it assumes a brownish-yellow, 
 then a blue tarnish, and at a higher temperature it burns off 
 to MoO 3 . It is speedily dissolved by nitric acid as molybdic 
 anhydride (Mo0 3 ), with evolution of nitrous fumes; slowly by 
 hot sulphuric acid, with evolution of SO 2 . Molybdenum forms 
 three classes of compounds, viz., molybdous oxide, MoO ; chlo- 
 ride, MoCl 2 , and other molybdous salts ; molybdic oxide, MoO 2 ; 
 chloride, MoCl 4 , and corresponding salts ; the two kinds of 
 bases are converted into molybdic acid, or molybdates, by 
 strong oxidizing agents, while molybdates are reducible to one 
 or the other of the bases by deoxidizing agents. From molyb- 
 dons salts, as Mo(NO 3 ) 2 , alkaline hydrates or carbonate pre- 
 cipitate dark-brown molybdous hydrate, becoming blue in the 
 air by oxidation to molybdic-molybdate, Mo(MoO 4 ) 2 and 
 Mo 2 O 6 . The hydrate is insoluble in alkalies, sparingly soluble 
 in alkaline carbonates, but easily soluble in biearbonates. For 
 analytical purposes the most important is molybdic anhy- 
 dride, MoO 3 . It is white, lemon-yellow when heated, fuses 
 at a red heat, and sublimes. Hydrochloric acid separates 
 from alkaline molybdates, e.g., K 2 MoO 4 white crystalline mo- 
 lybdic acid, soluble again in an excess of the acid. This latter 
 acid solution, or the HC1 solution, assumes, in contact with 
 zinc, at first a blue, then a green and brown color. The addi- 
 tion of sulphocyanide of potassium changes the brown solution 
 to red. The same red tint is obtained when the hydrochloric 
 acid solution of a molybdate is treated with sulphocyanide of 
 potassium. Ether withdraws this color from the liquid and 
 assumes an orange tint, which, exposed to the air, turns crimson 
 (the most sensitive reaction for molybdenum). H 2 S produces 
 in acid solutions of molybdic acid gradually a brown precipi- 
 tate, MoS 3 , soluble in (NH 4 ) 2 S, forming (NH 4 ) 2 MoS 4 , while 
 the supernatant liquid appears blue or green. The same pre- 
 cipitate is formed when the aqueous solution of an alkaline 
 molybdate, after being saturated with H 2 S, or after the addi- 
 tion of (NH 4 ) 2 $, is acidulated with HC1. When the powdered 
 compound of molybdic acid is mixed with a drop of strong 
 
180 MINERALOGY SIMPLIFIED. 
 
 sulphuric acid on platinum foil, a blue color is obtained, or 
 it is still better to heat the pulverized substance in a small 
 porcelain dish with a little cone, sulphuric acid, and then add 
 alcohol, when the liquid assumes a sky-blue color if molybdic 
 acid is present. For the reaction of molybdate of ammonium 
 with phosphoric acid see " Phosphates," page 183. 
 
 32. NICKEL, B. B Oxide of nickel gives, if cobalt is not 
 present, in the O. F. a reddish-brown bead when hot and 
 pale-yellow on cooling. With larger quantities of oxide these 
 colors are darker. In the R. F. the bead becomes gray and 
 opaque from the separation of metallic nickel, and on long con- 
 tinued blowing colorless. Upon Ch. in the R. F., especially 
 upon addition of granulated tin, the reduction is quickened and 
 the reduced nickel unites with tin to a metallic globule. 
 
 All the salts of the protoxide, or nickelous oxide, NiO, are 
 yellow when anhydrous ; as hydrates, or in solution, green ; 
 they redden litmus paper, arid are decomposed on ignition. 
 The neutral salts (containing no free acid) are only partially 
 decomposed by H 2 S ; and, when acidulated with HC1, not at 
 all ; acetate of protoxide of nickel or any nickel salt, previously 
 treated with acetate of sodium, is completely precipitated by H 2 S 
 when the solution is warmed, and contains riot too much free 
 acetic acid. The precipitated black sulphide of nickel (NiS) 
 is with difficulty soluble in dilute hydrochloric, and in acetic 
 acid, though very soluble in nitric, and nitro-hydrochloric 
 acid. (IS H 4 ) 2 S, likewise throws down from a neutral solution 
 sulphide of nickel, of which only a very small quantity remains 
 soluble in an excess, giving it a brown color. On this account 
 a brown cok>r of the liquid (which is poured off from the pre- 
 cipitate produced by (NHJ 2 S) indicates nickel. 
 
 Potassa throws down apple-green nickel hydroxide = 
 ^(OH)^, insoluble in excess, soluble in ammonia salts. Acid 
 salts, or such containing sal-ammoniac, are not precipitated by 
 NH 3 ; neutral salts only partially; the precipitate is soluble in 
 an excess of ammonia with a blue color. Caustic potash 
 throws down gradually from this solution Ni(OH) 2 . Carbo- 
 
DETECTING CERTAIN ELEMENTS. 181 
 
 nates of the alkalies precipitate basic carbonates ; the precipi- 
 tate being soluble in an excess of the precipitant. 
 
 Nitrite of potassium produces in very concentrated nickel 
 solutions only a brownish-red precipitate of potassio-nickelous 
 nitrite = (N0 2 ) 2 Ni -f- 4NO 2 K, soluble upon addition of water. 
 In the presence of carbonates of the alkaline earths (Ba, Sr, 
 CM), CO 3 , said reagent throws down, even in dilute nickel 
 solutions, nearly all the metal in the form of yellow crystalline 
 salt (NO 2 ) 6 NiMK 2 , (M = Ba, Sr, or Ca), which in cold water 
 is with great, difficulty, in boiling water easily, soluble, with a 
 green color, decomposition taking place. 
 
 Ferrocyanide of potassium yields a greenish-white, ferri- 
 cyanide of potassium a yellowish-green precipitate. 
 
 Cyanide of potassium precipitates nickelous cyanide, soluble 
 in excess, the solution contains potassio-nickelous cyanide = 
 (NiCy 2 , 2KCy), from which dilute HC1, or H 2 S0 4 , again 
 throws down NiCy 2 , with evolution of hydrocyanic acid. 
 
 If the solution of NiCy 2 , 2KCy, is treated with an alkaline 
 solution of hypochlorite of sodium, and heat applied, blackish- 
 brown nickelic oxide (peroxide) Ni 2 O 3 , is thrown down as 
 hydroxide. The same happens, when the. hydrated protoxide 
 of nickel, diffused in water (or better in dilute alkali) or a 
 solution of cyanide of nickel, is treated with chlorine. Free 
 acids, even acetic acid, prevent its formation. HC1 con- 
 verts it into chlorine and chloride of nickel. On this reaction 
 rests a method of separating nickel from cobalt. 
 
 33. NITRIC ACID (NITRATES) When nitrates are fused in 
 a glass tube with bisulphate of potasium, reddish-brown fumes 
 are evolved (N 2 3 ), which become readily visible when the 
 tube is held against a white background. All nitrates detonate 
 when heated on charcoal ; those of the alkalies and alkaline 
 earths (calcium nitrate) deflagrate with violence, being con- 
 verted into carbonates. 
 
 Osmium. See page 123. 
 
 Oxygen All combustible substances burn in oxygen gas 
 with great brilliancy, hence if this element is Driven off from 
 
182 MINERALOGY SIMPLIFIED. 
 
 some compound heated in a reagent tube, and an ignited splin- 
 ter of charcoal be brought into the gas, it will burn with 
 greatly increased brilliancy. 
 
 34. PALLADIUM Oxide of palladium, PdO, is reduced on 
 ignition by B. B., but the metallic particles cannot be fused 
 together. With borax on platinum wire in O. F. it is reduced 
 without dissolving in the flux. The metallic particles cannot 
 be united together to a globule even on charcoal in R. F. as in 
 O. F. With salt of phosphorus it gives the same reaction. 
 With soda on coal insoluble. The soda is absorbed by the 
 coal, leaving the Pd behind as infusible powder. 
 
 Palladium occurs in a tolerably pure state with Brazilian 
 platinum ore, also together with gold. It is darker than plati- 
 num ; heated in the air, it oxidizes and turns blue ; at a higher 
 temperature the oxide is again destroyed. In the alcohol flame 
 the metal becomes covered with soot; it is capable of condensing 
 enormous quantities of hydrogen gas.* In nitric acid it is with 
 difficulty dissolved. In hot hydrochloric and sulphuric acid 
 scarcely soluble ; in aqua regia readily soluble. With oxygen 
 it forms two oxides, PdO and PdO a , like platinum. PdO is 
 the common compound. PdCl 4 is produced with aqua regia, 
 and combines with other chlorides, viz., K a PdCl 6 . Palladic 
 chloride loses chlorine easily, passing into palladious chloride, 
 PdCl 2 , and to this correspond the other palladious salts. From 
 solutions of these caustic alkalies produce a dark-brown pre- 
 cipitate, PdO, soluble in excess; ammonia gives a flesh-red pre- 
 cipitate, PdCl 2 NH 3 , soluble in excess. By the action of HC1 
 on this solution, a yellow, precipitate is formed, Pd(NH 3 Cl) 2 . 
 Iron vitriol reduces palladium salt slowly to metallic palladium 
 (black). Stannous chloride induces a black precipitate, and 
 gives a green solution. Iodide of potassium produces, even in 
 dilute solutions, a black precipitate of palladious iodide, PdI 2 , 
 
 * Palladium hydrate, Pd 2 H 4 , is formed by passing hydrogen over 
 metallic palladium heated to redness. It possesses all the properties 
 of a metal ; it has metallic lustre, is tough, conducts electricity, and 
 is distinctly magnetic. (Graham.) 
 
DETECTING CERTAIN ELEMENTS. 183 
 
 quite insoluble in water, and suitable for the quantitative deter- 
 mination of iodine. 
 
 35. PHOSPHORIC ACID OR PHOSPHATES. The green color 
 (see flame reactions) which phosphates impart B. B. to the 
 flame, especially upon the addition of a drop of concentrated 
 sulphuric acid serves often for their detection. 
 
 If a previously pulverized and well-dried phosphate is heated 
 to a red heat in a closed tube with a piece of magnesium-wire 
 or metallic sodium, the phosphoric acid will be reduced. If 
 the tube is then broken, and the piece containing the fused 
 assay is, after cooling, moistened with a little water, phosphor- 
 etted hydrogen PH 3 is given off, having the characteristic dis- 
 agreeable odor of decaying fish. 
 
 If a phosphate salt is dissolved B. B. in a borax bead to 
 which some carbonate of sodium has been added, and tungstate 
 of sodium is introduced, the bead upon being heated in the R. F. 
 turns blue, while tungstic acid alone colors a borax bead in the 
 R. F. yellow. 
 
 In the * r et way it is traced, even in very minute quantities, 
 thus, a few drops of a neutral or acid solution containing phos- 
 phoric acid are poured into a test-tube which is then filled to 
 the depth of an inch with a solution of molybdate of ammonium 
 containing much free nitric acid, there is formed a pale yellow 
 precipitate termed ammonium phosphomolybdate. For the 
 full delicacy of the test, especially if mere traces of phosphoric 
 acid are present, the mixture should be set aside for several 
 hours at a temperature of 30 to 40 C. 
 
 Silicic acid, with which phosphoric acid might be confounded, 
 produces a strongly yellow coloration, but does not yield a 
 precipitate, whilst arsenic compounds in solution furnish a 
 yellow precipitate of ammonium arsenio-molybdate of variable 
 composition. 
 
 36. PLATINUM This metal is insoluble in IIC1, HF1, 
 H 2 8O 4 , and HNO 3 , but soluble in aqua regia to platinic chlo- 
 ride, Ptd 4 . From this reddish-yellow solution H 2 S throws 
 down dark-brown platinum sulphide PtS a , soluble in an excess 
 
184 MINERALOGY SIMPLIFIED. 
 
 of yellow ammonium sulphide. Stannous chloride colors the 
 solution of platinum dark brownish-red. For the reactions of 
 PtCl 4 with KC1 and NH 4 C1, consult potassium (below) and 
 ammonium, page 140. 
 
 37. POTASSIUM For flame reactions, see B. B. A glass of 
 
 borax containing potassa becomes blue when a little oxide of 
 nickel* is carefully added, with soda alone a brown bead is 
 obtained on cooling. 
 
 For the detection of potassium in compounds in the wet way, 
 platinic chloride (PtClJ is added to neutral and acid solutions 
 of the compound substance (not too dilute), together with HC1, 
 (if the compound be not a chloride)* when a yellow crystalline 
 precipitate of potassium platinic chloride (KCl) 2 PtCl 4 is thrown 
 down. Since ammonium salts are also precipitated by this 
 reagent with closely resembling color and form, these, if pre- 
 sent, must first be removed (volatilized). Minute portions of 
 potassa are detected by evaporating the solution with the rea- 
 gent nearly to dryness on the water-bath, and then dissolving 
 the mass in alcohol ; the yellow crystalline precipitate, octahe- 
 dral, remains undissolved, and may be identified under the 
 microscope. 
 
 38. RHODIUM Rhodium is contained in platinum ores (0.4 
 
 to 1.0 p. c.). It is soluble in aqua regia only when in an alloyed 
 condition (with Pt or Cu). It is soluble on fusion with bisul- 
 phate of potassium ; it is oxidized at a red heat when mixed with 
 potassa and nitre, forming brown RhO 2 . When Rh is mixed 
 with common salt, and a current of chlorine passed through the 
 mixture, a red double salt is formed, Rh 2 Cl 6 -f GNaCl, soluble 
 in water. From the warm solution, H 2 S precipitates slowly. 
 Rh 2 S 3 insoluble in (NH 4 ) 2 S. When the solution is treated with 
 some caustic potassa solution, and a few drops of alcohol added, 
 
 * Oxalate or carbonate of nickel may also be employed. It must 
 be free from cobalt (must not furnish a blue glass with borax). Ad- 
 mixtures of soda and lithia do not interfere with the reaction if the 
 potassa is present in sufficient quantity. 
 
DETECTING CERTAIN ELEMENTS. 185 
 
 a black precipitate of metallic rhodium falls at ordinary tem- 
 perature. 
 
 39. RUBIDIUM. The oxide rubidia, a very rare alkali, gives 
 B. B. a violet flame, and when mixed with caesia and potassa, 
 can only be distinguished by spectroscopic examination. 
 
 40. RUTHENIUM is alloyed with platinum, and found as 
 laurite, Ru 2 S 3 , in the platinum ore of Borneo. Insoluble in 
 acids. By fusion with caustic potassa and chlorate of potassium, 
 or saltpetre, an orange colored RuO 4 K 2 is formed, from the solu- 
 tion of which nitric acid separates black sesquioxide. Chlorine 
 throws down anhydrous RuO 4 . From the orange solution of the 
 sesquioxide in HC1, hydrosulphuric acid (which colors it at first 
 blue), throws down after a while brown sulpho-metal. Sulpho- 
 cyanide of potassium (in the absence of other platinum alloys) 
 causes a purple-red, and, when heated, a violet coloration. 
 
 41. SELENIUM and SELENIURETS yield in the closed tube at 
 a high temperature, a sublimate which is reddish or black, and 
 producing a red powder, give off at the same time the odor of 
 decaying horse-radish. In the open tube they evolve the 
 same characteristic odor, and yield a sublimate of selenium, 
 which near the assay is steel gray, and further off red. 
 
 Selenites and selenates are reduced to selenides B. B. on 
 charcoal in R. F. with the characteristic odor of selenium. 
 
 Selenium is steel-gray with a faint metallic lustre ; it fuses 
 very easily; volatilizes with brown fumes, giving the odor of 
 decaying horse-radish; is soluble in bisulphide of carbon, and 
 imparts B. B. a blue color to the O. F. Consult flame re- 
 actions, page 105. 
 
 42. SILICIUM, SILICON, or the oxide, SILICA, when heated 
 with soda gives a clear glass, if the soda be not in excess. 
 This reaction distinguishes silica from the earths ; silica may, 
 however, contain alumina, and still fuse with soda to a clear 
 glass. 
 
 In most silicates the silica may be detected by the help of 
 salt of phosphorus. Most silicates, when added to a bead of 
 that salt and heated, are decomposed ; the bases dissolve in the 
 
 1G* 
 
186 MINERALOGY SIMPLIFIED. 
 
 free phosphoric acid without interfering with its transparency 
 (unless the substance is present in too large a quantity), while 
 the silica, being almost insoluble, floats as a translucent spongy 
 mass* in the bead. The latter must be observed carefully 
 while hot, since many silicates form a glass, which, on cool- 
 ing, becomes opalescent or turbid. The spongy mass (Kiesel- 
 skelett) consists of an aggregate of most minute crystals which 
 almost defy a microscopical determination. According to a 
 great many experiments, however, they possess the crystal- 
 line form of tridynrite, which is hexagonal, the crystals being 
 tabular, formed by the prism and basal plane. They consist of 
 pure silica, like quartz. f 
 
 When a finely powdered silicate is fused with an excess of 
 carbonate of sodium, the resulting mass dissolved in dilute HC1, 
 and evaporated to dryness, the silica is rendered insoluble ; and 
 on moistening the residue with strong HC1, and dissolving it 
 in hot water, all the silica will remain behind; and can be 
 separated from the bases by filtration and washing. 
 
 Most of the hydrous silicates, and many which are anhy- 
 drous, but which contain an excess of base, are decomposed by 
 strong HC1, the bases uniting with the HC1. while the silica 
 separates, either as a gelatinous hydrate, or as a non-gelatinous 
 powder. 
 
 43. SILVER This metal is easily recognized by its physical 
 characters, as also by the brown coating it gives when heated 
 in O. F. on charcoal. When combined with easily oxidizable 
 metals, it may be separated by heating on charcoal in O. F. 
 If silver be associated with a large quantity of lead or bismuth, 
 it is best to subject it to cupellation. The following process 
 serves for .its complete separation from most argentiferous ores. 
 The finely powdered substance is mixed with an equal bulk of 
 borax glass, and an excess of pure granulated lead (except in 
 
 * Kieselskelett, Germ. 
 
 f J. Landauer's Lothrohranalyse, 2d ed. Berlin, 1881, p. 95. See 
 also " Tridyinite," p. 260, in E. S. Dana's Text-book of Mineralogy, 
 New York, 1877. 
 
DETECTING CERTAIN ELEMENTS. 187 
 
 cases where lead or its oxide already exists, as in litharge, mi- 
 nium, cerussite). The mixture is placed in a cylindrical cavity 
 of the coal, and fused in R. F. with Fletcher's blowpipe, Fig. 
 91, after the earthy matters have been dissolved, and the 
 metallic particles united into one globule ; this latter is subjected 
 for a short time to the O. F., thereby separating volatile and 
 easily oxidizable substances that maybe present. The" remain- 
 ing globule, containing a large excess of lead and all the silver, 
 together with the larger portion of the nickel and copper, is 
 then separated from the flux mechanically, and subjected to 
 cupellation. 
 
 For this purpose finely pulverized bone-ash is mixed with a 
 small quantity of soda and made into a stiff paste with water. 
 This paste is placed in a circular cavity in charcoal, half an 
 inch in diameter, and one quarter inch deep, and the surface 
 of it made concave and smooth by pressing it with an agate 
 pestle, or any other suitable convex surface. This cupel is now 
 carefully exposed to a gentle heat till perfectly dry. These cap- 
 sules may be bought ready-made. The lead globule freed from 
 adhering flux is then placed upon the cupel and exposed to 
 O. F. Should much nickel and copper be present an infusible 
 coating is formed which prevents the desired oxidation ; this 
 may be counteracted by the addition of a small quantity of 
 lead. The blast is kept up until all traces of lead have become 
 oxidized ; this is indicated by the cessation of the rainbow 
 colors of the oxide of lead which play over the surface of the 
 globule. When the quantity of litharge that is formed in the 
 process of cupellation is large, the globule of silver, still con- 
 taining lead, may be removed to a fresh cupel and there finally 
 refined. The instant when the last traces of lead disappear is 
 then readily perceived by the sudden brightening of the 
 globule. The remaining metal, when freed from gold, has a 
 silver-white color. It may be tested for gold as described 
 under that metal. See, also, cupellation of silver and gold, 
 page 165. 
 
 In the wet way silver is determined, in almost all cases, as 
 
188 MINERALOGY SIMPLIFIED. 
 
 chloride of silver, AgCl, and separated from other metals ; its 
 insolubility in acids and solubility in ammonia distinguish it 
 readily from all the other chlorides which are insoluble, or with 
 difficulty soluble. Some metals, such as zinc, iron, and copper, 
 the protosulphate of iron (or, perhaps better, the prot-acetate 
 of iron), stannous chloride, sulphurous acid, and many organic 
 compounds, precipitate metallic silver from its solutions. 
 
 44. SODIUM It is readily distinguished, even in compound 
 substances, by the intense yellow color it imparts to the outer 
 blowpipe flame. The sodium flame is invisible when observed 
 through cobalt-blue glass, and red glass ; with green glass it is 
 orange colored (sensitive reaction). Sodium is not precipitated 
 by platinic chloride, since it forms a compound soluble in water, 
 alcohol, and ether. Indeed, nearly all its salts are soluble, ex- 
 cept pyroantimoniate of sodium, Na a H 8 Sb a O 7 -f- 6H 2 O.* Pyro- 
 antimoniate of potassium, which is soluble, is hence the only 
 reagent that precipitates soda from its solutions, as a white 
 compound, of the above-mentioned composition, viz : 
 K 2 H 2 Sb 2 O 7 -f 2NaCl = Na 2 H 2 Sb 2 O 7 + 2KC1. 
 
 It must be precipitated from a neutral, or feebly alkaline 
 solution. Alkaline solutions must be neutralized with dilute 
 hydrochloric or acetic acid ; acid solutions with caustic potassa 
 (not ammonia). 
 
 Compare flame reactions. 
 
 * Prof. N. Menschutkin's Analytische Chemie. German edition 
 of Dr. 0. Bach, page 32. Fremy, the discoverer of this salt, calls 
 it metantimoniate of sodium, which, according toMenschutkin, is not cor- 
 rect. This author considers antimonic acid in some respects analo- 
 gous to phosphoric acid, viz : 
 
 Phosphoric acid = PH/) 4 . 
 
 Pyrophosphoric acid = 2PH 3 4 H 2 = P 2 H 4 7 . 
 
 Metaphosphoric acid = PH 3 4 H 2 = PH0 3 . 
 
 Antimonic acid = ShH 3 4 
 
 Pyroantimonic acid = 2SbH 3 4 H 2 = Sb 2 II 4 7 . 
 
 Metantimonic acid = SbH 3 4 H 2 = SbIlO 3 . 
 
DETECTING CERTAIN ELEMENTS. 189 
 
 45. STRONTIUM Strontium compounds color the flame 
 
 crimson. In the presence of barium the crimson color appears 
 at the moment when the substance, moistened with HC1, is first 
 brought into the flame. The paler, yellowish-red flame of 
 calcium is liable to be mistaken for the strontium flame. Con- 
 sult flame-colors, p. 104 et seq. 
 
 In solubility ', most compounds of strontium closely resemble 
 those of barium, the hydrate being a little less soluble, and the 
 sulphate and chromate more soluble in water than the corre- 
 sponding barium compounds, and the silico-fluoride quite 
 soluble. The chloride is soluble, the nitrate insoluble, in ab- 
 solute alcohol (100 per cent.). 
 
 Strontium sulphate (SrSO 4 ), like barium sulphate, is almost 
 insoluble in concentrated solution of ammonium sulphate, while 
 sulphate of calcium is soluble, and may thus be separated. A 
 saturated solution of calcium sulphate (CaSO 4 ) slowly pro- 
 duces a faint precipitate of SrSO 4 (prevented, or dissolved, by 
 the presence of HC1, and HN0 3 ), but quite insoluble in alcohol. 
 
 An aqueous solution of calcium sulphate (gypsum) may be 
 the simple means to distinguish calcium, barium, and strontium 
 salts, when soluble in water. No precipitate will be formed if 
 lime is present, while a baryta solution will at once be rendered 
 turbid, or afford a precipitate, and strontia gives a faint pre- 
 cipitate after some time only. An addition of alcohol, how- 
 ever, throws down completely sulphate of strontium and sulphate 
 of calcium. 
 
 46. SULPHUR Free sulphur fuses and forms a yellow sub- 
 limate in the closed tube. In an open tube, or on charcoal, it 
 burns, yielding sulphurous acid, SO 2 . The higher sulphides 
 (sulphurets) give off sulphur in the closed tube; the neutral 
 sulphides and subsulphides give off sulphurous acid gas when 
 heated in the open tube, recognizable by its odor and the red- 
 dening of moist blue litmus paper. Sulphur is soluble in bisul- 
 phide of carbon, benzine, and turpentine. 
 
 In the investigation B. B. of sulphur-compounds, a lamp or 
 candle-flame should be employed, since ordinary coal gas 
 
190 MINERALOGY SIMPLIFIED. 
 
 often contains considerable quantities of sulphur. The sulphur 
 in sulphides an<d sulphates may be detected B. B. by fusing 
 small quantities on coal with two or three parts of soda in the 
 R. F. The sulphur is hereby converted into sulphide of 
 sodium, which when placed on blank silver-foil, or on a bright 
 silver coin, and moistened with a drop of water, yields sulphu- 
 retted hydrogen, which blackens the silver, and also test-paper 
 containing acetate of lead. If selenium is present, the reaction 
 cannot be used. 
 
 The following delicate test in the wet way, given by von 
 Kobell, answers well in most cases: A small quantity of the 
 powdered mineral sample, and an equal volume of iron powder* 
 (Ferrum pulveratum, or alcoholizatum of the druggist) are 
 put with a spatula into a glass cylinder 2^ inches high and 
 1 inch in diameter, and barely covered with hydrochloric acid 
 (1 vol. cone, acid and 1 vol. of water). A strip of filtering 
 paper, previously dipped into sugar-of-lead solution and dried, 
 is fastened to a cork, and the mouth of the cylinder closed with 
 it. In about one minute the paper appears blackened by the 
 sulphide of lead thus formed, if any sulphur is present. All 
 those compounds giving any distinct sulphur reactions, react 
 also hepatic with iron powder. A dilute solution of ammonium 
 molybdate with an excess of hydrochloric acid is colored fine 
 blue by a small quantity of sulphuretted hydrogen or of sulphides 
 dissolved in water. One of 'the most sensitive tests for sulphur 
 (in the presence of an alkaline hydrate) is that of Prof. J. D. 
 Dana. Heat B. B. in the R. F. any sulphide or sulphate, or any 
 powdered mineral assay containing sulphur, upon charcoal 
 with Sd. Put the fused mass into a watch-glass, moisten with 
 a drop of water, and add a particle of a crystal, not larger than 
 a pin's head, of the sodium nitroprusside (or of the correspond- 
 ing potassium salt) ; there will be a magnificent purple color 
 displayed at once, but disappearing after some time. Vapors 
 
 * Iron filings, free from rust, are pounded in an iron mortar ; first 
 sifted through a fine sieve, and afterwards through linen. 
 
DETECTING CERTAIN ELEMENTS. 191 
 
 are tested for hydrosulphuric acid (H 2 S) by conducting them 
 into an ammoniacal solution of sodium nitroprusside.* 
 
 A glass made B. B. of eoda and silica becomes red, or orange, 
 when sulphur is present. 
 
 When soda is fused on charcoal in the R. F. with any com- 
 pound of sulphur (sulphide or sulphate), sulphide of sodium is 
 produced, and, if much sulphur is present in the sample, the 
 fused mass will show the characteristic color of "hepar" 
 (Hepar sulphuris, or liver of sulphur), being; an old term for 
 the higher sulphides of the alkalies, having a liver-brown 
 color. 
 
 47. TANTALUM See Columbium (Niobium), 72, p. 144. 
 
 48. TELLURIUM 1. Tellurides, heated in the open glass 
 
 tube, give a white or gray sublimate, fusible B. B. into color- 
 less, or nearly colorless, drops. On charcoal, they give a white 
 coating, and color the R. F. green-blue. 
 
 2. When a compound containing tellurium is triturated with 
 soda and charcoal dust and fused in a closed tube, then allowed 
 to cool, and a little hot water dropped into the tube, the water 
 assumes a beautiful purple color, owing to the dissolved tellur- 
 ide of sodium. 
 
 3. Tellurium compounds, when gently heated in a mattrass 
 with an excess of cone, sulphuric acid, impart to it a purple 
 
 * If this test for sulphur is made with any organic substance, as 
 pairings of nails, hair, albumen, etc., the carbonate of sodium should be 
 mixed with a little starch-powder, which appears to prevent the loss 
 of any of the sulphur by oxidation. On winding up a hair four inches 
 long, by coiling it around one point of a platinum support, moistening 
 it and dipping it into the mixture of carbonate of soda with starch, 
 and then heating by the blowpipe, the fused mass will give with the 
 nitro-prusside an unmistakable action indicative of sulphnr. By 
 careful management perfectly satisfactory results may be obtained 
 from a piece of hair less than an inch long. For theoretical deduc- 
 tions concerning nitro-ferricyanides or nitro-prussides, consult Qualitative 
 Chemical Analysis, by Professors Douglass and Prescott, 3d edition, 
 1880, pp. 187 and 196. 
 
192 MINERALOGY SIMPLIFIED. 
 
 color, which disappears on the addition of water, when a black- 
 ish-gray precipitate is formed. 
 
 Consult Bunsen's flame reactions, p. Ill et seq. 
 
 49. TIN In the metallic state, tin is recognized by its pecu- 
 liar physical properties. In nature it is found only as an oxide, 
 SnO (cassiterite). B. B. oxide of tin is slowly dissolved by 
 borax to a transparent glass, which is transparent on cool- 
 ing. With soda or cyanide of potassium on charcoal it is easily 
 reduced ; and if borax also be added, a very minute quantity of 
 tin may be detected when present in other minerals. 
 
 Sulphides containing tin must first be roasted, and the 
 roasted mass treated with a mixture of soda and borax in R. F., 
 the product is bright metallic tin, which can be further tested. 
 On Ch. in the O. F. it forms oxide, that " glows" strongly, 
 appears yellowish while hot, but becoming, on cooling, dirty yel- 
 lowish-white. Exposed to the R. F. the molten metal retains 
 it bright aspect. 
 
 Tin dissolves in cone. HC1 with evolution of hydrogen, forming 
 stannous chloride, SnCl 2 , corresponding to stannous oxide SnO ; 
 in cone, aqua regia.it is easily dissolved to stannic chloride, SnCl 4 ; 
 in cold nitric acid, or dilute aqua regia, without evolution of 
 gas, but with formation of ammonium salts, to stannous oxide or 
 stannous chloride, viz., Sn -f 4NO 3 H Sn(OH) 4 -{- 4NO 2 , or 
 Sn + 9HC1-+ NO 3 H = 4SnCl 2 + NH 4 C1 -f 3H 2 0. Cone, 
 sulphuric acid dissolves it with evolution of SO 2 , to stannous 
 sulphate, SO 4 8n. Of the stannous salts, the chloride, SnCl 2 , 
 is the most in use, soluble in water and HC1, absorbing oxygen 
 in the air, and separating oxide, or oxy-chloride. H 2 S pre- 
 cipitates, from neutral and acid solutions, brown stannous sul- 
 phide, SnS, scarcely soluble in ordinary (NH 4 ) 2 S, but more 
 readily soluble in yellow sulphide of ammonium. Alkaline 
 supersulphides, whereby ammonio stannic sulphide SnS 3 
 (NH 4 ) 2 is formed, from the solutions of which acids throw down 
 yellow stannic sulphide, viz : 
 
 1. SnS + (NH 4 ),S 2 = SnS 3 (NH 4 ) 2 . 
 
 2. SnS 3 (NH 4 ) 3 -f 2HC1 = SnS 2 + 2NH 4 C1 -f H 2 S. 
 
DETECTING CERTAIN ELEMENTS. 193 
 
 Stannous salts are oxidized to stannic salts by many oxidiz- 
 ing reagents. They are themselves powerful reducing agents. 
 
 Stannic oxide, or anhydride, forms two well-marked hydrates 
 or acids : stannic acid, H 2 SnO 3 , and metastannic acid, 
 H 10 Sn 5 O 15 (variable). Stannic acid is formed by precipitating 
 stannic salts with alkalies ; metastannic acid, by the action of 
 nitric acid on tin. Stannic acid is insoluble in water, but it 
 readily forms soluble stannic salts with HC1, H 2 SO 4 , and 
 HNO 3 ; and also soluble alkaline stannates with the alkaline 
 hydrates; other stannates being insoluble. Metastannic acid is 
 insoluble in acids, and does not form metastannates. 
 
 The stannic oxide, hydrate, sulphide, and phosphate are in- 
 soluble in water. 
 
 The alkaline hydrates, carbonates, and barium carbonate, 
 precipitate, from solutions of stannic salts, stannic acid, 
 H 2 SnO 3 , which is white, and soluble in an excess of fixed alka- 
 line hydrates and carbonates, but insoluble in ammonium hy- 
 drate and carbonate (distinctive from antimony), e. g., SnCl 4 -f- 
 4KOH H 2 SnO 3 + 4KC1 + H 2 O. 
 
 Copper and tin are separated by strong nitric acid until all 
 the metal is oxidized, the whole evaporated, to get rid of most 
 of the acid, hot water added, when all the stannic oxide (and a 
 trace of copper) can be filtered off; from the filtrate copper can 
 be thrown down with caustic potassa at a boiling heat as black 
 oxide. Should lead, zinc, and iron be present at the same 
 time, we proceed as follows : after the stannic oxide has been 
 removed, we separate the lead with sulphuric acid ; the copper 
 is precipitated from the acid solution by H 2 S ; zinc and iron 
 are separated by boiling with acetate of soda, or by adding an 
 excess of ammonia, when the iron is precipitated. From the 
 solution zinc is thrown down by (NH 4 ),S, or in the absence 
 of ammoniacal salts by carbonate of sodium at a boiling tem- 
 perature. 
 
 Tin from Bismuth To a strong HC1 solution of the two 
 metals, add an excess of water, when an insoluble white pre- 
 17 
 
194 MINERALOGY SIMPLIFIED. 
 
 cipitate of oxychloride of bismuth is produced. The tin will 
 remain in solution. 
 
 Tin from Antimony Advantage is taken of the solubility 
 of the sulphides of tin in oxalic acid. From the solution of 
 the two metals the sulphides are precipitated in the usual man- 
 ner, oxalic acid added in great excess, ^'. e., 20 grammes of the 
 reagent for every gramme of tin, so that the acid will crystal- 
 lize out in the cold. Then heat to boiling, and pass in H 2 S for 
 about twenty minutes. No precipitate appears at first ; but as 
 soon as the liquid is saturated with the gas the sulphide of an- 
 timony begins to fall, and, in a very few moments, is com- 
 pletely thrown down. 
 
 When a neutral solution of salts of tin acidulated with some 
 HC1 is brought in contact with metallic zinc, metallic tin is 
 thrown down in the form of scales, or as a gray spongy mass. 
 When this reaction is carried on upon platinum foil, no black 
 spot is produced, which is the case when a salt of antimony is 
 thus treated. 
 
 50. SEPARATION OF As, Sb, Sn The metals are precipi- 
 tated as sulphides from an acid solution and redissolved in 
 (NH 4 ) 2 S (to separate them from metals not precipitated from 
 acid solutions and not soluble in (NH 4 ) 2 S if present), then HC1 
 is added, when a yellow precipitate falls ; the mixture is slightly 
 heated, the sulphides filtered off and washed. The mixture of 
 sulphides is gradually and slightly heated with cone. HC1; the 
 yellow residue is sulphide of arsenic, the filtered solution con- 
 tains Sn and Sb. 
 
 The yellow As 2 S 3 * is dissolved in cone. HC1 with addition 
 of KC1O 3 , the solution saturated with NH 3 in excess, NH 4 C1 
 and MgSO 4 added; precipitate Mg(NHJAsO 4 . For further 
 confirmation the precipitate is filtered off, and, after washing, a 
 portion of it is dissolved in nitric acid, neutralized with ammo- 
 nia, and treated "with AgNO 3 , forming brownish-red Ag 3 AsO 4 , 
 which is soluble in ammonia and nitric acid. 
 
 * H 2 S precipitates the arsenic from an acid solution always as 
 As 2 S 3 ; but by the treatment with yellow (NH 4 ) 2 S it passes into 
 
 As 2 S 5 . 
 
DETECTING CERTAIN ELEMENTS. 195 
 
 51. TITANIUM Compounds of titanic acid treated with 
 
 S. Ph. B. B. dissolve in the O. F. to a clear bead, pale-yellow 
 when hot, and colorless when cold. The strong R. F. now 
 turns the bead yellow while hot, reddisli when cooling, and 
 violet when cold (titanous oxide). If iron is present, the cold 
 bead is brownish-yellow to brownish-red, and the violet color 
 only appears when the bead is acted upon with tin, in the R. F. 
 on charcoal. An excess of iron interferes with the reaction. 
 
 2. Ignition in the O. F. on charcoal with soda does not re- 
 duce titanic acid to the metallic state (distinction from tin). 
 
 3. If a substance containing titanium is fused with carbonate 
 of sodium, and the product obtained is dissolved in HC1, and 
 then heated with metallic tin or zinc, the titanic acid is reduced 
 to sesquioxide of titanium, coloring the liquid blue or violet, and 
 finally the violet hydrated sesquioxide separates as a powder, 
 retaining its color. 
 
 4. When the powdered mineral containing titanic acid is 
 fused with 6 to 8 parts of the bisulphate of potassium, and the 
 mass dissolved in very little water, then a few drops of water 
 added, and next 5 or 6 volumes more of water, and the mixture 
 is then boiled, a white precipitate results (titanic acid) which 
 may be further examined with salt of phosphorus, etc. 
 
 Native titanic acid (Rutile) is finely pulverized and fused 
 with 4 parts of its weight of alkaline carbonate. The mass, when 
 treated with water deposits crystalline acid, titanate of the alkali 
 remaining along with the iron. This should be digested with 
 cone. HC1, and the diluted solution boiled with sulphite of 
 sodium, when the titanic acid will be precipitated ; or we may 
 precipitate with sulphide of ammonium, and pour sulphurous 
 acid solution over the precipitated mixture, when the sulphide 
 of iron is dissolved out, and the titanic acid left as a white 
 powder. 
 
 52. TUNGSTEN ( Wolframium) This is found in the minerals 
 Wolframite (Fe,Mn)WO 4 ; in Scheelite, CaWO 4 ; Cuprotungs- 
 tite, Cu 2 WO 5 +aq; Stolzite PbWO 4 . B. B. the oxides of 
 tungsten impart to the bead of salt of phosphorus in the R. F. 
 
196 MINERALOGY SIMPLIFIED. 
 
 at first a dirty green, and then a blue color when cold (if iron 
 is present the bead appears blood-red). With tin the bead, in 
 the presence of iron, turns also blue or green. 
 
 The metal resembles iron, is brittle, and with difficulty 
 fusible. Treated with nitric acid, or aqua regia, it is converted 
 into anhydrous tungstic trioxide, WO 3 , which is a yellow pow- 
 der, insoluble in water and acids, but soluble in caustic alka- 
 lies ; when it is feebly heated (to 250 C.) and a current of hy- 
 drogen gas passed over it, it turns to blue oxide, i. e., tungstic 
 trioxide combined with tungstic dioxide, 2WO 3 -f WO 2 , at a 
 dull-red heat it forms brown tungstic dioxide, WO 2 . 
 
 When a tungstate is fused with carbonate of sodium, and 
 treated with hydrochloric acid and zinc, a beautifql blue color 
 is obtained (reduction to W 2 O 6 =WO 3 + WO 2 ). When a tungs- 
 tate is fused with bisulphate of potassium, and the fused mass, 
 consisting of tungstate of potassium, K 2 WO 4 , and free tungstic 
 acid, is treated with water, some of it is dissolved, especially in 
 the presence of carbonate of ammonium (distinction from silicic 
 acid). When a finely powdered tungstate is treated with cone, 
 hydrochloric acid, and a little nitric acid is added, yellow tung- 
 stic acid remains undissolved, but this is readily taken up by 
 ammonia, and this solution, mixed with hydrochloric acid and 
 zinc, assumes a blue color. 
 
 Tungstic acid and tungstates. Two modifications of tungstic 
 acid exist, termed normal and metatungstic acid; and the 
 tungstates may likewise be divided into two corresponding 
 classes, the ordinary or normal tungstates and the meta- 
 tungstates. 
 
 Tungstic acid, H 2 WO 4 . When a solution of a tungstate is 
 precipitated in the cold, a white precipitate is thrown down, 
 consisting of hydrated tungstic acid, H 2 WO 4 -f H 2 O. This is 
 soluble in water, has a bitter taste, and reddens blue litmus 
 paper. 
 
 Metatungstic acid, H 2 W 4 O 13 -f 7H 2 O. For this purpose the 
 barium salt is decomposed by dilute sulphuric acid, or the lead 
 salt with hydrosulphuric acid. The acid crystallizes in small 
 
DETECTING CERTAIN ELEMENTS. 197 
 
 yellow octohedrons. The salts are readily soluble in water. 
 When the solution is concentrated by boiling, a white hydrate 
 is deposited, and afterwards the trioxide separates. 
 
 With chlorine, tungsten forms four compounds, viz: 
 
 Tungsten dichloride, WC1 2 . 
 
 Tungsten tetrachloride, WC1 4 . 
 
 Tungsten pentachloride, WC1 6 . 
 
 Tungsten hexachloride, WC1 6 . 
 
 A characteristic reaction is the following : When a tung- 
 state is fused with carbonate of sodium, the mass dissolved in 
 HC1, and the solution boiled with metallic zinc, it becomes 
 intensely blue, but fades entirely on dilution with water. A 
 small amount of tungstic acid is detected thus : The assay is 
 fused with five parts of soda, the mass extracted with water, 
 and HC1 added, when the tungstic acid, insoluble in acid, falls 
 in the form of a white powder. The precipitate turns yellow 
 by boiling, is insoluble in an excess of acid (distinction from 
 molybdic acid), but soluble in ammonia. This solution, pre- 
 viously acidified, yields with ferrocyanide of potassium a deep- 
 brown solution, and after some time a precipitate of the same 
 color falls. With nitrate of silver it gives a white, with stan- 
 nous chloride (SnCl 2 ), a yellow precipitate, which appears fine 
 blue when the solution was previously acidulated wtih HC1. 
 (Laudauer.) 
 
 The mineral wolfram (tungstic acid, iron, and manganese), 
 the author found (confirming Dana's experience) to be suffici- 
 ently decomposable by boiling cone, sulphuric acid to give a 
 colorless solution, which, treated with metallic zinc, becomes 
 intensely blue, like Prussian blue, the color lasting several 
 hours. 
 
 53. URANIUM The reactions B. B. with borax and salt of 
 phosphorus lead to its detection. With salt of phosphorus it 
 dissolves to a clear yellow glass, turning to a greenish-yellow 
 when cold. In R. F. acted upon, this gJass assumes a dirty- 
 green color when hot, but a beautiful green when cold. 
 
 17* 
 
198 MINERALOGY SIMPLIFIED. 
 
 Treated upon charcoal with tin, tin's color becomes a darker 
 green. Uranium occurs chiefly in the minerals pitchblende and 
 uranite. It combines with oxygen in several proportions,* viz., 
 Uranium dioxide UrO 2 , and trioxide UrO 3 , and these combine 
 to form intermediate oxides, e. g., Ur 3 O 8 = UrO 2 + 2UrO 3 
 UrO 2 is basic, while UrO 3 is an acid-forming oxide. 
 
 Uranous dioxide, UrO 2 , is obtained by heating the uranos- 
 uranic oxide or uranic oxalate in a current of hydrogen. It 
 forms a brown or brick-red pyrophoric powder. When heated 
 in the air it takes fire and is converted into Ur 3 O g . It dis- 
 solves in strong acids, forming green uranous salts. Uranous 
 hydroxide is precipitated in reddish-brown flakes, which become 
 black on ebullition, by adding an alkali to a uranous solution. 
 It dissolves easily in dilute acids, while the calcined oxide is 
 soluble only with difficulty. 
 
 Uranium tetrachloride, or uranous chloride, UrCl 4 . It is 
 best prepared by passing chlorine over an intimate mixture of 
 charcoal and any of the oxides of uranium, strongly heated in 
 a tube of hard glass. It crystalizes in fine dark-green regular 
 octachedrons, volatilizing in red \apors. Dissolves in water, 
 forming an emerald-green solution. Caustic alkali throws 
 down uranous hydrate. 
 
 Uranic trioxide, UrO 3 or uranyl oxidef (UrO 2 )0. As an 
 anhydride it is brick-red ; as hydroxide, yellow. Reactions of 
 the trioxide salts dissolve in water with a yellow color. 
 
 Uranic sulphate, Ur0 2 SO 4 -f 3Aq, is obtained by heating 
 the nitrate with sulphuric acid. 
 
 Uranic nitrate, UrO 2 (NO 3 ) 2 -f- 6Aq, is prepared by dissolv- 
 ing any of the oxides in nitric acid. 
 
 * The atomic weight of uranium is, according to the recent investi- 
 gations of I). J. Mendelejeff, 240, while hitherto it was assumed to be 
 120, and, accordingly, the formulae of the oxygen compounds were 
 noted protoxide, UrO, sesquioxide Ur 2 O 3 , and the proto-sesquioxide, 
 UrA. 
 
 f Peligot regards UrO 2 as a compound radical. Uranyl, the tri- 
 oxide being the oxide of this radical, and the hydroxide has the 
 formula Ur0 2 (HO) r 
 
DETECTING CERTAIN ELEMENTS. 199 
 
 Hydrogen sulphide, in solutions acidulated with HC1, pro- 
 duces no precipitate ; sulphide of ammonium produces a dark- 
 brown one of oxy sulphide, UrO 2 S-f H 2 O somewhat soluble in 
 an excess, but quite insoluble in yellow sulphide of ammonium 
 (containing more S). 
 
 54. URANATES Uranyloxide not only forms the uranyl salts, 
 but also unites with basic metallic oxides to form the uranates. 
 Potassium uranate = K 2 Ur 2 O 7 . This orange powder is obtained 
 by precipitating an uranic salt with an excess of potash. 
 
 Ammonium uranate, (NH 4 ) 2 Ur 2 O 7 , a yellow precipitate, 
 obtained with NH 3 . Carbonate and bicarbonate of potassium 
 give a yellow precipitate of the double carbonate, UrO 3 K 4 (CO 3 ) 3 , 
 soluble in excess, and likewise soluble in carbonate of sodium 
 and carbonate of ammonium. Carbonate of barium precipitates 
 uranium salts completely in the cold. 
 
 For a process for the extraction of uranium from pitch- 
 blende, by Wohler, consult Roscoe and Schorlemmer, Treatise 
 on Chemistry, vol. ii. pt. ii. p. 218. 
 
 For reactions with borax see table, page 94. 
 
 55. VANADIUM. Vanadates, in the absence of other colored 
 metallic compounds, may be detected by their reactions with 
 borax and salt of phosphorus before B. B. 
 
 In the O. F. with S. Ph. the bead is soluble to a clear 
 glass which is dark yellow while hot, light yellow when cold. 
 This bead, when brought in the R. F., assumes a brownish 
 color when hot, and a beautiful chrome green color when cold. 
 Distinguished from chromium by its reaction in O. F. 
 
 Vanadium forms with oxygen a series of compounds, viz., 
 the. monoxide V 2 O, the dioxide V 2 O 2 , the trioxide V 2 O 3 , the 
 tetroxide V 2 O 4 , the pentoxide (vanadic acid) V 2 O 5 . Corres- 
 ponding with these a series of chlorides are known. The 
 most important compound, from an analytical point of view, is 
 vanadic acid. It forms a reddish-yellow powder, fusible at a 
 red heat, forming, when cold, a crystalline mass scarcely soluble 
 in water, but easily soluble in stronger acids and in 'alkalies. 
 
200 MINERALOGY SIMPLIFIED. 
 
 The vanadiates of the alkalies are all soluble in pure water, 
 but much less so in the presence of other alkaline salts. Vana- 
 diate of barium is insoluble ; hydro-sulphuric acid H 2 S, or sul- 
 phurous acid (SO 2 ), reduces an acidulated solution of V 2 O 5 to 
 dioxide (V 2 2 ), which latter remains dissolved with a blue 
 color. Sulphide of ammonium throws down a brown precipi- 
 tate, soluble in an excess with a brown color ; soluble in colorless 
 sulphide of ammonium or in sulphide of potassium with an 
 intense cherry-red color (the reaction is very characteristic, 
 but evanescent). Ferrocyanide of potassium produces a yellow 
 precipitate, which becomes green on exposure to the atmos- 
 phere. The acidulated solution of a vanadiate of alkali, when 
 shaken with ether containing hydrogen dioxide, H 2 O 2 , turns 
 red. V 2 O 5 , when heated in a current of hydrogen gas, is 
 reduced to V 2 O 3 . This same oxide is formed, as a soluble 
 salt, if a solution of the pentoxide in sulphuric acid is reduced 
 by metallic magnesium. The neutral solutions are brown, 
 the acid ones green. All the lower oxides of vanadium in an 
 acid solution are with permanganate of potassium oxidized to 
 vanadic acid, exhibiting with sulphide of ammonium the same 
 deportment as that acid itself. Compounds of vanadium can 
 be fused with soda and saltpetre in a platinum crucible. The 
 fused mass, when extracted with water and acidulated with 
 cone, acetic acid, forms, when filtered, upon addition of nitrate 
 of silver, a yellow precipitate. When the fusion is evaporated 
 with HC1, a yellow or brownish-yellow solution is obtained, 
 turning upon addition of protochloride of tin (stannous chlo- 
 ride) blue. 
 
 56. YTTRIUM Yttria, its oxide, is found in the minerals 
 gadolinite,* orthite, yttrotantalite, etc. B. B. the reactions 
 
 * Gadolinite contains, according to an analysis of Bahr and Bun- 
 sen (Anal. d. Chem. und Phys., Jan. 1866), silica 22.61, glucina 
 6.96, sesquioxide of iron 4.73, protoxide of iron 9.76, yttria 34.64, 
 erbia 2.93, protoxide of cerium (CeO) 2.86, oxide of didymium (DiO) 
 8.38, lanthanoxide (LaO) 3.21, magnesia 0.15, lime 0.83, soda 0.38, 
 water 1.93 = 99.37. 
 
DETECTING CERTAIN ELEMENTS. 201 
 
 of yttria (YO) are identical with those of the oxide of gluci- 
 num, or BeO (oxide of berryllium). From its salts caustic 
 potash, ammonia, and sulphide of ammonium precipitate white 
 hydrated oxide Y(HO) 3 not soluble in excess. Sal-ammoniac 
 prevents the reaction. YO is a strong base, decomposes salts 
 of ammonia, and attracts greedily carbonic acid from the atmo- 
 sphere. Carbonate of baryta does not precipitate it. 
 
 Analysis of the gadolinite (silicate of Y, Be, Fe, Mn, Ce, La). 
 After the removal of the silica, oxalate of ammonium removes 
 from the neutral solution, in the presence of ammonia and 
 sal-ammoniac, the insoluble oxalate salts of Y, Ce, La, while 
 Be, Fe, Mn remain in solution as oxalates. The separation of 
 Y from Ce and La is executed with cone, neutral sulphate of 
 potassium solution. The double sulphate, K 3 Ce(SO 4 ) 3 is but 
 slightly soluble in water, and quite insoluble in sulphate of po- 
 tassium solution, and the same is the case with the double sul- 
 phate, K 8 La 2 (SO 4 ) 7 . Hence these are precipitated, while from 
 the solution the yttrium oxide, YO, is thrown down by ammonia 
 and is determined as such. 
 
 57. ZINC -Oxide of zinc with borax gives a clear glass, 
 
 which is milk-white on flaming; or, with more assay, is enamel- 
 white on cooling. In the inner flame, on charcoal, fumes are 
 given off and a white coating surrounds the assay. With soda 
 on charcoal the ores, even when containing little zinc, afford 
 the peculiar bluish flame of burning zinc, and white oxide is 
 deposited on the coal. With cobalt solution a green color, 
 while tin gives a bluish-green. 
 
 From solutions of zinc all the alkali hydrates, including am- 
 monia, precipitate white hydrate of zinc, Zn(OH) 3 soluble in 
 an excess. 
 
 Hydrosulphuric acid precipitates a part of the zinc from 
 neutral solution of its salts with mineral acids, and the whole 
 from the acetate ('. <?., sulphide of zinc is not soluble in acetic 
 acid). Alkali sulphides as sulphide of ammonium (NH 4 ) 2 S 
 throw down all the zinc as sulphide, both from its salts with 
 acids, and from its soluble combinations with alkalies. Pure 
 sulphide of zinc is white. 
 
202 MINERALOGY SIMPLIFIED. 
 
 58. ZIRCONIA occurs in nature in the zircons or jargons. 
 B. B. infusible, when strongly heated a very brilliant light is 
 given out. 
 
 It forms only one compound with oxygen, viz., ZrO 2 , which 
 yields salts with acids, the sulphate is with difficulty soluble ; 
 the chloride, ZrCl 4 , is volatile. Fluoride of zirconium is solu- 
 ble in water (distinctive from thorium) and yields with fluoride 
 of potassium a double salt, K 2 ZrFl 6 , with difficulty soluble in 
 water. ZrO 2 , fused with soda, liberates CO 2 , forming a scarcely 
 soluble sodium compound, the composition of which differs. 
 The simplest Na 4 ZrO 4 is produced by the action of an excess 
 of soda. 
 
 Reactions of zirconium salts : 
 
 Caustic alkalies, ammonia, and sulphide of ammonium, throw 
 down hydroxide, Zr(OH) 4 , not soluble in an excess of caustic 
 alkalies and in sal-ammoniac (distinction from alumina and 
 glucina), but soluble in carbonate of ammonium. Zr(OH) 4 ob- 
 tained in the cold is easily soluble in acids, that produced at a 
 higher temperature, or the ignited oxide, is with difficulty 
 soluble (requiring two parts of cone, sulphuric acid to one of 
 water). 
 
 The carbonate of zirconium is soluble in carbonate of ammo- 
 nium, separating again by boiling. Neutral sulphate of potas- 
 sium precipitates white K 4 Zr(SO 4 ) 4 , insoluble in an excess, 
 but soluble in cold HOI (difference from Th, Ce). The pre- 
 cipitated salt furnished at a higher temperature is insoluble in 
 HC1. 
 
 Oxalic acid yields an oxalate insoluble in an excess but 
 soluble in HC1 and in oxalate of ammonium (difference from 
 thorium). Analysis of zircon: SiO 4 Zr, is fused with soda. 
 The mass is treated with water, which dissolves silicate of sodium, 
 and leaves behind a crystalline powder of zirconia-sodium, 
 which, after washing with more water, is dissolved in HC1, 
 from which solution NH 3 throws down Zr(OH) 4 . From oxide 
 of iron, zirconia is separated with oxalic acid or sulphite of 
 sodium. 
 
FUSION AND FLUXING. 203 
 
 CHAPTER VIII. 
 
 FUSION AND FLUXING. 
 
 THE term "fusion" is applied to the conversion of a solid 
 substance into the fluid form by the application of heat ; fusion 
 is most frequently resorted to for the purpose of effecting the 
 combination or the decomposition of bodies. The term " flux- 
 ing" is applied to the process in cases where substances insolu- 
 ble, or difficult of solution, in water and acids, are, by fusion, 
 in conjunction with some other body, modified or decomposed 
 in such a manner that the new-formed compounds will subse- 
 quently dissolve in water or acids. Fusion and fluxing are 
 conducted either in porcelain, silver, or platinum crucibles, 
 according to the nature of the compound. The crucible is sup- 
 ported on a triangle of medium stout platinum-wire, resting on 
 the ring of a blast lamp. (See Fig. 46, p. 53.) 
 
 Resort to fluxing is especially required for the analysis of 
 the sulphates of the alkaline earths, and also for that of many 
 silicates. The flux most commonly used is carbonate of sodium 
 or carbonate of potassium, or, better still, a mixture of both in 
 equal atomic proportions, i. e., 13 parts of pure carbonate of 
 sodium are mixed with 10 parts of pure anhydrous carbonate 
 of sodium.* 
 
 Silicates are fused with about 4 to 5 parts of the alkaline 
 mixture mentioned, or, still better, with carbonate of sodium 
 alone, provided the operation is carried on with Bunsen's 
 blast lamp, or a wind furnace. A basic alkaline silicate is 
 formed, which, being soluble in water, may be readily separated 
 from such metallic oxides as it may contain in admixture. 
 
 * The mixture is kept in a well-stoppered bottle. 
 
204 MINERALOGY SIMPLIFIED. 
 
 From this basic alkaline silicate, hydrochloric acid separates the 
 silicic acid as hydrate. If a fixed alkaline carbonate is fused 
 together with sulphate of barium, strontium, or calcium, there 
 are formed carbonates of the alkaline earths and sulphates of 
 the alkalies. In the new compounds both the base and the 
 acid of the originally insoluble salt may now be readily 
 detected. However, we do not employ carbonate of potassium 
 separately, nor carbonate of sodium, to effect the decomposition 
 of the insoluble silicates and sulphates ; but we employ for this 
 purpose the above described mixture of both, because this 
 mixture requires a far lower degree of heat than either of its 
 components alone, and hence the operation may be conducted 
 over an alcohol lamp with an argand burner, or a Bunsen 
 gas burner. The fusion with alkaline carbonates is always 
 effected in a platinum crucible provided no reducible metallic 
 oxides be present, which would ruin'it. 
 
 In cases where alkalies are present in the mineral submitted 
 to analysis, we employ hydrate of baryta* for its fusion. Upon 
 fusing silicates together with about four parts of hydrate of 
 baryta, a basic silicate of barium is formed, and the oxides are 
 liberated. If the fused mass is treated with hydrochloric acid, 
 the solution evaporated to dryness, and the residue digested 
 with hydrochloric acid, the silicic acid is left behind, and the 
 oxides are obtained in solution in the form of chlorides. Hy- 
 drate of baryta is preferable as a flux to test silicates for alka- 
 lies, to carbonate or nitrate of barium, since it does not re- 
 quire a very high temperature for its fusion, nor does it cause 
 any spurting in the fusing mass from the disengagement of gas, 
 as in the case with the nitrate. The operation is conducted in 
 a silver or platinum crucible. The mineral subjected to fusion 
 must in every case be very finely pulverized in an agate mortar 
 and sifted through the finest hair sieve. 
 
 * Hydrate of baryta fuses at a gentle red heat without losing its 
 water. 
 
FUSION AND FLUXING. 205 
 
 DEFLAGRATION. 
 
 In a very general sense " deflagration" signifies a process 
 of chemical decomposition attended with a detonation or explo- 
 sion. It is here used in a more restricted sense to designate 
 the deoxidation of a substance in the dry way at the expense of 
 the oxygen of another substance mixed with it, usually a ni- 
 trate or a chlorate, viz., saltpetre, potassium chlorate. Con- 
 nected with this process is a sudden or violent combustion, 
 attended with a very lively incandescence. Deflagration is 
 resorted to, either to produce the desired oxide e. g., ter- 
 snlphide of arsenic is deflagrated with nitrate of potassium to 
 obtain arsenate of potassium-*-or it is applied as a means to 
 prove the presence or absence of a certain substance. Thus salts 
 are tested for nitric or chloric acids by fusing them with cyanide 
 of potassium, and observing whether this process will cause 
 deflagration* or not. 
 
 To attain the former object, the perfectly dry mixture of the 
 substance under investigation, and of the deflagrating agent is 
 projected in small proportions into a red-hot porcelain crucible 
 With very small quantities the process is best conducted on 
 piece of platinum foil, or on a small platinum spoon. 
 
 ON THE USE AND PRESERVATION OF PLATINUM VESSELS. 
 
 Platinum apparatus being very expensive, should be handled 
 with great care and kept polished, i. e., by gently rubbing 
 witli moist sea-sand (the rounded grains of which do not 
 scratch the metal) ; by fusing borax upon the coated surface, 
 or by digestion with nitric acid, and lastly polishing again with 
 sea-sand. 
 
 1. Platinum is not attacked at any temperature by nitric, 
 
 * B. B. deflagrations of minute quantities, viz., common and Chili 
 saltpetre, chlorate of potassium, are executed on charcoal. If we place 
 upon the fused mass a moistened red litmus paper it turns blue (al- 
 kaline carbonates), and a drop of 11C1 causes effervescence (CO 2 ). 
 18 
 
206 MINERALOGY SIMPLIFIED. 
 
 hydrochloric, or sulphuric acid, but dissolves in nitro-hydro- 
 chloric acid, though less readily than gold. 
 
 2. Free chlorine and bromine attack platinum at an ordinary 
 temperature ; also free sulphur, phosphorus, arsenic, selenium, 
 and iodine attack ignited platinum. Hence the fusion of sul- 
 phides, sulphates, and phosphates with reducing agents (car- 
 bon, etc.) is injurious or fatal to platinum vessels. The igni- 
 tion of organic material containing phosphates acts in a slight 
 degree as free phosphorus. 
 
 3. The heating of ferric chloride, and the fusion of bromides, 
 and iodides affect platinum to some extent. 
 
 4. The alkali hydrates* (not their carbonates) and the alka- 
 line earths, especially baryta and lithia when ignited with plati- 
 num in the air, gradually corrode platinum vessels. The 
 nitrates of the alkalies or alkaline earths are also detrimental. 
 
 5. All metals which may be reduced by fusion, especially 
 salts of bismuth, lead, tin, and all metallic compounds mixed 
 with reducing agents (cyanide of potassium, etc.), including 
 the alkalies and earths, form fusible alloys at a high tempera- 
 ture with platinum. Oxides of mercury, lead, bismuth, tin, 
 antimony, zinc, copper, nickel, are, at a white heat, rapidly 
 reduced, unite with the platinum, and corrode it. 
 
 6. Silica with charcoal slowly corrodes ignited platinum. 
 Hence platinum crucibles should not be supported on charcoal 
 in the furnace, but packed in magnesia in an outer crucible of 
 clay. 
 
 Cracks and holes in platinum crucibles may be repaired with 
 gold solder, but such vessels cannot afterwards be exposed to a 
 high heat. 
 
 * Caustic alkalies must be fused, or evaporated in silver crucibles. 
 These can only be used at temperatures below full redness, and must 
 not come in contact with sulphur or be heated over coke, coal, or gas, 
 or other fuel containing sulphur. 
 
PART II. 
 
 DETERMINATIVE MINERALOGY. 
 
 CHAPTER IX. 
 
 ON THE DETERMINATION OF MINERALS BY MEANS OF SIM- 
 PLE EXPERIMENTS WITH THE BLOWPIPE, AIDED BY 
 HUMID ANALYSIS. 
 
 A FREE translation from the twelfth edition of Professor 
 Franz von Kobell's "Tafeln zur Bestimmung der Miner- 
 alien."* 
 
 INTRODUCTION TO THE TABLES. 
 
 The following tables are intended to assist in the discovery 
 and facilitate the determination of minerals by the most plain 
 and reliable methods of examination. They are based upon a 
 few simple experiments with the blowpipe or with chemicals 
 in the wet way, i. e., the substance, if not already fluid, is first 
 brought into the liquid state and is then operated upon by 
 chemical reagents in the form of a solution. These experi- 
 ments soon lead to a group containing a few species, among 
 which is the mineral sought its name and usual composition. 
 The species under examination can generally be distinguished 
 from others in the same group by some of its chemical charac- 
 ters. In any case where uncertainty or doubt might arise on 
 
 * Before the last edition was fully prepared for printing, the cele- 
 brated author von Kobell died (Nov. 11, 1882) ; hence this twelfth, 
 improved, and augmented edition has been issued by K. Oebbeke, 
 Miinchen, 1884. .1. Lindauer's Buchhandlung. 
 
208 MINERALOGY SIMPLIFIED. 
 
 account of similarity in the chemical reactions of two species, 
 we may be convinced of the correctness of our determination 
 by referring to any work on mineralogy, and comparing the 
 physical properties of the species. The correctness and advan- 
 tage of this method of determining, minerals have been suffi- 
 ciently demonstrated by practical exercises carefully conducted 
 for many years. 
 
 In order to perform successfully all the manipulations here 
 required, it is only necessary to be acquainted with the use of 
 the blowpipe, and also with the manner of making some simple 
 solutions and precipitations. 
 
 It is expected that these pages will be especially useful to 
 those who have neither time nor the inclination to devote 
 themselves to the study of larger works on mineralogy, but to 
 whom the determination of some few minerals is often a matter 
 of interest. For that reason it may be acceptable to the chem- 
 ist, the miner, the farmer, and the mechanic. 
 
 When an individual wishes to determine any mineral, the 
 arrangemenf is such that he will be constantly directed by the 
 divisions to the tests which he must make. After noting the 
 
 "Lustre of the Mineral" 
 
 there is generally required a single fusion of the sample, 
 either alone or with soda; then one trial by solution, and a 
 few precipitations, when the object sought is attained. Any 
 one who will follow the directions here given, and execute the 
 tests with accuracy, will soon become acquainted with many 
 reactions, and by a short practice he may acquire the abil- 
 ity to determine minerals with facility and certainty. Where 
 errors would be most likely to occur in the examination, 
 they are avoided by the arrangement of the divisions, ?'. <?., 
 some minerals have both a metallic and non-metallic lustre ; 
 some fuse under- or above 5, according to the skill of the 
 operator. As these minerals might appear of doubtful limit, 
 they are mentioned in both divisions. 
 
PHYSICAL PROPERTIES OF MINERALS. 209 
 
 PHYSICAL PROPERTIES OF MINERALS. 
 
 I. LUSTRE. In the group of minerals with metallic lustre 
 are placed only those which are perfectly opaque. A thin 
 splinter held between the eye and the light must show no 
 tmnslucency when it is considered as having metallic lustre; 
 otherwise as without it. 
 
 II. FUSIBILITY. 
 
 The following is the scale of fusibility : 
 
 1. Stibnite (antimony glance). 
 
 2. Natrolite. 
 
 These in coarse or fine splinters fuse in the mantle of a can- 
 dle flume (without the blowpipe). 
 
 3. Almandite. Alumina-iron garnet, does not fuse in a can- 
 dle flame like the preceding; but B.B. easily, even in some- 
 what larger pieces. 
 
 4. Actinolite. B. B., fusible in rather fine splinters. 
 
 5. Orthoclase. B. B., fusible in finer splinters. 
 
 6. Bronzite. (B. B. becomes rounded only on the finest 
 points and the sharpest edges.) Splinters or fragments of 
 these minerals are kept on hand, and their fusibility compared 
 with that of samples similar to them in size and edges. 
 
 Trials of fusibility should be made in the forceps, and mine- 
 rals difficult of fusion should be employed in thin splinters since 
 these might fuse on the edges, while an obtuse piece might 
 lead to the conclusion that the mineral is infusible. Nor 
 should the sample be regarded as infusible until it has been 
 heated just beyond the extremity of the blue flame where the 
 heat is most intense. 
 
 Minerals which decrepitate strongly (like common salt) are 
 finely pulverized, moistened with water and placed on charcoal ; 
 by heating the particles become sintered (if the sample be fusi- 
 ble), so that the mass may be taken in the forceps and further 
 heated in the flame. 
 
 18* 
 
210 MINERALOGY SIMPLIFIED. 
 
 III. HARDNESS. For the scale of hardness that of Mohs is 
 adopted, which is as follows, viz : 
 
 1. Talc, common foliated, light-green variety. 
 
 2. Gypsum, the crystallized variety (or rock-salt, Dana). 
 
 3. Calcite (calc-spar), transparent variety. 
 
 4. Fluor-spar, crystallized variety. 
 
 5. Apatite, transparent variety. 
 5.5. Scapolite, crystalline variety. 
 
 6. Orthoclase, white, cleavable variety. 
 
 7. Quartz, transparent variety. 
 
 8. Topaz, transparent crystal. 
 
 9. Corundum (sapphire), cleavable variety. 
 10. Diamond. 
 
 Trials of hardness are made by taking individuals of the 
 scale and attempting to scratch the mineral under examination, 
 or by using a file on similar edges of each ; both methods may 
 be employed. A few trials will give sufficient experience in 
 the use of this scale. 
 
 Sharp corners must be used in scratching, and particular 
 care should be taken in this, as in all other cases, that impuri- 
 ties do not come in to modify the result ; thus a grain of quartz 
 in some of the impure varieties of Galena, if it happened to 
 come upon the corner which is used, would make the mineral 
 appear quite hard, and without proper precautions many such 
 errors may occur. 
 
 IV. COLOR. Great care must be taken in forming any con- 
 clusions from the color of minerals. In minerals of metallic 
 lustre the color is generally constant and often very charac- 
 teristic in some of the non-metallic species the same is true, but 
 experience will teach how greatly the colors of non-metallic 
 minerals vary, and varieties are constantly found differing in 
 color from all that were previously known. Hence, especially 
 in non-metallic minerals, the color which is given should only 
 be regarded as an aid, or unimportant suggestion in the deter- 
 mination. 
 
SPECIFIC GRAVITY. 
 
 211 
 
 V. STREAK. The streak of a mineral is the color of the 
 powder obtained by scratching it with a knife or file, or bet- 
 ter, if not too hard, by drawing it across a piece of unglazed 
 porcelain. 
 
 SPECIFIC GRAVITY. 
 
 Determination of the specific gravity by an ordinary good 
 balance and weights. The specific gravity of a mineral is its 
 weight compared with that of an equal volume of water, which 
 is taken as a unit of comparison. 
 
 The direct comparison by weight of a certain volume of 
 water with an equal volume of a given solid is not often prac- 
 ticable. By making use, however, of a familiar principle in 
 
 Fig. 118.* 
 
 hydrostatics, viz., that the weight lost by a solid, immersed in 
 water, is equal to the weight of an equal volume of water, that 
 is, the volume of water it displaces the determination of the 
 specific gravity becomes a very simple process. 
 
 * Mohr's hydrostatic balance for determining the specific gravity of 
 liquids and solid objects. 
 
212 MINERALOGY SIMPLIFIED. 
 
 The weight of the mineral in the air (w) is determined by 
 weighing with the balance in the usual'manner, then the weight 
 in water is found (w r ), when the loss by immersion, or the dif- 
 ference of the two weights (w w') is the weight of a volume 
 of water equal to that of the mineral. Finally, the quotient 
 found by dividing the first weight (10) by that of the equal vol- 
 ume of water as determined (w w'}, gives the specific gravity 
 
 (G.) That is to say: G. = w ,. 
 
 w w' 
 
 For example, the weight of a fragment of quartz is found to 
 be 4.534 grammes. Its weight in water = 2.817 grammes, and 
 therefore the loss of weight, or the weight of an equal 
 volume of water = 1.717. Consequently the specific gravity 
 
 4534 
 
 = i?ni or 2 - 64L 
 
 The mineral is first accurately weighed on a good balance, 
 then suspended from one pan of the balance by a horse-hair, 
 silk thread, or, better still, by the finest possible platinum wire, 
 in a glass of distilled water conveniently placed beneath. The 
 platinum wire may be wound around the specimen, or, where 
 the latter is small, it may be made at one end into a little spiral 
 support. AVhile thus suspended, the weight is again taken with 
 the same care as before. Since the 
 Fig. 119. density of water varies with its tem- 
 
 perature, a standard temperature must 
 be selected for these experiments, in 
 order to obtain uniform results : 60 
 F. (15 C.) has been generally 
 adopted. 
 
 If the mineral is not solid, but pul- 
 verulent or porous, it is best to reduce 
 it to a powder and weigh it in a little 
 
 glass bottle, shown above (Fig. 110).* This bottle has a 
 stopper which fits tightly, and the neck of which is drawn out 
 
 * These glass bottles are capable of holding exactly a thousand 
 grains, or two hundred grains, or any known weight, of distilled 
 
 water. 
 
SPECIFIC GRAVITY. 213 
 
 to a fine tube, with a very fine opening. The bottle is filled 
 with distilled water, the stopper inserted, and the overflowing 
 water carefully removed with a soft cloth. It is now weighed, 
 and also the mineral whose density is to be determined. The 
 stopper is then removed,' and the mineral in powder form or in 
 small fragments inserted with care, so as not to introduce air- 
 bubbles. The water which overflows on replacing the stopper 
 is the amount of water displaced by the mineral. The weight 
 of the bottle with the inclosed mineral is determined, and the 
 w r eight of the water lost is obviously the difference between 
 this last weight and that of the filled bottle and the mineral 
 together, as first determined. The specific gravity of the min- 
 eral is equal to its weight in air, divided by the weight of the 
 equal volume of water thus determined. 
 
 Where this method is followed with sufficient care, especially 
 avoiding any change of temperature in the water, the results 
 are quite accurate. 
 
 If a mineral is soluble in water, it is weighed in a liquid in 
 which it is insoluble, and of which the specific gravity is known. 
 The specific gravity is then readily calculated. 
 
 Example 1 50 parts of rock-salt (w), when weighed in 
 spirits of turpentine, displace an amount the weight of which 
 is equal to 19.53 parts. The specific gravity of spirits of tur- 
 pentine is to that of water as 0.872 : 1 ; hence, we find that 
 
 0.872 : 1 = 19.53 : w w', and hence ww f = 1M? = 22.396, 
 
 0.872 
 ?'. <?., the weight of an equal volume of water. 
 
 Since G = ,= 5 =2.232, the latter number, 
 ww' 22.396 
 
 2.23, expresses the specific gravity of rock-salt. 
 
 Example 2 A substance soluble in water was weighed in 
 oil, and its specific gravity, compared with the oil, was 2.6, the 
 specific gravity of the oil was 0.87: then 2.6x0.87 = 2.262, 
 the specific gravity of the substance. 
 
 The specific gravity of a substance lighter than water, for 
 instance that of elmwood, is found as follows : 
 
214 MINERALOGY SIMPLIFIED. 
 
 The elmwood by itself weighs in the air = . .2 oz. 
 The wood is attached to a piece of lead which 
 
 weighs = . . . . . . 4 oz. 
 
 Total weight of both in air= .... 
 In water both together weigh = . 
 
 Loss of both united = 2.85 oz. 
 
 The lead alone weighs in the air = . . . 4.00 oz. 
 When submerged in water = .... 3.65 oz. 
 
 Loss of the lead alone in water . . . 0.35 oz. 
 
 By substracting from the loss of both solids in 
 
 water = ....... 2.85 oz. 
 
 The loss of lead alone in water = . 0.35 oz. 
 
 We obtain hence for the loss of the wood = . 2.50 oz. 
 
 Hence the specific gravity of elmwood is =. 0.8. 
 
 Since : 2 ' QQ ( absolute wei S llt in air ) = .8 (f. e., 
 
 2.50 (weight of an equal bulk of water) 
 
 the spec. grav. of the wood mentioned). 
 
 The specific gravity of minerals is most easily taken by means 
 of Prof. Jolly's spring-balance.* (Fig. 120). A wire wound in a 
 spiral form is suspended at , and has attached at its lower end, 
 &, two pans c and d. The pan, c?, dips into water. The vessel 
 containing the water in which the pan is suspended is placed 
 upon a shelf, which may be moved up or down on the 
 standard of the balance. A mark at m shows the extension of 
 the spiral on the mirror scale, which is also attached to the 
 standard. In reading, the mark is made to cover the reflection 
 on the mirror. 
 
 If weights increasing a tenth of a gramme are added succes- 
 
 * This spring-balance (Federwage) is furnished by Mechaniker 
 Berberich, in Miinchen, for 27 marks, about $6.75. 
 
SPECIFIC GRAVITY. 
 
 215 
 
 sively to the pan in the air, it is found that the extension of 
 
 the wire is in proportion to the weight added. Conically wound 
 
 wire, with its greatest diameter at a, and 
 
 its smallest at ft, shows precisely the rela- ^' * 2( ^ 
 
 tion between the size of the load and the 
 
 extension of the spiral. 
 
 The manner of using the balance is ex- 
 tremely simple. Before the substance is 
 placed on the pan, the place of the mark 
 is observed on the scale. A known weight 
 is then placed on the upper pan, and the ( 
 
 shelf, B, moved down as far as neces- 
 sary ; so far, that with the consequent ex- 
 tension of the spiral, the pan, c?, will again 
 sink into the water, when a second reading 
 is made. The difference in these figures 
 gives -the number of divisions on the scale 
 over which the spiral has been made to 
 pass by the weight. If it is found, for 
 example, that with a weight of 1 gramme 
 the extension of the spiral is 122.2 divi- 
 sions, while with some substance, as a 
 piece of mineral, the extension is only 
 54.4, the absolute weight of the substance 
 
 If, however, the 
 
 will be _5M = 0.445. 
 
 122.2 
 
 absolute weight is not required, only the 
 specific, it is not necessary to express the ab- 
 solute weight in grammes. Three readings 
 are made: first, with empty pan; second, 
 with substance placed on the upper pan ; and 
 the third, after placing the same substance 
 on the pan under water. The difference 
 between the first two gives the absolute 
 weight expressed in divisions of the scale, and the. difference 
 in the last two gives the weight of the displaced water. The 
 
216 MINERALOGY SIMPLIFIED. 
 
 quotient of these differences is, therefore, the specific weight. 
 If the mark with the empty pans stands at 64.2, and with the 
 substance placed in the upper pan at 275.3, and with the same 
 substance in the lower pan at 220.8, then the absolute weight 
 is 275.3 64.2 = 211.1, and loss of weight in water is 275.3 
 
 9111 
 
 220.8 = 54.5. Specific weight will be 1^ = 3.85. The 
 
 54.5 
 
 second decimal is not always certain, but, by proper arrange- 
 ment of the spiral, is found as reliable as the ordinary balance. 
 If the specific weight of a fluid is to be determined, both pans 
 are taken off, and in place of them a glass of about 1 c.c. in 
 size is suspended by a fine platinum wire. The loss of weight 
 in water and other liquids is shown by the scale as in the former 
 case. As is shown in the drawing, the shelf, B, is attached to 
 the standard, A. The movable standard, C, has the same 
 length as A ; can be raised or lowered, and made fast at any 
 point. C is drawn out according to the length of the spiral, so 
 far that the mark with the pans empty stands opposite one of 
 the upper divisions of the scale, which, to show the whole ex- 
 tension of the spiral, must be at least 600 mm. long. Every 
 spiral at first shows a little elasticity, which grows less, and 
 which, during any one experiment, amounts to really nothing. 
 
 PYRO-ELECTRICITY. 
 
 Electricity is developed in some minerals by heat, whereby 
 some light substances are attracted, such as deer's hair or fibres 
 of wool and cotton. 
 
 In determining whether a crystal be positively or negatively 
 electric, mistakes may easily happen, which may, however, be 
 avoided, according to von Kobell, by employing "chamois 
 beard" hair electroscope (. e., the long hair, hanging down the 
 back of a four year old chamois, is called its " beard.") These 
 hairs, when rubbed from the root toward the end point, become 
 strongly positive electric; on the contrary, rubbed from the 
 point toward the root they become negative electric, though 
 less so. 
 
CRYSTALLIZATION. 217 
 
 OPTICAL INVESTIGATION OF MINERALS. 
 
 When a mineral is transparent, a Nicol prism, and von Ko- 
 belFs Stauroscope* will be useful in determining the optical 
 properties of minerals. 
 
 Altered reactions of impure minerals. It is scarcely necessary 
 to remark that the reactions usually mentioned relate only to 
 pure or homogeneous specimens. When a mineral is presumed 
 to be impure we must take into consideration its adulterations 
 and judge of the reactions accordingly. Some varieties of 
 wollastonite, for example, effervesce with acids, and also react 
 alkaline after fusion ; neither of which reactions belongs prop- 
 erly to this material, but is caused by an admixture of calcite 
 or other carbonate. 
 
 CRYSTALLIZATION. 
 
 Crytallization,t if distinct, will often aid very materially in 
 determining the identity of a mineral. 
 
 The forms of crystals are exceedingly various, while the sys- 
 tems of crystallization based on their mathematical distinctions 
 are only six in number. 
 
 * See von Kobell's Mineralogie, 5te Auttage, Leipzig, 1878, page 65, 
 " Stauroscope ;" also, The Study of Rocks, by Frank Rutley, F.G.S., 
 London ;. Longmans, Green & Co., 1879, page 81, giving a description 
 of the instrument devised by vou Kobeli, and an improvement made 
 by Brezina. 
 
 f For the study of Crystallography and the Physical Characters of 
 Minerals, E. S. Dana's "Text-book of Mineralogy" is recommended, 
 3d ed., New York, 1880. 
 
218 
 
 MINERALOGY SIMPLIFIED. 
 
 SYSTEMS OF CRYSTALLIZATION. 
 
 Js T o. Some typical simple forms. 
 
 Cube and octahedron. 
 
 Right prism with square base. 
 
 Right prism with rectangular 
 or rhombic base. 
 
 Right rhomboidal and oblique 
 rhombic prisms. 
 
 Oblique disymetric rhomboidal 
 prism. 
 
 Rhombohedron and hexagonal 
 prism. 
 
 Axes. 
 
 3 axes, rectangular and equal. 
 3 axes, rectangular, 2 equal. 
 3 axes, rectangular and unequal. 
 
 3 axes, unequal, 2 rectangular. 
 
 3 axes, unequal, and unequally 
 inclined. 
 
 4 axes, 3 equal and equally in- 
 clined, 1, unequal at right 
 angles to the other three. 
 
 NAMES USED BY DIFFERENT AUTHORS. 
 
 No. 
 1 
 
 Nanmann. 
 
 Mohs. 
 
 Weiss & Rose 
 
 Phillips. 
 
 Delafosse. 
 
 Dana. 
 
 Tesseral. 
 
 Tessular. 
 
 Regular. 
 
 Cubic. 
 
 Cubic. 
 
 Isometric. 
 
 2 
 
 Tetrago- 
 nal. 
 
 Pyramidal. 
 
 2 and 1 
 axial. 
 
 Pyram 
 idal. 
 
 Tetrago- 
 nal. 
 
 Dimetric, 
 or Tetra- 
 
 
 
 
 
 
 
 gonal. 
 
 3 
 
 Rhom- 
 bic. 
 
 Orthotype. 
 
 1 and 1 
 axial. 
 
 Prisma- 
 tic. 
 
 Ortho- 
 rhombic. 
 
 Trimetric, 
 or Ortho- 
 
 
 
 
 
 
 
 rhombic. 
 
 4 
 
 Monocli- 
 nohedric 
 
 Hemior- 
 thotype. 
 
 2 and 1 
 membered. 
 
 Oblique 
 
 Clino- 
 rhombic. 
 
 Mono- 
 clinic. 
 
 5 
 
 Triclino- 
 hedric. 
 
 An ortho- 
 type. 
 
 1 and 1 
 membered. 
 
 Anor- 
 thic. 
 
 Clino- 
 hedric. 
 
 Triclinic. 
 
 6 
 
 Hexago- 
 nal. 
 
 Rhombohe- 
 dral. 
 
 3 and 1 
 
 axial. 
 
 Rhombo- 
 hedral. 
 
 Hexago- 
 nal. 
 
 Hexago- 
 nal. 
 
CHEMICAL PROPERTIES OF MINERALS. 219 
 
 CHEMICAL PROPERTIES OF MINERALS. 
 
 Preliminary proceedings for testing and properly classify- 
 ing them. In commencing examinations for ascertaining the 
 species and name of a mineral, it is always important to begin 
 with the first group, and pass on to those following, since a 
 mineral which is contained in a former group may also possess 
 the character of a succeeding group, but never the reverse. 
 
 For convenience of those making examinations, a SYNOPSIS 
 OF THE DIVISIONS AND GROUPS is PREFIXED. Instead of fur- 
 ther explanation, two examples will sufficiently illustrate the 
 method of determination. 
 
 1. EXAMPLE. Suppose we have a specimen of " ALUMI- 
 NITE" before us and are unacquainted with the mineral. It 
 has no metallic lustre, and therefore belongs to the Division 
 II., viz: Minerals without metallic lustre. 
 
 It is infusible, and therefore falls under subdivision C. Min- 
 erals infusible or fusible above 5. The first group of the 
 subdivisions is characterized by its behavior before the blow- 
 pipe, " turning blue" when moistened with cobalt solution. One 
 trial shows that it belongs to this group, and since it yields 
 much water in a matrass, it must be looked for under section 
 i, page 289. Among the minerals here mentioned, only alunite 
 and aluminite yield hepar with soda ; the specimen under ex- 
 amination shows this deportment, and must be one or the other ; 
 aluminite is described as being easily soluble in muriatic acid, 
 while alunite is scarcely attacked. A single trial with muri- 
 atic acid determines the mineral to be " aluminite" and its 
 white color distinguishes it further from the similar mineral, 
 "pissophanite" which is olive-green, and has a vitreous lustre. 
 
 To each species is added its chemical formula, for the pur- 
 pose of affording to those who are acquainted with chemistry a 
 ready means of obtaining a more intimate knowledge of its 
 composition than is developed in the characters mentioned. 
 For example, the formula of aluminite is A1SO 6 -|- 9Aq, from 
 which we see that the essential constituents of this mineral are 
 
220 MINERALOGY SIMPLIFIED, 
 
 alumina, sulphuric acid, and water; other trials, therefore, 
 could be made in addition to those just described, to verify its 
 composition. 
 
 TESTING FOR WATKR. 
 
 For the determination of water, a number of small fragments 
 of crystals, or compact mineral should be selected. Instead 
 of a matrass, an open glass tube about 5 inches in length is 
 used ; the sample is placed within it, and we can blow gently 
 on the outside, so as not to fuse the glass ; the water, if present, 
 collects in small drops on the cooler parts of the tube. 
 
 A trace of moisture may be found in almost any mineral, but 
 a very little practice will show whether a mineral is really 
 hydrous or not. Decrepitating minerals may be enveloped in 
 a piece of copper-foil, and thus placed in the tube and heated. 
 In order to determine the loss of water by ignition, quantita- 
 tively, we choose a small platinum crucible, holding some 2 
 grammes of the hydrated mineral. The heating is done over 
 a Bunsen burner, or blast-lamp, the flame of which envelops the 
 apparatus completely. In this manner some silicates of mag- 
 nesia, like chlorite, ripidolite, etc., will lose their water com- 
 pletely, but which could not have been expelled by a common 
 alcohol lamp. 
 
 SOLUTION is the liquefaction of a solid, or a gas, by mixture 
 with a liquid. The -most universal solvent is water; it is 
 always understood to be present in definite proportions, in 
 operations in the wet way. Other solvents are alcohol, ether, 
 disulphide of carbon, benzine, glycerine, and others less im- 
 portant. It must never be forgotten that there are degrees of 
 solubility, but there is hardly such a fact as absolute solubility, 
 or insolubility, regardless of the proportion of the solvent. 
 
 Substances are said to dissolve in acids, or in alkalies, and 
 this is termed a chemical solution ; or, more definitely, it is 
 both a chemical action and solution ; the solution being always 
 a mere physical change. We say that lime dissolves (chemi- 
 cally) in hydrochloric acid, ?*. <?., in the reagent thus called, 
 
DECOMPOSITION BY ACIDS. 221 
 
 which is a mixture of that acid in water. The acid unites 
 with the lime, forming a soluble solid, which the water dis- 
 solves. 
 
 DECOMPOSITION BY ACIDS. 
 
 To test whether a mineral is decomposable (soluble) in acids 
 or not, the sample should be as finely pulverized as possible in 
 an agate mortar. It is then treated with tolerably strong acid, 
 and, if necessary, heat is applied. The digestion is carried on 
 in a small glass flask, a large test-tube, or a small porcelain dish 
 for a quarter of an hour. In order to see whether silicates or 
 many compounds of the earths, and the allied metallic oxides, 
 have been partially dissolved, we separate the acid by decanta- 
 tion or filtration from the residue, and add ammonia in excess, 
 and then a few drops of phosphate of sodium. In case these two 
 reagents produce a decided precipitate, it is a sign that decom- 
 position has taken place, but when no precipitate is formed, or 
 but a few flakes appear, the mineral may be pronounced nearly 
 or quite insoluble. 
 
 If silicates in fine powder form are heated with cone, 
 phosphoric acid (until the latter begins to volatilize, forming 
 thereby dense vapors), and the cold mass is treated with water 
 and boiled, gelatinous lumps of silica separate. Many silicates 
 " gelatinize" when previously fused, viz., garnet, vesuvianite, 
 etc. For this purpose several splinters, or small pieces of the 
 sample are fused B. B., then wrapped in paper and crushed to 
 powder on a steel anvil, and then still finer ground in an agate 
 mortar. This fine powder is brought into a reagent tube or por- 
 celain dish, some hydrochloric acid added, and the whole boiled 
 until the acid is evaporated, when gelatinous lumps remain be- 
 hind ; or, after the lapse of about twelve hours a distinct im- 
 movable " gelatinous" mass is produced in the vessel. If this 
 is stirred up with water, it may be filtered off, and the filtrate 
 be further tested with ammonia, oxalate of ammonium, etc., for 
 alumina, lime, etc., that might be present. 
 
 19* 
 
222 MINERALOGY SIMPLIFIED. 
 
 2. EXAMPLE. Let us suppose that we have bornite, or 
 variegated copper pyrites to determine upon. 
 
 The mineral has metallic lustre ; B. B. it fuses without 
 giving off perceptible fumes. In the oxidizing flame we can 
 perceive the odor of sulphurous acid, and the sample would, of 
 course, when heated with carbonate of sodium, form hepar (sul- 
 phide of sodium) which an experiment confirms. From this 
 
 it follows that the mineral must be looked for under I A 5. 
 
 A single trial with soda shows that it cannot be one of the first 
 four minerals of this (o) group, and that it must belong to the 
 group Chalcocite, etc., whose solutions in nitric acid, treated 
 with an access of ammonia, give an azure-blue color, and which, 
 when fused on coal and moistened with muriatic acid, tinge 
 the blowpipe flame blue. Among minerals of metallic lustre 
 the color is usually characteristic ; it is therefore mentioned 
 when applicable for the purpose of shortening the process of 
 determination. The color of the specimen under examination 
 is copper-red, inclining to yellow ; this sufficiently distinguishes 
 it from the others of the same group, and we must call the 
 mineral bornite, or variegated copper pyrites. 
 
 On beginning the delightful study of determinative miner- 
 alogy, the student ought to exercise great patience and proceed 
 slowly, but surely. Jt is by far the best way to examine at 
 first well-known species. 
 
 Mineral species selected for the study of determinative 
 mineralogy. Von Kobell advises his own students to deter- 
 mine successively the following list of minerals according to 
 the method before us : 
 
 Aluminjte, Borax, Chalcocite, 
 
 Alunite, Bornite, . Cinnabar, 
 
 Anhydrite, Bournonite, Cryolite, 
 
 Antimony-glance, Calamine, Cuprite, 
 
 Apophyllite, Calcite, Datolite, 
 
 Argentite, Cassiterite, Diallogite, 
 
 A.rsenopyrite, Celestite. Dolomite, 
 
 Atacamite, Cerugsite, Lapis-lazuli, 
 
 Barite, Chalcopyrite, Ljevrite. 
 Lepidolite, 
 
WEIGHTS AND MEASUKKS. 
 
 2-2:3 
 
 Limonite, 
 
 Psilomelane, 
 
 Sphalerite, 
 
 Magnesite, 
 
 Pyrite, 
 
 Strontianite, 
 
 Magnetite, 
 
 Pyrolusite, 
 
 Talc, 
 
 Malachite, 
 
 Pyromorphite, 
 
 Witherite, 
 
 Manganite, 
 
 Pyrrhotite, 
 
 Wolfram, 
 
 Molybdenite, 
 
 Realgar, 
 
 Wollastonite, 
 
 Natrolite, 
 
 Scheelite, 
 
 Wulfenite. 
 
 Niccolite, 
 
 Smaltite, 
 
 
 Orpiment, 
 
 Smithsonite, 
 
 
 French Weights and Measures. 
 
 French. 
 
 One Milligramme 
 " Centigamme 
 " Decigramme 
 " Gramme 
 " Decagramme 
 " Hectogramme 
 " Kilogramme 
 
 English. 
 
 = .0154 grains Troy. 
 
 = .1543 " " 
 
 = 1.5434 " " 
 
 = 15.4336 " " 
 = 154.336 " 
 = 1543.36 
 = 15433.6 " 
 
 French. 
 
 One Millimetre 
 " Centimetre. 
 " Decimetre 
 " Metre 
 " Decametre 
 u Hectometre 
 " Kilometre 
 " Myriametre 
 
 2.679 Ibs. Troy. 
 2.205 " avoirdupois. 
 
 English. 
 .0394 inches. 
 .394 " 
 3.937 
 
 = 39.37 " 
 = 393.71 
 = 3937.1 
 = 39371. 
 = 393710. 
 
 1 pound avoirdupois = 7000 grains Troy, or 16 ounces. 1 ounce 
 avoirdupois = 437 grains Troy. 1 gramme = 15.43 grains. 2.35 
 grammes = 1 ounce avoirdupois. 453.60 grammes = 1 pound avoir- 
 dupois. 31.1 grammes = 1 ounce Troy. 1 pound Troy = 5760 grains 
 Troy. 1 kilogramme = 1000 grammes, or = 35.30 ounces avoirdu- 
 pois, or = 32.48 ounces Troy. 100 grammes = 3.53 ounces avoirdu- 
 pois, or 3.2 ounces Troy. 1 inch English = 25.4 millimetres, or 2.54 
 centimetres. 1 foot English = 30.48 centimetres, or 304.8 millimetres. 
 The imperial gallon contains of water at (62OF. 16fOC.) 70,000 grains. 
 The pint ( of gallon) " " " 8,750 " 
 
 Tho fluidounce ( 2 ^of pint) " " "' 437.5" 
 
224 MINERALOGY SIMPLIFIED. 
 
 Relations of the Scales of the Thermometers of Celsius- (Centi- 
 grade}, Reaumur, and Fahrenheit. 
 
 Rules to find the relative value of the three scales. 
 Since, 180 F. = 100 C. = 80 R., 
 Therefore, 9 F. = 5 C. = 4 R. 
 
 Consequently, 1 F. = '^C. = *R. 
 J ) 
 
 no 40 
 
 Also 1 C. F. R. 
 
 i) O. 
 
 n o r o 
 
 And 1 R. = F.sse- C. 
 
 4 4 
 
 From this and the fact that the temperature denoted by 32 
 on the Fahrenheit scale, corresponds to that denoted by on 
 the other two scales, the following rules are derived : 
 
 1. To convert F. degrees into C. degrees. 
 
 Subtract 32 from the number of F. degrees, and multiply the 
 
 remainder by -, according to the formula 
 
 y 
 
 . = (x .32 X ) C. Thus 
 
 212 F. === (21232) 5 = 180 x 5 - = 100 C. 
 
 2. To convert C, degrees into F. degrees. 
 
 9 
 
 Multiply the number of C. degrees by -and add 32 to the 
 
 o 
 
 product, according to the formula : 
 
 x C. *= (x x - + 32) F. Thus 
 ' 
 
 100 C. == 100 x 4- 32 = 180 -f 32 == 212 F. 
 5 
 
. SCALES OF THE THERMOMETER. 225 
 
 # 
 
 3. To convert F. degrees into R. 
 
 Subtract 32 from the number of F. degrees, and multiply 
 
 the remainder by - according to the formula: 
 
 t7 
 
 x F. = (x 32 x 1)B. Thus 
 212 F. = (212_ 32) = 180 X - = 80 R. 
 
 c/ 
 
 4. To convert R. degrees into F. 
 
 Q 
 
 Multiply the number of R. degrees by _ and add 32 to the 
 product, according to the formula : 
 
 xR.= (xx 9 -f- 32) F. Thus 
 
 80 R. = 80 x - + 32 = 180 + 32 = 212 F. 
 
 5. To convert C. derees into R. 
 Multiply 
 
 formula : 
 
 Multiply the number of C. degrees by ~, according to the 
 
 5 
 
 x C. = x x R - 
 
 5 
 
 100 C. = 100 x -=80 R. 
 5 
 
 G. To convert R. degrees into C. 
 
 g 
 Multiply by -, according to the formula : 
 
 4 
 
 x R. = x x -C. Thus 
 4 
 
 80 R. = 80 x - = 100 C. 
 
 The table on next page will give the comparative values of 
 degrees of Reaumur, Celsius, and Fahrenheit. 
 
2-20 
 
 MINERALOGY SIMPLIFIED. 
 
 Reaumur. 
 
 Centigrade. 
 
 Fahrenheit. 
 
 Reaumur. 
 
 Centigrade. 
 
 Fahrenheit. 
 
 Above freezit g-point. 
 
 Above freezing-point. 
 
 4-80 
 76 
 72 
 68 
 64 
 60 
 56 
 52 
 48 
 44 
 40 
 36 
 32 
 28 
 24 
 20 
 16' 
 
 4-100 
 
 95 
 90 
 85 
 80 
 75 
 70 
 65 
 60 
 55 
 50 
 45 
 40 
 35 
 30 
 25 
 20 
 
 4-212 
 203 
 194 
 185 
 176 
 167 
 
 fe 8 
 
 140 
 131 
 122 
 113 
 104 
 95 
 86 
 77 
 68 
 
 +12 
 
 8 
 4 
 
 
 4-15 
 10 
 5 
 
 
 4-59 
 50 
 41 
 32 
 
 Below freezing-point. 
 
 4 
 
 8 
 12 
 16 
 20 
 24 
 28 
 32 
 36 
 
 5 
 10 
 15 
 20 
 25 
 30 
 35 
 40 
 45 
 
 23 
 14 
 
 5 
 4 
 13 
 
 22 
 31 
 40 
 49 
 
 KEY TO THE GENERAL CLASSIFICATION OR SYNOPSIS OF 
 THE TABLES. 
 
 Group I. Minerals with metallic lustre. (Of those minerals whose 
 lustre may be doubtful, only such are here included as 
 are perfectly opaque, even on the thinnest edges.) 
 Class I. Native malleable metals and mercury (are easily dis- 
 tinguished from others), see page 230. The remaining 
 minerals form the following groups : 
 Class II. Fusible from 1-5, or readily volatile. 
 
 Division 1. B. B., on charcoal evolve the strong garlic odor 
 of arsenic, page 232. 
 
 Division 2. B. B., on charcoal, or heated in an open glass 
 tube, give the horseradish odor of selenium, page 236. 
 
 Division 3. B. B., on charcoal, a whitish deposit is obtained 
 which tinges the R. F. green ; in presence of selenium, 
 greenish-blue. Heated gently in a small flask or a test- 
 tube with an excess of concentrated sulphuric acid, 
 the latter assumes a purple-red or hyacinth-red color, 
 which upon the addition of water disappears, while a 
 grayish-black precipitate of tellurium is thrown down, 
 page 238. 
 
GENERAL CLASSIFICATION OR SYNOPSIS. 227 
 
 Division 4. B. B., on charcoal, or in an open glass tube, 
 evolve copious fumes of antimony, page 240. 
 
 Division 5. Heated in an open glass tube give off sulphu- 
 rous acid, which reddens moistened blue litmus paper. 
 B. B., with soda on ehnreoal, yield hepar, but do not 
 give reactions of the preceding divisions, page 243. 
 
 Division 6. Not belonging to the preceding divisions, page 
 
 248. 
 
 Class III. Infusible, or fusibility above 5, and not volatile, page 
 251. 
 
 Division 1. B. B., impart, even in small quantities, to the 
 borax bead in the 0. F., the amethystine color of man- 
 ganese, page 251. 
 
 Division 2. Are magnetic, or B. B., on charcoal become so 
 if perseveringly heated in the R. F., page 252. 
 
 Division 3. Not included, but in some respects related to 
 the preceding divisions, page 254. 
 
 Group II. Minerals without metallic lustre. 
 
 Class I. B. B., volatilize easily or are combustible, page 256. 
 Class II. B. B., fuse easily between 1-5, and volatilize only par- 
 tially or not at all, page 28. 
 
 Part A. B. B., fused with soda on charcoal yield a metallic 
 globule, or when fused alone, in the R. F., form a mass 
 which acts upon the magnetic needle. 
 
 Division 1. B. B., yield with soda alone, or with soda and 
 borax together, a silver globule. 
 
 Those decomposable by nitric acid yield, when their 
 solution is treated with hydrochloric acid, a white pre- 
 cipitate of chloride of silver, which B. B. on charcoal 
 is easily reduced to metallic silver, page 258. 
 Division 2. B. B., with soda, yield a lead globule. 
 
 The nitric acid solution gives, upon the addition of 
 sulphuric acid, a white precipitate of sulphate of lead, 
 which B. B. with soda on charcoal furnishes metallic 
 lead, page 260. 
 
 Division 3. Moistened with hydrochloric acid, communi- 
 cate to the blowpipe flame a transient blue color, and 
 produce with nitric acid a solution which, upon addi- 
 tion of an excess of caustic ammonia, turns, azure blue, 
 page 263. 
 
228 MINERALOGY SIMPLIFIED. 
 
 Section i. B. B., fused on charcoal, evolve a strong arseni- 
 cal odor, page 264. 
 
 Section ii B B., on charcoal, evolve no arsenical odor, 
 
 page 265. 
 Division 4. B. B., impart to the borax bead a sapphire-blue 
 
 color (cobalt), page 268. 
 
 Division 5. B. B., fused in forceps, or melted oh charcoal 
 in the R. F., give a black or gray metallic mass, acting 
 upon the magnetic needle, but do not belong to the pre- 
 ceding divisions, page 268. 
 
 Section i. Evolve, when fused, a strong arsenical odor, 
 page 268. 
 
 Section ii. Soluble in hydrochloric acid without leaving a 
 perceptible residue, and without gelatinizing, page 269. 
 
 Section iii. With hydrochloric acid form a jelly, or decom- 
 pose with separation of silica, page 272. 
 
 Section iv. Only slightly attacked by hydrochloric acid, 
 
 page 275. 
 Division 6. Not included in the foregoing divisions, page 
 
 276. 
 Part B. B. B., fused with soda on charcoal give no metallic 
 
 globule, or fused alone in R. F. do not become magnetic. 
 Division 1. B. B., after fusion and continued heating on 
 charcoal or in the forceps (or when easily fusible, in a 
 platinum spoon), have an alkaline reaction, turning the 
 moistened yellow turmeric paper brown,* or rendering 
 red litmus paper blue, page 277. 
 
 Section i. In water easily and perfectly soluble, page 
 277. 
 
 Section ii. Insoluble or very slightly soluble in water, 
 
 page 279. 
 
 Division 2. Soluble in hydrochloric acid, some also in 
 
 water, without perceptible residue ; the solution does 
 
 not form a gelatinous mass upon evaporation, page 282. 
 
 Division 3. Entirely soluble in hydrochloric acid, forming 
 
 a stiff jelly upon evaporation, page 286. 
 
 * Prof. Kenngott has shown that many silicates and other com- 
 pounds, before and after fusion, have an alkaline reaction when they 
 are placed on turmeric paper in the form of powder moistened with 
 water, but they do not show this reaction when in fragments. 
 
GENERAL CLASSIFICATION OR SYNOPSIS. 229 
 
 Section i. B. B., in the closed tube give water, page 286. 
 Section ii. B. B., in the closed tube, give none or only 
 
 traces of water, page 287. 
 
 Division 4. Soluble in hydrochloric acid, the silica sepa- 
 rating without forming a perfect jelly, page 289. 
 Section i. B. B., in the closed tube give water, page 289. 
 Section ii. B. B., in the closed tube yield 110 water or only 
 
 a trace, page 292. 
 
 Division 5. Are only slightly attacked by hydrochloric 'acid, 
 and B. B. impart to borax glass a deep amethystine 
 color of manganese, page 294. 
 Division 6. Not included in the preceding divisions, page 
 
 295. 
 Class III. Infusible, or fusible above 5. 
 
 Division 1. B. B., after previous ignition, assume a fine- 
 blue color when moistened with cobalt solution and 
 again ignited (alumina), page 303. 
 Section 1 i. B. B., yield much water in the closed tube, 
 
 page 303. 
 Section ii. B. B., in the closed tube yield little or no 
 
 water, page 306. 
 
 Division 2. Moistened with cobalt solution and ignited, as- 
 sume a green color (zinc), page 309. 
 
 Division 3. After ignition, B. B. have an alkaline reaction, 
 and change the color of moistened turmeric paper to 
 reddish-brown, or red litmus paper to blue, page 309. 
 Division 4. Completely soluble in hydrochloric acid, or 
 when this has no effect, in nitric acid, without gelatin- 
 izing by evaporation or leaving a considerable residue 
 of .silica, page 311. 
 
 Division 5. Gelatinize with hydrochloric acid, or are decom- 
 posed with separation of silica, page 316. 
 Section i. B. B., in the closed tube yield water, page 31(5.' 
 Section ii. B. B., in the closed tube yield no water or but 
 
 traces, page 320. 
 Division 6. Not included in either the foregoing divisions, 
 
 page 321. 
 
 Section i. Hardness under 7, page 321. 
 Section ii. Hardness 7 or above, page 325. 
 
 20 
 
230 MINERALOGY SIMPLIFIED. 
 
 GROUP I. MINERALS WITH METALLIC LUSTRE, 
 
 Of the minerals which show an imperfect metallic lustre, 
 only such are included in this division which are also opaque, 
 as wolframite (tungstate of iron), chrome iron ore, etc. The 
 following are ductile and malleable, arid are easily distinguished 
 from, others by their physical properties : 
 
 Class i. Native Malleable Metals and Mercury, 
 
 MALDONITE, Au 2 B5. Color, silver-white (tarnishing black). 
 B. B. upon coal readily fusible, producing inodorous bismuth 
 fumes (covering the coal with dark-brown oxide, which turns 
 pale-yellow on cooling) ; at the same time the gold collects in 
 a globular mass on the coal. By fusing the mineral together 
 with sulphur and iodide of potassium, the coal becomes coated 
 with red iodide of bismuth. G. 8.2-9.7. 
 
 NATIVE SILVER, Ag." Color, silver-white; is easily solu- 
 ble in nitric acid ; the solution even when much diluted gives 
 with muriatic acid a white curdy precipitate of chloride of 
 silver, which, exposed to the light, changes color, becoming 
 bluish-gray. It is easily soluble in ammonia from which 
 copper foil precipitates it in the form of metallic, spongy silver, 
 assuming its natural white color and lustre when rubbed in an 
 agate mortar. H. 2.5-0. G. 10-11. Moistened with sulphide 
 of ammonium, bright silver at once becomes yellowish-brown 
 to gray. (Compare Amalgam.') 
 
 NATIVE GOLD, Au and Electrum (gold alloyed with silver, 
 Ag + x Au, more or less of a gold-yellow color). Native gold 
 is soluble only in nitro-muriatic acid (aqua regia), without 
 perceptible residue. The alloy with silver is partly or entirely 
 decomposed by nitro-muriatic acid with the formation of chlo- 
 ride of silver, which remains undissolved. If we dilute a few 
 drops of the gold solution, concentrated by evaporation with much 
 water until the yellow color has almost disappeared, and then 
 
MINERALS WITH METALLIC LUSTRE. 231 
 
 heat this liquid in a porcelain dish, together with tin-foil (stan- 
 niol), a beautiful purple color is produced, yielding, when left 
 standing, a purple-red deposit of stannate of protoxide of gold, 
 the so-called "purple of Gassius." Heated to boiling with some 
 crystals of oxalic acid, the metallic gold is precipitated as a 
 brown powder, which by rubbing assumes metallic lustre. The 
 solution gives with proto-sulphate of iron (copperas) the same 
 reddish-brown precipitate of gold, which, by rubbing, assumes 
 the color and metallic lustre of gold. H. 2.5-3. G. 15.6-19.5. 
 
 NATIVE COPPER, Cu, is of a copper-red color; dissolves in 
 nitric acid, forming a sky-blue solution which yields with 
 caustic ammonia a blue precipitate, soluble in excess to a 
 deep azure-blue liquid. H. 2.75. G. 8.5-8.9. 
 
 NATIVE LEAD, Pb. Of a lead-gray color; B. B. easily 
 fused, fuming and coating the coal with a greenish-yellow 
 oxide. Dissolves easily in nitric acid, and the solution gives, 
 with muriatic acid, if much diluted, no precipitate,* but, on 
 the addition of sulphuric acid, a heavy white precipitate of 
 sulphate of lead. H. 1.5. G. 11.3.. 
 
 NATIVE PLATINUM, Pt (H. 4.5-5. G. 17-18), and 
 
 PALLADIUM, Pd. Both are infusible. Platinum is of a steel- 
 gray color, soluble in nitro-muriatic acid, but not in nitric. 
 Palladium is between a steel-gray and silver-white; soluble in 
 nitric, but more easily in nitro-muriatic acid. The solution of 
 platinum gives with carbonate of potassium a yellow preci- 
 pitate, insoluble in excess. That of palladium gives a brownish 
 precipitate soluble in excess of the reagent. H. 4.5-5. G. 
 11.8-12.2. 
 
 NATIVE IRON, Fe ; color steel-gray ; attracted by die mag- 
 net ; infusible; soluble in muriatic acid. H. 4.5. G. 7-7.8. 
 
 Argentine (sulphuret of silver), is malleable. (Compare, also, 
 Hessite.) 
 
 NATIVE MERCURY, Hg; is easily recognized, since it is 
 fluid at common temperature ; color, tin-white. G. 13.5-13.6. 
 
 * In a concentrated solution a white precipitate of chloride of lead 
 is formed, soluble in much watr. 
 
232 MINERALOGY SIMPLIFIED. 
 
 The other minerals with metallic lustre may be divided into 
 the following groups : 
 
 Class ii. Fusibility from 1 5, or easily volatilized, 
 
 Division 1 B. B. on coal evolve the strong garlic odor of 
 arsenic. 
 
 NATIVE ARSENIC, As ; volatilizes B. B. without fusing, and 
 sublimes in a bolt-head as a grayish-white crystalline coating. 
 In some varieties the last portion fuses before volatilizing. 
 Streak and fracture, tin-white. H. 3.5. G. 5.7-5.8. 
 
 Binnite.* Composition probably Cu 6 As 4 S B . B. B. fused 
 and then moistened with HC1 colors the flame blue (chloride of 
 copper). A nitric acid solution is rendered blue. Ammonia 
 and this reagent give no precipitate (iron). In the closed 
 tube gives a sublimate of arsenic sulphide; in the open tube, a 
 crystalline sublimate of arsenic trioxide (As 2 O 3 ) with vapor of 
 sulphur dioxide (SO a ). B. B. on coal gives a faint, white coat- 
 ing and odor of arsenic ; with soda fuses to a globule, giving 
 metallic copper. Lustre, metallic ; color, black on fresh frac- 
 ture; streak, cherry-red; brittle, H. 4.5. G. 4.4. A similar 
 deportment is exhibited by 
 
 Arsenomelane and 
 
 Jordanite (Pb a As 4 S 9 ). The latter exhibits a lead-gray color 
 and a black streak. 
 
 Dufrenoysite^ Pb 2 As 2 S 6 . 
 
 Tennantite, Graukupfererz, Cu 8 As 2 S 7 (or 4Cu a S-}-As 2 S s ). 
 
 Polybasite (Ag,Cu) 9 (Sb,As)S 6 . 
 
 JSnart/ite, Cu 3 AsS 4 , 
 
 Rionite (Cu,Fe) 6 (As,Bi) 2 S 8 . 
 
 Domeykite, Cu 3 As. B. B. when fused on coal, and then 
 
 * According to von Kobell this species, found in the valley of 
 "Binnen," Switzerland, consists of arsenite of lead, containing no 
 copper. Consult Dana's Syst. of Min., p. 90. 
 
 f According to the nomenclature of Prof. Kenngott. 
 
MINERALS WITH METALLIC LUSTRE. 233 
 
 moistened with HC1, give to the flame a blue color. The solu- 
 tion in nitric acid yields, with caustic ammonia in excess, a 
 sky-blue liquid. The solution of polybasite in nitric acid, 
 yields, with HC1, a heavy precipitate of chloride of silver, while 
 the others give only a slight one or none at all. A strong solu- 
 tion of caustic potassa extracts on long boiling from all. except 
 dorneykite, sulphuret of arsenic (and sulphuret of antimony), 
 which, when the previously diluted solution is treated with HC1, 
 is precipitated in lemon-yellow flakes (if the sulphuret of anti- 
 mony predominates, the flakes are of a yellowish-red color). 
 
 Rionite, when fused B, B. on coal with sulphur and iodide 
 of potassium, produces a red deposit of iodide of bismuth on 
 the coal, while the others do not. 
 
 Enurgite is plainly cleavable at an angle of 98 ; the others 
 show no cleavage at all. 
 
 Dufreiioysite has a dark steel-gray color and a reddish-brown 
 streak. 
 
 Tennantite is of a light steel-gray color, 
 Dorneykite is silver-white, with a yellow tarnish. The nitric 
 acid solution of most varieties of tennantite yields with am- 
 monia a reddish-brown precipitate of hydrated sesquioxide of 
 iron. The solution of dufrnoysite does not. Similar to that 
 of tennantite is the deportment of epigenite. The latter, how- 
 ever, crystallizes in the orthorhombic ; the former in the iso- 
 metric system. In the neighborhood of domeykite (G. 7 to 
 7.5) belong 
 
 Alyodonite (of Chile), Cu 6 As (with 83.5 per cent, of Cu). 
 H. 4; G. 7.G. 
 
 WTiitneyile, Cu 9 As (88.4 per cent. Cu), color bronze to red- 
 dish-white, becoming brown on exposure, Malleable. H. 3.5 ; 
 G. 8.3. Less fusible than algodonite. 
 
 Smaltite (Speisskobalt), Co (Fe,Ni) As 2 . II. 5.5 ; G. G.37- 
 7.3 
 
 Skutterudite (Tesseralkies), CoAs 3 . 
 
 Cobaltite (glance-cobalt, arsenio-sulphuret of cobalt), Co, 
 AsS. H. 5.5; G. l.-fU. 
 
 20* 
 
234 MINERALOGY SIMPLIFIED. 
 
 Glaucodot (Co,Fe),AsS, and 
 
 Alloclasite (Co,Fe,Zn) 4(As,Bi 7 S 9 ). B. B. in small quanti- 
 ties all impart to a borax bead a fine sapphire-blue color. By 
 concentrated nitric acid they are dissolved, with separation of 
 arsenious acid. The solutions have a red color. The concen- 
 trated solution of alloclasite becomes turbid upon the addition 
 of water (bismuth) ; the others give no such reaction. The 
 solution yields with soluble glass (silicate of potassium solution) 
 a blue precipitate. 
 
 Smaltite (smaltine), skutterudite, and glaucodot yield B. B. 
 in a bolt-head, heated until the glass begins to melt, a gray 
 sublimate of metallic arsenic. Cobaltite gives no sublimate at 
 all. The much diluted nitric acid solution of cobaltite (cobal- 
 tine) and glaucodot give, with chloride of barium, a heavy 
 deposit of sulphate of barium. 
 
 Cobaltite crystallizes in the isometric system, and has octa- 
 hedral cleavage ; skutterudite a cubical one. Glaucodot* crys- 
 tallizes in the orthorhombic system ; cleavage, basal perfect ; 
 prismatic less so. The nitric acid solutions of smaltite and 
 skutterudite yield, when pure, no precipitate with chloride of 
 barium, otherwise a slight one of sulphate of barium. Smaltite 
 shows no cleavage, while skutterudite cleaves in distinct cubes. 
 
 Some varieties of smaltite contain much nickel, approaching 
 chloanthite ; in which case their solutions in nitric acid exhi- 
 bit a greenish color. The nickel is recognized distinctly as 
 follows: The mineral powder is decomposed with a small quan- 
 tity of concentrated nitric acid, and, without filtration, ammo- 
 nia gradually added, until the last few drops of that reagent 
 produces a distinctly alkaline reaction, when the mixture, with- 
 out further dilution with water, is filtered. The filtrate is sky- 
 blue if nickel is present. 
 
 Compare the following (also native bismuth, which is often 
 contaminated with cobalt ores). Bismuth is, however, readily 
 recognized from the fact that water precipitates it white from 
 
 * A similar behavior like glaucodote is exhibited l>y glancopyrite, 
 Fe, Co, Cn, Sl>, As, S. 
 
MINERALS WITH METALLIC LUSTRE. 235 
 
 its concentrated nitric acid solution, the same as alloclasite, 
 whose color is, however, steel-gray, while that of metallic bis- 
 muth is reddish silver-white. 
 
 NICCOLITE (nickeline or .copper nickel, or rothnickelkies), 
 Ni 2 As. H. 5.25. G. 7.5. 
 
 doanthite,* or weissnickelkies (Co,Ni)As 2 , and 
 
 Gersdorjfite, or nickel glance, or arsenio-sulphuret of nickel, 
 NiSAs. H. 5. G. 6. 
 
 These give, when boiled with nitro-muriatic acid, an apple- 
 green solution. Caustic ammonia in excess produces a sap- 
 phire-blue liquid. Potnssa and silicate of potassium (soluble 
 glass) added to the solutions give greenish precipitates. Chlo- 
 ride of barium produces in the dilute acid solution of gersdorf- 
 fite a heavy precipitate ; in the other two none, or only a feeble 
 one. 
 
 Niccolite and gersdorffite, when heated in closed glass tube, 
 give no sublimate of metallic arsenic, but cloanthite* does. A 
 similar deportment is shown by chatamite, whose solution yields, 
 however, with an excess of ammonia, a reddish-brown precipi- 
 tate (hydrated ferric oxide). Further, 
 
 Corynite^i Ni( As,Sb)S, and 
 
 Wolfachite, Ni(As,Sb)S, B. B. on coal yield arsenic and 
 antimony fumes, and produce with soda hepar.f These min- 
 erals usually show the reaction for cobalt. 
 
 The color of niccolite is light copper-red ; of chloanthite and 
 chatamite, tin-white; that of gersdorffite, light lead-gray, 
 inclining to tin-white. Corynite, is silver-white to steel-gray; 
 wolfachite, silver-white. Compare ulmannite (riickeliferous 
 gray antimony) which contains arsenic, and in that case re- 
 sembles gersdorffite in its behavior. 
 
 ARSENOPYRITE, or arsenio-sulphuret of iron, or mispickel, 
 FeS 2 4-FeAs. B. B. in a bolt-head yields a sublimate of metal- 
 
 * Chloanthite is, according to Dana, only a variety of smaltite ; it 
 crystallizes in the isometric system, whilst rammelsbergite, NiAs, of 
 like composition, crystallizes in the orthorhombic system. 
 
 f Corynitc is isometric; wolfachito, orthorhombic. 
 
236 MINERALOGY SIMPLIFIED. 
 
 lie arsenic; on coal it fuses to a black, and, after long blowing, 
 to a magnetic globule,* thereby covering the coal with white 
 arsenious acid. In nitric acid it is soluble with separation of 
 sulphur and arsenious acid. The solution gives, with caustic 
 ammonia, a reddish-yellow precipitate. Fracture, silver-white, 
 inclining to gray. H. 5-5.5 G. 6-6.2. 
 
 Compare native bismuth and native antimony, which often 
 contain arsenic, but are easily recognized by their fusibility at 
 a low temperature, and the white or yellow coating which they 
 give to coal. Some proustite and pyrargyrite show often a 
 submetallic lustre, but are readily distinguished by their cochi- 
 neal-red streak. 
 
 Division 2. B. B. on coal, or in open glass tube, evolve the 
 strong horseradish odor of selenium. 
 
 GuANAJUATiTEf (Frenzelite), selenide of bismuth (B5 2 Se 3 ). 
 B. B. fuses readily, colors the flame blue, and gives when fused 
 with sulphur and iodide of potassium upon charcoal a red coat- 
 ing of iodide of bismuth. H. 2.5-3.5. G. 6.25. 
 
 Tiemannite (selenide of mercury) (HgSe,) and Lehrba- 
 chite (selenide of mercury and lead) (P,Hg)8e. B. B. yield 
 with soda, in a bolt-head, metallic mercury ; this is likewise 
 the case when the mineral powder is mixed with iron powder, 
 and the mixture wrapped in copper foil is heated in a glass 
 tube. Lehrbachite gives with soda on coal, globules of lead ; 
 tiemannite does not. Both volatilize readily, tiemannite while 
 fusing, lehrbachite before fusing. Color of the former is 
 steel-gray to blackish lead-gray, that of the latter lead-gray. 
 
 Guadalcazarite (Hg,Zn), (S,Se). Gives the reaction of 
 mercury and also of sulphur. Hence, when the mineral powder 
 
 * A similar behavior is exhibited by liillingite, leucopyrite, arse- 
 niuret of iron, FeAs 2 , which, after the expulsion of arsenic, fuses im- 
 perfectly and with difficulty on its edges. Specific gravity 7.2. With 
 iron it produces no hepar, or the reaction is but feeble. 
 
 f See E. S. Dana's Text-book, 1880, page 211. 
 
MINERALS WITH METALLIC LUSTRE. 237 
 
 is heated together with iron-powder and the mass treated with 
 muriatic acid, sulphide of hydrogen is evolved. Color is iron- 
 gray, streak black. H. 2. G. 7.15. 
 
 CLAUSTHALITE (seleniuret of lead, Selenblei, PbSe). B.B. 
 volatilizes chiefly without fusion, and coats the coal with a 
 feeble metallic gray, and then with a white and greenish -yellow 
 color. It yields with some difficulty, by means of soda, a glo- 
 bule of lead. Dissolved in nitric acid it is precipitated by 
 sulphuric acid, sulphate of lead being formed. Heated with 
 concentrated sulphuric acid until the latter commences to 
 escape in vapor form, it yields a fine green solution, from which 
 water throws down a fine red precipitate, or produces cloudi- 
 , ness of the same color (selenium). Color, lead-gray. H. 2.5-3. 
 G. 8.2-8.8. 
 
 NAUMANNITE (seleniuret or silver, Selensilber ( Ag,Pb) 5 Se 3 ). 
 B. B. fuses easily, and in the O. F. quietly ; in the R. F. with 
 intumescence ; with soda and borax it yields a globule of silver. 
 Dissolves in concentrated nitric acid ; the solution throws down 
 with muriatic acid a strong precipitate of chloride of silver. 
 Color, iron-black. H. 2.5. G. 8. 
 
 Berzelianite (seleniuret of copper, Selenkupfer), Cu 2 Se. 
 
 Raphanosrnite (seleniuret of copper and lead}, Seleribleikup- 
 fer, (Pb,Cu 2 )Se, and 
 
 Jtucairite (seleniuret of silver and copper), (Cu,Ag) 2 ,$e. 
 B. B. on coal fuse to a metallic globule, which, moistened with 
 muriatic acid, imparts to the flame a blue color. They are 
 soluble in concentrated nitric acid, and the solutions treated 
 with caustic ammonia in excess assume an azure-blue color. 
 The solution of eucairite gives, with muriatic acid, a heavy 
 precipitate of chloride of silver ; that of raphanosmite with sul- 
 phuric acid, a precipitate of sulphate of lead ; that of berzelia- 
 nite affords no precipitate with either of the acids. Color of 
 berzelianite is silver-white; that of eucairite and raphanosmite, 
 lead-gray. 
 
 Crookesite (Cu 2 Tl,Ag)8e is similar to berzelianite, con- 
 taining 17.25 per cent, of thallium, and coloring the flame 
 vivid jrreen. 
 
238 MINERALOGY SIMPLIFIED. 
 
 Division 3. B. B. on coal yield a whitish deposit, which colors 
 the reducing flame greenish or greenish-blue.* Impart to 
 concentrated sulphuric acid, when gently heated with it in 
 a test-tube, a purple-red or hyacinthine color, which, 
 upon the addition of water disappears, while a blackish- 
 gray precipitate forms (tellurium}. 
 
 Collecting the precipitate upon a filter and drying it, it im- 
 parts to concentrated sulphuric acid, when heat is first applied, 
 a purple color, which again disappears upon continued heating. 
 B. B. most compounds of tellurium evolve on charcoal the 
 horseradish odor of selenium, caused by an accidental trace of 
 this element. 
 
 The ores of tellurium may, by their color, be divided into 
 two groups. 
 
 (a) Those of a tin or silver-white color. 
 
 NATIVE TELLURIUM, Te. B. B. fuses easily ; can be 
 entirely volatilized ; fumes strongly, and burns with a greenish 
 flame. In nitric acid it is soluble without residue ; the solu- 
 tion gives with potassa a white precipitate mostly soluble in 
 excess ; muriatic or sulphuric acid causes no perceptible precipi- 
 tate. Color, tin-white to silver-white. H. 2-2.5. G. 6.1-G.3.. 
 
 MELONITE, Ni 2 Te 2 . Hexagonal, reddish-white, dark-gray 
 streak. 
 
 HESSITE (telluret of silver, Tellursilber), Ag 2 Te (sectile) 
 and .: 
 
 ALTAITE (telluret of lead, Tellurblei), PbTe, are soluble 
 in nitric acid without residue. The solution of the first in 
 excess of nitric acid forms no precipitate with sulphuric acid, 
 while the second gives a heavy deposit of sulphate of lead. 
 B. B. the first mineral gives, with soda, a globule of silver, 
 
 * If the ificrusted coal is held over a watch glass containing sulphide 
 of ammonium, the vapors of the latter render the coat brownish, while, 
 under the same circumstances, a coat of antimony would turn oranye- 
 red. 
 
MINERALS WITH METALLIC LUSTRE. 239 
 
 containing sometimes gold. Hessite is malleable. Altaite is 
 only sectile. Color, tin-white. 
 
 MUELLERITE (cwrotellurite, Weisstellur), (Au,Ag,Pb),Te 3 , 
 Sb. Is chiefly soluble in nitric acid with separation of the 
 gold ; with muriatic acid the solution affords a precipitate of 
 sulphate of lead. Color, silver-white, inclining to brass-yellow. 
 Brittle. (Belongs probably to Sylvanite.) 
 
 Compare the following : 
 
 (6) Those which have a lead-gray or steel-gray color. 
 
 TETRADYMITE (telluret of bismuth), Bi,(Te,S) 3 . B. B. fuses 
 to a silver-white, brittle, metallic globule ; yields, when fused 
 upon coal with iodide of potassium, a red precipitate. Dissolves 
 easily in nitric acid, with separation of sulphur ; the solution 
 yields with sulphuric or muriatic acid, no precipitate; with 
 potassa, a white precipitate insoluble ,in excess. Color, light 
 lead-gray. The thin laminae somewhat elastic. A similar 
 compound is Joseite, Bi 12 Te 4 SeS 3 . H. Ig2. G. 7.5. 
 
 SVLVANITE (graphic tellurium 3 Schrifterz), (Au,Ag)Te 3 .* 
 B. B. soon fuses, and after long blowing is reduced to a ductile, 
 metallic globule. In nitric acid it is imperfectly soluble, in 
 nitro-muriatic acid entirely so, with precipitation of chloride 
 of silver. The solution gives no precipitate on the addition of 
 sulphuric acid. Color, light steel-gray. 
 
 Nagyagite (telluret of gold and lead, Blattererz), Pb,Au, 
 T<',S. B. B. fuses easily, and after long blowing, to a mallea- 
 ble, metallic globule. In nitric acid it is easily and chiefly 
 soluble; the solution yields, with sulphuric acid, a heavy pre- 
 cipitate of sulphate of lead. When heated with concentrated 
 sulphuric acid, a solution is obtained of a hyacinthine or brown- 
 ish-yellow color, not exhibiting, as in the previous cases, a fine 
 red hue. Water discolors the liquid with separation of tellu- 
 rium. Color, blackish lead-gray. H. 1-1.5. G. 6.8-7.2. 
 
 (Compare, also, belonite.) 
 
 * Petzite (Ag,Au) 2 Te, shows a similar composition, but contains 
 more silver. 
 
240 MINERALOGY SIMPLIFIED. 
 
 Division 4. B. B. on charcoal evolve copious fumes of anti- 
 mony. 
 
 The fumes are nearly inodorous, or smell of sulphurous acid, 
 or have a feeble, arsenical odor caused by the sulphur in the 
 ores, or an accidental trace of arsenic. 
 
 By the first action of the flame, the vapor coats the coal 
 white (oxide of antimony), which coating submitted to the R. 
 F. does not alter the color of the flame. When this coating is 
 collected in a glass tube, and exposed to the vapors of sulphide 
 of ammonium, it turns orange, sulphide of antimony being pro- 
 duced. 
 
 NATIVE ANTIMONY, Sb. H. 3.3-5. G. 6.6-6.8. 
 
 STIBNITE (sulphuret of antimony, Antimonglanz), SbS 3 . 
 
 ZINKENITE (antimonial sulphuret of lead), PbSbS 4 . 
 
 J.VMESONITE (sulphuret of antimony and lead), Pb 2 SbS 5 . 
 
 BOURNONITE (antimonial sulphuret of lead and copper), 
 3(Cu,Pb)SSbS 3 . B. B. volatilizes entirely or principally. 
 Native antimony is distinguished by its tin-white color. Heated 
 B. B. it continues to burn without further blowing, and covers 
 the globule of metal with white, needle-shaped crystals of oxide.* 
 Stibnite (antimonite, antimony glance), in powder form, it is 
 soon changed to an ochre-yellow by a strong solution of potassa, 
 in which it is also chiefly soluble ; hydrochloric acid precipitates 
 it in yellowish-red flakes. Color of this mineral is lead-gray, 
 inclining to steel-gray. 
 
 Zttikenite, jamesonite, and bournonite are of a steel-gray 
 color. Digested in powder form with potassa solution they do 
 not change their color ; the potassa, however, when boiled down 
 nearly to dryness, extracts the sulphuret of antimony, which 
 may be precipitated by hydrochloric acid in yellowish-red or 
 orange flakes. ZinJcenite and jamesonite are converted by 
 nitric acid into a white pulverulent oxide without changing the 
 color of the acid, which dissolves only a small portion. Bour- 
 
 * Compare native bismuth and bismuthinite. 
 
AIINEliALS WITH METALLIC LUSTRE. 241 
 
 nonite partially dissolves to a sky-blue solution, yielding, with 
 sulphuric acid, a white precipitate of sulphate of lead, and with 
 caustic ammonia in excess an azure-blue liquid (copper). 
 
 Stylotypite (Cu a ,Ag,Fe) 3 SbS 6 , shows a similar deportment 
 to bournonite, but its solution in aqua regia yields no precipi- 
 tate with sulphuric acid. H. 3. G. 4.8. 
 
 ' Zinkenite is not cleavable. Hardness, 3.5. Jamesonite is 
 generally cleavable in one direction. Hardness, 2.5. These 
 minerals are related in their chemical characters to the follow- 
 ing rare compounds, which are all sulphurets of lead and anti- 
 mony, viz : 
 
 Boulangerite, Pb 3 SbS 6 . 
 f Geocronite, Pb 5 SbS 8 . 
 I Kilbrickenite.* 
 
 Plagionite, PbSbS. 
 
 Meneghinite, Pb 4 ShS 7 . 
 
 Some antimonites mixed with gatenite (galena) behave similarly, 
 likewise kobellite = Pb 3 BiSbS 6 (or 3PbS+ (Bi.Sb). 2 S 3 ), which con- 
 tains 35 per cent, of sulphide of bismuth. B. B. when fused together 
 with sulphur and iodide of potassium on charcoal, it affords a red and 
 yellow coating. When the nitric acid solution is treated with sul- 
 phuric acid, white sulphate of lead is precipitated. 
 
 DYSCRASITE (antimonial silver, Antimonsilber= Ag 3 Sb). 
 
 STEPHANITE (antimonial sulphuret of silver), Ag 5 $bS 8 (or 
 5AgS -f SbS 3 ). H. 2-5.5. G. 6.2. 
 
 TETUAiiEDUiTEt (gray copper ore, Fahlerz.) 
 
 Antimonfahlerz, Cu g Sb 2 S 7 , with (Cu 2 ) replaced by (Fe), 
 (Zn), (Ag 2 ) or (Hg). 
 
 * According to Dana and Brush identical with Geocronite. 
 
 f Polytelile, v. Kobell. Varieties of Antimonfahlerz, when poor in 
 silver, are distinguished from those rich in silver, by yielding from 
 their nitric acid solution a slight precipitate with HCl. All the varie- 
 ties containing copper furnish nitric acid solutions, which turn azure 
 blue by an excess of ammonia. (See Polytelite, Dana's Syst. of Min., 
 pp. 101, 104, 804.) 
 21 
 
242 MINERALOGY SIMPLIFIED. 
 
 Miarygyrite (sulphuret of antimony and silver), AgSbS 4 . 
 B. B. yields with soda, or soda and borax, a malleable silver 
 globule, and the nitric acid solution yields, with muriatic acid, 
 a precipitate of chloride of silver. Dyscrasite has a silver- 
 white color, and gives with soda no hepar. Is not attacked by 
 potassa. All the others give, with soda, hepar, and potassa 
 solution extracts sulphuret of antimony, which is precipitated 
 in orange-colored flakes by muriatic acid. Stephanite and 
 miargyrite are partially soluble in nitric acid, oxide of anti- 
 mony being deposited ; the solution treated with caustic am- 
 monia in excess acquires none or only a feeble bluish tint ; 
 that of tetrahedrite (polytelite, v. Kobell) assumes a sky-blue 
 color. The color of stephanite is between an iron-black and a 
 blackish lead-gray. Streak, black. Hardness, 2.5. Miargyrite 
 is iron-black, inclining to light steel-gray. Streak, dark cherry- 
 red. Hardness, 2.5. Tetrahedrite (polytelite) is between steel- 
 gray and iron-black. Hardness, 3.5. Streak, grayish -black. 
 
 Broyniardite (Pb,Ag) a SbS 5 , is an ore which shows a 
 similar deportment like the preceding. It crystallizes in the 
 isometric system (octahedrons). "When decomposed by nitric 
 acid, sulphate of lead separates. 
 
 Freieslebenite (Pb,Ag).,Sb 2 ,S 11 , and 
 
 Diaphorite, Ag 3 SbS 3 . 
 
 The former crystallizes in the monoclinic and the latter in 
 the trimetric (orthorhombic) system. 
 
 (Compare also pyrargyrite (ruby silver ore), Ag 3 SbS 6 .) 
 
 SPANIOLITE (gray copper, Quecksilberfahlerz), (Cu,Hg) 
 SbS. The nitric acid solution is colored azure-blue by an 
 excess of ammonia. It affords mercury when ground together 
 with iron-powder and soda, then the whole wrapped in copper- 
 foil and heated in a glass tube. H. 3.5. G. 8.1. 
 
 CHALCOSTIBITE (sulphuret of copper and antimony, Kupfer- 
 antimonglanz), Cu 2 SbS 4 . B. B. roasted on coal with soda 
 for some time yields' a copper globule. HC1 (hydrochloric 
 acid) produces no precipitate in the nitric acid solution. An 
 
MINERALS WITH METALLIC LUSTRE. 243 
 
 excess of ammonia renders the solution azure-blue. Color, 
 lead-gray to iron- black. H. 3.5. G. 4.8. 
 
 ULLMANNITE (nickeliferous gray antimony, Nickelantimon- 
 glanz), Ni 2 SbS 2 . H. 5.5. G. 6.8. 
 
 BREITHAUPTITE (antimonial-riickel, Antimonnickel), Ni 2 , 
 Sb, and 
 
 BERTHIERITE (sulphuret of antimony and iron), FeSbS 4 . 
 B. B. on coal yield, after long blowing, a magnetic globule. 
 Breitliauptite fuses with difficulty ; muriatic acid attacks it 
 with difficulty ; aqua regia readily and completely dissolves it. 
 Color, between copper-red and violet. Ullmannite fuses 
 readily ; muriatic acid attacks it with difficulty ; aqua regia 
 dissolves it with separation of sulphur.* Color, between lead- 
 gray and steel-gray. Berthierite fuses without difficulty ; and is 
 easily dissolved in muriatic acid with evolution of sulphuretted 
 hydrogen. Color, steel-gray inclined to brown. 
 
 Division 5 Heated in an open glass-tube give sulphurous 
 acid,, which reddens a strip of moistened blue litmus 
 paper placed in the end. B. B. with soda give hepar, 
 without presenting the general characters mentioned in 
 the preceding numbers. 
 
 ARGENTITE (sulphuret of silver, silverglance, Glaserz), 
 AgS and Jalpaite (Ag,Cu 2 )S can easily be distinguished from 
 the following by being malleable and sectile like lead. 
 
 The nitric acid solution yields with hydrochloric acid, a heavy 
 precipitate of chloride of silver. The addition of ammonia 
 colors the solution of Jalpaite blue, that of Argentite remains 
 colorless. B. B. on charcoal, heated with cyanide of potassium, 
 Jalpaite yields a silver globule containing copper. 
 
 Acanthite, AgS, is distinguished from argentite only by the 
 crystalline form. " The former crystallizes in the trimelric, 
 the latter in the isometric system. 
 
 * In other respects the solutions of the first two show, with am- 
 monia, the s:imr deportment that is mentioned in (1) of nickeliiie. 
 
244 MINERALOGY SIMPLIFIED. 
 
 Alabandite, MnS, and 
 
 flauerite, Mn8 2 , can be distinguished by the color of their 
 powders. That of the first is leek-green, that of the second 
 brownish-red. Both yield, when boiled down with a mixture 
 of phosphoric and nitric acid, a handsome violet liquid. 
 
 Cinnabar, HgS, usually of a red, in many varieties of a 
 lead-gray color, is characterized by the red streak. When 
 mixed with iron-powder, wrapped in copper-foil, and heated 
 in a glass-tube, metallic mercury is produced. 
 
 (Compare proustite and pyrargyrite.) 
 
 GALENITE (sulphuret of lead, galena, Bleiglanz), PhS. B. B. 
 with soda is easily reduced to metallic lead, coating the coal 
 with a greenish-yellow oxide. In concentrated nitric acid it 
 readily dissolves with separation of sulphur and sulphate of 
 lead. Color, lead-gray. Cleavable in cubes. The nitric acid 
 solution of galenite is not colored blue with an excess of ammo- 
 nia, which is, however, the case with the next. H. 2.5. G. 7.5. 
 
 CUPKOPLUMBITE (Kupfcrbleiglanz), Cu 2 S,2PbS. B. B. the 
 latter exhibits otherwise a deportment similar to' that of galenite. 
 
 HUASCOLITE is a zinciferous variety of the preceding, and 
 very similar in its behavior. 
 
 CiiALCOCiTE (suphuret of copper, Kupferglanz), Cu 2 $. 
 H. 2.5-3. G. 7.5. 
 
 STROMEYERITE (sulphuret of silver and copper, Silberkup- 
 forglanz), AgCu 2 S. 
 
 WITTICHENITE (sulpuhuret of copper and bismuth, Kupfer- 
 wismutherz), Cu 3 BiS 3 . 
 
 STANNINE (tin pyrites, sulphuret of tin, Zinnkies), (Cu,Sn, 
 Fe, Zn,) S. 
 
 CHALCOPYRITE (copper pyrites, sulphuret of copper and 
 iron, Kupferkies), Cu 2 Fe 2 S 4 . H. 3.5. G. 4.3. 
 
 CUBAN (Cubanite), Cu 2 Fe 4 S 4 . 
 
 BORNITE (erubescite, variegated copper, Buntkupfererz),* 
 (Cu 2 Fe)S. H. 3. G. 5. 
 
 * A copper ore of similar color and tarnishing like bornite, is cas- 
 tillite = (CuAg) 2 -\- 2(Cu,Pb,Zn,Fe)S. It is considered to be an 
 
MINERALS WITH METALLIC LUSTRE. 245 
 
 BELONITE, aikinite (acicular bismuth, Nadelerz), CuPb 
 BiS r 
 
 SAYNITE griinanite (bismuth nickel, Nickelwismuthglanz), 
 Ni,Bi,Fe,Cu,S. 
 
 CUPROPLUMBITE, Cu 2 S,2PbS, and 
 
 PENTLANDITE (sulphuret of iron and nickel, Eisennickel- 
 kies), (Fe,Ni)S, are partially soluble in nitric acid to a sky- 
 blue or greenish liquor, which, with ammonia in excess, 
 assumes an azure-blue or a deep blue color. If the blue 
 ammoniacal liquor is strongly acidulated with sulphuric acid, 
 and a strip of blank sheet-iron put into it, all the previously 
 mentioned minerals, with exception of saynite and pentlandite 
 (provided these two are free from an admixture of chalcopyrite), 
 throw down metallic copper. The color of chalcopyrite* and 
 cubanite is brassy-yellqw, the latter cleavable in hexadrons, the 
 former not. The color of bornite is between copper-red and 
 pinchbeck-brown. That of pentlandite, light bronze yellow. 
 B B. these ores melt to a steel-gray, brittle globule which is 
 attracted by the magnet. Pentlandite acts upon the magnetic 
 needle. H. 3.5-4. G. 4.6. 
 
 In order to distinguish the others (the colors of which are 
 gray), we proceed as follows : 
 
 a. The saturated nitric acid solution gives, upon the addition 
 of water, a white precipitate with wittichite, saynite, and 
 belonite. B. B. all three yield, when mixed in powder form 
 with sulphur and iodide of potassium and then fused on char- 
 coal (by continuous blowing), a red coat of iodide of bismuth. 
 In the acid solution of belonite, sulphuric acid produces a 
 white precipitate of sulphate of lead, which does not take place 
 with the others. (Compare chiviatite.) 
 
 argentiferous bornite. When decomposed by nitric acid, a residue of 
 sulphate of lead remains behind. 
 
 * A mineral much resembling chalcopyrite is barnhardtite (homich- 
 line) Cu 4 Fe 2 S 5 . Color, brass-yellow ; the fresh fracture tarnishes to a 
 golden-yellow in twenty-four hours. 
 
 21* 
 
246 MINERALOGY SIMPLIFIED. 
 
 B. B. on coal, ivittichite yields with soda a copper globule ;* 
 saynite, a gray, nickeliferous, strongly magnetic globule. 
 
 b. The saturated nitric acid solution furnishes with water no 
 precipitate, but with sulphuric acid a white one of sulphate of 
 lead ; the mineral is cuproplumbite. 
 
 c. The nitric acid solution produces neither with water nor 
 sulphuric acid, any precipitate, but if muriatic acid throws 
 down white chloride of silver the mineral is stromeyerite. 
 
 d. Neither of the reagents alluded to having any effect, or 
 producing but a very slight precipitation, we arrive at chal- 
 cosite and stannite. 
 
 (Compare tetrahedrite.) 
 
 Chalcosite on coal B. B. gives, after long blowing, a malle- 
 able copper globule ; is soluble in nitric acid with separation of 
 sulphur; color, between blackish lead-gray and steel-gray. But 
 stannite alone gives no malleable or metallic globule ; is dis- 
 solved by nitric acid with separation of sulphur and oxide of 
 tin ; color, between steel-gray and brass-yellow. 
 
 Chalcosite crystallizes in the trimetric system. Other simi- 
 lar sulphides of copper are : 
 
 Carmenite.^ 
 
 Digenite. 
 
 Cupreine (hexagonal). 
 
 Millerite (sulphuret of nickel, Ilaarkies), NiS. 
 
 Linneite, linnceite (cobalt pyrites, Schwefelkobalt), CO S S 4 
 (or 2CoS + Co8 2 ). A variety is called siegenite, carrollite, 
 =Co 2 CuS 4 . 
 
 PYRITE (iron pyrites, bisulphuret of iron, Eisenkies), 
 FeS 2 . H. 6-6.5. G. 4,9. 
 
 * A deportment similar to wittichite is exhibited by tannenite and 
 klaprothite. 
 
 f According to Dana (System of Min. 1872, p. 53), carmenite is 
 a mixture of chalcocite and covellite. Digenite and cupreine result 
 also probably from alterations according to him, see p. 53. 
 
MINERALS WITH METABLIC LUSTRE. 247 
 
 PYRROTIIITE (Pyrrhotine, magnetic pyrites, Magnetkies), 
 Fe 7 S 8 , and 
 
 STERNBERGITE (sulphuret of silver and iron), (AgFe)S. 
 B. B. are reduced to a magnetic globule which, moistened with 
 muriatic acid, imparts to the flame no perceptible change of 
 color except carrollite which, under these circumstances, colors 
 the flame blue ; the partial nitric acid solution is not blue. B. 
 B. linnaeite and carrollite render a borax bead sapphire-blue ; 
 in nitric acid both dissolve perfectly and easily, forming a rose- 
 red solution which gives, with chloride of barium, a white pre- 
 cipitate. From the solution of carrollite, iron wire precipitates 
 metallic copper. Color, between tin-white and light steel-gray. 
 Sternbergite B. B. is partly reducible to silver ; the partial 
 nitric acid solution gives, with muriatic acid, a heavy precipi- 
 tate of chloride of silver. Color, dark tombac-brown. Pyrite 
 and pyrrhotite B. B. give only the reaction of iron and 
 sulphur. 
 
 Pyrite* before fusion does not act on the magnetic needle ; 
 is only slightly attacked by muriatic acid. Aqua regia forms 
 a solution which with ammonia yields a brownish red precipi- 
 tate insoluble in an excess and not rendering the solution 
 blue. Color, pale yellow. 
 
 Pyrrhotite acts upon the needle ; is principally soluble in 
 muriatic acid with evolution of sulphuretted hydrogen. Color, 
 between brown-yellow and copper-red (usually tarnished tom- 
 bac-brown). 
 
 Millerite is scarcely affected by nitric acid ; with nitro- 
 muriatic acid it forms a greenish solution, in which potassa 
 causes a greenish precipitate. Ammonia produces a precipitate 
 which dissolves in an excess with a blue color. Color, between 
 a brass-yellow and bronze-yellow. Has been heretofore found 
 only in hair-like crystals. 
 
 Closely related to the preceding is beyrichite Ni 6 S r 
 
 * Marcasite (ortho-rhombic iron pyrite) and pyrite (isometric iron 
 pyrite) are only distinguishable by their crystalline form. Are de- 
 composed by nitric acid. 
 
248 MINERJPLOGY SIMPLIFIED. 
 
 Color, lead-gray. B. B. in a closed tube affords a sublimate 
 of sulphur. Millerite does not. 
 
 BISMUTHINITE (sulphuret of bismuth, Wismuthglanz), 
 BiS 3 . B. B. in the reduction flame fuses with boiling and 
 spirting. Yields a globule of bismuth, and coats the coal yel- 
 low. Dissolves in nitric acid with separation of sulphur. 
 The concentrated solution diluted with water becomes turbid, 
 and then yields a white precipitate of bismuth. Color, light 
 lead-gray, inclining to steel-gray. H.2. G. 6.4. 
 
 A similar behavior is shown by chiviatite (Pb. 2 ,Cu 2 )Bi 3 S n . 
 It is decomposed by nitric acid with separation of sulphate of 
 lead. Emplectite CuBiS 2 affords with nitric acid a bluish- 
 green solution, which turns, with an excess of ammonia, azure- 
 blue. Behaves otherwise like bismuthite. (Compare native 
 bismuth.) 
 
 Division 6 Not belonging to the preceding divisions. 
 
 AMALGAM (native), AgHg 2 and AgHg 3 . B. B. gives off 
 quicksilver in a matrass, with boiling and spirting, and leaves 
 a swollen mass of silver. Dissolves easily in nitric acid. Color, 
 silver-white. The amalgam richest in silver is arquerite, 
 Ag,,Hg. 
 
 Metacinnabarite, HgS. Mixed with iron powder, it affords, 
 in a matrass, mercury and sulphide of iron, which latter evolves 
 sulphide of hydrogen when treated with hydrochloric acid. 
 Rarely crystallized, constituting amorphous cinnabar. Color, 
 grayish-black. Streak, black. 
 
 BISMUTH (native), Bi. B. B. fuses easily, arid does not 
 continue to burn after removal from the flame ; evaporates after 
 long blowing, and imparts to the coal, at first, a white coating, 
 which becomes partly yellow and partly orange. The color 
 slightly fades on cooling. B. B. The mineral powder when 
 fused together with sulphur and iodide of potassium on char- 
 coal affords, after continuous blowing, a cinnabar-red coating. 
 It is easily soluble in nitric acid. The concentrated solution 
 
MINERALS WITH METALLIC LUSTRE. 249 
 
 yields with much water a white precipitate. Color, reddish 
 silver-white. Brittle. H. 2.5. G. 9.7. 
 
 Rabdionite (Cu,Mn,Co,Fe). Colors the borax bead cobalt- 
 blue. Heated with phosphoric acid, gives a violet solution 
 (manganese). Is dull, but gives a metallic greasy streak. 
 Color, black. H. 1. G. 2.8. 
 
 HAEMATITE (specular iron, red iron ore, Rotheisenerz), 
 Fe 3 O 3 . Difficult of fusion ; in the reduction flame becomes 
 magnetic. Streak, cherry-red. H. 5.5-6. G. 5. 
 
 Cuprite (red copper ore), Cu 2 O ; has sometimes a metallic 
 lustre ; easily reducible to a copper globule B. B. 
 
 Magnetite (magnetic iron, Magneteisenerz), Fe 3 O 4 . B. B. 
 fuses with great difficulty, usually above 5. It may be easily 
 recognized by its action on the needle, and its black streak. 
 
 Hortonolite (Fe,Mg) 2 SiO 4 . Fuses at 4. Color, yellow to 
 dark yellow-green. It has partly a metallic lustre and with 
 an admixture of magnetite is magnetic. 
 
 Roepperite (Fe,Mn,Zn,Mg) 2 SiO i . Color, dark-green to 
 black. 
 
 Fayalite^ Fe 2 SiO 4 . Fuses at 3. Color, dark-green, brown 
 to black. 
 
 The three latter minerals gelatinize with hydrochloric acid. 
 
 WOLFRAMITE (Wolfram, tungstate of iron and manganese), 
 (Fe,Mn,) W0 4 == W 75.56, F0 20.17, Mn 3.54 (Fe and Mn 
 varying greatly). B. B. fuses at 3 to a gray and often crystal- 
 line globule ; with borax it yields an amethystine colored bead. 
 Boiled with phosphoric acid and strongly concentrated it yields 
 a fine blue liquid, whose color is heightened on cooling. 
 When diluted with water a reddish-yellow, and later a color- 
 less liquid is obtained. Upon the addition of iron powder and 
 sulphuric acid it turns, when shaken, intensely sapphire blue. 
 This liquid, when diluted with much water, loses in a few 
 minutes its blue color. If we add to the blue solution with 
 phosphoric acid, a little nitric acid, the color is changed to 
 violet (manganese reaction). Color, grayish-black to iron 
 black. Streak, dark reddish-brown to black. H. 5.5. G. 7.3. 
 
250 MINERALOGY SIMPLIFIED. 
 
 BLACK SILICATE OF MANGANESE (Schwarzer Mangan- 
 kiesel)* MnSiO 3 -f- 2H 2 0. B. B. fuses with intumescence, 
 and in a bolt-head yields much water ; imparts to a borax bead 
 in the oxidizing flame a strongly amethystine color. It is -dis- 
 solved by muriatic acid with separation of silicic acid, without 
 gelatinizing. Color, between lead-gray and iron-black. 
 
 (Compare KLIPSTEINITE, Mn 2 3 ,MnOSiO 2 ,H 2 0.) 
 
 PSILOMELANE (name alludes to its smooth botryoidal form 
 and black color). General formula =RO-f 4MnO 2 . Many va- 
 rieties ; compact; amorphous. B. B. fusible; reacts strongly 
 of manganese with borax. Boiled with muriatic acid it gives 
 off chlorine. Color, dark bluish-gray. H. 5-6. G. 3.7-4.7. 
 
 LIEVRITE (Ilvaite, Yenite), H 2 Ca 2 Fe 4 1?eSi 4 18 . 
 
 ALLANITE (Ce,La,Di,Fe,Ca) 3 (Al,Fe)Si 8 12 . 
 
 Both gelatinize completely with hydrochloric acid. Al- 
 lanite fuses easily and swells up. Xievrite fuses easily and 
 quietly. 
 
 PLATTNERITE (superoxide of lead, Schwerbleierz), Pb0. 2 . 
 Of adamantine lustre; spec, gravity, 9.3. Color, iron-black. 
 Streak, brown. B. B. with soda on charcoal yields a globule 
 of lead. 
 
 /S'mars^e(uranotantalite),(Fe,Y,UO^) 5 (Cb,Ta) < O 15 . Fuses 
 at 4-5 to a steel-gray mass. Lustre of surface of fracture 
 shining and submetallic. Color, velvet-black. Streak, dark red- 
 brown. 
 
 When the powdered mineral is fused with caustic potassa in 
 a silver crucible, and the mass afterwards extracted with water 
 and filtered, a green solution is obtained, which, when neu- 
 tralized with hydrochloric acid, yields a whitish precipitate. If 
 the latter is boiled with a sufficient quantity of fuming hydro- 
 
 * A name given by v. Leonhard to a mineral as yet imperfectly 
 known, and containing 14.9 per cent, of water. The analysis is by 
 Klaproth. It is mentioned by v. Kobell, and in Nan maim' s Miner- 
 alogie, Leipzig, 1871. Is not described in Dana's Syst. of Min., 5th 
 edit. ; but the closely related mineral Klipsteinite, which gives 9 per 
 cent, of water on ignition. 
 
MINERALS WITH METALLIC LUSTRE. 251 
 
 chloric acid and tinfoil for some minutes, and then diluted 
 with an equal volume of water, a sapphire-blue solution results. 
 
 Glass in. Infusible, or Fusibility above 5, and Non- 
 volatile, 
 
 Division 1. B. B. impart, in ever so small quantity, to the 
 borax bead in the oxidizing Jlame an amethystine color 
 of manganese. 
 
 The oxides of manganese belonging to this group dissolve 
 more or less easily in muriatic acid with evolution of chlorine 
 gas. They yield, when the powdered minerals are boiled down 
 with phosphoric acid to syrupy consistency, a beautiful violet 
 liquid, which becomes, when diluted with water, and then 
 shaken with some crystals of iron-vitriol, entirely discolored. 
 
 (Compare FRANKLINITE in the following division. It at- 
 tracts the magnetic needle.) 
 
 LITHIOPHORITE = MnO, CuO,CoO,Li J O,BaO,Al 2 O 3 ,MnO a , 
 H 2 O. Colors the flame carmine-red (lithia). With salt of 
 phosphorus gives reactions for copper and cobalt. 
 
 CREDNERITE (mangankupferoxide), Cu 3 M 2 9 . B. B. moist- 
 ened with muriatic acid it imparts to the flame a fine blue 
 color. The solution yields, with ammonia in excess, a brown 
 precipitate and an azure-blue liquid, which is not the case with 
 the following. 
 
 BRAUNITE (sesquioxide of manganese), 2MnO,MnO 2 + 
 MnSiO^. Color, dark brownish-black. Streak blackish, inclin- 
 ing to brown. Hardness G-G.5 (between orthoclase and quartz). 
 B. B. in a matrass affords none, or only traces of water. H. 6. 
 G. 4.7. 
 
 HAUSMANNITE (red oxide of manganese), 2MnO-f-IVInO 2 . 
 Color brownish-black. Streak reddish and chestnut-brown. 
 Hardness 5-5.5, between apatite and orthoclase. B. B. in a 
 bolt head affords no water. 
 
 MANGANITE (hydrated oxide of manganese), Mn 2 O 3 ,H 2 O. 
 Steel-gray to iron-black. Streak, dark reddish-brown. Hard- 
 
252 MINERALOGY SIMPLIFIED. 
 
 ness 4, between calcite and fluorspar. B. B. in a b'olt head 
 affords much water. 
 
 PSILOMELANE (compact oxide of manganese), (Mn, Ba, 
 K 2 ) 5 O 9 -f- Aq (compos, doubtful). Color, bluish to grayish- 
 black and blackish-gray. Streak, brownish black to black. 
 Hardness 5-6. B. B. in a bolt head it affords water. The 
 solution of most varieties in muriatic acid yields with sulphuric 
 acid a heavy precipitate of sulphate of barium. (At present 
 only found amorphous, but more generally diffused than any of 
 the ores of manganese.) 
 
 PYROLUSITE (polianite, peroxide of manganese), MnO a . 
 Color, iron-black, steel-gray. Streak, black. Hardness 2-2.5, 
 between rock-salt and calcite. B. B. in a bolt head it yields 
 none or only a trace of water. 
 
 (Compare Alabandine and Hauerite.) 
 
 Division 2 Are magnetic, or B. B. when heated on charcoal 
 perseveringly in the R. FL become so. 
 
 Lolingite. 
 
 Arsenopyrite. 
 
 In different varieties; imperfectly fusible, are distinguished 
 from the next following by evolving an arsenical odor B. B. on 
 charcoal. 
 
 HcBinatite (specular iron, red iron ore, Rotheisenerz), Fe 2 O 3 . 
 Distinguished from the following by its cherry- red streak and 
 its iron-black, steel-gray, or brownish-red color. Dissolves 
 slowly in muriatic acid. 
 
 Franklinite^ (Zn,Mn,Fe)O,(Mn,Fe) 2 O 8 , and 
 
 Magnetite (magnetic iron ore, Magneteisenerz), Fe 3 O 4 , 
 are strongly magnetic ; both are slowly dissolved in concen- 
 trated muriatic acid, by which the former evolves chlorine ; 
 the latter does not. Pulverized franklinite, boiled down with 
 phosphoric acid, yields a beautiful violet color; magnetite does 
 not. The color of both is iron-black. The streak of frank- 
 linite is reddish-brown, that of magnetite black. A similar 
 deportment to franklinite is shown by 
 
 Jacobsite (Mn,Mg)O,(Fe,Mn) 2 O 3 . Color, deep black. Is 
 
MINERALS WITH METALLIC LUSTRE. 253 
 
 magnetic, and occurs in distorted octohedrons. Its phosphoric 
 acid solution turns violet upon addition of nitric acid only after 
 heating. 
 
 Magnoferrite, or magnvsioferrite, MgO,Fe 2 O 3 . Soluble with 
 difficulty in hydrochloric acid. In the solution after the oxi- 
 dation of the protoxide of iron with chlorate of potash and its 
 precipitation with an excess of ammonia, phosphate of soda gives 
 a precipitate of ammonio-phosphate of magnesia in the filtrate. 
 H. 6-6.5. G. 4.5. 
 
 MENACCANITE (titanic iron, ilmenite, hystatite, Titan- 
 eisen, Kibdelophan, Iserin, etc.), (Ti, Fe) 2 O 3 . Influences 
 the magnetic needle, but is easily distinguished from the pre- 
 ceding by the following process : Pulverize and boil the 
 powder with concentrated muriatic acid, and filter ; the fil- 
 tered liquid boiled with tinfoil assumes gradually a fine blue or 
 violet color turning a pink-red when diluted. Streak, black. 
 Color, iron-black, inclining to steel-gray. H. 5-6. G. 4.5-5. 
 
 We may also boil the powder of menaccanite, at first with 
 cone, sulphuric acid, then evaporate to dryness and add to 
 the residue cone, hydrochloric acid and tinfoil. In this way 
 the mineral is more easily dissolved. Sometimes the hydro- 
 chloric acid solution boiled with tinfoil passes through the filter 
 with a brownish color, in which case it must again be boiled 
 with additional cone, hydrochloric acid and tinfoil, in order to 
 obtain a violet solution, turning to a rose-color when diluted. 
 
 (Compare rutile and arkansite, which through an admixture 
 of menaccanite frequently exhibit magnetic properties. Muri- 
 atic acid attacks them but slightly.) 
 
 LIMONITE (brown hematite, Brauneisenerz), Fe 2 O s ,3H 2 O. 
 The lustre in many varieties is submetallic ; is distinguished 
 from the preceding by its ochre-yellow streak. H. 5.5. G. 3.6-4. 
 
 SPHALERITE (Zincblende) (Zn, Fe)S. containing often- 
 times iron, and having a submetallic lustre, is recognized by 
 the fact that muriatic acid evolves sulphuretted hydrogen. 
 H. 3.5-4. G. 3.9-4.2. 
 
 Compare the following division : 
 22 
 
254 MINERALOGY SIMPLIFIED. 
 
 Division 3 Not included, but in some respects related to, the 
 preceding are : 
 
 CHROMITE (COLUMBITE AND NIOBITE) FERROILMENITE 
 CHROMITE (chromic iron, Chromeisenerz), FeO,Cr 2 O 3 , or 
 (Fe,Mg)0,( Al,Cr) 2 O 3 . In many varieties strongly magnetic, in 
 others only very feebly so. Hydrochloric acid has little effect on 
 it. Evaporated with phosphoric acid an emerald-green solution 
 is obtained ; those varieties containing oxide of manganese yield 
 a violet solution (manganese) which, agitated with crystals of 
 green vitriol, disappears while the green color of oxide of 
 chromium appears. B. B. alone it remains unchanged. 
 Borax and phosphorus slowly and perfectly dissolve it, form- 
 ing beads of a fine emerald green when cold. Color, iron-black, 
 pitch-black. Streak , yellowish-brown. H. 5.5. G. 4.3. 
 
 Some varieties of Cassiterite, SnO 2 , have a metallic lustre. 
 B. B. on charcoal heated with cyanide of potassium, metallic 
 tin is obtained. 
 
 MOLYBDENITE (sulphuret of molybdenum, Molybdanglanz), 
 MoS 2 (H. 1-2. G. 6.2), and 
 
 GRAPHITE (carburet of iron and black lead), C, are both 
 very soft and leave a gray trace on paper. H. 1.5. Color of 
 the former is lead-gray inclining to red ; of the latter, iron- 
 black, steel-gray. B. B. molybdenite, confined with the 
 forceps, colors the flame light green ; with soda it gives hepar. 
 Heated in a platinum spoon with nitre, it explodes with evolu- 
 tion of light and heat. The mineral boiled down with con. nitric 
 acid, furnishes a white mass (molybdenum trioxide) which, 
 when boiled with caustic potash, yields a partial solution that 
 upon being acidulated with hydrochloric acid, and afterwards 
 diluted, assumes, when stirred with a strip of tin, a fine blue 
 color. 
 
 A splinter of graphite, held in forceps made of zinc, becomes 
 covered quickly with copper when dipped into a solution of 
 sulphate of copper. 
 
 PEROFSKITE, CaTi0 3 , as also some RUTILK, TiO 2 , with 
 
MINERALS WITHOUT METALLIC LUSTRE. 255 
 
 sub-metallic lustre. When the fine powder of these minerals 
 is fused together with caustic potash, water added, and the 
 solution evaporated after addition of an excess of HC1 and a 
 piece of tinfoil, the liquid becomes violet-colored, and, on dilu- 
 lution with water, rose-red. (Reaction of TiO 2 .) Perofskite 
 crystallizes in cubes. 
 
 (Compare rutile and brookite.) 
 
 IRIDOSIMINE, Ir, Os, Rh, Ru. Fused in a matrass with nitre 
 evolves the peculiar odor of oxide of osmium. Not perceptibly 
 attacked by Bx and S. Ph. or aqua regia. Color, tin-white. 
 Streak, gray. H. 6-7. G. 19.3-21.1. 
 
 .TANTALITE, Fe(Mn)Ta,O 6 , and 
 
 COLUMBITE, FeCb 2 (Ta 2 )O 6 ; 
 
 YTTROTANTALITE, (Fe, Ca, Y) 2 (TaCb) 2 O 7 . 
 
 The color of these minerals is iron-black. Yttrotantalite 
 loses its color before the blowpipe, and becomes yellowish or 
 white ; that of the others remains unchanged. Acids affect 
 them but little. If tantalite and columbite are powdered, fused 
 with caustic potash in a silver crucible, dissolved in water, and 
 filtered, a precipitate is formed with hydrochloric acid, which, 
 boiled with dilute sulphuric acid, becomes white ; on the addi- 
 tion of zinc the precipitate from the columbite becomes intensely 
 blue in the hot solution, and retains this color on the addition 
 of water for a considerable time. The precipitate from tanta- 
 lite is lighter colored, and loses its color quicker with water. 
 
 (Compare polycrase and aeschynite.) 
 
 URANITK, U 8 O 4 . Color, usually velvet-black; lustre, greasy; 
 partially soluble in nitric acid to a yellow liquid ; the solution 
 gives a sulphur-yellow precipitate with ammonia. Boiled with 
 phosphoric acid gives an emerald-green solution. G. 6.4-7. 
 
256 MINERALOGY SIMPLIFIED. 
 
 GROUP II. MINERALS WITHOUT METALLIC 
 LUSTRE, 
 
 Class i. Easily Volatile or Combustible, 
 
 NATIVE-SULPHUR, S. H. 1.5; G. 2. Completely vola- 
 tile ; burns with a blue flame and evolution of sulphur dioxide, 
 SO 2 . Color, sulphur-yellow, honey-yellow, and brown from 
 impurities. 
 
 REALGAR, As 2 S 2 . Arsenic disulphide, orange-yellow. H. 
 1.5-2. G. 3.5. 
 
 ORPIMENT, As 2 S 3 . Arsenic trisulphide (auripigmentum), 
 yellow sulphide. Both fuse easily and volatilize with emission 
 of arsenical fumes. Soluble in potassa. HC1 precipitates from 
 this solution lemon-yellow flocks. 
 
 ARSENITE (arsenious acid, white arsenic), As 2 O 3 . B. B. 
 on ch. with soda emits an arsenical odor, and in a bolt head 
 gives a white crystalline sublimate. Color, white. H. 1.5. 
 G. 3.8. 
 
 VALENTINITE (oxide of antimony, Weisspiessglanzerz, 
 Germ.), Sb 2 O 3 and 
 
 KERMESITE (pyrostibite, red antimony, Antimonblende, 
 Germ.), 2Sb 2 S 2 -f Sb 2 O 3 . B. B. fuse and evaporate easily, 
 coating the charcoal white. Are insoluble in water. Valen- 
 tinite dissolves readily in muriatic acid without evolution of 
 gas. Kermesite (pyrostibite) is partly soluble with the 
 escape of sulphide of hydrogen (H 2 S). The powder of the 
 first, treated with potassa, does not change color; that of the 
 second, immediately assumes an ochre-yellow. The former is 
 white, the latter cherry-red. 
 
 SENARMONTITE (Sb 2 O 3 ), has the same composition as valen- 
 tinite, but crystallizes in the isometric system, whilst valentinite 
 is trimetric. 
 
 SAL AMMONIAC (ammonium chloride, Salrniak, Germ.), 
 NH 4 C1, and 
 
 MASCAGNITE (hydrous ammonium sulphate), (NH 4 ) 2 SO 4 
 
MINERALS WITHOUT METALLIC LUSTRE. 2o / 
 
 -[-Aq. B. B. volatilize with abundant fumes; the first without 
 fusing; the second fusing and puffing up at the first applica- 
 tion of heat. Both dissolve easily in water. The solution of 
 sal ammoniac gives no precipitate with chloride of barium. 
 Mascagnite yields a heavy precipitate of sulphate of barium. 
 When treated with potassa liquor they both evolve.an ammo- 
 niacal odor. Color, white. 
 
 CINNABAR (sulphuret of mercury, Zinnober, Germ.), HgS. 
 Streak, red. When the mineral powder is ground together 
 with iron powder, wrapped in copper foil, and heated in a 
 closed tube, metallic mercury sublimates, and the residue 
 yields with hydrochloric acid, hydrosulphuric acid (SH 2 ). H. 
 2-2.5. G. 9. 
 
 CALOMEL (horn quicksilver, Mercurous chloride), HgCl. 
 B. B. in a bolt head with soda yield metallic mercury. For 
 trial not too little of the substance must be taken. The 
 mixture may be wrapped up in thin paper, and introduced 
 into the middle of an open tube, and the flame applied to this 
 spot until the glass begins to melt. The metal may be col- 
 lected in globules on the sides of the tube by means of a feather. 
 Calomel is white, but potassa . renders it black, mercurous 
 oxide (Hg 2 O) being produced. The alkaline solution, acidu- 
 lated with nitric acid, after being filtered off, yields with nitrate 
 of silver a heavy precipitate of chloride of silver. H. 1.5. 
 G. 6.5. 
 
 COTUNNITE* (Chlorblei, Germ.) Chloride of lead, PbCl 2 . 
 
 Color, yellowish-white. Streak, white. May be scratched 
 by the nail. Soluble in about 22 parts of hot water. B. B. 
 partly volatile. Fuses on charcoal readily, and deposits a 
 white coating, the inner edge of which is tinged yellow from 
 oxide of lead. With soda on coal gives lead globules. See 
 mineral coals in the appendix to ores. 
 
 * Dana^Syst. of Min., 5th edit., p. 117 ; also, Brush's Determinat. 
 Min., etc., p. 72. 
 
 22* 
 
258 MINERALOGY SIMPLIFIED. 
 
 Class ii. Fuse easily between 1 and 5, and volatilize 
 only partially or not at all. 
 
 Part A. B. B. FUSED WITH SODA ON CHARCOAL YIELD A 
 
 METALLIC GLOBULE, OR, FUSED ALONE IN THE R. F., 
 FORM'A MASS* WHICH ACTS ON THE MAGNETIC NEEDLE. 
 
 Division 1. -7?. B. yield with soda or soda and borax together 
 a silver globule. Those decomposable by nitric acid yield, 
 when this solution is treated with hydrochloric acid, a 
 white precipitate of chloride of silver, which B. B. is 
 easily reduced on charcoal to metallic silver. (It is well 
 to fuse the globule once more with borax, to obtain the 
 silver entirely pure and ductile.} 
 
 Proustite. Light red, silver ore. 
 
 Lichtes Rothgiiltigerz, Germ., Ag 3 As8 3 (or 3Ag 2 S -j- As 2 $ 3 ), 
 and 
 
 Pyrargyrite (dark-red, silver ore. Dunkles Rothgultigerz, 
 Ag 3 SbS 3 (or 3Ag 2 S-|-Sb 2 S 3 )). May be distinguished from 
 the following by their cherry-red streak. B. B. the first 
 evolves the strong odor of arsenic ; the second coats the coal 
 with the fumes of antimony. Either mineral reduced to 
 powder and heated with potassa assumes a black color, and is 
 partly decomposed and dissolved. If this potash solution be 
 neutralized with muriatic acid, proustite will form lemon-yellow 
 flocks of sulphuret of arsenic, pyrargyrite, orange flocks of 
 sulphuret of antimony. Color of the former is cochineal-red ; 
 of the latter dark-red to blackish lead-gray. A similar 
 behavior is shown by proustite. 
 
 Xanthoconite (Xanthokon), 3AgS -f As 2 O 5 ) -f 2(3AgS -f 
 As 2 S 3 ) (Da).| Color, dull red to clove-brown. Crystals, 
 orange-yellow on the edges by transmitted light. Streak, 
 powder yellow. Brittle qualities which readily distinguish it. 
 
 * All minerals with non- metallic lustre, which emit an arsenical 
 odor before the blowpipe belong to this class, except pharmacolite. 
 \ According to Brush, Ag 9 As 3 S 10 . Determin. Min., etc., p. 72. 
 
MINERALS WITHOUT METALLIC LUSTRE. 259 
 
 (Compare miargyrite, AgSbS 2 (or Ag 2 S-f-Sb 8 S 2 ), which 
 sometimes resembles very much the pyrargyrite. The specific 
 gravity of the former is 5.2, that of the latter 5.7.) 
 
 Cerargyrite (Kerargyrit, Horn Silver, Silberhornerz), 
 AgCl. 
 
 lodyrite (iodargyrite, lodsilber, Germ.), Agl, and 
 
 JEmbolite, Ag (ClBr) are ductile, and maybe hammered out. 
 In closed tube fused with bisulphate of potassa, the following 
 phenomena take place. The bead of Agl* swimming in the 
 flux is dark, almost black, whilst hot, turning by the gradual 
 cooling process to red. The bead of AgCl, when hot, has a 
 pale hyacinth-red color; that of AgBr an intense garnet-red 1 , 
 both turning to yellow when cold. When these silver com- 
 pounds are mixed with zinc filings in a cylindrical glass, and 
 next treated with very dilute sulphuric acid, they assume after 
 a while, a blackish color. If the solution is poured off, some 
 starch added, and a few drops of potassic permanganate solu- 
 tion (MnKO 4 ) acidulated with cone. HC1, the liquor of iody- 
 rite shows a blue or bluish-black color, that of embolite a 
 yellow color, that of cerargyrite is not colored at all. When 
 the above solution of embolite (without starch solution) is 
 treated with solution of MnKO 4 , acidulated with HC1, then 
 mixed with ether, and diligently stirred, the layer of ether 
 assumes a yellow color, whilst the liquor beneath is colorless. 
 This department is very characteristic for bromine after we 
 have convinced ourselves that no iodine is present, since that 
 body yields similar reactions. Chlorine produces under these 
 circumstances no coloring of the ether. 
 
 SELBITE (carbonate of silver), AgCO 3 , dissolves easily in 
 nitric acid, with effervescence. Color, ash-gray inclining to 
 black. Streak has metallic lustre. According to Walchner 
 it is only a mixture ; and according to Sandberger, one of 
 Selb's original specimens, examined under the lens, showed to 
 
 * lodyrite by this fusion process gives off iodine vapors ; and embolitv 
 bromine vapors. 
 
2GO MINERALOGY SIMPLIFIED. 
 
 contain earthy argentite, besides dolomite and silver, and all 
 parts afforded a sulphur reaction.* 
 
 Division 2. B. B. 'with soda yield a lead globule. The 
 compounds of this group are soluble in nitric acid ; zinc 
 precipitates metallic lead from the solution ; sulphuric 
 acid forms a heavy white precipitate of sulphate of lead. 
 
 When boiled with caustic potash solution a liquid is obtained, 
 which, either with chromate of potassium alone, or after treat- 
 ment with some acetic acid, gives an orange or yellow precipi- 
 tate of chromate of lead. 
 
 BINDHEIMITE (Bleinierc), Pb 3 Sb 2 O 8 -f- 4Aq, and 
 
 NADORITE, PbSb g O 4 + PbCl 2 . 
 
 B. B. on charcoal both yield metallic lead and coatings of 
 lead and antimony. Bindheimite affords water in a closed 
 tube. Nadorite fused in a salt of phosphorus bead, which 
 has previously been saturated with oxide of copper, colors the 
 flame blue (chloride of copper). 
 
 MiMETiTE,MiMETisiTE(leadarsenate), 3Pb 3 As 2 O 8 + PbCl . 
 B. B. on coal is reduced ; evolves a strong arsenical odor. 
 Confined with the forceps and fused in the external flame, 
 some varieties crystallize like pyromorphite (phosphate of lead). 
 Color, yellowish-green, brownish. Closely related to this 
 mineral is 
 
 HEDYPHANE (arsenate and chloride of lead with phosphate 
 of lime), 3(l > b,Ca) 3 As 2 O 8 -i- (Pb,Ca)Cl 2 . B. B. alone on 
 coal gives arsenical odors and, containing phosphate of cal- 
 cium, gives the reaction for phosphoric acid. 
 
 PYROMORPHITE, 3Pb 3 P 2 O 8 -f PbCl 2 . B. B. is not re- 
 duced alone on coal ; fuses to a bead which, after cooling, is 
 distinctly crystalline. The nitric acid solution gives, when 
 boiled with molybdate of ammonium, an ochre-yellow precipi- 
 tate of phospho-molybdate of ammonium. Color, generally 
 green, of different shades; also brown and white. H. 3.5-4. 
 G. 6.5-7. 
 
 * Dana, Syst. of Min., fifth ed., p. 804. 
 
MINERALS WITHOUT METALLIC LUSTRE. 261 
 
 i'M (Mennige), Pb s O 4 = PbO 2 -f 2PbO. 
 
 CROCOITE (crocoisite, cbromate of lead), PbCrO 4 . 
 
 PHCENICOCHROITE, PHONICITE (melanochroite, sesqui- 
 chromate of lead), Pb 8 CrO 6 == 2PbOO 4 -j- PbO. 
 
 DECHENITE (araeoxene, PbZn) V 2 O 6 . Have a red color. 
 B. B. Crocoisite, pboenicite, and dechenite, added in small 
 quantities, impart to a borax bead an emerald-green color 
 which, with dechenite, turns, in the oxidizing flame, gradually 
 light olive-green, then yellow, and next disappears. They are 
 soluble in boiling muriatic acid without effervescence, with 
 separation of chloride of lead, and form an emerald-green 
 liquid.* This liquid concentrated by the addition of alcohol, 
 and poured off from the separating chloride of lead, assumes 
 upon dilution with water a sky-blue color if dechenite is 
 present, with the others it remains green. Crocoite yields 
 with phosphoric acid at first a reddish-yellow solution which,- 
 when concentrated, turns emerald-green, and diluted with 
 water loses it entirely. Uechenite treated thus produces, not 
 a green, but a yellow solution. Minium gives with borax a 
 yellow bead which becomes colorless on cooling. It does not 
 change the color of muriatic acid. The streak powder of 
 crocoite and dechenite is ot^nge ; of phocnicite, brick-red. 
 
 LINARITE (cuprous sulphate of lead, Kupferbleispath), 
 1*1)3 -|- CH is characterized by its deep azure-blue color. 
 Nitric acid, at the commencement of heating, discolors it, 
 while sulphate of lead is precipitated. 
 
 CERUSSITE (carbonate of lead, Weissblcirz), PbCO 3 . 
 
 LANARKITE (sulphato-carbonate of lead), PbSO 4 -{- PbCO 3 . 
 
 PHOSGENITE (Hornblei, Kerasin), PbCO 3 -j- PbCl 2 are dis- 
 solved by nitric acid with effervescence. Lanarkite only 
 incompletely. The solution of phosgenite gives, with nitrate 
 of silver, a heavy precipitate of chloride of silver, that of 
 lanarkite with nitrate of barium a precipitate of sulphate of 
 barium, that of cerussite affords none with either reagent. 
 
 * Provided, that sufficient HC1 was present and the boiling con- 
 tinued long enough. 
 
262 MINERALOGY SIMPLIFIED. 
 
 Color of cerussite, white, of lanarkite, greenish-white to yellow- 
 gray, of phosgenite, white. Similar to lanarkite is 
 
 LEADHILLITE, PbSO 4 + 3PbCO 3 , crystallizes in the ortho- 
 rhombic system. Of the same composition is 
 
 Siisanmte, PbSO 4 -f 3PbCO 3 , crystallizing in the hexagonal 
 system (rhombohedrons). Lanarkite crystallizes in the mono- 
 clinic system. 
 
 ANGLESITE (sulphate of lead), PbSO 4 , soluble in nitric 
 acid with difficulty. B. B. with soda yields hepar and is re- 
 duced to metallic lead. H. 3. G. 6.1-6.3. 
 
 WULFENITE (molybdate of lead), PbMo0 4 . Boiled with 
 concentrated muriatic acid is dissolved with separation of 
 chloride of lead, forming a green liquid, which diluted some- 
 what and stirred with tinfoil, assumes immediately a blue color. 
 Boiled with concentrated phosphoric, acid, a pale green solu- 
 tion is obtained, which, when diluted with four times its bulk 
 of water, sometimes becomes turbid. If now this liquid is 
 agitated with a very little iron powder, it turns blue, with 
 more iron olive-green (at a common temperature)! 
 
 After the mineral powder has been heated in a porcelain dish 
 with concentrated sulphuric acid, the addition of alcohol, on cool- 
 ing, colors the liquor, especially at^he sides of the dish, a fine 
 blue. Color, honey, wax, and orange-yellow. H. 3. G. 6.9. 
 
 STOLZITE (tungstate of lead, schuletine, Wolframsaures 
 Bleioxyd), PbW0 4 . Boiled with phosphoric acid, like the pre- 
 ceding solution, does not grow turbid when diluted and the 
 liquid turns, with a little iron powder, a beautiful blue, but not 
 before heat is applied. A greater addition of iron-powder does 
 not alter the color. Sulphuric acid colors the powder lemon- 
 yellow, while the acid remains colorless. Color, yellow, 
 yellowish-brown. H. 3. G. 7.9. 
 VAUQUELINITE (chromate of lead and copper), Pb 2 CuCr 2 O 9 . 
 
 Vanadinite, Vanadinbleierz, 3Pb 3 V 2 O 8 -j-PbCl 2 . 
 
 Eusynchite* P 
 
 * A variety of Dechenite. See Brush Manual of Determinative 
 Mineralogy, pp. 73 and 74. 
 
MINERALS WITHOUT METALLIC LUSTRE. 263 
 
 B. B. they impart to borax glass an emerald-green color 
 which remains so with vauquelinite even in the O. F. while 
 the others turn yellow. They are soluble in nitric acid. The 
 solution of vauquelinite is green, that of vanadinite and eusyn- 
 chite, yellow or colorless. The solutions of vauquelinite and 
 eusynchite yield with nitrate of silver no precipitate, that of 
 vanadinite gives a precipitate or becomes turbid. All three pro- 
 duce with concentrated hydrochloric acid upon the addition of 
 alcohol, an emerald-green solution which concentrated until 
 the PbCl separates, turns, upon the addition of water, sky-blue, 
 by vanadinite and eusynchite, while it remains green with 
 vauquelinite. Color of the last is blackish to olive-green ; 
 that of vanadinite, brown or yellowish ; that of eusynchite 
 yellowish red to ochre-yellow. Vanadinite crystallizes in the 
 hexagonal, and the chemically related 
 
 Descloizite, Pb V 2 7 , cryst in the orthorhombic system. 
 
 (Compare plumbo-resinite, Bleigummi, Germ.) 
 
 Closely related to vauquelinite are : 
 
 Laxmanm'te* (PbCu) 6 (P,Cr) 4 17 and 
 
 Phosphochromite. 
 
 Their nitric acid solution reacts with molybdate of ammo- 
 nium, of phosphoric acid, and when gently heated, forms after a 
 lapse of time a yellow precipitate. t 
 
 Division 3. Moistened with hydrochloric acid they communi- 
 cate to the blowpipe flame a transient blue color ; with 
 nitric acid, form a sky-blue or a green solution^ which 
 becomes azure-blue by the addition of ammonia in excess. 
 
 The compounds of oxide of copper belonging to this class are 
 principally so much decomposed by boiling with potassa, that 
 their acids combine with the potassa. 
 
 * Held by Beresqfto be a phosphocliromite. See Text-Book of Min- 
 eralogy, p. 3U4. E. S. Dana's. 
 
 f The yellow precipitate (often termed phospho-molybdate of am- 
 monium) contains molybdic acid, ammonia, water, and about 3 per 
 cent, of phosphoric acid. Is soluble in phosphoric, and other acids. 
 
264 MINERALOGY SIMPLIFIED. 
 
 Section i. B. B. evolve a strong arsenical odor (and generally give 
 alone on coal a white, brittle metallic glolule of arsenical 
 copper}. Are of a green color. 
 
 Chenevixite, (Pe,Cu 3 ) 2 As 2 O n + 3Aq. 
 
 Fuses to a black magnetic slag. The following yield no 
 magnetic product : 
 
 Bayldonite, ( CuPb) 4 As 2 O 9 -f 2 Aq. 
 
 The nitric acid solution affords, with sulphuric acid, a white 
 precipitate of sulphate of lead. 
 
 Olivenite (prismatic arsenate of copper), Cu 5 As 2 O 9 -f-Aq. 
 B. B. in the forceps affords on cooling a blackish, radiating crys- 
 talline mass, the surface of which is covered with prismatic 
 crystals. It yields but little water (4 per cent.) in a bolt head. 
 Color, olive-green, passing into leek or blackish-green. A 
 similar mineral with 7 per cent, of water is : 
 
 Abichite (clinoclasite) Cu 6 As 2 O n -f3Aq. 
 
 Tyrolitz (Kupferschaum), Cu 5 As 2 O 10 -j-9Aq. 
 
 Chalcophyllite (copper mica, Kupferglimmer) Cn 8 As 2 O 13 -f 
 7Aq. 
 
 B. B. decrepitate violently, and in a bolt head afford much 
 water. The second is soluble in ammonia without residue ; 
 the first with separation of carbonate of calcium. Both are per- 
 fectly cleavable in one direction. Tyrolite is apple-green and 
 verdigris-green. Chalcophyllite emerald-green, grass-green. 
 
 Closely allied to these is : 
 
 Conichalcite, (Konichalcit) 2(Cu,Ca) 4 (As,P,V) 2 O 9 + 3Aq. 
 
 Reniform and massive. Fraction splintery brittle. Color, 
 pistachio-green to emerald-green. Some vanadic acid re- 
 places part of the phosphoric. The fused assay has an alkaline 
 reaction. 
 
 LIROCONITE (Linsenerz), (Cu 8 Al) J{ (As,P) 2 11 -f 12Aq. 
 
 B. B. does not crepitate, and heated slightly, assumes a 
 smalt-blue color. In ammonia it is soluble with separation of 
 white flocks. Contains a large quantity of water, and loses by 
 ignition 22 per cent, of its weight. Color, sky-blue, also 
 green. 
 
MINERALS WITHOUT METALLIC LUSTRE. 205 
 
 EUCHROITE, Cu 4 As 2 O 9 +7Aq, and 
 
 KiuxiTE, Cu.As 2 O 10 -f 2Aq, are distinguished principally 
 by their loss of weight on ignition. The former loses 18^ per 
 cent., the latter 5 per cent, of water. Color, emerald-green. 
 Amorphous. A mineral similar to the preceding is : 
 
 Cornwallite, Cu 5 As 2 O IO + 3Aq==Cu 3 As 2 O 8 + 2H 2 Cu 2 O 2 + Aq. 
 
 Amorphous, with about 13 per cent, of water. Color, green 
 (emerald to verdigris green). 
 
 Section ii. B. B. evolve no arsenical odor, but generally give 
 alone on c#al a malleable globule of copper. 
 
 ATACAMITE (chloride of copper), CuCl 2 -4-3II 2 CuO a , with- 
 out being moistened with muriatic acid communicates to the 
 blowpipe flame a fine blue color, and thereby may be easily dis- 
 tinguished from all similar minerals. The nitric acid solution 
 yields with nitrate of silver, white chloride of silver. Color, 
 leek, blackish-olive, emerald-green. H. 3.5. G. 4.25 
 
 Closely allied are : 
 
 TaUingite, CuCl 2 -J;4H a CuO 2 -f iAq. Color blue to green. 
 
 Percylite, (Pb,Cu) (C1 2 ,O) + Aq. Color sky-blue. 
 
 Both color the flame blue like the preceding. 
 
 Percylite dissolved in nitric acid yields with sulphuric acid 
 a white precipitate of sulphate of lead. 
 
 Nantokite, CuCl. Color when fresh, white ; colors the flame 
 blue and yields no water in a closed tube. 
 
 (Compare Atlasite, 7Cu 2 CO 4 +CuCl a + 10 Aq.) 
 
 Chalcanthite (blue vitriol, sulphate of copper), Cu'SO 4 -l-5Aq. 
 
 jBroc&afcVeCu 4 SO 7 + 3Aq. and Corc.Uite (Covellin, Kupfer- 
 indif/) CuS, 
 
 B. B. with soda give hepar, which is not the case with the 
 remaining minerals of this division. Blue vitriol dissolves 
 easily in water. Color, sky-blue. The second and third are 
 insoluble in water, but soluble in nitric acid. The solutions 
 of the first two give, with nitrate of barium, a heavy precipitate 
 of sulphate of barium. Covellite in the exterior flame burns 
 and emits the odor of sulphurous acid. It is not reduced until 
 23 
 
2GG MINERALOGY SIMPLIFIED. 
 
 ;ill the sulphur is expelled by roasting. Color, indigo blue- 
 blackish. Brochantite exhibits no such deportment. Color, 
 emerald green. 
 
 Related to brochantite is : 
 
 Lanyite,CufiO ( .-}-4Aq. Color, greenish-blue. Brochantite 
 contains 12, langite 16 per cent, water. 
 
 Pisanite* FeO, CuO, SO 3 -f 7H S O; or a copperas with three- 
 fifths of the iron replaced by copper. In concretionary and 
 stalactitic forms, color light-blue. Occurs with chalcopyrite 
 at a copper mine in the interior of Turkey. Gives B. B. with 
 fluxes reactions for copper, otherwise like copperas. 
 
 CUPRITE (red oxide of copper, Bothkupfererz) Cu 2 O, and 
 
 BLACK COPPER ORE (Kupferschwaerze), CuO, are easily 
 and quietly dissolved in acids. The concentrated solution of 
 the former in muriatic acid gives, when diluted with water, a 
 white precipitate (of protochloride of copper) ; with potas.su, an 
 ochre-yellow deposit. The solution of the black oxide of cop- 
 per, with water, does not give any; with potassa, a bluish pre- 
 cipitate. Color of the first is cochineal -red ; of the second, 
 brown or brownish-black. The last mineral generally slightly 
 effervesces in acids owing to impurities. 
 
 Pure black oxide of copper constitutes : 
 
 Tenosite, melaconite, CuO, of dark steel-gray color, in thin 
 laminre transparent, brown. 
 
 MALACHITE (green carbonate of copper), Cu 2 CO 4 +H 2 O. 
 
 AZURITE (blue carbonate of copper), Cu 3 C 2 O 7 -fH 2 O, and 
 
 MYSORINE (anhydrous carbonate of copper), CuC0 3 , dissolve 
 in nitric acid with effervescence, caused by the escape of carbonic 
 acid. The first two in a matrass afford a large amount of 
 water ; the third only a little or no water. Color of the first 
 is always green ; the second blue, usually sky-blue ; the third 
 brownish-black. 
 
 Aurichalcite, (Zn, Cu) 3 CO 5 + 2Aq. 
 
 Buratite (according to J. D. Dana identical with the former, 
 System of Min., 5th ed., p. 712). 
 
 * Daua's System of Min., 5th ed., p. 646-47. 
 
MINERALS WITHOUT METALLIC LUSTRE. 2<>7 
 
 B. B. Give with soda on charcoal a zinc coating. Atlasite, 
 Cu 2 CO H -fCuCl 2 -f-10Aq. 
 
 The nitric acid solution gives with nitrate of silver a precip- 
 itate of chloride of silver. 
 
 LIBETHENITE (phosphate of copper), Cu 4 P 2 O 9 -|-H 2 O, and 
 
 Lunnite (phosphochalcite, pseudomalachite), Cu 6 P 2 O a -}- 
 3H 2 O. 
 
 Easily and quietly soluble in nitric acid. The solution 
 yields with molybdate of ammonia a yellow precipitate (P 2 O 5 ). 
 Color of libethenite dark olive-green, .when ignited loses 7 
 percent, of water ; color of lunnite dark green, loses 14 per 
 cent, of water by ignition. 
 
 A similar deportment is shown by 
 
 Eldite* (prasine), Cu 3 P 2 O 8 -f 2H 2 CuO 2 -f- Aq. Ramm. 
 Cleavage in one direction perfect. Color, dark olive-green. 
 
 Tagilite, Cu 4 P 2 <) 9 -f 3Aq = Cu 3 P 2 O 8 + H 2 CuO 2 + 2Aq. 
 Color, emerald-green. Lose on ignition 9 to 10^ per cent, of 
 water. 
 
 Torbernite (Chalcolit, Kupfer-Uranit, Germ.), CuU 2 P 2 O 12 
 _j- 8Aq*= 2(UO 2 ) 3 P/) 8 + Cu 3 P 2 () 8 + 24Aq. The solution in 
 nitric acid has a yellowish-green color, and forms, with ammo- 
 nia in excess, a blue liquid, with a bluish-green precipitate; 
 by this it can be distinguished from the preceding minerals, 
 since the precipitates which they form with ammonia are 
 almost entirely soluble in excess of ammonia. The solution 
 gives, when warmed with molybdate of ammonium, a yellow 
 precipitate;. Color, emerald-green. In one direction perfectly 
 cleavable. 
 
 Volborthite, (CuCa) 4 V 2 O -f H 2 O. Melts very easily, 
 yielding with soda a copper globule. Its powder, ground with 
 soda and heated to fusion in a platinum crucible, furnishes a 
 mass which, extracted witli boiling water, produces, upon 
 addition of hydrochloric acid and proper evaporation, an eme- 
 rald-green liquor, changing to a sky-blue when more water is 
 added. Color of the mineral yellowish-green. 
 
 * Pseudomalachite, Cu^On-p- 3Aq. Brush's Determ. Miu., p. 75. 
 
2G8 MINERALOGY SIMPLIFIED. 
 
 Division 4. B. B. impart to a borax lead a fne sappJtirc- 
 blue color. (Cobalt.) 
 
 Erythrite (cobalt bloom, Kobaltbluethe), Co 3 As 2 O 8 + 8Aq. 
 B. B. in a matrass affords water and becomes smalt-blue. 
 Dissolves in muriatic acid to a rose-red liquid. Color, carmine- 
 peach, rose-red. 
 
 ANN ABERGITE, NICKELBLUETIIE (Nickelocker), Ni 3 As. 2 O 8 -f- 
 8Aq (always containing oxide of cobalt). B. B. in a matrass 
 yields a large quantity of water. Its solution in muriatic or 
 nitric acid is of a green color. Ammonia gives a greenish 
 precipitate soluble in excess to a sapphire-blue liquid. Color, 
 fine apple-green. 
 
 Heterogenite, (CoO -f 2Co 2 O 3 ) -f 6Aq.) Soluble in IIC1 
 with evolution of chlorine, colors the flame green. Color, black, 
 red, brown. 
 
 Division 5 Fused B. B. in the forceps or on coal in the 
 reduction flame, yield a black mass which acts upon the 
 magnetic needle (this includes none contained in the pre- 
 ceding divisions). 
 
 In order to discover the magnetism of a mineral it is well 
 to use large masses of such as fuse easily, and to expose them 
 for some time to the reduction flame. 
 
 Section i. Evolve when fused upon coed strong arsenical odor. 
 
 PITTICITE (Pittizit, iron sinter, Eisensinter). Composi- 
 tion uncertain ; contains As. 2 4 1?e0 3 S0 3 H 2 0. 
 
 PIIARMACOSIDERITE (beudantite, cube ore, Wuerfelerz), 
 Fe 4 As 6 27 + 15Aq, and 
 
 SCORODITE (Skorodit), eAs 2 Oj-f 4Aq. B. B. fuse easily to 
 a magnetic globule. In potassa the powder immediately 
 assumes a reddish-brown color. The last two are found crys- 
 tallized, the former one in the isometric (or cubic), the latter in 
 trimetric (or rhombic) system. Their color is green of dif- 
 ferent shades. Iron sinter is amorphous. Lustre, opalescent 
 or vitreous. Color, brownish, blood-red, also white. 
 
MINERALS WITHOUT METALLIC LUSTRE. '200 
 
 ARSENIOSIDERITE (atsenocrocite), (Ca 3 Fe)As/) 8 -l- H^FcOg. 
 Fibrous, of silky lustre, and brownisli-yellow color. 
 
 MORENOSITE (pyromeline, nickel vitriol), NiSO 4 -{- 7Aq. 
 Light blue-green; mostly soluble in water; with caustic 
 ammonia in excess it yields a blue liquid. (Sometimes con- 
 tains arsenic.) 
 
 Section ii. Soluble in HCl without perceptible residue, and without 
 gelatinizing. (Evolve B. B. no arsenical odor when fused on 
 Ch.) 
 
 Ludwigite.* Comp. R 4 FB 2 0, . Contains Mg, Fe, 3?e (von 
 Kob.) 
 
 Sussexite.* General formula R 2 B 2 O 5 + Aq = (Mn, Mg) 2 
 B 2 5 -\- H 2 O. Both give the boric acid reaction with sulphuric 
 acid and alcohol. B. B. sussexite imparts a violet color to the 
 hot borax bead (oxide of manganese). 
 
 Rabdionite (Cu, Mn, Co) (Fe, Mn)0 4 . B. B. gives much 
 water in a closed tube (13 p. c.), and colors the borax bead 
 blue. Soluble in strong HCl with evolution of chlorine. 
 Soluble in phosphoric acid to a violet fluid. Color, black. 
 
 Pettkoite (Fe 3 , Fe) S 3 12 . B. B. gives little or no water in the 
 closed tube (1 J p. c.), is soluble in water. Chloride of barium 
 gives a white precipitate of sulphate of barium. Color, black. 
 Streak, dirty-green. 
 
 Melanterite (copperas, iron vitriol). FeSO 4 -f 7 Aq, and 
 
 BOTRYOGEN (red iron vitriol), (Fe, Mg) Fe 2 S 4 16 + 12Aq. 
 B. B. intumesce strongly, and in the reduction flame fuse to a 
 magnetic slag. Copperas is entirely soluble in water. Botry- 
 ogen leaves a yellow residue of peroxide of iron. The solu- 
 tion gives with chloride of barium a heavy precipitate of 
 sulphate of barium. With ammonia it forms a greenish pre- 
 cipitate, which exposed to the air changes to a brownish-red. 
 
 * According to Brush (Determ. Min., p. 82), ludwigite is only a 
 sub-species of sussexite. See, also, E. S. Dana's Textb., p. 358. 
 
 23* 
 
270 MINERALOGY SIMPLIFIED. 
 
 Color of botryogen, ochre-yellow to red. Streak, yellow. 
 Melantcr'de is green. 
 
 A deportment similar to botryogen is exhibited by 
 
 Coguimbite, J?eS 3 12 -f 9Aq. 
 
 Roemerite, (Fe, Zn)$e8 4 O M -f l^Aq (i s yellowish-brown). 
 
 Jarosite, K^e^O^ -f- 6Aq. 
 
 Fibroferrite (stypticite), FeS 2 9 + lOAq. 
 
 All of these are yellow. Fibroferrite occurs in fibres of a 
 silken lustre and pale yellow color. Their powders are imme- 
 diately turned brownish-red by solution of potassa (Fe 2 O 3 ). 
 Melanterite at first greenish, then black. 
 
 Here belong (likewise furnishing a yellow powder) 
 
 Copiapite, Pe,S 5 21 -f- 18Aq. 
 
 Raimondite, 3Pe 2 S 3 15 4-7Aq. 
 
 Pastreite orjarosife (Brush), K 2 Fe 3 S 4 22 -f- 6Aq. 
 
 Carphosiderite, ^ 4 s 6 27-f 18A( 1- Insoluble in water. Pow- 
 ders yellow. 
 
 Voltaite, 3eS 3 12 -f 20Aq. Characterized by its black to 
 dark-green color and octahedral crystallization. All these 
 sulphates B. B. in the closed tube yield water. 
 
 SIDERITE (spathic-iron, Eisenspath), FeC0 3 . With diffi- 
 culty fusible, becomes by heating black and magnetic. Dissolves 
 .in warm HC1 with effervescence*. H. 4. G. 3.75. Compare 
 Mesi tine-spar (Mesitite). 
 
 The following minerals, inclusive of beraunite, contain phos- 
 phoric acid, and their nitric acid solution yields with molyb- 
 date of ammonium, at a gentle heat, a yellow precipitate. 
 
 HUREAULITE (Huraulith, hydrous phosphate of iron and 
 manganese), (Mn, Fe, H 2 ) 3 P a O 8 -[- 4Aq, and 
 
 TRIPLITE (phosphate of iron and manganese), (Fe, Mn) s 
 P 2 O 8 (Fe, Mn, Fl). B. B. fuse easily, and, when moistened 
 with sulphuric acid, tinge the flame with a feeble bluish-green. 
 They dissolve with borax in the exterior flame to an amethys- 
 tine bead. -Hureaulite in a matrass yields a considerable 
 amount of water; the other only a trace. With phosphoric 
 acid, boiled down, both yield a colorless liquid, which, upon 
 
MINERALS WITHOUT METALLIC LUSTRE. 271 
 
 
 
 addition of nitric acid, turns violet. Hureaulite is of a red- 
 dish-yellow color ; is not cleavable. Triplite is brownish or 
 black, cleavable at right angles in three right angular direc- 
 tions. A similar deportment to triplite is shown by zwieselite.* 
 Both give the reaction for fluorine when fused in a close tube 
 with bisulphate of potassa. 
 
 Sarcopside 4(Mn, Fe) 3 P,0 8 -f H 4 Fe() 5 . Color, flesh -red to 
 lavender-blue. Streak, straw-yellow. Compare the follow- 
 ing \r- 
 
 Trlpltyliie. Triphyline, (Fe, Mn, Li 2 ) 3 P 2 O 8 . 
 
 B. B. gives a deportment similar to the preceding ; the re- 
 action of manganese with borax is less distinct, but the bead 
 is colored more strongly with iron. When the solution in 
 HC1 with addition of nitric acid is evaporated to dryness, 
 and alcohol added, then heated to the boiling point and 
 lighted, purple-red stripes will be visible occasionally in the 
 flame, especially towards the last. This behavior (caused by 
 the presence of lithia) easily distinguishes it from similar phos- 
 phates of iron. Color, greenish-gray, bluish, etc. Cleavable 
 in four directions. 
 
 .Diadochite, Fe 2 O 3 , SO 3 , P 2 O 5 , H 2 O. Easily soluble in hydro- 
 chloric acid, the solution yields with chloride of barium a heavy 
 white precipitate of sulphate of baruim. Amorphous. Color 
 red to yellowish-brown. The powder is yellow. 
 
 Vivianite (blue iron earth), Fe 3 P 2 O 8 + Aq. 
 
 Dufrenite, kraurite (green iron ore), 5 ? ^J ) a !i+ 3Aq. 
 
 Cacoxenite, kacoxene, Fe. 2 P 2 8 -{-12Aq, and borickite 
 (Fe, Ca 3 ) 5 P0 4 0,5+15Aq. 
 
 B. B. fuse easily, and when moistened with sulphuric acid 
 they exhibit the same reaction as the preceding. They impart 
 to borax bead only the color of oxide of iron (i. e. in the ex- 
 terior flame it is red when hot, after cooling yellow) ; in the 
 reduction flame it is bottle-green. The hydrochloric acid solu- 
 tion yields with chloride of barium no precipitate. In a 
 
 * Brush considers both identical. 
 
272 MINERALOGY SIMPLIFIED. 
 
 matrass they yield "a large proportion of water. Cocoxene 
 loses by ignition 3.3, vivianite 28, borickite 19, and dufrenite 
 8^ per cent, of water. Color of vivianite is blue of different 
 shades ; that of anglarite gray inclining to blue ; that of dufre- 
 nite dark leek-green ; that of cacoxene ochre-yellow ; and that 
 of borickite reddish-brown. Another phosphate resembling 
 these is beraunite. 
 
 Beraunite, FeP 2 8 4- Aq, exhibits a hyacinth-red, or red- 
 dish-brown color. 
 
 Hematite, peroxide of iron, red iron ore, specular iron, is 
 easily distinguished by the cherry-red color of its streak (gene- 
 rally fusible above 5). Compare limonite. H. 6-6.5. G.4.5. 
 
 Section iii. With hydrochloric acid form a jelly, or is decomposed 
 ivith separation of silica.* 
 
 Cronstedtite, 3(Fe, Mg),Si0 4 + Pe 2 Si0 8 + 6Aq. In a matrass 
 affords water, and B. B. fuses with intumescence to a black 
 bead. With muriatic acid it forms a perfect jelly. (Sidero- 
 schisolite^ shows a similar deportment, and belongs probably 
 to the same species.) Color, raven-black. Streak, dark leek- 
 green. Hardness between 2 and 3. 
 
 A similar deportment is shown by thuringite. The analysis! 
 yielded : SiO 2 23, Fe 2 3 15, A1 2 O 3 17, FeO 33, H 2 O 12 = 100. 
 The solution in aqua regia yields, with ammonia, a precipitate 
 of Fe a O 3 and Al a O 3 . If this mixture is boiled with caustic 
 potash, A1 2 O 3 is extracted, leaving Fe 2 O 3 behind. From the 
 potassa solution, rendered acid with HC1, ammonia throws 
 down A1 2 O 3 . Found in Thiiringen, and in the United States 
 at the Hot Springs, Ark., and at Harper's Ferry. 
 
 * The residue may be recognized as pure silica when it is easily 
 and perfectly soluble in potassa, or at least the greater portion. The 
 solution yields by the addition of a sufficient quantity of dissolved 
 sal ammoniac, a white flaky precipitate of hydrous silica. B. B. silica 
 fuses readily with soda to a transparent glass (the soda should be 
 added gradually). 
 
 t J. D. Dana's Syst. of Min., 5th ed., p. 504. 
 
 t F. von KobelPs Mineralogie, 5 Aufl. Leipzig, 1878, p. 225. 
 
MINERALS WITHOUT METALLIC LUSTRE. 273 
 
 Chalcodite, (Fe, Mg) 2 (Fe, Al)Si 5 13 -f- 3Aq, and stilpnomelane, 
 of nearly the same composition, yield water in a bolt-head (9 
 per cent.), are decomposed by hydrochloric acid without gela- 
 tinizing. The color of chalcodite is green, inclining to 
 bronze ; that .of stilpnomelane black. Their streak is greenish- 
 gray. Related closely with chalcodite are : 
 
 Voiytite, 3tl, e, Mg, Si, Aq. 
 
 Ekmannite, Fe, Mn, Pe, Si, Aq and 
 
 Euralite, Fe, Mg, Si, Pe, gi, Aq. 
 
 Whilst chalcodite is radiated and sometimes foliated, voigtite 
 is micaceous, and the last two are massive. In the matrass 
 yield water, and are decomposed by HC1 without gelatinizing. 
 
 Palagonite, l> 3?> Mg, Ca, Si, Aq. Is amorphous, and has a 
 brownish-yellow streak. Yields much water (16 p. c.), fuses 
 at 3 to a black, lustrous, magnetic glass. Sometimes gelatin- 
 izes, sometimes does not, with HC1. Compare jollyte. 
 
 Lievrite (Ilvaite), H,Ca,Fe 4 FeSi 4 18 . 
 
 Allanite (Orthite), (Ce, La, Di, Fe, Ca) 3 (AlFe)Si 3 12 . Are not 
 cleavable, gelatinize with HC1. Give little or no water in the 
 closed tube. Allanite swells much and fuses easily to a bulky 
 brown or black glass. After separation of SiO 3 from the HC1 
 solution, ammonia gives a heavy precipitate, which dissolves 
 in oxalic acid, leaving a white residue, which, ignited and 
 treated with dilute HC1 to separate carbonate of calcium and 
 again ignited, gives a brick-red mass (oxide of cerium). Color, 
 pitch-brown to greenish-black. Streak, greenish-gray. Hard- 
 ness, 5.5-6 (orthaclase). 
 
 Lievrite (ilvaite). Intumesces slightly; decrepitates slightly 
 and fiises easily to an iron black magnetic bead. Color brown, 
 ish-black ; streak, black. Hardness, between apatite and ortho- 
 elase. 
 
 Fayalite, Fe 2 SiO 4 , and 
 
 Hortonolite, (Fe,Mg) a SiO 4 . Crystalline and cleavable ; gela- 
 tinize perfectly. Decomposed by phosphoric acid. The jelly 
 of hortonolite turns immediately violet when treated with nitric 
 acid. 
 
274 MINERALOGY SIMPLIFIED. 
 
 The same deportment is exhibited by 
 
 Knebelite, (Fe,Mn). 2 8iO 4 , and 
 
 Ropperite, (Fe,Mn,Zn,Mg),SiO 4 . 
 
 Tlie latter gives, with soda on coal, a deposit of oxide of 
 zinc. 
 
 Pyrosmalite, ((FeMn)Cl 2 -f 7(Fe,Mn)SiO. { ) + 5Aq, and 
 
 Astrophyllite, (K,Na) 6 (Fe,Mn) 15 (Pe,Al) 2 (Si,Ti) 16 5f) , are decom- 
 posed by HC1, leaving a residue of silica without gelatinizing. 
 B. B. they fuse easily at 2-2.5. 
 
 Pyrosmalite mixed with salt of phosphorus and oxide of 
 copper tinges the flame bluish-green (chlorine). Astrophyllite 
 does not. 
 
 Both distinctly cleavable in one direction ; the latter often 
 micaceous. 
 
 The hydrochloric acid solution of the latter when boiled with 
 tin is colored violet, turning rose-red when diluted (titanic acid 
 reaction). 
 
 Lepidomelane, K^Fe-jCAljFejgSigO^. In small six-sided tables, 
 or an aggregate of minute scales. Color, raven black. Streak, 
 grayish-green. Decomposed easily by HC1, leaving a residue 
 of silica in the form of scaly flakes. 
 
 Allochroite (iron-lime garnet, Eisenkalkgranat), Ca 3 FeSi 3 12 in 
 some varieties forms an imperfect jelly with cone. IIC1. Not 
 cleavable, easily fusible. Color, green, yellow to black. 
 
 Gillingite, V,Fe,Mg,Ca,Si, Aq, and 
 
 Xylotile (Bergholz, Germ.), 3?e,Mg,Si, Aq, are fusible with 
 difficulty, and become magnetic only after long blowing. They 
 are decomposed by muriatic acid without gelatinizing. The 
 former is brownish-black ; amorphous ; the last is brown ; 
 fibrous, like wood. In a matrass both give water.* 
 
 * Many limonites (hydrated peroxide of iron, Thoneisenstein), 
 F<'. 2 -H 3 . fuse and become magnetic-; they dissolve in concentrated mu- 
 riatic acid with separation of clay. Streak, mostly ochre-yellow or 
 brownish-red. 
 
MINERALS WITHOUT METALLIC LUSTRE. 27~> 
 
 Section iv. Only sliyhtly attacked by hydrochloric acid. 
 
 CROCIDOLITE (Krokydolitb, blue asbestos), Fe, Na 2 , Mg, 
 Si, Aq. 
 
 AKFVEDSOMTK (black hornblende), Na Si-4-Fe 3 Si r 2(Na 2 , 
 Fe, Ca) Si0 3 -f Fe, Si 3 O 9 B. B. fuse easily at from 1.7 to 2 
 with intumescence and frothing, to a black mass. In a matrass 
 the second affords no water ; is perfectly cleavable under 
 123 55'. Color, black. Streak, grayish to green. Crocido- 
 lite in a matrass affords some water. Color, green to lavender- 
 blue ; has been noticed only in aggregated fibres. 
 
 (Compare ampltibole and tourmaline (some varieties of which 
 act feebly upon the magnet after fusion).) 
 
 GLAUCONITE. SELAUONITE (green earth, Griinerde), 
 Fe, Mg, K 2 , Xl, Si, Aq B. B. fuses at 3 quietly without intumes- 
 cence. In a matrass yields some water. Color, olive to sea- 
 green. Hardness 1. 
 
 Ac MITE (Achmit), (Na 6 Fe 3 Fe) Si 3 9 , and 
 
 Babingtonite, e,Ca,Fe,Mn,Si, fuse quietly. Acmite at 2, 
 babingtonite at 2.6 to a black glistening mass. Acmite is 
 cleavable at an angle of about 93. Babingtonite when fused 
 with potassa and dissolved in muriatic acid gives with ammonia, 
 or better with oxalate of ammonium, a heavy precipitate of lime ; 
 acmite gives none or only a very slight precipitate. 
 . (Compare augite (black crystallized pyroxene).) 
 
 Almandite ( Almandine garnet, Thoneisengranat), Fe 3 A:lSi 3 O ir 
 B. B. fuses quietly at 3. Gelatinizes after fusion. Is not 
 ch-avable. Hardness, 7-7.5. Color, red, brown-red. Sp. gr. 
 3.7-4. 
 
 (Compare also allochroite (Eisenkalk-granat).) 
 Wolframite (Wolfram), (Fe,Mn)WO 4 , and 
 
 Ferberite (of the same composition).* 
 
 Color, black. Streak, ochre-yellow. Lustre, submetallic. 
 Boiled with cone, phosphoric acid give a blue liquid, which 
 
 * The ferberite of von Kobell is considered identical with wolframite. 
 Sec Brush, Deterin. Min., p. 78. 
 
270 MINERALOGY SIMPLIFIED. 
 
 diluted with water becomes colorless. Upon addition of iron 
 powder and shaking the solution turns fine blue again. 
 
 B. B. with soda and nitre on platinum foil give the bluish- 
 green manganese reaction. 
 
 A similar deportment is shown by 
 
 Megabasite (Blumit), (Mn,Fe)WO 4 . Color, brown. Streak, 
 ochre-yellow. 
 
 Rhodonite (Mangankiesel), MnSiO 3 . Color, rose-red, brown- 
 ish-red. Lustre, vitreous. 
 
 B. B. some varieties become, after fusing, magnetic. Im- 
 parts a violet color to the borax bead. 
 
 Lepidolite (lithionite, Lithionglimmer), (K,NaLi) c Al 4 Si 12 39 . 
 After fusion frequently magnetic. Tinge the flame distinctly 
 purple-red (lithia) ; eminently cleavable in one direction (mi- 
 caceous). 
 
 (Compare Lepidomelane, K 1 Fe 2 (Ali J e) 3 Si 6 24 .) 
 
 Division Not included in the foregoing divisions. 
 
 Molybdite (Molybdiinocker), MoO 3 . B. B. on coal fuses, 
 fumes, and is absorbed. By fusion with soda and elutriation 
 of the coal we can obtain a steel-gray powder oflreduced molyb- 
 denum. With salt of phosphorus in the reduction flame a dark 
 glass is formed, which on cooling acquires a clear green. In 
 muriatic acid it dissolves easily, the solution being colorless, 
 but when stirred with tinfoil immediately assumes a blue color. 
 Color, sulphur-yellow, inclining to orange. 
 
 Eulytite (WismuthWende). 
 
 Silicate of bismuth, Bi 4 Si 3 O 12 , and 
 
 Bismutite, 2Bi 8 C 3 O ]8 -f 9H 2 O, B. B. fused with sulphur 
 and iodide of potassium on charcoal give a fine red sublimate 
 on the coal (bismuth). 
 
 Eulytite gelatinizes perfectly with HC1. 
 
 Bismutite dissolves with effervescence in it. 
 
 Pucherite, BiVO 4 . B. B. reacts of bismuth like the pre- 
 ceding ; gives with HC1 a greenish-blue solution which, diluted 
 
MINERALS WITHOUT METALLIC LUSTRE. 277 
 
 with water, yields a yellow precipitate, whilst the filtrate has 
 a sky-blue color. Color, reddish-brown. Streak, ochre-yellow. 
 
 (Compare samarskite.) 
 
 Also allanite in the preceding division, which after fusion 
 is not always magnetic. 
 
 (Compare likewise lepidomelane.) 
 
 Part B. B. B. FUSED WITH SODA ON COAL YIELD NO ME- 
 TALLIC GLOBULE, OR FUSED ALONE IN THE R. F. DO 
 NOT ACT ON THE MAGNETIC NEEDLE. 
 
 Division 1 After fusion and continued ignition on coal in the 
 forceps or the platinum spoon, give an alkaline reaction, 
 turning moistened red litmus paper blue; and yelhw tur- 
 meric paper, broivn. The assay must be employed in 
 splinters and not in powder form * 
 
 Section i. In water easily and perfectly soluble. 
 
 Nitrate of potassium (saltpetre), KNO 3 . 
 
 Nitratine (nitrate of sodium, sodanitre), NaNO 3 . B.B. heated 
 gently on charcoal they deflagrate in a lively manner, which 
 does not occur with those following. Fused on platinum wire, 
 nitrate of potassium tinges the flame bluish, inclining to red. 
 Nitrate of sodium colors it strongly yellow. In the solution of 
 nitrate of potassium, chloride of platinum causes a yellow pre- 
 cipitate (potassa). In nitrate of sodium solution it occasions 
 none. 
 
 Sodium carbonate, Na a CO 3 -f lOAq. 
 
 Thcrmonatrite, Na 2 CO 3 + Aq, and 
 
 Trona or sesquicarbonate of sodium, Na 4 C,O 8 -f 3Aq. 
 
 li. 1>. in the closed glass tube give much water. Their solu- 
 tion in water is alkaline and effervesces on the addition of an 
 
 * Konngott has shown that many silicates and other compounds 
 react before, or only after fusion, (ilhiliuc, when they are placed in 
 iiotn/rr form upon moist turmeric paper, but not wbcn in tbe sliapo of 
 sjillii/t'.rs. The above-mentioned minerals, however, exhibit an alka- 
 line reaction even in splinter form. 
 24 
 
278 MINERALOGY SIMPLIFIED. 
 
 acid. The crystals of the former soon deliquesce by exposure 
 in the air. Sesquicarbonate of sodium does not. 
 
 Mirabilite (sulphate of sodium, Glauber's salt), Na 2 SO 4 + 
 lOAq. 
 
 Thenardite (anhydrous sulphate of sodium), Na 2 SO 4 . 
 
 Aphthitalite (glaserite, sulphate of potassium), K 2 SO 4 . 
 
 JEpsomite* (sulphate of magnesium, 'Epsom salt), MgS0 4 -f- 
 7Aq. 
 
 Kalinite (sulphate of potassium and aluminium, potash alum), 
 K 2 AlS 4 16 -f24Aq. Their solution in water does not give an 
 alkaline reaction or effervesce by the addition of an acid ; 
 chloride of barium causes a heavy precipitate of sulphate of 
 barium which is insoluble in acids. In the solutions of alum 
 and of ep somite, carbonate of potassium produces white precipi- 
 tates. They are easily distinguished B. B., since the mass that 
 remains after expulsion of the water and continued strong 
 ignition, assumes, moistened with cobalt solution and heated 
 again, in the former (alumina) a fine blue, in the latter a flesh- 
 red color (magnesia). In the solutions of the other minerals 
 alkalies cause no precipitates. A concentrated solution of 
 glaserite yields a yellow precipitate with chloride of platinum, 
 while the first two give none. In a matrass, mirabilite affords 
 a large quantity of water, but thenardite gives none. 
 
 Taclthydrite, CaMg 1 Cl 6 + 12Aq = CaCl > + 2MgCJ, + 12Aq 
 (Kammelsb.). Gives in the closed tube much water. B. B. 
 fuses at first on its surface when a non-fusible mass remains, 
 which colors the flame finely red and reacts alkaline. In 
 water easily and completely soluble. The solution reacts of 
 lime and magnesia. Color, yellowish. Deliquescent. 
 
 * Epsomite contains 50 per cent, of water. Similar compounds are 
 Loweite, 2Na 2 MgS 2 O g -j- 5Aq, and 
 
 Kieserite, MgS0 4 -f- Aq ; both with 14 per cent, of Aq. 
 Bloedite, Na 2 MgS 2 O 8 + 4Aq, and 
 
 iSimoityitc, Na 2 MgS 2 8 -f- 4Aq ; both with 21 per cent, of Aq. 
 Picromerite (kainite), K 2 MgS a O 8 + GAq. 
 
 The aqueous solution of the last yields with nitrate of silver a white 
 precipitate of chloride of silver. 
 
MINERALS WITHOUT METALLIC LUSTRE. 279 
 
 CarnaUitc, KMgCl 3 + GAq = KC1 _J-MgCl 2 -f 6Aq. B. B. 
 fuses easily. After continued fusion on platinum foil, tlie 
 remaining mass reacts alkaline. Sohvble in water. Gives no 
 reaction of lime, but of magnesia with phosphate of sodium ; 
 when free ammonia is present, a white, crystalline precipitate 
 of ammonio-magnesium phosphate being formed. A solution 
 of chloride of platinum indicates the presence of K 2 O by fur- 
 nishing a yellow, crystalline precipitate in moderately dilute 
 solutions of the mineral. 
 
 HALITE (rocksalt, common salt, chloride of sodium), NaCl 
 and sylvite, KC1. Are anhydrous, and easily recognized by 
 their taste. The aqueous solution gives with chloride of 
 barium and alkalies no precipitate; with nitrate of silver a 
 curdy precipitate of chloride of silver. Chloride of platinum 
 produces with the first, none ; with the second, a yellow pre- 
 cipitate (K 2 O). The solution shows no alkaline rea-ction. 
 
 BORAX (tinkal, biboratc of sodium), Na 2 B 4 7 -{- lOAq. The 
 solution has an alkaline reaction, and does not effervesce with 
 acids. After being treated with sulphuric acid and evaporated 
 to dryness, if alcohol be added, it burns with a green flame 
 (caused by boric acid). B. B. bubbles, swells up, and fuses 
 lo a clear bead. 
 
 Section ii. Insoluble in water, or dissolving with difficulty. 
 
 ULKXITE* ' ; (fforocalcite, boronatrocalcite), NaCaB.O () '-f 
 5Aq. Fuses at 1. Alone it tinges the flame yellow. Moistened 
 with sulphuric acid imparts to it a beautiful green (boric acid). 
 Yields much water in a matrass. Partially soluble in hot 
 water. The solution is alkaline in its character. In muriatic 
 acid easily and quietly soluble. The solution when evaporated 
 leaves a residue which imparts to alcohol the property of burn- 
 
 * Von Kobell describes under the name of " borocaleite" a mineral, 
 CaO, 2BO 3 (containing no sod-iuni), and a mineral " ul<>xite" of the above 
 formula, both from southern 1'ern. According to J. I). Dana's Syst. 
 of Mineralogy, 5th ed., p. f>99, both minerals are alike, sodium bring 
 an rssciitial constituent found in both. A. A. Hayes, who analy/ed 
 it, had overlooked tlic sodium. 
 
280 . MINERALOGY SIMPLIFIED. 
 
 ing with green color. The mineral' is insoluble in sulphuric 
 acid.* (Occurs in delicate, fibrous, felt-like masses.) 
 
 Gay-lussite (carbonate of calcium and sodium), Na 2 CO 3 -{- 
 CaCO 3 -f 5Aq. 
 
 Wither ite (carbonate of barium), BaC0 3 , and 
 
 Staffelite, Ca s P 1 O 8 -f CaCO 3 . Are dissolved in dilute hydro- 
 chloric acid with effervescence. The acid solutions of gay- 
 lussite and staffelite, largely diluted with water, give with 
 sulphuric acid no precipitate ; that of witherite an abundant 
 deposit of sulphate of barium. In a matrass gay-lussite affords 
 much water ; willierite and staffelite none. The solution of 
 staffelite in HC1 gives with NH 3 a precipitate, the others do 
 not. The HC1 solution of staffelite yields with molybdate of am- 
 monium at a gentle heat a yellow precipitate (phosphoric acid). 
 
 (Compare strontianite, which colors the flame purple (stron- 
 tium).) 
 
 ANHYDRITE (anhydrous sulphate of calcium), CaSO 4 . 
 
 GYPSUM (hydrated sulphate of calcium), CaSO 4 -f- 2Aq. 
 
 POLYIIALITE (sulphate of potassium, calcium, and magne- 
 sium), Ca 2 MgK 2 S 4 O 16 + 2Aq. 
 
 BRONGNIARTINE (glauberite, sulphate of sodium and calcium), 
 Na 2 CaS 2 O g . Are quietly soluble in sufficient muriatic acid. 
 The solution gives with chloride of barium a heavy precipitate 
 of sulphate of barium, and with oxalate of ammonium, after 
 being neutralized with caustic ammonia, it yields a precipitate 
 of oxalate of calcium. In a matrass polyhalite yields some water; 
 gypsum, a large amount ; the others only traces of water.' 
 Poll/halite and brongniartine are soluble in water with separa- 
 tion of sulphate of calcium. If a small quantity of these minerals 
 is boiled with water, a solution is obtained, yielding a slight 
 precipitate with oxalate of ammonium (lime), and after that is 
 filtered off, phosphate of sodium, in the presence of free ammonia, 
 thrown down a heavy precipitate of phosphate of ammonium- 
 
 * Compare strassfurtite (boracite), Mg 7 B 16 Cl 2 30 . Soluble in sul- 
 phuric acid.. Reacts alkaline after fusion, from an admixture of 
 NaCl and MgCl,. 
 
MINERALS WITHOUT METALLIC LUSTRE. 281 
 
 i)itf(/n.(>si'nm in the filtrate of polyhallite, but none in that of 
 bronyniartine (glauberite). Their fusibility is 1.5. 
 
 In the solution of polyhalite, chloride of platinum gives a 
 yellow precipitate (K 2 O) ; in that of brongniartine, none. 
 
 Anhydrite and gypsum are only slightly soluble in water, 
 and their fusibilities = 2.5-3. Hardness of anhydrite is 3.5, 
 all the others are softer. 
 
 Closely related to brongriiartine is 
 
 Syitgenite (kaluszite), CaS0 4 -f K 2 SO 4 -f Aq, from Kalusz 
 in Gallizien. 
 
 BAKITE. Heavy spar, sulphate of barium, BaSO 4 , and 
 
 Celestite (celestine, sulphate of strontium), SrS0 4 . Are not, 
 or but very little, attacked by H'Cl. When finely pulverized 
 celestite is boiled with HC1 enough is dissolved to form, upon 
 the addition of chloride of barium, a slight precipitate of 
 sulphate of barium. B. B. with soda yield hepar. Heated in 
 the forceps, barite tinges the flame a pale yellowish-green ; 
 celestite a feeble purple-red. By moistening with a drop of 
 IIC1 the particles which have been fused arid long heated in 
 the reduction flame, and then holding the mass in the blue 
 portion of a candle flame (without blowing) it colors it purple- 
 red, when the assay is celestite, but does not with barite. 
 
 FLUORITE (fluespath, Germ.), CaFl 2 . 
 
 CRYOLITE (fluoride of sodium and aluminium, Kryolith), 
 Na (i AlF 12 (or GNaF-f- A1F 6 ). 
 
 PIIARMACOLITE (arsenate of calcium), Ca 2 ls + OH. B. B. 
 with soda do not give hepar. Do not effervesce with muriatic 
 acid. Arsenate of calcium is easily distinguished by its alliace- 
 ous odor when fused on coal (the fragments used should be as 
 large as possible). The other two heated in a glass tube with 
 sulphuric acid give off much hydrofluoric acid gas, which 
 strongly attacks the glass, the water which condenses at the 
 upp<T end of the tube reacts for fluorine with Brazil-wood 
 paper. Fusibility of liparite 3, of cryolite 1.* Phosphores- 
 
 * Fuses in the flame of a candle. 
 24* 
 
282 MINERALOGY SIMPLIFIED. 
 
 cence is obtained from the coarsely-powdered fluor-spar below 
 a red heat. At a high temperature it ceases, but is partially 
 restored by an electric discharge. Cleavage, octahedral. 
 
 Closely related with cryolite is 
 
 Chiolite, Na 3 A-lF 9 (or 3NaF -4- A1F 6 ) , occurs in granular masses, 
 while cryolite is found in large crystalline lumps, cleavable in 
 three rectangular directions. Also related is 
 
 Pachnolite (thomsenolite), Na 2 Ca 2 A-lF 12 -f- 2Aq. Heated in 
 the closed tube yields water which has a strongly acid reaction. 
 Similar compounds not containing water are 
 
 Arksutite, CaNa 2 A-lF 10 . 
 
 Chodneffitv, Na 4 A-lF 10 . 
 
 Others containing water are 
 
 Thomsenolite. * 
 
 Gearksutite, Ca 2 AlF ]0 -f- 4Aq (19 p. c. water). 
 
 Cancrinite, Na 2 A-lSi 2 8 , effervesces' with concentrated hydro- 
 chloric acid, and gelatinizes when heated with it. B. B. it 
 turns white and turbid ; fuses at 2.5 with intumescence, and 
 foaming to a white, porous glass, which, when moistened and 
 placed upon turmeric paper, reacts alkaline (brown). Related 
 to nephelite (nepheline), (NaK) 2 &lSi 2 8 . 
 
 Division 2. Soluble in hydrochloric acid; some also in water 
 without perceptible residue; the solution does not form a 
 gelatinous mass. 
 
 (Compare from the preceding division those minerals which 
 after fusion react only feebly alkaline, viz., kieserite, kainite 
 (picromerite, Brush), and epsomite.) 
 
 * Prof, von Kobell in his tables, llth edit. v 1878, mentions " pach- 
 itolite" and J' thomsenolite" under two heads as distinct minerals, 
 while the chemical identity of thomsenolite and pachnolite was shown 
 by the analyses of Knop and Wohler to he merely varieties of one and 
 the same species. Consult Textbook of Mineralogy, by E. J. Dana. 
 New York, 1877, p. 243. Also, Brush's Manual of Determinative 
 Mineralogy, '3d edit., 1878, p. 81, giving both names to the same 
 mineral. 
 
MINERALS WITHOUT METALLIC LUSTRE. 283 
 
 Durangite (NaLi) 2 (AlPeMn)As 4 (0,F) 9 . Fuses easily, with 
 strong sulphuric acid it gives off hydrochloric acid, which 
 corrodes glass. B. B. on charcoal evolves fames of arsenic. 
 Color, orange-red. Streak, yellowish. 
 
 Chondroarsenite, Mn 6 As 2 O n -|-3Aq. 
 
 Trdgerite, U 3 As 2 O 14 -f 12Aq, and 
 
 Walpuryite (Walpurgin), Bi 10 U 3 As 4 O S4 -j- 12Aq. All have 
 a yellow color, and B. B. on charcoal develop arsenical fumes. 
 Chondroarsenite colors a bead of salt of phosphorus amethys- 
 tine (oxide of manganese) ; the others color it green. Wal- 
 purgitewith S -}- KI fused together gives a red sublimate on 
 charcoal (iodide of bismuth). 
 
 Adamite (Adamin, Germ.), Zn 4 As 2 O 9 -f Aq. B. B. easily 
 fusible. On charcoal evolves arsenical fumes, giving at the 
 same time a zinc coating. Color, honey-yellow. 
 
 Fauserite (Mn, Mg) SO 4 -j- Aq. Soluble in water. Heated 
 with P 2 O 5 and HNO 3 , forms a violet solution. B. B. colors 
 the borax bead violet when hot (oxide of manganese). Con- 
 tains 40 p. c. of water. 
 
 Tschermigite (ammonia-alum) (NH) 2 AlS 4 O l6 -f-24Aq. 
 
 Keramohalite (alunogen), AlS 3 ]2 -J-lSAq, and 
 
 Goslarite (sulphate of zinxi), ZnSO 2 -|-7H 2 O. Fuse when first 
 heated, puff up, and form an infusible mass, which, moistened 
 with cobalt solution and again heated, assumes a fine blue color 
 when it is tschermigite and alunogen, but a green color when 
 it is sulphate of zinc. With soda they give hepar, and are 
 soluble in water. Tschermigite evolves ammonia vapor when 
 treated with caustic potash solution, alunogen does not. 
 
 Struvite, NH 4 MgPO 4 -f 12Aq. Fuses easily. Gives much 
 water in a matrass, but with soda no hepar ; evolves when 
 treated in powder form with caustic potash (KHO) or soda 
 (NaHO)* the odor of ammonia, and forming white fumes when 
 any volatile acid as HC1 is brought in contact with it. This 
 
 * Caustic lime (CaII./) 2 ) may also be employed ; in that case, how- 
 ever, it must be in the solid state, not in solution. 
 
284 MINERALOGY SIMPLIFIED. 
 
 experiment is best performed by inserting a glass rod moistened 
 with IICl into the mouth of a test-tube in which the decom- 
 position of the ammonium salt is being effected, and immediately 
 withdrawing it. The HC1 employed should not be concentrated 
 but should be diluted with an equal volume of water. The 
 presence of vapor of free ammonia may be recognized by turn- 
 ing red litmus paper blue. 
 
 Sassolite (boron trioxide, boric acid), H 6 B a O 6 .- 
 
 Boracite (borate of magnesium), Mg 7 B 16 Cl 2 O 30 , and 
 
 Stassfurthite, 2Mg 3 B 8 O ]5 + MgCJ 2 .* 
 
 Hydrob or acite (hydroborate of calcium and magnesium), 
 CaMgB 6 O n + 6Aq. 
 
 LarderelliteJ NH,OB 4 + 4H 2 0. 
 
 Sussexite (Mn,Mg) 2 B 2 5 -f- H 2 O. Fuse easily with intum- 
 escence and color (except stassfurthite)t the flame green (boric 
 acid). When the powdered minerals are heated with sulphuric 
 acid, then alcohol added and set on fire, the flame is tinged in- 
 tensely green (boric acid). Larderellite evolves, when treated 
 in powder form with caustic potash or soda-solution, the odor 
 and test of ammonia. Sussexite is easily distinguished from 
 the others, that it yields a violet liquid when boiled with phos- 
 phoric acid and nitric acid (manganese). 
 
 B. B. Boracite gives none or only traces of water, whilst 
 the others yield water abundantly. Sassolite is soluble in water 
 and alcohol ; the others are not. Hydroboracite contains 2G 
 per cent, of water, while the similar mineral szaibelyite, Mg 5 
 B 4 O n -f- 3Aq, contains only 7 per cent, of water. Very closely 
 .related to boracite is stassfurthite,| and similar to hydro- 
 boracite is 
 
 * Prof. v. Kobell mentions boracite and stassfurtliite as two distinct 
 minerals, although of an identical chemical composition ; while Profs. 
 Dana and Brush consider both under one head, "boracite." 
 
 f J. I). Dana's Syst. of Min., fifth edit., p. 600; also Am. Jonrn. 
 Sci., ii. xvii. 130. A rare borate from the Tuscan lagoons. Analysis 
 by E. Bechi. 
 
 J Constitutes only a variety ofboracite, as already stated. 
 
MINERALS WITHOUT METALLIC LUSTRE. 285 
 
 Lunebitrgite, Mg 3 P 2 B 2 O u -f 8Aq. It yields, however, in a 
 nitric acid solution with molybdate of ammonium a yellow pre- 
 cipitate (P 2 O 5 ), which is not the case with the others. 
 
 (Compare : Tinkal, NaO,B 2 O 3 + lOAq.) 
 
 Alabandite (alabandine) MnS, and 
 
 Hauerite, MnS 2 . When boiled with phosphoric acid and 
 nitric acid is added, violet solutions are produced. The roasted 
 minerals give, with borax, a violet bead in O. F. (manganese). 
 The powder of alabandite is leek-green, that of hauerite 
 brownish-red. 
 
 (Compare : I. A. 5.) 
 Wagnerite, Mg 3 P 2 O 8 + MgF,. 
 
 Apatite, 3Ca 3 P 2 O 8 + Ca(Cl,F) 2 , and 
 
 Kjeralfine, 2Mg s P 2 O 8 + CaF 2 . 
 
 B. B. Apatite fuses quietly at 5. Wagnerite and kjerulfine 
 with bubbling at 3-3.5. Kjerulfine in the closed tube phos- 
 phoresces with a faint white light. Moistened with strong 
 sulphuric acid all color the flame bluish-green. The nitric acid 
 solutions give with molybdate of ammonium a yellow precipitate 
 (phospho-molybdate of ammonium). Wagnerite is soluble in 
 dilute sulphuric acid. Apatite is not. Kjerulfine is with sepa- 
 ration of sulphate of calcium. The solution of the latter, in some- 
 what concentrated HC1, yields with sulphuric acid at once a 
 heavy precipitate of gypsum. Wagnerite gives none, or fur- 
 nishes one only after a lapse of time. 
 
 Brushite, HCaPO 4 -f- 2Aq. Reacts like apatite in the wet 
 way, but gives much water in the closed tube (26 per cent.). 
 
 Likewise : 
 
 Isoclasite, Ca 4 P a O 9 -f 5Aq, with 18 per cent, of water. 
 
 Ambhjgonite, 2A1P 2 8 + 3(Li,Na)F. Fuses easily at 2, coloring 
 the flame purple-red (lithia). Soluble with difficulty in cone. 
 HC1 and H 2 SO 4 ; with the latter evolves hydrofluoric acid, also 
 when fused with bisulphate of potassium. The nitric acid solu- 
 tion gives a yellow precipitate with molybdate of ammonium 
 
 O'A)- 
 
 A closely related mineral is 
 
2S() MINERALOGY SIMPLIFIED. 
 
 Helronite, with 4 per cent, of water give a pure lithia flame. 
 Both are cleavable at an angle of 105. Hardness, C. Phos- 
 phoresce with a light-blue color. 
 
 Autunite (uranite, Kalk-Uranit, Germ.), CaU a P a 12 -f lOAq, 
 or 2(UO^ 3 P 2 O 8 +C;i 3 P 2 O 5 4-30 Aq. B: B. fuses easily in the 
 closed tube, and, with salt of phosphorus in O. F., a yellow 
 glass, which in R. F. turns handsomely green. The solutions 
 in HC1 and HNO 3 have a yellow color, and yield with ammo- 
 nia a yellow precipitate. Give like amblygonite the phos- 
 phoric acid reaction with molybdate of ammonium. 
 
 (Compare chalcolite (phosphate of uranium and copper).) 
 
 Division 3. Are entirely soluble in muriatic acid, forming a 
 stiff jelly upon partial evaporation. 
 
 Section i. B. B. in a matrass afford 'water. : . 
 
 DATOLITE (Datolith, borosilicate of calcium), H a Ca 2 B 2 Si s O 10 . 
 In a matrass gives but little water (the others much water) ; 
 fuses to a dense, clear, and mostly colorless bead, tinging the 
 ilame green. Gives the boric acid reaction likewise with 
 sulphuric acid and alcohol, the latter burning with a green 
 flame when set on fire. Prismatic cleavage perfect. 
 
 EDINGTONITE, BaAlSi 3 10 +3Aq. The diluted hydrochloric 
 acid solution produces, with sulphuric acid, a white precipitate 
 of sulphate of barium. Sp. gr. 2.7. 
 
 NATROLITE (mesotype). B. B. fuses at 2, quietly without 
 any perceptible intumescence. The HC1 solution yields, after 
 the alumina has been thrown down by caustic ammonia, no 
 precipitate, or a very slight one, by carbonate of ammonium. 
 Loss by ignition 9^ p. c. (Compare analcime.) 
 
 Scolecite (Skolezit, Germ.), CaAlSi 3 10 -j-3Aq, an( ] laumont- 
 ite, CaAlSi 4 12 4-4Aq. B. B. curl up in worm-like forms on 
 fusion, especially scolecite, which, in the O. F., gives a volu- 
 minous, frothy, shining slag, that, in the R. F., fuses further 
 into a vesicular slightly transparent glass. Laumontite fuses, 
 emitting few air-bubbles, to a white translucent enamel. 
 
MINERALS WITHOUT METALLIC LUSTRE. *2<S7 
 
 H. of scolecite, 5.5; of laumontite, 3. Scolecite becomes 
 electric on heating. Closely related to scolecite are : 
 
 Jl/csolite (Ca,Na 2 )AlSi 3 Oj -}-3Aq, an j thomsonite (comptonife), 
 2(Ca,Nf4)&lSi s Og4-&A<li but neither of them is pyro-electrical. 
 
 PIIILLIPSITE (lime harmotome) (Ca,K 2 )AlSi 2 8 -f 5Aq. Fuses 
 at 3, with slight intumescence ; many varieties fall to powder 
 like arragonite ; occurs crystallized only in rectangular prisms, 
 terminated with rhombic pyramids, and generally in twins, one 
 individual being united to another by a common main axis 
 at 1)0. 
 
 Here belong also 
 
 Gismondite (Ca,K._,)AlSi 3 0, 4-4 Aq. Usually has the appear- 
 ance of the square octahedron. Fuses at 3 with slight intu- 
 mescence. 
 
 Jtfnerite, &l,Ca,]S"a 2 ,ir>,S,Si. Fuses with intumescence. In 
 the I1C1 solution, chloride of barium produces a slight precipi- 
 tate (BaS0 4 ). 
 
 (Compare also the following division, apophiUitc, okcnitc, 
 and analciinc, which are decomposed by muriatic acid to a, 
 gelatinous mass, but not to a thick jelly.) 
 
 Section ii. B. B. in a matrass give none, or only traces of water. 
 
 (Compare datolite, of the preceding division.) 
 
 TEPIIROITE (mangan-chrysolite), Mn 2 SiO 4 . 
 
 HELVITE (Helvin), 3(Be,Mn,Fe) 2 SiO 4 -f (Mn,Fe)S. Boiled 
 with P 2 O 5 , with addition of HNO 3 , both give a violet solution. 
 
 B. B. in the oxidizing flame impart to a borax bead an 
 amethystine hue. Helvite evolves, with muriatic acid, sulphu- 
 retted hydrogen. Tephroite does not. Tephroite is cleav- 
 able at right angles (in one direction perfectly), the other not. 
 Color of helvite is honey-yellow, wax-yellow ; of tephroite, 
 reddish-brown, grayish. 
 
 Closely related with helvite is 
 
 Danalite, 3(Be,Mn,Fe,/n) 2 SiO 4 + (Fe,Mn,Zn)S. This min- 
 eral, containing zinc, gives B. B.* a slight coating of zinc. 
 
288 MINERALOGY SIMPLIFIED. 
 
 With soda on charcoal and with borax the iron reaction. 
 Heated with HC1 evolves H 2 S. Color, flesh-red, gray. 
 
 HAUYNITE (HAUYNE), 2(Na,Ca)AlSi,O 8 -f (N*,C*)SO 4 . LAPIS- 
 LAZULI, and LASUKSTEIN (ultramarine) of similar composi- 
 tion, are of sky-blue and azure-blue color. Haiiynite fuses 
 with difficulty at 4.5 ; lapis-lazuli easily at 3 ; both to a white 
 glass. B. B. both yield with soda upon coal hepar, with char- 
 acteristic brownish-red spots. 
 
 Nosite (Nosean, Nosin), a soda haiiynite, 2Na 2 -f AlSi0 8 -f 
 Na 2 S0 4 , and 
 
 Scolopsite (Skolopsite}, 3tl,Ca.Na 2 ,S,Cl,Si,H" 2 . Color, grayish 
 or brownish. Nosite melts at 4.5 ; skolopsite at 3, with foam- 
 ing and spirting. The hydrochloric acid solutions of both 
 yield, with chloride of barium, a white precipitate of sulphate 
 of barium. Nosite occurs mostly in rhombic dodecahedrons; 
 skolopsite massive with splintery fracture. 
 
 SODALITE (Sodalith), 3Na 2 AlSi 2 8 -f 2NaCl, and 
 
 EUDIALYTE (eucolite), 6Na 2 (Ca,Fe) 2 (Si,Zr) 6 O 15 -f NuCl. 
 B. B. heated with a flux of phosphorus salt and oxide of 
 copper give the reaction of chlorine, by imparting to the flame 
 a transient blue color. The solution in nitric acid gives with 
 nitrate of silver a curdy precipitate of chloride of silver. The 
 diluted IIC1 solution of eudialyte colors turmeric paper orange 
 (reaction for zirconia). When the solution is boiled down sul- 
 phate of potassium to crystallization, and this mass boiled with 
 water, the solution is rendered turbid from precipitated zirco- 
 nia. Sodalite fuses B. B. to a clear, colorless bead. Eudia- 
 lyte to an opaque pistachio-green glass. Spec. grav. of sodalite, 
 2.3 ; of eudialyte, 2.9. 
 
 Wollastonite (tabular spar), CaSiO 2 . B. B. fuses to a color- 
 less semi-transparent bead. After separation of the silica, from 
 its muriatic acid solution, it gives with ammonia none, or only 
 a slight precipitate; with carbonate of ammonium an abundant 
 precipitate of carbonate of calcium. (Compare pectolite (Pek- 
 tolith), HNaCa 2 Si 3 OJ. 
 
 Nephelite (elaeolite, Davyne), (Na,K) 2 AlSi a 8 . 
 
MINERALS WITHOUT METALLIC LUSTKK. 289 
 
 Meionite (Mejonit), Ca 6 Al 4 Si 9 36 , and 
 
 Melilite (Humboldtilite), ( v Na 2 Ca,Mg) 12 (Al,Fe) 2 Si 9 36 . 
 
 In the HC1 solution of these minerals, after separation of 
 the silica, ammonia gives a precipitate (Fe 2 O 3 and A1 2 O 3 ). 
 Meionite fuses, with intumescence and evolution of light, to a 
 vesicular glass, which cannot be perfectly rounded by fusion. 
 The others fuse quietly without intumescence. The solution 
 of nephelite gives, after separation of alumina by NH 3 and fil- 
 tration with oxalate of ammonium, none or a slight precipitate. 
 That of melilite a heavy precipitate (lime). The decomposed 
 nephelite, when containing lime, reacts alkaline after fusion. 
 Melilite does not. (Compare cancrinite.) Nephelite crystallizes 
 hexagonal. Melolite in the tetragonal (dimetric) system. A 
 variety of nephelite (elaeolite) has a fatty lustre. 
 
 A similar deportment to melilite is shown by 
 
 Barsowite* (variety anorthite), CaAlSi 2 8 . B. B. fuses at 4, 
 Melilite at 3 ; the latter with some intumescence, the former 
 quietly. 
 
 (Compare gehlenite, Ca 3 (AlFe)Si 2 10 . Fusible in very thin 
 splinters ; does not swell. Also 
 
 Tachylite, Fe,Mg,Ca,Na. 2 ,l,Si,H: 2 .) 
 
 Division 4. Dissolve in hydrochloric acid, the silicic acid 
 separating without forming a perfect jelly. 
 
 (Many must be finely pulverized before being treated with 
 concentrated acid.) 
 Section i. B. B. in a matrass afford water. 
 
 Klipsteinite, Mn 3 Mn,gi 2 B: 2 . Treated with HC1, evolves 
 chlorine, and silica separates as a slimy powder. With cone, 
 phosphoric acid it yields a violet solution. Gives 9 per cent, of 
 water on ignition. B. B. with borax gives the amethystine 
 color of manganese. 
 
 * Brush (Manual of Determinative Mineralogy, pp. 84 and 86) con- 
 siders amorthite to be a variety of barsowite, both having an identical 
 composition. (Compare also Dana's Syst. of Mineralogy, p. 340.) 
 
 2$ 
 
290 MINERALOGY SIMPLIFIED. 
 
 Apophyllite, 4(H f CaSi a O 6 +Aq)-fKF. 
 
 'Pectolite (Pektolith), HNaCa 2 S5 3 9 , and 
 
 Okenite, H 2 CaSi 2 O 6 + Aq. 
 
 Easily decomposed by HC1, the silica separating in gelatin- 
 ous lumps, without forming a stiff jelly. After the separation 
 of the silica* the solution gives (with an excess of HC1) with 
 ammonia no, or only a slight, precipitate. Pectolite fuses B. B. 
 with slight intumescence to a white enamel, like glass. Yields 
 but little water (4 per cent.). After fusion gelatinizes perfectly 
 with HC1. The others yield much water. Apophyllite 16 per 
 cent., okenite 17 per cent. After fusion are but slightly attacked 
 by HC1. Apophyllite fuses at 1.5 to a vesicular white glass. 
 Okenite at 2.5-3, with frothing to a porcelain-like mass.t 
 
 (Compare xonaltite, 4CaSiO 3 + H 2 O.) 
 
 Anolcite (Analcime), Na.,A:lSi 4 12 -f-2Aq, like the preceding, is 
 decomposed by HC1 to a gelatinous mass, but after separation 
 of the silicic acid, the solution gives, with ammonia, a copious 
 precipitate of alumina. B. B. the first action of the flame 
 renders it white and turbid, but when fusion takes place it be- 
 comes clear, like water, and gives, without intumescence, a 
 shining glass. It is usually found crystallized in cubes and 
 trapezohedrons. Not cleavable. 8 per cent, of water. 
 
 Pyroschrite (Pyrosklerit), Mg 12 Al 2 Si 9 36 +12Aq. 
 
 Chonicrite (Chonikrit), (Ca,Mg) 10 Al 2 Si 7 30 -}-6Aq, and 
 
 Jottyte (Fe,Mg) 6 Al t Si 9 36 -j-12Aq, are readily distinguished from 
 the preceding, and following, by their lower degree of hardness, 
 which is equal to that of calc-spar (=3). B. B. chonicrite fuses 
 at 3.5 to 4, with escape of bubbles ; pyrosclerite at 4 without 
 bubbles ; pyrosclerite is perfectly cleavable in one direction ; 
 color, green ; 1 1 per cent, of water. Chonicrite is not cleavable ; 
 white-yellow ; 9 per cent, of water. Jolyte swells up, fuses 
 with difficulty, is amorphous ; color, brown ; streak, light-green ; 
 
 * In order to separate all the silica completely, the solution in HC1 
 must be evaporated to dryness in a porcelain dish, again digested 
 (moistened) with some HC1, then water added and filtered. 
 
 f Compare sepiolite (meerschaum, sea foam), Mg.,Si 3 8 -f-2Aq. 
 
MINERALS WITHOUT METALLIC LUSTRE. 291 
 
 water, 13 per cent. The following have a similar composition 
 to pyrosclerite : 
 
 Vermiculite (Mg,Fe) 12 Al 2 Si 9 36 +12Aq, an d 
 
 Jeff'erisite, Mg 4 (Alfe) 2 Si 5 20 +6Aq, which B. B. swell up ex- 
 ceedingly. The first exfoliates in wormlike masses, the second 
 swells up prodigiously. 
 
 Mosandrite, &yi*^&,Si^4H,&,$, and 
 
 Catapleiite (Katapltit), (Na a ,Ca)(Si,Zr) 4 O 9 + 2Aq. Have 
 a hardness of 4-4.5, and exhibit cleavage. The former fuses 
 at first with frothing, and then quietly at 2.5-3 to a yellowish- 
 brown glass. The second quietly at 3 to a white porcelain- 
 like bead. The diluted HC1 solution of catapleiite colors yellow 
 turmeric paper orange, and furnishes a precipitate of zirconia 
 (r) when boiled down with sulphate of potassium. The boiling 
 down must be carried on nearly to dryness, and the mass again 
 treated (dissolved) with water. Mosandrite shows no such 
 deportment.* They contain 9 per cent, of water. 
 
 Brewstrite, (Sr,Ba)A-lSi 6 0, 6 -f-5Aq. B. B. fuses at 3 with 
 frothing and swelling. May easily be distinguished from 
 similar minerals by its solution in muriatic acid, giving with 
 sulphuric acid a heavy precipitate of sulphate of barium which 
 is insoluble in acids. Contains 13 per cent, of water. 
 
 Stilbite, (Ca,Na 2 )A-lSi 6 16 -f 6Aq. 
 
 Hipostilbite (desmine), (Ca,Na,) 2 Al 2 Si 9 26 + 12 Aq. 
 
 Chabazite (clmbasite), (HK 2 Ca)A-lSi 5 13 + 6 Aq. 
 
 Prehnite, H 2 CaA-lSi 3 12 . B. B. swell up more or less, and 
 fuse, curling up to an enamel-like mass.f Prehnite yields but 
 little water (4.3 per cent.). The others give in a bolthead 
 much water, losing by ignition 15 to 20 per cent. Clmbasite 
 
 * The titanium in mosandrite is recognized by boiling of the 
 muriatic acid solution with tin-foil; it may contain so little that the 
 liquid thus obtained turns merely reddish. 
 
 f Von Kobell states that, although operating with perfectly normal 
 crystals of stilbite and hypostilbite, he could never verify a dillVivnce 
 in the point of fusion between the two minerals, while according to 
 Fischer desmine fuses to a vesicular glass. 
 
292 MINERALOGY SIMPLIFIED. 
 
 is distinguished by its rbombobedral crystallization and imper- 
 fect cleavage. Stilbite and hypostilbite are perfectly cleavable 
 in one direction. 
 
 Stilbite crystallizes in the monoclinic (Dana), hypostilbite 
 in the trimetric system. A similar, small hemispherical, reni- 
 form or cylindrical fibrous mineral is 
 
 Mordenite (Ca,Na 2 )AlSi 9 22 -f- G Aq. The mineral yields 12 
 per cent, of water. B. B. fuses without intumescence. 
 
 Sepiolite (meerschaum, sea-foam) = [MgSi-fiJ] (Dana), is 
 distinguished from the above by being difficult to fuse, and by 
 absorbing moisture with avidity. 
 
 Deweylite (gymnite), Mg 4 Si 3 ]0 -f 5 Aq, melts" with diffi- 
 culty at 5 ; is amorphous, of a waxy lustre, and resembles 
 somewhat gum-arabic. Absorbs no water. Contains 20 per 
 cent, of water. 
 
 Sordavalite (Sordawalit), Si,l,Fe,Mg,H 2 . Amorphous, fuses 
 at 2.5 quietly to a dense, black, shiny glass. With difficulty 
 decomposed with hydrochloric acid. The solution yields, 
 with caustic ammonia, a heavy greenish-gray precipitate. 
 Color, grayish-black ; streak, liver-brown. Contains 4 per 
 cent, of water. 
 
 Section ii. B. B. in a matrass yield no water, or only a trace. 
 
 (Compare pectolite, chronicrite, and prehnite of the preced- 
 ing section.) 
 
 Some specimens of Lapis-Lazuli (Lasurstein) afford no com- 
 plete jelly, but may be easily recognized by their sky-blue color. 
 B. B. with soda on charcoal yield hepar in characteristic 
 brownish-red spots. 
 
 Cryophyllite (Kryophyllit), (KjLO^FesCAl^e^Si^Og,,. Mica- 
 ceous ; also, scaly, massive. Color, by transmitted light, dull 
 emerald-green ; transverse to the axis, brownish-red. Fuses 
 easily in the candle flame, and B. B. with intumescence to a 
 gray enamel, giving a red lithia flame. 
 
 Tachylite, e,Mg,Oa.:iS T a 2 ,&l,Si,S 2 . Amorphous. B. B. fuses 
 at 2.5 easily and quietly to a black, shining glass. Muriatic 
 acid decomposes the mineral with separation of gelatinous 
 
MINERALS WITHOUT METALLIC LUSTRE. 203 
 
 silica. The solution boiled down with tin-foil does not assume 
 a violet color. 
 
 Schorlomite, Ca 9 Fe 2 (Si,Ti) 12 39 , and Tschejfkinite (Tscliero- 
 kinite), Ce,Fe,Ca,Ti,i. The first fuses quietly, the second 
 with much effervescence, at 3-4, to a black glass or a gray 
 mass. Schorlomite is decomposed by HC1 with some difficulty, 
 leaving the silica behind as a slimy powder. The HC1 solution 
 of both, when evaporated with addition of tin-foil, assumes a 
 violet color, turning to a rose-red by dilution with water 
 (titanic acid). Tscheifkinite is easily decomposed by cone. 
 HC1, the silica separating in gelatinous lumps. Both are black, 
 with a vitreous lustre on a fresh fracture. Streak-powder, gray. 
 
 A similar behavior to schorlomite is exhibited by ivaarite, 
 both of which ought perhaps to be united. 
 
 Wernerite (scapolite*), (Ca,Na 2 ,K 2 )l3i 2 8 . 
 
 Porcellanite^ (porcelain-spar), 8i,&l,Ca,Na. 2 , 1, fuse B. B. 
 at 2.5 with intumescence and emission of light, forming a white 
 blebby glass which is not easily rounded. They are distinctly 
 cleavable in two right angular directions. 
 
 To wernerite belong, according to v. Kobell, nuttalite, glaii- 
 colite, stroganowite. 
 
 Wohlerite, Oa,Na 2 Zr,Cb,gi, B. B. easily fusible at 3 to a 
 light-green, much blistered glass. HC1 dissolves it with sepa- 
 ration of silicic acid in flakes. This solution boiled down 
 with tin-foil assumes at last a fine blue color; after a slight 
 dilution with water a blue filtrate is obtained, which turns 
 yellow turmeric paper orange. Color, wine-yellow to honey, 
 yellow. 
 
 Eukolite probably belongs here. 
 
 Labradorite, (Ca,Na 2 )AlSi 3 1Q , and 
 
 Anorthite, CalSi 2 O 8 . B. B. fuse quietly at 3^4 to a tolerably 
 dense, clear glass. Labradorite is cleavable unequally in two 
 
 * See Brush's Manual of Det. Min., 3d edit., p. 86; also E. S. 
 Dana's Textbook of Min., p. 204. 
 
 f EkebergHe, scapolite, wernerite, porcellanite (v. Kob.), Syn. 
 under wernerite. See Dana's Syst. of Min., 5th edit., p. 324. 
 
 25* 
 
294 MINERALOGY SIMPLIFIED. 
 
 directions at an angle of 86 40' ; on the perfect faces of cleav- 
 age slight striae are visible ; on the less perfect, none. Shows 
 frequently a play of colors, from blue to green, also red and 
 yellow. Anorthite is perfectly cleavable at 85 48'. 
 
 Labradorite is not completely decomposed by HC1. 
 
 Grossularite, or lime-alumina-garnet. The general formula of 
 garnet is R 3 AlSi 3 ]2 , and grossularite is usually Ca 3 AlSi 3 Oi 2 . Many 
 varieties are in a great measure decomposed by concentrated 
 muriatic acid. B. B. fuse quietly at 3, and are readily dis- 
 tinguished from the above by want of cleavage. Many varie- 
 ties of sphene are also decomposed by concentrated acid with 
 separation of silicic acid. The solution boiled with metallic 
 tin assumes a violet color. 
 
 See danburite, which colors the blowpipe flame beautifully 
 green. Compare tephroite, which imparts to a borax bead an 
 amethystine color (manganese oxide). 
 
 Division 5 Are only slightly attacked by hydrochloric acid, 
 and B. B. impart to borax ylass the deep amethystine 
 color of manganese. 
 
 They yield, when boiled down with phosphoric acid to a 
 syrupy consistency, a mass which, with piemontite, assumes 
 directly a violet color ; with the others, only after stirring with 
 a glass rod previously dipped into nitric acid. 
 
 Carpholite (Karpholit), H 4 Mn (Al,Fe,Mn) Si. 2 0, and Arden- 
 nite* Analysis, Si0 2 = 29. GO, A10 3 = 23.50, MnO = 25.88, Fe0 3 = 
 1.86, CaO = 1.6S, MgO = 3.38, V 2 5 ==9.20, ign. 4.04 = 99.09. 
 
 In the closed tube yield water, the first contains 11 p. c. the 
 second 5 p. c. of water. Carpholite fuses at 2.5-3 ; ardennite, 
 at 2. Carpholite is fibrous ; color, straw-yellow. Ardennite, 
 radiated. Locality, Ottrez, in the Ardennes, Belgium. Analy- 
 ses by Lasaulx and Bettendorf. Color, brownish-yellow. 
 
 Spessartite (Spessartin), manganese garnet, (Mn,Fe) 3 AlSi 3 12 . 
 
 * E. S. Dana's Textbook of Alin., page 288. 
 
MINERALS WITHOUT METALLIC LUSTRE. 295 
 
 B. B. fuses quietly at 3. Cleavage indistinct, sometimes do- 
 decahedral. Color, brownish-red. 
 
 Piedmontite (Piemontit), manganese epidote, H 2 Ca 4 (Mn,Fe, 
 Al) 3 Si 6 26 . B. B. fuses with intumescence at 2-2.5. In one 
 direction the cleavage is distinct ; less so in another. Color, 
 cherry-red, reddish black. 
 
 Rhodonite (Rother Mangankiesel), MnSi0 3 , fuses quietly at 
 3 ; distinctly cleavable at 92 55'. Color, rose-red, peach- 
 blossom red. 
 
 Richterite* (Manganamphibol), which resembles it, cleaves 
 at 124. 
 
 Division 6 Not included in the preceding divisions. The 
 remaining minerals are all silicates, except sclteeltte, which 
 "are not attacked, or are imperfectly decomposed by hydro- 
 chloric acid. 
 
 (Compare pyrophyllite, B. B. swelling up and becoming par- 
 tially rounded.) 
 
 DANBURITE,! CaB 2 Si 2 O 8 . B. B easily fuses at 3 to a bead 
 which is clear while hot ; opaque when cold. It tinges the 
 flame green. Boiled with sulphuric acid to dryness the residue 
 imparts to burning alcohol a green color. 
 
 Very closely related is 
 
 Howlite, Ca 4 B 5 Si. 2 23 -f 5Aq. 
 
 SciiEELiTE(tungstate of calcium), CaWO^. B. B. fuses with 
 difficulty at 5. The powder dissolves in HC1, leaving a 
 greenish-yellow or lemon-yellow residue of tungstic acid, 
 soluble in caustic ammonia. If this residue, while yet moist, 
 
 * Brush and E. S. Dana call this mineral pyroxene, including many 
 varieties, from the colorless diopside and u-hite malacolite to black augite ; 
 light-colored varieties fuse to a white glass, while the dark ones give 
 a black glass. 
 
 f I was the first who discovered the presence of boracic acid in 
 danburite, at that time a very rare mineral, but, owing to impurities, 
 gangue, etc., my analysis proved not entirely correct. To Prof. 
 Brush chiefly, belongs the honor of setting matters right, and estah- 
 lishing the above formula. H. K. 
 
296 MINERALOGY SIMPLIFIED. 
 
 be rubbed with a knife blade on paper, it at once changes to a 
 green or bluish-green color. It' the solution is boiled down 
 with phosphoric acid until volatilization begins, the cold mass 
 becomes blue ; dissolved in water, the color disappears, but 
 reappears permanently upon the addition of iron powder. 
 
 Lepidolite (lithia mica, Lithionglimmer, Germ.), (K,Li) 6 , 
 Al 4 Si 12 42 , and 
 
 Cookeite, K^i^^SiJL}. Are micaceous. Cleavage in one 
 direction very perfect. Give to the blowpipe flame the purple- 
 red color of lithia. Lepidolite fuses at 2. Gives in the 
 closed tube little or no water. B. B. cookeite exfoliates, ver- 
 micular, and gives much water. 
 
 Therm ophyllite* (serpentine), Mg 3 Si 2 O 7 -j- 2 Aq. 
 
 Euphyllite (&l,K 2 ,]Sra 2 ,gi,:& 2 ), and 
 
 Margarite, emerylite, H 2 Ca&l 2 Si 2 Q 12 . Are, like the preced- 
 ing, micaceous. 
 
 Thermophyllite. B. B. swells up and gives much water in 
 the closed tube (11 p. c.). The others fuse without, swelling 
 at 44.5, and give little water. Their laminne are not elastic. 
 Euphyllite is easily decomposed by sulphuric acid. Margarite 
 with difficulty. Compare 
 
 Muscovite, K 2 AlSi 2 8 , and 
 
 Biotite, K 2 (Fe,Mg) 7 Al,Si 7 28 . 
 
 Gumbelite, &l,K 2 ,Si,IT 2 . Occurs in thin, short, fibrous 
 layers. B. B. swells up to a fan-like mass, fuses in thin fibres,.- 
 and yields water in the closed tube (7 p. c.). Color, green- 
 white. Not attacked by HC1 and H 2 SO 4 . 
 
 Petalite (Li 6 Al)Si 6 15 , and 
 
 Spodumene(Triphane) (Li 6 Al)Si 3 9 . Do not exhibit the ready 
 and perfect cleavage of the preceding, and their hardness is 
 6.5 ; give to the blowpipe flame the purple-red color of lithia, 
 especially so when the assay held in the forceps is fused together 
 with some bisulphate of potassium. This reaction is rendered 
 more perceptible by taking in the forceps a piece of the mineral 
 
 * Identical with serpentine, see Brush's Determ, Min., p. 87. 
 
MINERALS WITHOUT METALLIC LUSTRE. 297 
 
 and fusing on it bisulphate of potassium, which is repeated 
 several times ; during the blowing the bead is gently moved 
 through the flame. It then shows occasionally purple-red 
 streaks. Petalite fuses quietly to a white enamel. 
 
 Spodumene intumesces, throwing out fine branches, which 
 fuse to a clear transparent glass. Specific gravity of petalite 
 = 2.45, that of spodumene = 3.2. To petalite belongs the 
 variety called 
 
 Castor (Kastor), which distinctly colors the blowpipe flame 
 red. 
 
 Leucophanite (Leucophan), 4NaF -f- 3(Ca,Be) 4 Si 3 O 10 , fuses 
 quietly at below 3 to a transparent colorless glass ; with salt of 
 phosphorus in the open tube gives the fluorine reaction. Phos- 
 phoresces when heated, or when struck with a hammer, emit- 
 ting a reddish-violet light. Cleavage in one direction excel- 
 lent. H."= 3.5-4. 
 
 Wilsonite,* Xl,K 2 ,Mg,Si,S 2 . Fusible at 2 with intumescence 
 to a whitish glass ; yields in a matrass some water. Hardens 
 3. Distinctly cleavable at right angles. 
 
 Nohlite, $b,J?r,Y,IT2' Amorphous ; color, blackish-brown ; 
 lustre, vitreous. B. B. fuses with difficulty, and yields in the 
 closed tube 4^ per cent, of water. In its chemical deportment 
 it is near samarskite. 
 
 Compare sordavvalite, Div. 4, a. 
 
 DIALLAGE'J' (pyroxene). Malacolite or white augite, 
 
 * According to Brush, it is only altered scapolite. See Determina- 
 tive Min., page 88. 
 
 f Professors Dana and Brush consider this mineral a thin, foliated 
 lime-magnesia-pyroxene, t. e., a variety of pyroxene or augite, the 
 general formula of which is RSi0 3 , where R may be Ca,Mg,Fe,Mn, 
 and sometimes also Zn,K 2 Na. 2 . Usually two or more of these bases 
 are present. The first three are most common ; but calcium is the 
 only one that is present always and in large percentage. Besides 
 the substitution of the above bases for one another, these same bases 
 are at times replaced by Al,#e,Mn, though sparingly, and the silicon 
 occasionally by aluminum. Consult James D. Dana's Manual of 
 Mineralogy and Lithology, 3d edition, page 245. New York, 1881. 
 
298 MINERALOGY SIMPLIFIED. 
 
 CaMgSi 2 O 6 . Fusibility, 3.5 ; is distinguished by its pearly, 
 subrnetallic lustre, and distinct cleavage in one direction. 
 Harmotome (Baryt-harmotome), BaAlSi 5 O u + 5 Aq. Distin- 
 guished from the preceding and following by yielding a con- 
 siderable amount of water in a matrass ; and the partial 
 solution in muriatic acid is rendered turbid or gives a precipi- 
 tate with sulphuric acid of sulphate of barium. It occurs like 
 lime-harmotome in twin crystals. 
 
 Axinite, (Ca,Fe,K 2 ) 7 (Al,Fe,B) 3 Si 8 32 , and 
 
 Tourmaline, Al,B,Fe,Mn,Mg,K iJ ,lS r a 2 ,Li 2 ,Si,Ti, with a mixture 
 of fluor-spar and bisulphate of potassium, impart to the blow- 
 pipe flame a transient green color.* Axinite fuses readily and 
 with strong intumescence to a shining dark-green glass. When 
 finely pulverized and fused, axinite gelatinizes in muriatic acid. 
 Different species of tourmaline show different deportments ; 
 some fuse easily and with intumescence, some curl up to a 
 white greenish-gray, rarely black glass ; others fuse with diffi- 
 culty (and a few lithia tourmalines are infusible). Most tour- 
 malines become strongly electric when heated ; axinite does not. 
 
 J)iops!de-\ (Pyroxene, Dana), Ca,Mg,Si 2 O 6 , and 
 
 * By taking the mixture on a hot platinum wire and covering the 
 surface of the flux with the mineral in fine powder form, and heating 
 it, without blowing, in the blue point of a good flame, the color is 
 perceptible at the first moment of fusion. When axinite and tour- 
 maline are reduced to fine powder and fused, then treated with 
 sulphuric acid and evaporated to the consistence of syrup, then 
 alcohol added to it, the latter will, when lighted, burn with a green 
 flame. If about 1 gram, each of finely-powdered axinite or tourma- 
 line are ground together with 3 grams, of bisulphate of potassium, and 
 the mixture fused in a small platinum dish at a red heat, and next a 
 small quantity of alcohol is added, this latter, when lighted, will 
 burn with a distinct green flame, especially towards the end. The 
 platinum dish can be cleaned again with boiling dilute HC1. 
 
 f Diopside is, according to Dana, a pyroxene of the same composition 
 as the previously described lime-magnesia-pyroxene or malacolite, 
 occurs in greenish-white or grayish-green crystals. See Dana's 
 Manual of Min., 3d edition, 1881, page 246. 
 
MINERALS WITHOUT METALLIC LUSTRE. 299 
 
 Augite.* An analysis from Montreal by Hunt gave Si0 2 49.40, 
 A10 3 6.70, *?e0 3 7.83, MgO 13.66, CaO 21.88, Na 2 0.74, H 2 0.50 = 
 100.11. Their hardness is 6 ; fuse at 3.5-4, some quietly, 
 some with slight effervescence. Diopside forming a white, 
 augite a black glass. Both are distinctly cleavable at 93 and 
 87. Diopside is colorless, or light green and gray; augite, 
 black or dark-green. 
 
 Tremolite (grammatite), (Ca,Mg)SiO 3 , and 
 
 Arnphibok (Strahlstein, hornblende), RSiO 3 , as for pyrox- 
 ene. Hardness, 5.5. B. B. they swell up, and at 3-4 fuse with 
 effervescence ; tremolite to a white or slightly colored ; am- 
 phibole to a black or grayish glass. Both are distinctly cleav- 
 able at 124^ and 5j^. Color of the first is white, inclining 
 
 * Hedenbergite is, according to von Kobell, an iron-lime augite, 
 containing but little magnesia. Polylite, hudsonite, and jeffersonite 
 come in here. By the mutual action of acids or negative oxides, 
 three classes of salts are produced, viz., normal, acid, and basic. Nor- 
 mal salts are those in which the acid and base .saturate each other, 
 in which, therefore, all the hydroxyles, whether of acid or base, are 
 eliminated (in the form of Aq.), and the acid radical remains united 
 to metal by means of oxygen, c. </., potassium nitrate and potassium 
 and zinc sulphates (see above). A cut salts are those which retain a 
 part of the acid hydroxyle, e. y., hydrogen potassium sulphate. Basic 
 salts are those in which a part of the hydroxyl of the base, or of the 
 oxygen of the positive oxide, remains in the combination, e. g., basic 
 zinc sulphate (see above). The sulphur acids may be regarded as 
 compounds of negative radicals with hydrosulpburyl (SII) ; e. </., 
 sulphocarbonic acid CS(SH) 2 , and hydrosulphuric acid (hydrogen 
 sulphide) H(SH). Sulphur bases are K(SH).Ca(SH) 2 , etc. Sulphur 
 salts result from the reaction of sulphur acids upon sulphur bases. 
 Most sulphur salts, however, are produced by the action of negative 
 anhydrosulphides on sulphur bases, or on positive anhydrosulphides, 
 e.g., 
 
 As 2 S 5 -f 6(KSH) = 2[AsS(SK) 3 ] + 3H 2 S. 
 
 Arsenic, potassium, potassium, hydrogen. 
 
 sulphide, hydrosulphide, sulphursenate, sulphide. 
 
 (Manual of Qualitative Chemical Analysis ; Fresenius's New Sys- 
 tem. New York, Wiley & Sons, publishers, 1883.) 
 
300 MINERALOGY SIMPLIFIED. 
 
 to green, gray, etc.; of the second, green inclining to black. 
 To these belong asbestos (Ca,Mg,Fe)SiO 3 , and 
 
 Amianthus,* a name applied to the finer and more silky 
 kinds of asbestos. 
 
 Richterite\ is a tremolite containing manganese. Boiled 
 down with concentrated phosphoric acid yields upon addition 
 of some HNO 3 a beautiful violet mass. Chemically related 
 with tremolite is also 
 
 Nephrite. Compact, fine-grained tremolite, having a tinge 
 of green or blue, and breaking with a splintery fracture. H.=6. 
 Feels greasy to the touch. 
 
 Titanite (sphene) CaTiSiO 5 . B. B. fuses with slight intu- 
 mescence to a blackish glass. Partially decomposed by cone, 
 hydrochloric acid. The solution, when boiled with tin, becomes 
 violet (titanic acid), the violet color turning into a rose-red 
 upon dilution with water. We obtain the HC1 solution more 
 readily when the mineral powder is boiled previously with 
 H 2 SO 4 , and the latter completely evaporated, and the residue 
 treated with cone. HC1. System of crystallization, clinorhom- 
 bic. (Monoclinic. Dana.) 
 
 Guarinite is of the same composition, but crystallizes in the 
 rhombic system. (Oythorombic. D.) 
 
 YTTROTITANITE (keilhauite), Ca,Y,3Pe,Xl,Si,Ti. Fuses im- 
 perfectly at its edges, with lively frothing, to a blackish mass. 
 Muriatic acid attacks it but little. If the mineral is fused 
 with caustic potash and the mass treated with muriatic acid, 
 so as to separate the silicic acid, the remaining solution, when 
 boiled with tinfoil, gives the same reactions as sphene. 
 
 * Mountain leather, mountain cork, and mountain wood are similar 
 varieties. 
 
 f Richertite, tremolite, and nephrite -are varieties of Dana's 
 pyroxene, one of the most common minerals. It occurs in almost all 
 basic eruptive rocks, like dolerite, as an essential constituent, and 
 is frequently met with in rocks of other kinds. Common also in 
 granular limestone. In basalt the crystals are generally small and 
 black, or greenish-black. 
 
MINERALS WITHOUT METALLIC LUSTRE. . 301 
 
 ORTHOCLASE (common feldspar, potash-feldspar), K 2 AlSi 6 16 , 
 and 
 
 ALBITE (soda-feldspar), Na 2 AlSi 6 16 . Hardness, 6. They 
 fuse quietly; the former at 5, the latter at 4. Are not attacked 
 by acids. Cleavage of orthoclase is distinct in two directions 
 at right angles (90). Albite in two directions at an angle 
 of 931. 
 
 Closely related to Albite stands 
 
 OLIGOCLASE. Soda-lime feldspar (Ca,Na. 2 ,K 2 )AlSi 5 O u . Fuses 
 at 3.5. Shows striations on one cleavage surface, like 
 
 Labradorite (Labrador feldspar), (Ca,Na 2 )AlSi 3 10 . The 
 latter is, however, mostly decomposed" by HC1, which is not 
 the case with oligoclase. The lime in oligoclase is easily 
 traced, thus : The finely powdered mineral is mixed with fluor- 
 ide of ammonium and the mixture fused in a platinum dish. 
 The residue is boiled with IIC1, and the ensuing solution neu- 
 tralized to excess witli ammonia and filtered. In the filtrate 
 oxalate of ammonium produces a white precipitate of oxalute of 
 calcium. 
 
 Similar to orthoclase is 
 
 Hyalophane, (Ba,K a )AlSi 4 O 12 . This mineral, when fused 
 with soda, hydrochloric acid added, and the silica separated 
 from the HC1 solution, gives with H 2 SO 4 a precipitate of white 
 sulphate of barium. 
 
 ZOISITE, H 2 Ca 4 (AlFe) 3 Si 6 26 , and 
 
 PISTACITE (epidote) of the same composition. H. = 6.5. 
 B. B. fuse at 3-3.5, with swelling and intumescence to a slaggy 
 mass which with zoisite is white or yellowish, with pistacite, 
 black or dark brown. After fusion, they gelatinize with HC1. 
 The color of zoisite is gray, yellowish-gray, grayish-white ; 
 that of pistacite, green (pistachio-green). Zoisite cleaves 
 finely and very distinctly in one direction ; pistacite, pretty 
 distinctly in two directions at 115. 
 
 Grossularite (Grossular, lime-alumina- garnet), Ca 3 AlSi 3 12 . 
 Vesuvianite ( Vesuvian. idocrase), Ca 8 (Al.Foj. 2 Si 7 E8 . 
 
 Pyrope (Magnesia-alumina-garnet), (Mg,Ca,Fe,Mn) 3 Al 
 20 
 
302 MINERALOGY SIMPLIFIED. 
 
 Si 3 Oj,. Hardness, f>.5-7.5. The first and second fuse at '3 ; 
 the first quietly, the second with intumescence; both gelatiniz- 
 ing with HC1 after fusion. The third melts quietly at 3, f>-4. 
 Vesuvian is cleavable in the planes of a quadrangular prism. 
 Grossular and pyrope are not cleavable. Grossular is strongly 
 attacked by concentrated muriatic acid ; its color is green, 
 yellowish -brown, hyacinth-red, and also white. Pyrope is not 
 attacked by acids, and occurs only of a blood-red color. B. B. 
 with borax yields a chrome-green glass. 
 
 MONZONITE, XljFejCajNa^Si, resembles grossolurite, but does 
 not gelatinize after fusion, and is not decomposed either by 
 II Cl or II 2 8O 4 . 
 
 EDELFORSITE* (AEDELFORSITE) (or red zeolite of Adel- 
 fors), CaSi -f Xl5i 3 (v. Kob.) 
 
 SpiiENOCLASEt (Spherioklas, v. Kob.), Ca,Mg,Fe,lSi, have 
 nearly the hardness of 6 ; are not much attacked by acids. The 
 first fuses at 4, with frothing, and, when heated, phosphoresces 
 strongly with a greenish light. The second fuses at 3 quietly ; 
 phosphoresces feebly with a yellow light. 
 
 Compare the following division, C., emerald (beryl), eu- 
 clase, cordierite (iolite), also biotite (uniaxial mica), and 
 muscovite (biaxial mica). 
 
 Obsidian, or volcanic glass. 
 
 Pitch*, Pechstein, a.Jh.faAJra.SL 
 
 Pearlstone, Perlstein, 
 
 Pumice, Bimsstein. 
 
 These fuse with swelling at 3.5 to 4, to a blebby white glass 
 or a porcelain-like mass. They are amorphous. Obsidian is 
 characterized by its glassy lustre, conchoidal and sharp-edged 
 fracture. Pitchstone by its greasy lustre. Pearlstone by its 
 mother-of-pearl lustre, and pumice by its porous, scoria-like 
 form. They are volcanic products. Many pitch 8 tones afford 
 water in the closed tube. 
 
 * Dana (Man. of Min., p. 245) considers this impure Wollastonite 
 (CaSi0 3 ). 
 
 f Dana's Syst. of Min., p. 280. 
 
MINERALS WITHOUT METALLIC LUSTRE. 803 
 
 Class ii r. Infusible, or fusibility above 5, 
 
 Division 1 Some assume a fine blue color when, after previous 
 ignition B. B., they are moistened with cobalt solution and 
 again heated, (alumina.) 
 
 (Some minerals should be first calcined and pulverized.) 
 The hardest anhydrous minerals belonging to this class show 
 this color most distinctly after they are finely pulverized and 
 then moistened with cobalt solution and ignited; the color 
 appears as the mass cools, and is distinctly seen only by day- 
 light. 
 
 Section i. B. B. yield much tvater in a matrass. 
 
 RALSTONITE, Xl,Mg,lS'a 2 .F,l3r 2 , fused in a closed tube with 
 bisulphate of potassium, gives the fluorine reaction. The water 
 yielded in the closed tube reacts for fluorine. 
 
 ALUNITE (alum-stone), K 2 A1 3 S 4 22 -f 6 Aq. 
 
 ALUMINITE (sulphate of aluminium), A1S0 6 -f- 9Aq. "With 
 soda on coal give hepar, which is not the case with the others. 
 Aluminite is easily soluble in muriatic acid ; alunite is not 
 perceptibly attacked, but when it has been ignited, water 
 extjxtcts alum, which may be obtained in octohedral crystals 
 by the slow evaporation of the aqueous solution. The alunite 
 loses 13 per cent, of water by ignition, the aluminite 47 per 
 cent. A similar mineral, felsobanyte, A1 2 S0 6 + 10 Aq, loses 37 
 per cent, of water. A similar behavior to'aluminite is shown by 
 
 PISSOPHANITE (pissophane, garnsdorffite), Xl,Fe,3,H 2 . It 
 occurs at Garnsdorf, near Saalfeld, and at Reichenbach, Sax- 
 ony, on alum slate. B. B. it becomes black, and colors the 
 flame slightly greenish. The aluminite is white or opaque. 
 Pissophane is pistachio-asparagus, or olive-green, and trans- 
 parent. 
 
 Compare potash-alum, ammonia-alum, and KeramoJtaUte 
 (alunogen), which are soluble in water, which is not the case 
 with the preceding minerals. 
 
304 MINERALOGY SIMPLIFIED. 
 
 PLUMBOGUMMITE (plumbo-resinite, Bleigummi), 
 decrepitates and affords water in a matrass, carefully heated. 
 B. B. it swells up, and at a strong heat softens without liquefy- 
 ing. With soda on coal yields metallic lead. Is soluble in 
 nitric acid. The solution yields with molybdate of ammonium, 
 at a gentle heat, a yellow precipitate (P.^OJ. 
 
 CALAMINE (electric-calamine, Kieselgalmei), Zn 2 Si0 4 , forms 
 with muriatic acid a perfect jelly. B. B. on coal with soda 
 it yields, after long blowing, a yellowish-white coating, which, 
 treated with cobalt solution and heated, becomes green 
 in specks. After the separation of silica, the muriatic acid 
 solution is precipitated white by ammonia, and the oxide of 
 zinc thus formed redissolved by an excess of ammonia. 
 
 WAVELLITE (subphosphate of aluminium), A1 3 P 4 ]9 -{- 12Aq. 
 
 Evansite, A1 3 P 2 U + 18Aq. 
 
 Peganite, Al a P 2 O n -f- 6Aq. 
 
 Fi seller ite, Al 2 P 2 O n +8Aq. 
 
 JJerlimte, 2A]P 2 O 8 + Aq. 
 
 Richmondite, P\Xl,ET 2 , and 
 
 Zepharovichite, AlP 2 8 -f- 6Aq. Are principally soluble in 
 caustic potassa. When this solution is mixed with HNO 3 in 
 excess, some molybdate of ammonium added, and heat applied, 
 a yellow precipitate is obtained (P a O t ). 
 
 Berlinite loses by ignition only 4 per cent, of water ; pegan- 
 ite 24 per cent. ; wavellite and 
 
 Zepharovichite 27 per cent.; fischerite 29 per cent. 
 
 Richmondite 35 per cent. ; evansite 40 per cent. 
 
 Similar compounds are : 
 
 Trolleite, A1 4 P 6 27 + 3Aq., with 6 per cent, of water. 
 
 Spaeri-te, A1 5 P 4 23 + 16Aq. 
 
 Redondite, ll,Fe,^ 2 . 
 
 The last two contain 23 per cent, of water each. 
 
 Tavistockite, Ca s AlP 2 O n -|- 3Aq. 
 
 Amphithalite, *l,Ca,^ 2 ,fl a . 
 
 The last two contain 12 per cent, of water each. 
 
 Coeruleolactite, A1 3 P 4 19 -|- IGAq, with 21 percent, of water. 
 
MINERALS WITHOUT METALLIC LUSTKE. 305 
 
 Gibbsite (Hydrargillite), H 6 A10 6 . 
 
 Diaspore, H 2 A10 4 . 
 
 Xanthophyllite (Seybertite), il,ffe,gr,&,Si,l. 
 
 Phokrite (Nacrite),* Al 2 Si 3 12 -f- 4Aq. 
 
 Gibbsite is tolerably easily dissolved by caustic potash, loses 
 by ignition 34J per cent, of water. The others are not soluble 
 in caustic potash. They cleave distinctly in one direction. 
 Xanthophyllite is wax-yellow, loses by ignition only 4J per 
 cent, of water. Diaspore and pholerite nearly \p per cent, 
 of water. Distinguished by their hardness, as nearly 6 for 
 diaspora to only 1 for pholerite. This latter (v. Kobell's na- 
 crite) occurs in scales with a pearly lustre. 
 
 Allophane, AlSi0 5 -f 5Aq. 
 
 Halloysite, AlSi 2 7 +4Aq. 
 
 Samoite, Al*Si 2 10 -f- lOAq. and 
 
 Collyrite (Kollyrit),t Al 2 Si0 6 -f 9Aq, are decomposed by HC1 
 with separation of gelatinous silica. H. of allophane 3 ; it 
 gelatinizes perfectly and colors the blowpipe-flame usually 
 green from an accidental admixture of copper, and loses by 
 ignition 42 per cent, of water ; is amorphous. H. of samoite 
 is 4, has a lamellar structure, and loses 30 per cent, of water. 
 The remainder have a hardness of 1-2. Halloysite contains 
 16, collyrite 33J per cent, of water. 
 
 Oimolite, Al 2 Si 9 24 + 6Aq., and 
 
 Kaolinite (kaolin, porcelain earth), AlSi() 5 -|- 2Aq. (v. Kob.) 
 are with difficulty affected by HC1. Usually amorphous. 
 
 Porcelain earth feels smooth, not greasy, but rather pulve- 
 rulent ; is decomposed by H 2 SO 4 . 
 
 Cimolite is tough, and gives by scraping, shavings. Is im- 
 
 * Brush considers nacrite identical with kaolinite, &lSi 2 O 7 -4-2Aq, 
 whilst pholerite is looked upon as a separate species with the above 
 formula. See Brush's Determ. Min.. p. 89. 
 
 f Von Kobell's " Kollyrit," analyzed by Klaproth, has the same 
 formula with lOAq. Restates in a note that he refers to a species found 
 in the " Stephani mine," at Chemnitz, which gelatinizes with acids, 
 while other kinds, like that from Weissenfels, do not gelatinize. 
 
 26* 
 
300 MINERALOGY SIMPLIFIED. 
 
 perfectly decomposed by sulphuric acid. These minerals lose 
 by ignition 12 to 16 per cent, of water. Many " aluminous 
 earths, argillites, or clays, which are not sufficiently known, 
 but form with water a doughy mass, and develop the odor of 
 clay, might be appended here ; also lithomarge (Steinmark), 
 with 14 per cent, of water; also schiotterite (opal allophane), 
 with 35 per cent, of water ; miloschite and bolus, with 24 to 26 
 per cent, of water. These form with water no dough ; the 
 latter Udft on the contrary, fall to pieces with crackling. 
 
 (Co4>are from the following division, lazulite, svanbergite, 
 pyroJ)Si\lite, agalmatolite, disterite, wbrthite, myeline, which 
 in a matfUss likewise yield water, but only a small quantity. 
 Compare also ripidolite.) 
 
 Section ii. B. B. in the closed tube yield little, or no water. 
 
 Alumian, A1S 2 7 . B. B. yields with soda on charcoal hepar. 
 
 Lazulite, (Mg,Fe)&lP 2 O 9 +H,0. B. B. tinges the flame with 
 a feeble greenish color,* swells up, and crumbles to small 
 pieces, thereby losing its blue color, and becoming white. 
 By acids it is not directly attacked, and its blue color under- 
 goes no change. Caustic potash produces a partial solution, 
 which, treated with HNO 3 in excess, yields, when boiled witli 
 molybdate of ammonium, a yellow precipitate (P 2 O 5 ). 
 
 Svanbergite, &l,Ca,]?}"a 2 ,^ 2 ,, ET 2 . B. B. with soda on coal 
 gives a sulphur reaction. The partial nitric acid solution gives 
 a reaction for phosphoric acid with molybdate of ammonium. 
 Col0r, yellow or yellowish-brown, 
 
 WILLEMITE (Hebetine, anhydrous silicate of zinc), Zn 2 SiO 4 . 
 B. B. assumes with cobalt a blue, and in places a green color. 
 Gelatinizes in muriatic acid. The solution yields with ammo- 
 nia, after separation of silicon, a precipitate (ZnO) soluble in an 
 excess. From the ammoniacal solution sulphide of ammonium 
 throws down white sulphide of zinc. 
 
 MYELINE (Talksteinmark), AlSi0 5 . 
 
 AGALMATOLITE (figure stone), Al,l 2 ,S,I"I r 
 
 * Rendered distinct if previously moistened with sulphuric acid.. 
 
MINERALS WITHOUT METALLIC LUSTRE. 307 
 
 PYKOPHYLLITE, Al,Si 3 9 -f- H 2 0, have a low degree of hard- 
 ness, 1-3. " Pyrophyllite in one direction is perfectly cleavable. 
 B. B. it spreads out into fan-like shapes, and increases to 
 twenty times its former bulk. It is infusible, but partially 
 crumbles to pieces and glows with a white light. Loses by 
 ignition 5 per cent, of water. The others are not cleavable, 
 and B. B. unalterable. Myelin is somewhat decomposed by 
 acids. Related to pyrophyllite is 
 
 Westanrte, 3tl,Si,IT 2 , which has a brick-red color. 
 
 Muscovite (bi-axial mica, potash mica), H 2 AlSi 2 O g , 
 direction is perfectly cleavable ; the thin laminae ape^nexible 
 and elastic. B. B. does not expand perceptibly, and with diffi- 
 culty fuses in very thin scales. With cobalt solution it acquires 
 partially a pure blue color ; is not attacked by acids. Hard- 
 ness, 2.5. 
 
 Disterrite* (brandisite) (variety of clintonite, see Dana), 
 (Mg G ,Ca 6 ,Al 2 ,Fe 2 )Si0 20 . Orthorhombic. Cleavable in one direc- 
 tion. Fresh laminae B. B. turn grayish-white and turbid, and 
 thence moistened with cobalt solution and reheated, assume a 
 blue color. Hardness, 4-5. Concentrated sulphuric acid de- 
 composes it. 
 
 ANDALUSITE (chiastolite), AlSi0 5 , and 
 
 DISTHENE (cyanite, kyanite), AlSi0 5 , are only slightly 
 attacked by acids. B. B. phosphorus salt decomposes them, 
 and separates a siliceous skeleton. Aridalusite cleaves tole- 
 rably well in two directions at an angle of 91 J ; its hardness 
 7.5. The crystals called chiastolite have undergone decompo- 
 sition, and have usually a hardness of 5.5. They are generally 
 in twins consisting of four individual prismatic crystals, so 
 grown together with their principal axes parallel, that a cavity 
 remains between them which contains generally clay slate. 
 Disthene is distinctly cleavable in two directions at 100, 
 especially distinct in one direction. Hardness, 6, and some- 
 
 * Brush considers it identical with sr.ylnrlite (Determ. Min., p. 90.) 
 
308 MINERALOGY SIMPLIFIED. 
 
 times less. The spec. grav. of andalusite is 3.2 ; that of 
 disthene 3.6. Closely approaching to disthenite is 
 
 Sillimanite (worthite, monrolite, tribolite),* AlSi0 5 . Its 
 spec, grav., however, is less, namely, 3. 
 
 TOPAZ (fiuosilicate of aluminium), AlSi(0,F 2 ) 5 . 
 
 Rubellite^ (lithia tourmaline), (Li,Na,K) 6 Al 6 B 2 Si 9 45 , are not 
 attacked by acids. B. B. not perfectly dissolved by phosphor- 
 ous salt, the bead becoming opalescent on cooling. Topaz 
 retains its transparency, and does not swell when ignited. 
 Heated in larger pieces the yellow varieties turn white, assum- 
 ing upon cooling a rose-red hue. Rubellite becomes white, 
 puffs sometimes to a slaggy mass. Topaz is in one direction 
 distinctly cleavable. Hardness, 8. Rubellite is not cleavable. 
 Hardness, 6.5. The last-named mineral becomes electric when 
 heated, which happens only witH a few varieties of topaz. 
 The spec. grav. of topaz is 3.5 ; that of rubellfte, 3. 
 
 CORUNDUM (sapphire, emery, crystallized alumina), A10 3 . 
 
 CHRYSOBERYL, Be,A10 4 . These minerals are not attacked 
 by ordinary acids, but when they are heated with phosphoric 
 acid until volatilization commences the fine powder of corun- 
 dum is completely dissolved, less so that of chrysoberyl. The 
 solutions yield with caustic potash a precipitate which is 
 redissolved by an excess (alumina). B. B. in fine powder 
 form they are slowly but perfectly dissolved by salt of phos- 
 phorus, and the bead is not opalescent when cold. Hardness 
 of sapphire, 9 ; its specific gravity, 4. Hardness of chrysoberyl, 
 8.5 ; its specific gravity, 3.7. 
 
 (Compare spinel.) 
 
 Many varieties of spinel and leucite, when pulverized, 
 moistened with cobalt solution and ignited, become blue. Some 
 kinds of cassiterite, or tin stone, in powder form assume, when 
 moistened with cobalt solution upon ignition, a bluish or 
 
 * Dana (Man. of Min. and Lithol., New York, 1881, p. 285) calls 
 the mineral "tribolite," syn. with sillimdnite and bucholzite. 
 
 f Rubellite is a variety of tourmaline. See Brush, Determ. Min., 
 etc., p. 90. 
 
MINERALS WITHOUT METALLIC LUSTRE. 309 
 
 greenish tint, but readily yield with cyanide of potassium on 
 coal globules of tin. 
 
 The blue color, which quartz in a fine powder form acquires 
 with cobalt solution, differs from that of the preceding minerals 
 by inclining to red, and by the blue being less intense. 
 
 Division 2 __ Moistened with cobalt solution, and ignited, as- 
 sume a green color (zinc}. 
 
 It is sufficient to heat the moistened bead to a red heat. 
 
 The compounds of oxide of zinc belonging to this division 
 give to the coal a coating which is yellow while hot, but becomes 
 paler on cooling, and when moistened with cobalt solution and 
 again ignited assumes a green color. 
 
 SMITHSONITE (Zinkspath, carbonate of zinc), ZnCQ 3 . 
 
 Hydrozincite (Zincbliithe), Zn 3 CO 5 + 2Aq, dissolve in HC1 
 with effervescence by the escape of carbonic acid ; the solu- 
 tion yields with caustic ammonia a precipitate soluble in 
 excess. In a matrass smithsonite affords little or no water; 
 hydrozincite, a large quantity. 
 
 WILLEMITE (hebetine, anhydrous silicate of zinc), 2n 2 8i. 
 
 C ALAMiNE,(hydrous silicate of zinc, Kieselgalmei),^!!^!-}-^, 
 with muriatic acid form a perfect jelly. In a matrass the latter 
 yields water, the former none. B. B. silicates of zinc, when 
 treated with cobalt solution, become green in places, with a 
 large share of blue. 
 
 (Compare zinc vitriol and zincblende ; also kassiterite.) 
 
 Division 3 After ignition, give an alkaline reaction, and 
 color moistened turmeric paper brown, or red litmus paper 
 blue. 
 
 BUUCITE* (hydrate of magnesia), H 3 MgO a . 
 
 IIVDROMAGNOCALCITE, (6a, 
 
 * A manganese brucite is pi/rorhroite, H 2 fMnMg)0. 2 , showing a 
 similar deportment to Inn-itf, yielding, however, when boiled with 
 cone, phosphoric acid, and addition of some nitric acid, a violet color 
 (manganese). 
 
310 MINERALOGY SIMPLIFIED. 
 
 HYDROMAGNESITE (hydrocarbonate of magnesium), 2CaCO 3 
 -|- H 2 Mg0 2 , in a matrass affords much water, \vhich is not the 
 case with the remaining ones. Brucite dissolves easily and 
 quietly in muriatic acid ; the other two minerals with effer- 
 vescence. The concentrated muriatic acid solution of brucite 
 and hydromagnesite yields no precipitate with sulphuric acid ; 
 that of hydromagnocalcite a heavy one (gypsum). 
 
 A similar behavior as the last is exhibited by 
 
 Predazzite, 2CaC0 3 + H 2 MgO 2 , and 
 
 Pencatite, CaCO 3 + H 2 MgO 2 . 
 
 Related to hydromagnesite is nemalite, H 2 MgO 2 . (Pro- 
 bably a mixture of hydromagnesite and brucite, v. Kob.) 
 
 Calcite (carbonate of calcium), CaC0 3 , and 
 
 ARRAGONITE (needle spar), CaC, effervesce strongly when 
 moistened with muriatic acid, and are soluble even in large 
 lumps without th aid of heat. The concentrated solution 
 gives, without sulphuric acid, a precipitate of sulphate of calcium, 
 but none when largely diluted. B. B. arragonite crumbles to 
 powder; calcite decrepitates, but does not crumble like arra- 
 gonite. Specific gravity of calcite, 2.G-2.8 ; that of arragonite, 
 2.0-3. 
 
 (Compare Strontianite.) 
 
 DOLOMITE (magnesian limestone), (Ca,Mg)CO 3 . 
 
 MAGNESITE (carbonate.of magnesium), MgCO 3 , moistened 
 with muriatic acid dorfot effervesce, unless reduced to a 
 powder, and then only slightly ; but by application of heat they 
 effervesce/4trongly and dissolve. The concentrated solution of 
 dolomite gives with sulphuric acid a precipitate of sulphate of 
 calcium; that of magnesite, none. Magnesite is entirely or 
 chiefly dissolved in sulphuric acid ; the other only partially.* 
 
 (Compare the next following minerals.) 
 
 STRONTIANITE (carbonate of strontium), SrCO 3 , and 
 
 * Brown spar (mesetine spar) shows a behavior similar to dolomite, 
 but it becomes by ignition black and feebly magnetic. Compare also 
 siderite (ironspar) and diallogite (manganese spar), many varieties 
 of which upon ignition exhibit an alkaline reaction. 
 
MINERALS WITHOUT METALLIC LUSTRE. 311 
 
 BAIIYTO-CALCITE (carbonate of barium and calcium), (Ba, 
 Ca)CO 3 , are readily distinguished from the preceding, since 
 in small lumps they do not, or only transiently, effervesce with 
 cone. HC1, but are soluble with effervescence in very dilute 
 muriatic acid ; the solution, even when largely diluted, gives 
 with sulphuric acid a precipitate, with baryto-calcite at once, 
 with strontianite only after a while. B. B. strontianite spreads 
 out into cauliflower-like ramifications, which emit a brilliant 
 white light, and tinge the flame with a purple-red. Baryto- 
 calcite tinges the flame with a feeble greenish-yellow, while 
 the mineral acquires a green color. 
 
 (Compare yttrocerite ; likewise talc and muscovite, some 
 varieties of which after ignition react alkaline.) 
 
 Division 4 In hydrochloric acid, or, if this has no effect, in 
 nitric acid, entirely or chiefly dissolved, without forming 
 a jelly or leaving any considerable residue of silicic acid. 
 
 Lithiophorite, Mu,Cu,CojLi 2 ,Ba,Xl,Mn,fl 2 , color, bluish-black ; 
 lustre, dull. B. B. colors the flame carmine-red (lithia). With 
 salt of phosphorus gives reactions for copper and cobalt. 
 
 Ludwigite,* Comp. R 4 FeB 2 10 . R. 5 iron protoxide and mag- 
 nesia, combined with iron sesquioxide, and boron trioxide. 
 Color, black. Fusible with difficulty. Gives with sulphuric 
 acid and alcohol the green reaction of boric acid. 
 
 Cervantite, SbO 2 = Sb 2 O 3 -f Sb 2 O 6 . B. B. on coal infusible, 
 but with soda on coal easily reduced to metallic antimony, 
 yielding also the antimony coating. Affords little or no water 
 in the closed tube. 
 
 Siderite (carbonate of iron, spathic iron), FeCO 3 (Mn, 
 CaMg) ; 
 
 Mesitite, Mesitine (mesitine spar, breunnerite, braunspath), 
 Mg 2 FeC 8 ; 
 
 DIALLOGITE (rhodochrosite, carbonate of manganese), 
 MnCO 3 ; and 
 
 * Brush considers it only a variety of sussexite. Man. of Detenu. 
 Min., page 82. Consult E. S. Dana's Textbook of Min., 1880, page 358. 
 
312 MINERALOGY SIMPLIFIED. 
 
 Zaratite (emerald nickel, Nickelsmaragd), Ni 3 CO 5 -\- 6Aq, 
 are soluble in muriatic acid (by the aid of heat) with 
 effervescence caused by the escape of carbonic acid ; the 
 remainder do not effervesce. Siderite, mesitite, and emerald 
 nickel B. B. form a black or gray mass which is attracted by 
 the magnet. Emerald nickel is recognizable by its green color, 
 and the fact that its muriatic acid solution turns pale blue by 
 an excess of ammonia. Siderite in most varieties decrepitates 
 very strongly ; to borax glass it imparts a bottle-green color. 
 Mesitite dissolved in nitric acid, and the oxide of iron preci- 
 pitated with ammonia, yields with oxalate of ammonium no 
 precipitate, but if ammonia be added, and then phosphate of 
 soda, a heavy precipitate (of phosphate of magnesium and ammo- 
 nium) falls. The solution of siderite gives with the last-named 
 reagents only a slight precipitate 'or none. Diallogite B. B. 
 becomes gray or black, and sometimes magnetic ; to borax 
 glass in the oxidizing flame it imparts an amethystine-red. 
 
 Hydrotalcite (vblknerite), l,Mg,fi,,<3. Yields in a ma- 
 trass much water. B. B. in the R. F. does not become mag- 
 netic. The powder effervesces with muriatic acid, and is 
 thence dissolved. Neutralizing the acid solution with bicar- 
 bonate of sodium and filtering off the precipitate, the filtrate 
 gives with oxalate of ammonium none, but with phosphate of 
 sodium and ammonium a heavy white precipitate. 
 
 Parisite, 3(Ce,La,Di)CO 3 -f (Ca,Ce)Fl. ' Slowly soluble 
 in HC1 ; the not too acid solution gives with oxalic acid a 
 white precipitate, which on ignition becomes brick-red (oxide 
 of cerium). 
 
 GOETHITE (pyrrhosiderite, Eisenrutil), H 2 Fe0 4 . 
 
 LIMONITE (brown hematite, brown ochre), Hgf'e.jOg,* heated 
 
 * The yellow clay iron stone, Bohnerz, bog iron ore, Eisenniere 
 (reuiform iron ore), are mixtures of limonite, clay, sand, phosphate 
 of calcium and of iron, etc. They are generally fusible, sometimes 
 easily so, and are dissolved by muriatic acid witli separation of clay, 
 etc. Anthosiderite, Fe0 3 35.7,SiO 2 60.3,H 4 040= 100. 
 
MINERALS WITHOUT METALLIC LUSTRE. 313 
 
 before B. B. in the reduction flame become black and magne- 
 tic ; in a matrass afford water ; they dissolve slowly and with- 
 out effervescence in concentrated muriatic acid ; the solution 
 with ammonia gives a reddish-brown precipitate. Goethite 
 occurs crystallized, and in one direction is distinctly cleavable ; 
 color is hyacinth-red, also brown, and blackish-brown; by 
 ignition it loses 10 per cent. Limonite occurs sometimes in 
 fibrous, but generally in dense masses, of a brown color ; upon 
 ignition it loses 14-J per cent. The streak of each is ochre- 
 yellow. 
 
 Targite (hydro-hematite}, H 2 Fe 2 7 , has a brownish-red streak ^ 
 and loses in the closed tube 5-7 per cent, of water. B. B. 
 heated in R. F. becomes black and magnetic ; soluble with 
 difficulty in HC1. Compare 
 
 Hematite (specular iron, red hematite), Fe 2 O 3 , which in 
 many varieties is without metallic lustre. Can easily be dis- 
 tinguished by the cherry-red color of its streak, and by its 
 yielding no water, or only traces of it in the closed tube. 
 
 SPHALERITE* (zincblende, black jack, sulphuret of zinc), 
 ZnS. 
 
 MARMATITE* (sulphuret of zinc and iron), (Zn,Fe)S, and 
 
 GREENOCKITE (sulphuret of cadmium), CdS, boiled with 
 muriatic acid give off sulphuretted hydrogen (and if previously 
 mixed with iron powder, even at ordinary temperature). B. 
 B. with soda they form hepar. On coal, greenockite deposits a 
 brownish-red ring of oxide of cadmium ; the others leave a 
 yellowish coat of oxide of zinc. Concentrated nitric acid dis- 
 
 From Antonio Pereia, Brazil, where it is intimately associated with 
 magnetic iron, appears to be a mixtiire of limonite with quartz, for 
 the silica separated by the decomposition with HC1 behaves with caus- 
 tic potash like quartz powder. 
 
 * Von Kobell. Brush makes no distinction between the two mine- 
 rals, but considers marmatite a ferriferous variety of sphalerite, and 
 gives to the latter the formula (Zn,Fe)S. A part of the Zn being 
 often replaced also by cadmium ; also containing in minute quantities 
 thallium^ indium, and gallium. 
 27 
 
314 MINERALOGY SIMPLIFIED. 
 
 solves all three with separation of sulphur; in this solution 
 ammonia causes a precipitate, which is principally redissolved 
 in excess when the mineral is sphalerite or greenockite, while 
 marmatite leaves a perceptible amount of oxide of iron as a 
 residue. The ammoniacal solution yields with sulphide of 
 ammonium either a white precipitate of sulphide of zinc, or a 
 yellow one of sulphide of cadmium. 
 
 WAD (bog manganese, earthy manganese), H 2 Mn a O 5 . 
 
 ZINCITE (red zinc ore, manganesian oxide of zinc, Roth- 
 zinkerz), ZnO (with MnO). B. B. with borax give the reac- 
 tion of manganese. The first has a brown, the second a red 
 color. 
 
 (Compare psilomelane (is of a gray color). Also pyrochroite 
 and the next mineral.) 
 
 ASBOLITE* (earthy cobalt), Mn,Co,Ou,#r B. B. with borax 
 forms a fine sapphire-blue glass (Co). With soda on platinum 
 foil yields a green color (Mn). On charcoal generally emits a 
 slight arsenical odor. (Some varieties of asbolite fuse.) 
 
 Uraninite (Uranpecherz, pitchblende), U 3 O g , and 
 
 Zippeite (Uranocker), U 3 S 2 O, 5 + 12Aq. B. B. give with 
 salt of phosphorus in O. F. a yellow bead, which in R. F. 
 becomes deep green (uranium). In nitric acid they are soluble, 
 forming a yellow liquid, from which ammonia throws down a 
 sulphur-yellow precipitate. The nitric solution of zippeite 
 gives a heavy precipitate with nitrate of barium. 
 
 The color of uraninite is pitch-black, that of zippeitef 
 yellow.' The spec. grav. of uraninite is 6.5, that of zippeite 3. 
 
 Turquoisl (callaite, Kalait, Germ.), A^O^n- 5Aq, con- 
 taining Cu, colors the blowpipe flame green ; when mois- 
 tened, muriatic acid tinges it with a transient blue color. In 
 potassa it is chiefly soluble, leaving only a cupreous residue. 
 The nitric solution gives a yellow precipitate with molybdate 
 
 * A variety of wad. 
 
 f Many impure varieties of uranochre are fusible. 
 J Turrjuois receives a good polish, and is highly esteemed in Persia, 
 where it is mainly found, as a gem. 
 
MINERALS WITHOUT METALLIC LUSTRE. 315 
 
 of ammonium (phosphoric acid). In the closed tube much 
 water (19 per cent.). Color, sky-blue to green. Spec. grav. 
 2-2.8. 
 
 APATITE (phosphate of calcium), 3CaP.p s +CaCl,F) 2 . Fusi- 
 bility, 5. B. B. moistened with sulphuric acid it colors the 
 flame feebly green. The nitric acid solution gives with molyb- 
 date of ammonium a yellow precipitate of phosphoric acid. The 
 nearly neutral solution gives with oxalate of ammonium a white 
 precipitate of oxalate of calcium. B. B. in a matrass yields no 
 water. Spec. grav. 3.2. 
 
 MONAZITE (mengite, emerite), 5(Ca,La,Di) 3 P 2 8 ,Th 2 P 2 O . 
 Infusible. The mineral powder in the loop of a platinum wire, 
 moistened with sulphuric acid, tinges the flame green. Soluble 
 in muriatic acid with difficulty. The powdered mineral fused 
 with caustic potash, and the mass treated with water and fil- 
 tered, and the filtrate, acidulated with nitric acid, produce*, 
 with molybdate of ammonium,, a yellow precipitate (P S O 5 ). The 
 residue not dissolved by water is dissolved in a little HC1, and 
 oxalic acid added, when a heavy precipitate is thrown down, 
 which, ignited in a platinum spoon, turns brick-red (oxide of 
 cerium). At present found only in small, tabular crystals of a 
 reddish-brown or yellow color. Spec. grav. 4.9-5.2. 
 
 CHILDRBNITE, (Fe,Mn) 8 Al 2 P 6 29 + 15Aq. B. B. frits (bakes) 
 only on the surface, affects after ignition in the reducing flame 
 the magnetic needle. Moistened with sulphuric acid it colors 
 the flame greenish. Soluble with difficulty in muriatic acid. 
 The partial solution yields with molybdate of ammonium a yel- 
 low precipitate (P 2 O 6 ). 
 
 POLYCRASE (polymignite), Y,LT,^e,Ti,Cb 2 ,*fi 2 . B. B. decrep- 
 itates when heated suddenly, but is infusible and unchange- 
 able. If the powder is melted with caustic potassa, and the 
 mass boiled with muriatic acid and then filtered, the liquid 
 assumes, if boiled down in contact with tinfoil, a blue color 
 
 * Or $l> 2 (niobic acid of Continental chemists). Cl> 2 (columbic 
 acid according to Dana). 
 
316 MINERALOGY SIMPLIFIED. 
 
 (the liquid must be considerably concentrated however), which 
 upon the addition of very little water becomes more clear, and 
 yields a blue filtrate ; or, the mineral may be fused with bisul- 
 phateof potassium, the mass dissolved in dilute HC1, and boiled 
 with tin, when the same blue solution is obtained. The dilute 
 acid solution colors turmeric paper orange-yellow (zirconia). 
 Color, black. Spec. grav. 4.7-5. H. 0.5-6.5. 
 
 FLUOCERITE (fluoride of cerium), Ce,Fl 4 , and 
 
 Bastnasite (bamartite), CeF,2(Ce,La)C, evolve with bisul- 
 phate of potassa or strong sulphuric acid hydrofluoric acid 
 gas, corroding glass (a watch glass or glass tube may be ex- 
 posed to the fumes).* Bastnasite gives off at the same time 
 carbon dioxide (CO 2 ). Their color is yellow. Spec. grav. of 
 fluocerite 4.7, that of bastnasite 4.93. 
 
 A similar deportment is shown by 
 
 Yttrocerite, (Cu,Ce,Y)F 2 . Like fluorecite ; but has an 
 imperfect cleavage in two directions in the planes of a quadra- 
 tic prism. Color, violet-blue, inclining to white arid gray or 
 grayish-red. Lustre, weak, vitreous. 
 
 Division 5 With muriatic acid form a jelly, or are decom- 
 posed with separation of silicic acid, without gelatinizing ; 
 do not exhibit the characters of the preceding numbers. 
 
 Section i. In a matrass afford water. 
 
 DIOPTASE (emerald copper), H 2 CuSi0 4 . 
 
 CHRYSOCOLLA (copper-green, Kieselmalachit), CuSi0 3 -j- 
 2Aq. 
 
 CYANOCHALCITE, 6u, a ,-&i,lI 2 , and 
 
 Asperolite} (chrysocalla), CuSiO 3 -f 3Aq. B. B. fused 
 with soda on charcoal effervesce and yield a glass which in- 
 
 * Must not be inhaled, being corroding and poisonous. 
 
 f Hermann has given this -name to an amorphous mineral from 
 Tagilsk, Russia, so named on account of its great brittleness. Dana 
 considers it a variety of chrysocolla. See System of Min., pp. 402, 
 403, and 404. 
 
MINERALS WITHOUT METALLIC LUSTRE. 317 
 
 closes a ductile copper globule. Dioptase gives with acids a 
 perfect jelly. Chrysocolla, cyanochalcite, and ..asperolite are 
 decomposed without gelatinization. When the powdered 
 minerals are boiled with caustic potash, a deep blue solution 
 is obtained, and the powder turns a brownish color. By con- 
 tinued boiling, the blue color of the lye diminishes again, and 
 the powder turns brownish-black. From the filtered solution, 
 sal ammoniac, when added in sufficient quantity, throws down 
 hydrous silica. Dioptase loses by ignition 11 per cent, of 
 water. Cyanochalcite 16 per cent. Chrysocolla 20 per cent. 
 Asperolite 27 per cent, of water. Cyanochalcite as an azure- 
 blue color; the others are either green or bluish-green. 
 
 Uranotil, Ca 2 U 6 Si 5 O 30 -|- 15Aq. Color, lemon-yellow, turn- 
 ing" black by ignition. The HC1 solution yields after separa- 
 tion of the silica, with ammonia, a sulphur-yellow precipitate 
 (tf). Loses by ignition 12.7 per cent, of water. Crystallizes 
 in needles. 
 
 Xonaltite, 4CaSiO 3 -f H 2 O. Infusible according to Ram- 
 melsberg. The HC1 solution gives, after separation of the 
 silica, with ammonia no precipitate, but oxalate of ammonium 
 throws down oxalate of calcium. Yields 3.7 per cent, of water. 
 Massive ; color, white. 
 
 Thorite, ThSiO 4 + H 2 O, and 
 
 Cerite, (Ce,La,Di) 2 SiO 4 -|- H a O, gelatinize with hydro- 
 chloric acid.* B. B. witli soda on charcoal give no copper 
 globule. The solution of cerite yields (when not too acid) with 
 oxalic acid a white precipitate, which, upon being heated in a 
 platinum spoon, turns brick-red (cerium oxide). The color of 
 thorite is black ; streak, dark brown. Color of cerite, red- 
 dish-gray ; streak, white. Their spec, gravities are from 
 4.7-5. 
 
 Chloropal (nontronite), (*-'eSi 3 O 9 -f 5Aq. 
 
 * The jelly of cerite produced with dilute HCl is som-'wh it soft, 
 that obtained with oonc. HCl forms a gelatinous mass. 
 
 27* 
 
318 MINERALOGY SIMPLIFIED. 
 
 Rottisite (gentliite), H 4 (Ni,Mg) 4 S5 3 O 12 , are amorphous and of 
 a green color. Wolchonskoite of a dark leech-green, the others 
 yellowish-green. B. B. wolchonskoite gives to the borax bead 
 in both O. F. and R. F. an emerald-green color which, on 
 cooling, does not fade (chromium). Chloropal gives a green 
 glass which fades on cooling. If the powdered mineral is 
 treated with caustic potash, it turns without boiling, blackish, 
 if the species is chloropal ; if rbttisite, the color is, only after 
 boiling and with a strongly concentrated solution, changed to 
 brown. Wolchonskoite undergoes very little change. The 
 HC1 solution of rottisite assumes with ammonia a blue color. 
 
 Rottisite closely resembles 
 
 Genthite (v. Kob.)* 
 
 Thraulite (hisingerite, gillingite), ^e,Fe,Mg,Ca,Si,Aq. 
 
 Xylotyh (mountain wood, Bergholz), Fe,Mg,Si,Aq. B. B. 
 after fusion or long heating in the reduction flame become 
 magnetic ; are readily decomposed in muriatic acid without 
 forming a perfect jelly. The solution of the second, after 
 separation of the oxide of iron by ammonia, gives a heavy 
 precipitate with ammonia and phosphate of sodium ; that of 
 the first gives none. Thraulite is friable and brittle; its color 
 brownish-black. Mountain wood has been found only in tough, 
 fibrous, wood-like masses, exhibiting a wood-brown color. 
 
 SEPIOLITE (meerschaum), MggSi 8 O g -}- 2Aq, is very light; 
 specific gravity, 1.5. B. B. burns white and shrinks. Muriatic 
 acid decomposes it easily into a gelatinous mass. Absorbs 
 water greedily. Contains 10 per cent, of water. 
 
 BASTITE (Schillerspath). 
 
 CHRYSOTILE (an asbestiform variety of serpentine allied to 
 picrolite, Dana), show submetallic, opalescent, pearly lustre, 
 the first upon one cleavage plane, the second upon its compos- 
 ing fibres. Roasted B. B. bastite turns brown ; chrysotyle 
 white. Both are decomposed by concentrated muriatic acid 
 
 * Brush calls both minerals "gentliite." 
 
MINERALS WITHOUT METALLIC LUSTRE. 319 
 
 with gelatinization, still easier by sulphuric acid without gela- 
 tinization. Loss by ignition, 12 per cent. 
 
 MKTAXITE* resembles chrysotile, but is of feeble, silky 
 lustre both in its massive and fibrous variety. 
 
 Cerolite (kerolite), H 2 Mg 2 Si 3 7 -f- H 2 O. Hardness, .2-3. 
 Assumes, when moistened with cobalt solution, and heated 
 B. B., a pale flesh color. When heated loses 30 per cent, of 
 water. 
 
 SERPENTINE (hydrated silicate of magnesium), Mg 3 Si 2 O 7 -f- 
 2Aq. Concentrated muriatic acid dissolves it without gelati- 
 nization. Usually massive and dense. Hardness, 3-4. Loss 
 by ignition 12 to 13 per cent. The following hydrous magne- 
 sium silicates show a similar deportment, but exhibit, however, 
 a crystalline structure and cleavage. 
 
 PYCROPIIYLL,! hardness, 2.5. Loss by ignition 10^ per 
 cent. 
 
 PICROSMINE,J hardness, 2.7. Loss by ignition 9 per cent. 
 
 MARMLITE, hardness, 2.5 to 3. Loss by ignition 15.7 
 per cent. 
 
 Kdm mererite\\ (penninite), Mg 5 AlSi 3 O u -\- 4Aq, hardness, 1.5 
 to 2. Loss by ignition 13 per cent. Color, crimson-red; the 
 others are of a greenish or greenish-gray color. Kammererite 
 is chemically identical with Kotschubeit (ripidiolite, Brush), 
 Mg 5 AlSi 3 O u -f- 4Aq, but are distinguished optically, the former 
 being mon-axial, the latter bin-axial. 
 
 (Compare also chlorite and ripidolite, which are decomposed 
 by muriatic acid, though with difficulty, 6. Compare gymnite.) 
 
 * Dana (Manual of Min. and Lithol., pp. 307-9) considers bastite, 
 chrysotile, and nietaxite as different varieties of serpentine, H 2 Mg 3 Si 2 8 
 -f- lAq. Consult likewise Dana's Textbook of Min., p. 328, and 
 Brush's Determinative Min., p. 94, " serpentine." 
 
 f Pycrophyll and 
 
 J Picrosmine are varieties of pyroxene (Brush, Determ. Min., p. 88). 
 
 Marmolile is a thin, foliated, and pearly variety of serpentine 
 (Brush, Ibid., p. 94). 
 
 || According to Kenngott, kammererite is only a variety 
 colored red by chromic acid. 
 
320 MINERALOGY SIMPLIFIED. 
 
 ANTIGOKITE* (a foliated variety of serpentine). 
 
 MONRADITE (pyroxene), (Mg,Fe)SiO 3 -f H 2 O. 
 
 NEOLITE, Mg,l,Si,H 2 . 
 
 CLiXTONiTEf (seybertite), (Mge^Ca^Xl^Pe)^!. Likewise 
 decomposed by concentrated muriatic acid with formation of 
 jelly. Loss by ignition amounts only from 4 to 6 per cent. 
 Antigorite is found in foliated masses, cleavable perfectly in 
 one direction. Hardness, 2.5. Monradite, crystalline, foliated. 
 Hardness, 6. Clintonite distinctly cleavable in one direction. 
 Hardness, 4.4 to 5. Neolite very soft. Hardness, 1. Is 
 greasy like soap to the touch. 
 
 Section ii. In a matrass (jive no water, or only a trace. 
 
 (Compare the last-named minerals of the preceding division.) 
 
 GADOLINITE, (Y,Ce,Be,Fe) 3 $i0 5 , and 
 
 GEHLENITE,]: Ca 3 (AlFe)Si 2 10 . Gelatinize perfectly with 
 muriatic acid. B. B. gadolinite swells up, and many varieties 
 exhibit a momentary glow. At a long-continued heating assume 
 a dirty green color, some varieties becoming rounded on their 
 sharp edges ; is not cleavable. Color, black, blackish-green. 
 Specific gravity, 4 to 4.3. Gehlenite does not swell up. In 
 thin scales becomes rounded on the edges without showing any 
 peculiar phenomena. Color, grayish-white. Specific gravity, 3. 
 
 CHRYSOLITE (olivine), (Mg,Fe) 2 SiO 4 , and 
 
 CHRONDRODITE, Mg 8 Si 3 O u (contains F). Gelatinize per- 
 fectly with muriatic acid. With sulphuric acid the second 
 evolves a large proportion of hydrofluoric acid gas; the former 
 gives none. B. B. chrysolite is but little alterable. Color, 
 olive-green. Hardness, 7. H. of chondrodite, 6.5. Color, 
 
 * A variety of serpentine, Mg 3 Si 2 7 -f- 2Aq., with a small amount of 
 ^e, according to Brush's Determin. Min., p. 94. 
 
 f Analysis by G. Brush obtained Si0 2 , 20.24; &10 3 , 39.13; fe0 3 , 
 3.27; MgO, 20.84; CaO, 13.69; H 2 0, 1.04; Na 2 0(K 2 0), 1.43; Zr0 2 , 
 0.75 = 100.39 from Amity, N. Y. Dana's Textbook, p. 336. 
 
 J The mineral foun.d at Monzoni, called massive gehlenite, fuses 
 much more easily, and forms a separate species. 
 
MINERALS WITHOUT METALLIC LUSTRE. 321 
 
 yellow, brownish, greenish. Hyalosiderite is" an olivine con- 
 taining iron. The solution in aqua regia yields, after separa- 
 tion of the silica, with ammonia a brownish-red precipitate of 
 hydrated sesquioxide of iron. 
 
 Monticellite (batrachite), (Ca,Mg) 2 SiO 4 . The solution 
 gives after the precipitation by ammonia of some iron, with 
 oxalate of ammonium a white precipitate (lime). 
 
 (Compare ropperite.) 
 
 BOLTONITE (forsterite), Mg 2 SiO 4 , in one direction perfectly 
 cleavable ; hardness, 5 ; specific gravity, 3 ; color, yellow. Cone. 
 HC1 decomposes it, and the silica separates as a slimy powder. 
 
 LEUCITE (amphigene), K 2 Al,Si 4 Oi 2 . Decomposed by HC1 
 without gelatinizing ; the silicic acid being separated as fine 
 powder. Many varieties give with cobalt solution a fine blue. 
 Not cleavable. It occurs crystallized almost always in trapezo- 
 hedrons. Hardness, 5.5 ; specific gravity, 2.5 ; color, grayish 
 or yellowish-white. 
 
 Division G -The species yet remaining, ichich could not be 
 arranged tinder the foregoing divisions, may be separated 
 into tivo groups distinguished by their hardness. 
 
 Section i. Hardness under 7 {quartz). 
 
 BIOTITE, HEXAGONAL MICA (uniaxial mica, Einaxiger 
 Glimmer), K 2 (Fe,Mg) 7 Al 3 Si 7 O 28 . 
 
 MUSCOVITE, OBLIQUE MICA (biaxial mica, common mica, 
 Zweiaxiger Glimmer, Germ.), K 2 AISi 2 O 8 . 
 
 TALC (soapstone, steatite, Speckstein), H 2 Mg 3 Si 4 O 12 . B. B. 
 in a matrass yield none, or little water. Talc and soapstone (mas- 
 sive talc) do not lose more than 5 per cent. All, except the last, 
 distinctly cleavable in one direction ; hardness, 1-2.5. Talc 
 has a greasy feel, the others have not. Biotite is decomposed 
 by concentrated sulphuric acid, the others are not. Biotite 
 is optically uniaxial, sometimes biaxial, but the angle of 
 divergence does not exceed 5 and seldom 1. Turned in the 
 stauroscope, the black cross is not changed, while with the 
 
322 MIXER ALCHJY SIMPLIFIED. 
 
 others it is changed with various colors. The optical angle of 
 muscovite is 44-48 ; of rnagarite, the same ; and of phlogo- 
 pite, 3 20, seldom less than 5. The lamina? of muscovite 
 are elastic, flexible ; those of talc are flexible but not elastic. 
 Steatite (Speckstein) is a dense talc, feels also greasy to the touch. 
 
 (Compare pyrophyilite.) 
 
 A similar behavior to biotite is shown by 
 
 Margarodite, K 2 AlSi 2 8 (-{- Aq), and 
 
 Phlogopite, K 2 Mg 6 AlSi 5 O 20 , which are decomposed by concen- 
 trated sulphuric acid. They are optically biaxial, and alter 
 the cross in the stauroscope of Kobell with different colors. 
 
 Chlorite, Mg,Fe,l,Si,II 2 . 
 
 DELESSITE, M^Fe^l^gi,!^. 
 
 RIPODOLITE (Klinochlor) Mg 6 AlSi 3 14 + 4Aq. B. B. in a 
 matrass affords a considerable amount of water. Loss by 
 ignition, 12 per cent ; cleavage distinct in one direction ; 
 laminaB not elastic. Chlorite usually forms micaceous, granular 
 masses. Delessite is fibrous ; their hardness 1 to 2.5. By 
 boiling with muriatic acid (or still more easily with sulphuric 
 acid) they are decomposed. Ripidolite B. B. burns white, and 
 fuses at 5.5 to a grayish-yellow enamel. Chlorite turns black, 
 and moves a delicate magnetic needle. B. B. ripidolite gives 
 when fused together with the proper amount of borax a green 
 bead (oxide of chromium). Chlorite gives the reaction for 
 iron. 
 
 Closely related to ripidolite is 
 
 Lei.tchtenbergite of a yellow color, is optically uniaxial, while 
 
 Ripidolite, especially the variety clinochlor, is binaxial. 
 
 Here belongs 
 
 Pennitite (Pennin), Mg 6 AlSi 3 14 -f 4Aq. Color, green, like 
 chlorite ; is uniaxial, and crystallizes in rhombohedrons of 
 
 Related with the preceding minerals are 
 
 CMoritoid (Sismondin, masonite), (Fe,Mg)(Al,Fe)Si0 6 +H 2 0, 
 is not essentially attacked by muriatic acid, but is decomposed 
 by concentrated sulphuric acid. It is easily distinguished by its 
 
MINERALS WITHOUT METALLIC LUSTRE. 323 
 
 hardness, 5-G, and its loss by ignition amounting to only 7^ 
 per cent. 
 
 Cerolite (Kerolitli). (Compare Division 5, .) Amorphous, 
 yellowish-white; hardness, 2-3; loses 30 per cent, by heating. 
 HC1 decomposes it mostly. 
 
 Bawxite (beauxite) (AH?e)0 3 -f- 2 Aq. Amorphous, grayish- 
 white, reddish-brown. In the closed tube loses 20 per cent, of 
 water. Hydrochloric acid affects it but little, while concen- 
 trated phosphoric acid dissolves it almost entirely. Soluble, 
 also, in sulphuric acid. 
 
 (Compare argyllite.) 
 
 WoLCHONSKOiTE,^r,&'l,Pe Mg,Si,H 4 . Amorphous, dark green. 
 Boiled down with phosphoric acid it furnishes an emerald-green 
 solution, not altered by dilution with water, while gelatinous 
 silicic acid separates. Chromite, sometimes of a metal-like 
 fatty lustre, gives also the above chromium reaction, but the 
 mineral is black, and the streak yellowish-brow r n. 
 
 (Compare I. B. 3.) 
 
 WARWICKITE, 2MgTi0 3 + Mg 4 B 6 O 13 . Its powder is de- 
 composed by concentrated sulphuric acid. The solution when 
 evaporated to dryness imparts to burning alcohol a green 
 color. When this mass is boiled with hydrochloric acid and 
 tin-foil, the liquid, when duly concentrated, assumes a violet 
 color, which upon the addition of water turns into a rose-red. 
 
 BRONZITE (broncite, hypersthene), (Mg,Fe)SiO 3 . 
 
 ANTHOPIIYLLITE, Fegi + Mg 3 gi 2 . The former is perfectly 
 cleavable in one direction, and shows a pearly, metallic lustre ; 
 the second is distinctly cleavable in two directions at 124^, 
 and presents a similar but inferior lustre. Their hardness, 
 5-5.5. Hypersthene, while closely approaching to bronzite, 
 cleaves distinctly at 86^. 
 
 Tungstite (tungstic acid, Wolfrarasaeure), WO 8 . Color, 
 yellow. Gives, when boiled with phosphoric acid, a bluish solu- 
 tion, which, when stirred while warm with iron powder and a 
 little water, assumes at once a dark-blue color. Soluble in 
 
324 MINERALOGY SIMPLIFIED. 
 
 alkalies. B. B. gives with salt of phosphorus in O. F, a color- 
 less bead, which in R. F., or better with tin on charcoal, turns 
 blue on cooling. Occurs in soft earthy masses. 
 
 Scheelite (tungstate of calcium), CaWO 4 . Fuses at 5. When 
 boiled in nitric acid there remains a lemon-yellow residue of 
 tuns-tic acid, which is soluble in alkalies. Boiled down with 
 phosphoric acid yields a blue mass, which diluted with much 
 water forms a colorless solution, which, when agitated with 
 iron powder, assumes a fine blue color. H. 4.5-6. Spec. grav. 6. 
 
 Cassiterite (tinstone, peroxide of tin), SnO 2 B. B. fused 
 on coal with cyanide of potassium the splinters are reduced to 
 metallic tin (alone, only with much difficulty) ; is considerably 
 heavier than similar minerals. Specific gravity, 6.8-7. Hard- 
 ness, 6.5. 
 
 Octahedrite (anatase) also rutile (titanic acid), Ti0 2 . 
 When the fine powder has been fused with potassa and then 
 dissolved in muriatic acid, the solution boiled with metallic 
 tin assumes a violet color, which, upon addition of water, turns 
 red without further change. The fine powder may, before 
 treating it with HC1, also be first fused with bisulphate of pot- 
 assium, or dissolved with hot cone, sulphuric acid. Anatase is 
 perfectly cleavable in the planes of a quadratic pyramid at 
 136 22'. Rutile in the planes of a quadratic or equiangular 
 octagonal prism. Hardness of anatase 5.5. Color, indigo- 
 blue, brown, rarely red. Hardness of rutile, 6.5. Color, 
 generally red, brownish-red, blackish. Both possess a strong 
 metallic adamantine lustre. A similar deportment is shown by 
 
 Brookite^ also TiO 2 . Crystallization rhombic, primary 
 form, a right rhombic prism. Hardness, 5.5-6. Color, yel- 
 lowish to reddish-brown. 
 
 (Compare perofskite, which is sometimes hyacinth-red, and 
 crystallizes in cubic crystals. Compare sphene.) 
 
 ^Eschynite, (Ce,La,Di,Fe,Y) 3 Cb 2 (Ti,Th) 3 O u , and 
 
 * The opaque, iron black crystals with submetallic lustre, from 
 Arkansas, have been named by Sbeppard arkansite. 
 
MINERALS WITHOUT METALLIC LUSTRE. 325 
 
 Euxenite (Y,Fe,U) 3 Ti 2 Cb 2 O 12 ,H 2 O. When the powder is 
 fused with caustic potash in a silver crucible, and the mass 
 lixiviated with water, the filtered solution neutralized with 
 muriatic acid yields a precipitate, which, boiled with an excess 
 of concentrated muriatic acid and tin-foil, furnishes, upon the 
 addition of water, a blue solution, which turns olive-green in 
 the air, and then fades. If the residue from the lye is boiled 
 with muriatic acid and tin-foil, a rose-red solution is obtained, 
 upon dilution with water, which turns turmeric paper orange 
 if the mineral is asschynite. B. B. asschynite swells up and 
 becomes yellow or brownish. Color of the mineral, black ; 
 streak, light brown. Euxenite is not altered B. B. Its color 
 is brownish-black ; the streak, reddish-brown. Both possess a 
 fatty, metal-like lustre. 
 
 A very similar chemical compound is 
 
 Pyrochlore (from Miask), Cb 2 ,Ti,ThCe,Ca,^e,lS T a 2 ,F. Found 
 in octahedrons. Color, brown-red. Streak, light yellow. 
 
 OPAL, SiO 2 -(- Aq, in a matrass affords water. B. B. with 
 soda effervesces and forms a transparent glass ; infusible by 
 itself. Hardness, 6-6.5 ; amorphous. Boiled in potassa liquor 
 it is mostly, or entirely, dissolved. The solution treated with 
 a sufficient quantity of sal ammoniac throws down hydrous 
 silicic acid. Colorless, milk-white, yellow, brown, red. 
 
 Xenotime (phosphate of yttrium), ( Y,Ce) 3 P 2 O 8 . B. B. moist- 
 ened with sulphuric acid it colors the flame feebly green ; in 
 phosphorus salt it dissolves with difficulty, forming a colorless 
 glass. Hardness, 5. 
 
 (Compare childrenite, also orthoclase, and hyalophane.) 
 
 Section ii. Hardness, 7, and above 7. 
 
 (Compare of the preceding division cassiterite, rutile, and 
 opal, the hardness of which approaches 7 closely.) 
 
 QUARTZ (amethyst, chalcedony, jasper, flintstone, rock 
 crystal), SiO a . B. B. on coal, with soda, effervesce and fuse 
 easily to a transparent glass (too much soda must not be added). 
 Alone they remain infusible and unchanged in the strongest 
 heat of the blowpipe. The powdered mineral fused with caus- 
 28 
 
326 MINERALOGY SIMPLIFIED. 
 
 tic potash yields, with water, a more or less complete solution, 
 which, when mixed with a sufficient quantity of chloride of 
 ammonium, gives a heavy white precipitate of hydrous silica. 
 Hardness of quartz, 7. Struck with a steel gives sparks. Its 
 usual crystalline form is a hexagonal prism, sometimes termi- 
 nated at both ends by six-sided pyramids. Spec. grav. 2.5-2.8. 
 Crystals often as pellucid as glass, and colorless ; sometimes 
 topaz-yellow, red, green, blue, and brown colors to black. In 
 some varieties the colors are in bands or stripes (agate). 
 Here belongs 
 
 Tridymite, a hexagonal form of silica with a spec. grav. 
 2.2-2.3. 
 
 COKDIERITE (iolite), (Mg,Fe) 2 Al 2 Si 3 18 . 
 
 STAUROTITE (staurolite), H 2 (Mg,Fe) 3 Al 6 Si 6 3i . Hardness, 7. 
 B. B. do not form a transparent glass with soda. The former 
 is fusible at 5-5.5. Color, blue and grayish-blue. Spec, grav., 
 2.6. The latter is infusible. Color, brown, reddish-brown. 
 Spec, grav., 3.6. 
 
 BERYL (emerald, aquamarine, Smaragd), Be 3 AlSi 6 18 . 
 EuCLASE, H 2 Be 2 AlSi 2 10 . 
 PHENACITE (Phenakit), Be 3 Si. 
 
 ZIRCONITE (Zirkon), ZrSiO 4 . Their hardness, 7.5. B. B. 
 beryl and euclase, at a strong heat, become milk-white and 
 rounded on the thin edges. Beryl crystallizes in hexagonal 
 prisms ; cleavage basal and pretty distinct. Euclase crystal- 
 lizes in clino-rhombic prisms; is perfectly cleavable in two 
 directions at right angles. Phenacite arid zirconite B. B. are 
 unchangeable, except that the last loses its color. If powdered 
 zircon is fused with caustic potassa, and the mass boiled with 
 muriatic acid, the diluted acid colors turmeric paper orange 
 (zirconia). If the HC1 solution is evaporated to crystallization 
 and the mass boiled with a saturated solution of sulphate of 
 potassium, a white precipitate falls (zirconia) ; both occur only 
 crystallized. Phenacite in hexagonal pyramids, prisms, or 
 rhombohedrons ; its specific gravity, 2.7 to 3. Zirconite in 
 quadratic pyramids and prisms. Specific gravity, 4.4-4.6. 
 
MINERALS WITHOUT METALLIC LUSTRE. 327 
 
 TOPAZ* (topaz, fluosilicate of aluminium, physalite), (3tl,Si, 
 Fl). Hardness, 8 ; crystallizes in rhombic prisms ; basal 
 cleavage distinct. The yellow varietyf by exposure to a 
 gentle heat changes from yellow to pink or pale crimson, only 
 seen after cooling. If boracic acid is fused and heated on 
 platinum wire until the flame ceases to be tinged with green, 
 the bead, upon the addition of finely pulverized topaz, again 
 imparts, after continued blowing, a green color to the flame 
 (fluo-boron gas). Gives with salt of phosphorus in the open 
 tube the fluorine reaction. 
 
 UWAROWITE (Ouuarovite, lime-chrome garnet), Ca 3 rSi 3 lr 
 Color, emerald-green. B. B. infusible ; changes upon heating 
 to a blackish-green, but resuming, upon cooling, its former 
 color; with borax it fuses to an emerald-green glass. Hard- 
 ness, 7.5-8. Spec, grav., 3.5. 
 
 Spinel (aluminate of magnesium), (Mg,Fe)(Al,*-'e)0 4 . 
 
 Pleonaste (ceylonite, ceylanite, iron-magnesia spinel). 
 
 GAIINITE (zinc spinel), (Zn,Mg)(Al,Fe)0 4 . 
 
 CHLOROSPINEL (magnesia-iron spinel). Their hardness 
 7.5-8 ; they occur nearly always crystallized in octahedrons. 
 The mineral powder heated together with phosphoric acid in a 
 platinum crucible until volatilization commences, produces, 
 when cold, upon the addition of water, an almost complete 
 solution. This solution, treated with an excess of caustic 
 potash, yields a copious white precipitate when the mineral is 
 spinel. Chlorospinel gives a yellowish, pleonast a greenish 
 precipitate. The liquid filtered off from these deposits gives, 
 with sulphide of ammonium, no precipitate. Gahnite gives, 
 in the phosphoric acid solution with caustic potash, a slight 
 precipitate, and the liquid portion, when filtered off, yields with 
 sulphide of ammonium a greenish-black deposit, which later 
 
 * According to St. Claire-Deville, and Fanque, topa/,, and some 
 other silicates containing fluorine, when highly heated lose the fluo- 
 rine as fluoride of silicon. Topaz thus loses 23 per cent, of this 
 fluoride; (Dana). 
 
 f Brazilian topaz. 
 
328 
 
 MINERALOGY SIMPLIFIED. 
 
 B. B. on charcoal gives a heavy coating of zinc oxide. Spinel 
 and pleonast in powder form are B. B. rather easily soluble in 
 a bead of salt of phosphorus. The glass does not become 
 opalescent on cooling. Gahnite B. B. treated with borax and 
 phosphorus salt is nearly insoluble. Spinel has a red or 
 bluish color ; pleonast is black ; gahnite dark-green ; chloro- 
 spinel olive-green and translucent. Very similar to gahnite 
 are 
 
 Dysvlite* and 
 
 Kreittonite* The latter acts before ignition upon a delicate 
 magnetic needle. The spec. grav. of gahnite, dysluite, and 
 kreittonite, 4.3-4.6; that of other spinels, 3.6. 
 
 CARBON GROUP, 
 
 DIAMOND (Diamant,Germ.), C. Crystallizes in the tesseral 
 (isometric, D.) system. In octahedrons, dodecahedrons, and 
 more complex forms (Fig. 121). Faces often curved. Cleav- 
 
 Fig. 121. 
 
 age. octahedral and perfect. Color, white or colorless, also 
 yellowish, red, orange, green> blue, brown, and black. Lustre, 
 adamantine. Transparent; translucent when dark-colored. 
 H. 10. G. 3.5-3.6. When rubbed exhibits positive or vitre- 
 ous electricity. Diamond consists of pure carbon ; it is infu- 
 sible, and not attacked by any acids. At a high temperature, 
 and in contact with air (oxygen), it is consumed, producing 
 carbonic acid gas, C0 2 (carbon dioxide). Diamonds are dis- 
 
 * Brush considers both these as varieties of galmite. 
 
CARBON GROUP. 329 
 
 tinguished by their superior hardness and brilliant reflection of 
 light. Some specimens exposed to the sun for a short time 
 give out light when carried to a dark place. Diamond strongly 
 refracts and disperses light (sparkles). No other gems, unless 
 they are polished, become positive ( -f- ) electric when rubbed. 
 It may also be easily distinguished by the use of a small 
 writing or scratching diamond, which fails to mark the faces 
 of a real diamond when drawn lightly across them. The coarse 
 diamonds, unfit for jewelry, are called "bort," and the kind 
 in black pebbles or masses, from Brazil, " carbonado." The 
 latter occur sometimes in pieces 1000 carats* in weight; they 
 have a spec, grav., 3 to 3.42. Another kind is much like 
 anthracite. Spec- grav. 1.06, although as hard as diamond 
 crystals. 
 
 Goppert states that he found algoe-like plants inclosed in 
 diamonds. 
 
 They occur principally in alluvial soil and in rocks of second- 
 ary formation in the East Indies, Golconda, and in Brazil. 
 They are also found in the sands of the rivers which have 
 their sources in the Uralian Mountains in Russia. In South 
 Africa, where they were first discovered in 1867, they occur 
 in the gravel in the Vaal River. In the United States the 
 diamond has been met with in North Carolina, Georgia, 
 Virginia, Calfornia, Oregon, and Idaho. The prevalent opinion 
 is that diamond, like coal and petroleum, is of vegetable or 
 animal origin. 
 
 Diamonds are valued according to their color, transparency 
 and size. The rose diamond is more valuable than the pure 
 white, owing to the great beauty of its color and its rarity. 
 The green diamond is also much esteemed. The blue is prized 
 
 * A carat is a conventional weight, and is divided into 4 grains, 
 which are a little lighter than 4 grains Troy ; 74^ carat grains are 
 equal to 72 Troy grains. The term carat is derived from the name of 
 a Ix-an in Africa, which in a dried state has long been used in that 
 country for weighing gold. These beans were early carried to India, 
 and were employed there for weighing diamonds. 
 
 28* 
 
330 MINERALOGY SIMPLIFIED. 
 
 only for its rarity, as the color is seldom pure. The brown, 
 gray, and yellow varieties are of much less value than the pure 
 white or limpid diamond. The black diamond is exceedingly 
 rare, but without beauty. 
 
 1 carat (4 grains) .of small diamonds, employed for polishing 
 the larger ones, for cutting glass, etc., costs from $5 to $6. 
 
 A polished diamond (brilliant) weighing 1 carat is valued at 
 from $40 to $50. The prices of diamonds increase to such an 
 extent with their size that a brilliant weighing 5 carats may 
 cost as much as $750 to $1 000. The largest diamond at present 
 in Europe is in the possession of the Queen of Portugal; it 
 weighs 215 carats, and is valued at upwards of $750,000. 
 
 Mock diamonds. " Bristol stones," " Irish diamonds," 
 " Cape May diamonds," and u California diamonds" are skill- 
 fully cut quartz crystals. They are easily detected by the file 
 and their lightness. 
 
 CHAPTER X. 
 
 CHARACTERISTIC BEHAVIOR OF THE MOST IMPORTANT ORES 
 BEFORE THE BLOWPIPE AND WITH SOLVENTS.* 
 
 AN ore is a mineral compound in which some metal, usually a 
 valuable metal, forms a prominent constituent. Although a na- 
 tive metal is in this sense .not an ore, still, where a native metal 
 or other valuable compound mineral is distributed intimately 
 through the gangue, the mineral and gangue together constitute, 
 in the language of the miner, the ore of the metal it produces. 
 
 The more common ores are compounds of the metals with 
 metalloids, such as sulphur, arsenic, oxygen, chlorine, bromine, 
 iodine, phosphorus, silicon, etc. 
 
 * On this subject the author has made free use of Elderhorst- 
 Nason's Manual on Blowpipe Analysis and Dana's Manual of Mineral- 
 ogy and Lithology, 3d edit. New York, 1881. 
 
ORES OF ANTIMONY. - 331 
 
 Ores of Antimony. 
 
 NATIVE ANTIMONY Rhomboheclral. Color and streak, 
 tin-white. Lustre, metallic. Brittle. 
 
 Composition: Antimony, containing sometimes silver, iron, 
 or arsenic. 
 
 B. B. on charcoal fuses easily, and gives a white coating in 
 both O. F. and R. F. If the blowing be intermitted, the 
 globule continues to glow, giving off white fumes, until it is 
 finally covered with antimonious oxide, tinging the R. F. 
 bluish-green. 
 
 Stibnite, gray antimony, antimony sulphide. Color and 
 streak, lead-gray. Lustre, metallic. Brittle. H. 2. G. 4.5. 
 Tri metric. 
 
 Composition: Sb 2 S s = S. 28.2, Sb. 71.8. Fuses in the 
 flame of a candle. 
 
 B. B. on coal it is absorbed, giving off white fumes and a 
 sulphurous odor. When pulverized and treated with caustic 
 potassa, is rapidly colored ochre-yellow, and mostly dissolved. 
 The solution, when mixed with an acid, yields an orange- 
 colored precipitate. When pure entirely soluble in hot HC1, 
 with evolution of H a S. 
 
 Berthierite, (iron sulphantimonite): Composition : FeSbS 
 = S. 29.12, Sb. 56.61, Fe. 10.09, Mn. 4.9. 
 
 Color, dark steel-gray. Lustre, metallic, less bright than 
 gray antimony. H. 2-3. G. 4.2. Trimetric. On charcoal 
 coats the coal with white oxide of antimony, and after long 
 heating yields a magnetic globule (iron). Gives with fluxes 
 the iron reaction. Easily dissolved by hydrochloric acid with 
 evolution of sulphide of hydrogen. 
 
 Kermesite (red antimony). In tufts of cherryred capillary 
 crystals. Lustre, adamantine. II. 1.5, G. 4.5. Monoclinio. 
 Streak, brownish-red. 
 
 Composition: Sb a O 3 -f 2Sl> 2 S 3 = Sb. 75.3, O. 4.9, S. 19.8. 
 Is an antimony oxide and sulphide. 
 
 B. B. on charcoal behaves like gray antimony. It dissolves 
 
002 MINERALOGY SIMPLIFIED. 
 
 mostly in HC1 with evolution of sulphide of hydrogen. The 
 powdered mineral, when heated with potash solution, turns 
 yellow and dissolves. 
 
 Minerals containing antimony : allemontite, valentinite, senarmon- 
 tite, cervantite, livingstonite, etc. 
 
 Ores of Arsenic. 
 
 NATIVE ARSENIC Rhombohedral. Color and streak, tin- 
 white, but usually dark-grayish from tarnish. Brittle. II. 
 3.5. G. 5.G. Hexagonal. 
 
 Composition : As, with traces of Sb, Ag, Fe, Co, and Ni. 
 
 B. B. volatilizes readily before fusing, with the odor of 
 garlic ; also burns with a pale bluish flame when heated just 
 below redness. 
 
 Orpiment, yellow arsenic sulphide. In foliated masses. 
 
 Color and streak, fine yellow. Lustre, brilliant pearly. 
 H. 1.5. G. 3.4. Trimetric, 
 
 Composition : As 2 S 8 = S. 39.0, As. 61.0. 
 
 B. B. it wholly evaporates with an alliaceous odor, and on 
 charcoal burns with a blue flame. Soluble in aqua regia and 
 caustic potassa. 
 
 Realgar, red arsenic sulphide. Color, bright red to orange. 
 Lustre, resinous. H. 1.5. M. 3.5. Monoclinic. 
 
 Composition : As8= S. 29.9, As. 70.1. Fuses readily and 
 volatilizes like the former. 
 
 B. B. on coal with soda in R. F. gives off arsenical fumes, 
 burns with a yellowish-white flame. Aqua regia dissolves it 
 with difficulty, sulphur being precipitated. Boiled with caustic 
 potassa it is decomposed, leaving a brown powder (As 6 S) 
 undissolved. 
 
 Arsenolite, white arsenic. Color, white. Lustre, silky. 
 II. 1.5. G. 3.7. Isometric. 
 
 Composition: As 2 O 3 As. 75.8, O. 24.2 100. Heated 
 in a tube gives a crystalline sublimate octahedrons. 
 
ORES OF BISMUTH. 333 
 
 B. B. on coal with soda gives a strong garlic odor. Slightly 
 soluble in water, more so in water acidulated with IIC1. 
 
 Minerals containing arsenic: arsenopyrite, scorodite, polybasite, 
 enargite, domeykite, whitneyite, algodonite, smaltite, cobaltite, uic- 
 colite, pharmacosiderite, arseniosiderite, etc. 
 
 Ores of Bismuth. 
 
 NATIVE BISMUTH Bi. Color, reddish-white; streak, white; 
 subject to tarnish : brittle when cold, but somewhat malleable 
 when l.eated. H. 2.5. G. 9.7. Hexagonal. 
 
 Composition: Pure bismuth, with traces of arsenic, sulphur, 
 or tellurium. 
 
 B. B. on charcoal vaporizes, and leaves a yellow coating on the 
 coal. Fused with sulphur and iodide of potassium, coats the coal 
 with a red sublimate of iodide of bismuth. Readily dissolved 
 by nitric acid ; the solution is precipitated white by water. 
 
 Tetr ad y mite (telluric bismuth) Massive or granular. Lus- 
 tre, splendent metallic. H. 2. -2. 5. G. 9.7. Hexagonal. 
 Color, steel-gray ; soils paper. 
 
 Composition : Consists of Bi and Te, with sometimes S and 
 Se. General formula mostly Bi 2 (Te,!S) 3 = Te. 48.1, Bi. 51.9 
 (when free of S). . 
 
 The sulphurous variety contains some 5 per cent, of S, re- 
 placing Te. 
 
 In the open tube yields a white sublimate of tellurous acid, 
 which B. B. fuses to colorless drops. On coal fuses, gives 
 white fumes, and entirely volatilizes; tinges the R. F. bluish- 
 green ; coats the coal at first white (tellurous oxide), and finally 
 orange-yellow (bismuth oxide). Fused together with sulphur 
 and iodide of potassium, coats the coal red, like native Bi. 
 
 Bismutite ( Wismuthspath, Germ.). Color, white, or light 
 green ; streak, greenish-gray to colorless. Lustre, vitreous. 
 Brittle. H. 4. G. G.9. In acicular crystallizations (pseudo- 
 morphous), also incrusting or amorphous ; pulverulent. 
 
 Composition : Bi,C,lT[ 2 Carbon dioxide 6.08, bismuth 
 oxide 89.75, water 3.87 = KM). 
 
334 MINERALOGY SIMPLIFIED. 
 
 B. B. fuses readily, and on coal is reduced to Bi, and coats 
 the coal with yellow bismuth oxide. Fused with sulphur and 
 iodide of potassium, behaves like bismuth. Dissolves in HC1 
 with effervescence. The solution has a yellow color. 
 
 Bismuthinite (bismuth glance} Color and streak, lead- 
 gray, inclining to tin-white. H. 2. G. 6.4. In acicular crys- 
 tals, also massive. 
 
 Composition: Bi a S 3 = S. 18.75, Bi. 81.25. 
 
 In the open tube yields sulphurous fumes, and a white sub- 
 limate which B. B. fuses into drops, brown, while hot, and 
 opaque-yellow on cooling. On charcoal gives sulphurous fumes, 
 then fuses with spirting, and coats the coal yellow. When 
 fused with sulphur and iodide of potassium it behaves like Bi. 
 Dissolves in nitric acid, and water produces white precipitate. 
 
 Bismite (bismuth ochre). Composition : Bi 2 3 , contain- 
 ing sometimes traces of Fe 2 O s , CuO and As 2 5 . Occurs mas- 
 sive, earthy. G. 4.36. 
 
 B. B. it behaves like pure oxide of bismuth. Soluble in 
 HNO 3 . Addition of H 2 O causes a white precipitate. 
 
 Minerals containing bismuth : maldonite, josite, aikinite, chivia- 
 tite, emplectite, wittichonite, englytite, bismutoferrite, etc. 
 
 Ores of Chromiurrt. 
 
 CHHOMITE ( CHROMIC IRON) Color, iron-black ; streak, 
 dark-brown. Lustre, submetallic. II. 5.5. G. 4.3. Isometric. 
 In octahedral crystals or massive. In small fragments attracted 
 by the magnet. Possesses a less metallic lustre than other 
 black iron ores. 
 
 Composition : General formula, RK0 4 or Fer0 4 . Analysis 
 gives FeO. 32, Cr 2 O 3 . 68 = 100. Only slightly attacked by 
 HC1. B. B. infusible alone. Imparts a beautiful green color 
 to the beads of borax and salt of phosphorus when cold. The 
 powdered mineral, when fused with caustic potassa, forms 
 potassium chroma te. 
 
 The compounds of chromium, used extensively as pigments. 
 
ORES OP COBALT. 335 
 
 tire obtained mostly from this ore, for which reason it has been 
 described here. 
 
 Daubredite is a chromium sulphide found in some meteorites. 
 
 Minerals containing chromium : crocoite, melanochroite, vanque- 
 linite, walchonskoite, etc. 
 
 Ores of Cobalt. 
 
 Smaltite (smaltine, Speis-cobalt, Germ.) Color, tin-white. 
 Streak, grayish-black. Brittle. H. 5.5. G. 6.4. Isometric. 
 Occurs in octahedrons, cubes, dodecahedrons, and massive. 
 
 Composition : (CoN5)As 2 , the ore being either a cobalt 
 arsenide or cobalt-nickel arsenide, and graduating into nickel 
 arsenide, called chloanthite. The cobalt in the ore may consti- 
 tute 23.5 per cent., or it may be wholly absent in the chloan- 
 thite. 
 
 In the closed tube gives a sublimate of metallic arsenic ; in 
 the open tube a white sublimate of arsenous oxide, and some- 
 times traces of sulphurous acid. B. B. on charcoal affords a 
 garlic odor, fuses to a magnetic globule, which, with fluxes, gives 
 the indications of Fe, Co, and Ni. Gives with HNO 3 a pink 
 solution, As 2 O 3 being deposited. 
 
 Diff. : Has the white color of mispickel, but this latter yields 
 S and' As, and in a closed tube affords arsenic sulphide, orpi- 
 ment, and realgar. 
 
 Cobaltite (glance cobalt, Kobaltglanz, Germ.) Crystals like 
 those of pyrite, but silver-white in color with a tinge of red, 
 or inclined to steel-gray. Streak, gray-black. Brittle. H. 
 5.5. G. 6-6.3. Isometric. 
 
 Composition : CoS 2 -f CoAs 2 = CoAsS = As. 4.52 ; S. 19.3 ; 
 Co. 3 ).5 = 100. Contains often much iron and a little copper. 
 
 Unaltered in the closed tube, but in the open tube yields 
 sulphurous fumes and a white sublimate of arsenous oxide. 
 B. B. on coal, yields copious arsenical and sulphur fumes, and 
 fuses to a black metallic globule, which is magnetic ; with borax 
 a cobalt-blue globule. 
 
336 MINERALOGY SIMPLIFIED. 
 
 Linnaeite (cobalt pyrites, cobalt sulphide) Color, pale 
 steel-gray, tarnishing copper red. Streak, blackish-gray. II. 
 5.5.' G. 4.8-5. Isometric. 
 
 Composition : (Co,Ni) 8 S 4 = S. 42.0 ; Co. 58.0, but having 
 the Co partly replaced by Ni or Cu. 
 
 B. B. on coal yields sulphurous odor and a magnetic globule, 
 often also arsenical fumes. 
 
 Erythrite (cobalt bloom, hydrous cobalt arsenate) Color, 
 crimson or peach-red, having a cleavage like mica. Lustre of 
 laminae, pearly; earthy varieties without lustre. H. 1.5-2. 
 G. 2.9. Monoclinic. Valuable for the manufacture of smalt. 
 
 Composition : Co 3 O 8 As 2 -f 8Aq = arsenic acid, 38.4 ; oxide 
 of cobalt, 37.6 ; water, 24.0. 
 
 B. B. on coal gives arsenical fumes and fuses ; yields a blue 
 glass with borax (cobalt). 
 
 Acids dissolve it readily to a rose-colored liquid. The solu- 
 tion in concentrated HC1 appears blue while hot. 
 
 Asbolite (black cobalt oxide, earthy cobalt) is a variety 
 of " wad" (see Manganese Ores), containing cobalt oxide, 
 which sometimes amounts to 32 per cent. 
 
 Composition : MnO 2 ,CoO,CuO,H 2 O. 
 
 Color, black. Lustre, dull. H. 2-2.5. G. 3.1-3.3. 
 
 B. B. gives a blue bead with salt of phosphorus in 0. F. 
 (cobalt), and when heated in R. F. on coal with tin some 
 specimens yield a red, opaque, copper bead. With soda on 
 platinum gives a manganese reaction. Soluble in HC1 with 
 evolution of Cl ; the solution is usually blue, turning rose-red 
 on addition of water. 
 
 Minerals containing cobalt : carrollite, glaucodot, chathamite, 
 skutterudite, alloclasite, bieberite, roselite, etc. 
 
 Ores of Copper. 
 
 NATIVE COPPER Color, copper-red, contains often a little 
 silver disseminated throughout it. Ductile and malleable. 
 H. 2.5-3. G. 8.84. Isometric. 
 
ORES OF COPPER. 337 
 
 B. B. it fuses readily, and on cooling is covered with black 
 oxide. Dissolves in nitric acid, and produces a deep azure- 
 blue solution on the addition of ammonia. 
 
 Obs. : Native copper accompanies the ores of copper, and 
 usually occurs in the vicinity of dykes of igneous rocks. 
 
 Ghalcopyrite (copper pyrites). Color, brass-yellow, often 
 tarnished deep yellow and also iridescent. Streak, non-metal- 
 lic, greenish-black, and but little shining. H. 3.54. G. 4.15 
 4.3. Tetragonal. 
 
 Composition : (CuFe)S 2 = S, 34.tf ; Cu, 34.6 ; iron, 30.5 = 
 100. 
 
 B. B. fuses to a globule which is magnetic (Fe). Gives 
 sulphur fumes on coal. With soda on coal affords a globule of 
 metallic iron with copper. With fluxes the pulverized mineral 
 after roasting gives the reaction of copper and iron. Moistened 
 with HC1 it colors the flame blue, even previous to fusion. 
 Dissolves easily in aqua regia, less so in nitric acid. 
 
 Bornite (varieyated copper pyrites, erubescite). Color, 
 between copper-red and pinchbeck-brown. Tarnishes rapidly 
 on exposure. Streak, pale grayish-black, and but slightly 
 shining. Brittle. H. 3. G. 5. Isometric. 
 
 Composition : (Cu 2 Fe)S 3 = S, 28.6 ; Cu, 55.58 ; Fe, 16.36, 
 but varies much. 
 
 B. B on coal fuses to a brittle globule, attractable by the 
 magnet. Dissolves in nitric acid with separation. of sulphur. 
 
 Clialcocite (copper gliince). Third vitreous copper ore. 
 Color and streak, blackish lead-gray; often tarnished blue or 
 green ; streak sometimes shining. II. 2.53. G. 5.5. Ortho- 
 rhombic. 
 
 Composition : Cu 2 S = S, 20.2 ; copper, 79.8 = 100. 
 
 B. B. on coal gives off fumes of sulphur, fuses easily in the 
 exterior flame, and after the sulphur is driven off, a globule of 
 copper remains. Dissolves in nitric Moid, leaving a residue of 
 sulphur. 
 
 Tetrahedrite (gray copper, Fattier z). Color, between steel- 
 gray and iron-black ; streak, nearly like the color, sometimes 
 29 
 
338 MINERALOGY SIMPLIFIED. 
 
 inclined to brown and cherry-red. Rather brittle. Occurs in 
 tetrahedral forms. H. 3-4.5. G. 4.5-5. Isometric (hemi- 
 hedral). 
 
 Composition : Cu 8 S 7 Sb 2 (= 4Cu 2 S + Sb 8 S 3 ). Contains fre- 
 quently iron and zinc, and sometimes quicksilver. 
 
 B. B. the roasted mineral gives with soda on charcoal, after 
 long heating, a globule of copper. Heated in closed tube, fuses 
 and finally yields a dark-red sublimate of tersulphide of anti- 
 mony, with antimonious acid, and if an excess of soda be added, 
 a sublimate of mercury. The nitric acid solution gives no pre- 
 cipitate with hydrochloric acid, but usually the reaction of iron 
 and zinc. 
 
 Domeykite (arsenical copper) Color, tin-white to steel- 
 gray, with a yellow or iridescent tarnish. Lustre, metallic. 
 H. 3-3.5 G. 7-75. Reniform, massive, or disseminated. 
 
 Composition: Cu 3 As = As, 28.3; Cu, 71.7 = 100. 
 
 In an open tube fuses and gives a white crystalline sublimate 
 of arsenious oxide. B. B. on charcoal, arsenical fumes and a 
 malleable metallic globule, which on treatment with soda gives 
 a globule of pure copper. Not soluble in hydrochloric, but 
 soluble in nitric acid. 
 
 Atacamite (copper oxy chloride). Color, various shades of 
 bright-green, sometimes blackish-green ; streak, apple-green ; 
 translucent. Lustre, adamantine, vitreous. H. 3-3.5. G. 3.7. 
 Trimetric. 
 
 Composition: CuCl 2 -f 3H 2 CuO 2 = Cl, 16.64 ; Cu, 59.45; O, 
 11.25; water, 12.66 = 100. 
 
 In the closed tube gives off much water of an acid reaction, 
 and forms a gray sublimate. B. B. on coal fuses, coloring the 
 O. F. azure-blue, with a green edge, and giving two coatings, 
 one brownish and the other grayish-white ; continued blowing 
 yields a globule of metallic copper; the coatings touched with 
 the R. F. volatilize, coloring the flame azure-blue. In acids 
 easily soluble. 
 
 Cuprite (red copper ore, Rothkupfererz, Germ.) Color, 
 deep red, of various shades ; streak, brownish-red. Lustre, 
 adamantine or submetallic. Subtransparent ; brittle. H. 3.5-4. 
 
ORES OF COPPEK. 339 
 
 G. .5.8. Isometric. In regular octahedrons, and modified 
 forms of thii same ; also massive and earthy. 
 
 Composition : Cu a O = O, 11 .2 ; copper, 88.8 = 100. 
 
 B. B. on coal yields a globule of copper. In the forceps fuses 
 and colors the flame emerald-green ; if previously moistened 
 with HC1 the flame is momentarily azure-blue. With the 
 fluxes gives reactions for oxide of copper. Soluble in cone. HC1. 
 
 Malachite (yreen copper carbonate) Color, light green ; 
 streak, paler. Usually nearly opaque ; crystals, translucent. 
 H. 3.5-4. G. 3.7-4. Monoclinic. 
 
 Composition : Cu a O 4 C + H 2 O = CO 2 , 1 9.9 ; CuO, 71 .9 ; water, 
 8.2=: 100. Dissolves with effervescence in nitric acid (distinc- 
 tion from other green ores), also in ammonia. 
 
 B. B. Decrepitates and blackens, colors the flame green, and 
 becomes [tartly a black scoria. With borax it fuses to a deep- 
 green globule, and ultimately affords a bead of copper. 
 
 Azurite (blue malachite). Color, deep blue. Streak, bluish, 
 transparent to nearly opaque. Lustre, vitreous. H. 3.5-4. 
 G. 3.5-3.8. Monoclinic. 
 
 Composition : Cu 3 O 7 C 2 + H 2 O = CO,, 25.6; CuO, 69.2; 
 H 2 O, 5.2 = 100. 
 
 B. B. and in acids like the preceding. 
 
 Chalcanthite (copper vitriol, blue vitriol) Color, deep 
 
 sky-blue. Streak, colorless. Lustre, vitreous. Soluble in 
 water. Taste, nauseous and metallic. H. 2-2.5. G. 2.21. 
 Triclinic. 
 
 Composition: CuSO 4 + f>HO = SO s , 32.1 ; CuO, 31.8; II 2 O, 
 36.1 = 100. 
 
 B. 1>. on coal, colors the outer flame green, fuses, and affords 
 a globule of copper, crusted with a coat of sulphide. After 
 calcination, gives, with fluxes, the reactions of copper. A 
 piece of polished iron introduced into the solution becomes 
 coated with copper. 
 
 Olivenite (hydrous copper arsenate). Color, usually olive- 
 green. Streak, the same. Brittle. II. 3. G. 1.1-1.1. 
 Tri metric. 
 
310 MINE HA LOGY SIMPLIFIED. 
 
 Composition : Cn 4 O 9 As,= As,O B , 40.00; CuO, f)0.ir>; water, 
 3.19 = 100. Fuses easily, coloring the flame bluish-green. 
 B. B.j fuses with deflagration, giving off arsenical fumes, and 
 affords a little globule, which, with soda, yield metallic copper. 
 Dissolves in nitric acid, also in ammonia. 
 
 Tyrolite (copper froth) Color, verdigris-green or pale 
 
 apple-green. 
 
 Composition : Cu 5 As 2 O 10 -f- 11 Aq, 45.2 per cent, of copper. 
 A hydratecl arsenate of copper, containing also calcium car- 
 bonate (as an impurity ?) H. 1-2. G. 3. Tri clinic. 
 
 B. B. on coal, heated with soda and borax until the copper 
 oxide is completely reduced, and the slag dissolved in HC1, 
 a solution is obtained which shows the presence of lime. Dis- 
 solves in nitric acid with effervescence ; also in ammonia, with 
 a blue color. 
 
 Chrysocolla (hydrous copper silicate). Usually as incrusta- 
 tions. Also in thin seams and stains. Color, bright green, 
 resembling malachite. H. 2-4. G. 2-2.4. Usually as an 
 incrustation. 
 
 Composition : Cu0 3 Si + 2Aq. = SiO 2 , 34.2 ; CuO, 45.3 ; 
 H 2 O, 20.5 = 100. 
 
 B. B. it blackens in the R. F., and yields water without 
 melting. With soda on coal yields a globule of copper. 
 Heated in a glass tube, yields water and blackens. In the for- 
 ceps, infusible, coloring the O. F. intensely green. Borax 
 and salts of phosphorus dissolve in it with the usual reactions 
 of copper. It is decomposed by acids, silica remaining behind 
 (distinction from malachite, which is completely soluble with 
 effervescence in nitric acid). 
 
 General remarks. The most valuable sources of copper for 
 the arts are : native copper, chalcopyrite, or " yellow copper 
 ore," chalcocite, or " copper (/lance," bornite, or u variegated 
 copper ore," malachite, or " green carbonate of copper," 
 cJirysocolla, or " silicate," cuprite, or " red oxide of copper," 
 and occasionally, melaconite, or " black copper." 
 
 Minerals containing copper: Dioptase, algodonite, wliitneyite, en- 
 argite, tenorite (melaconite). 
 
ORES OF GOLD, PLATINUM, ETC. 341 
 
 Ores of Gold, Platinum, Iridium, and Palladium. 
 
 NATIVE GOLD. Color and streak, various shades of gold- 
 yellow, becoming pale from alloy with silver; occasionally 
 almost silver-white from the silver present. Easily distin- 
 guished by its malleability, its cutting like lead, its high speci- 
 fic gravity, and its resistance to acid. H. 2.5-3. G. 12-20, 
 varying according to the metals alloyed with the gold. Fuses 
 at 2016 F. (1102 C.). Isometric. 
 
 Composition : Native gold usually contains silver in various 
 proportions. The finest native gold from Russia yielded gold 
 9<S. 90, silver, 0.16, copper, 0.3;), iron, 05. G. 19.0!)9. 
 
 The following proportions of gold and silver have been ob- 
 served in other varieties : 
 
 Gold. Silver. 
 
 3 to 2 
 3J " 2 
 
 5 " 2 
 
 4 " 1 (most common). 
 
 6 " 1 (also frequent). 
 
 Average of California native gold is 88 per cent, gold, and 
 the range mostly between 87 and 89 ; the range of the Cana- 
 dian, mostly between 87 and 89 ; the range of the Australian, 
 between 90 and 9G per cent. The Chilian gold affords 84 to 
 90 per cent, of gold, and 15-3 per cent, of silver. The more 
 argentiferous gold has been called electrum. 
 
 Gold resists the action of heated concentrated nitric acid, 
 and is soluble only in aqua rcyia. 
 
 Copper is occasionally found in alloy with gold, and some- 
 times also iron, bismuth, palladium, and rhodium. A rho- 
 dium gold from Mexico, gave the spec, gravity lf>.f>-10.S, and 
 contained 34-43 per cent, of rhodium. A bismuth gold has 
 been called maldonite. 
 
 Calaverite is a bronze-yellow gold telluride, AuTe 4 = Te 55.5, 
 Au 1 1.5 = 100, with a little silver, occurriiiir massive at the 
 
 29* 
 
MINEIJAUHIY SIMPLIFIED. 
 
 Stanislaus mine, California, and the Red Cloud mine, Colo- 
 rado, and also the Keystone and Mountain Lion mines, in the 
 Magnolia district. 
 
 Krennerite is another gold telluride. 
 
 Sylvan-ite, or graphic tellurium. A telluride of gold and 
 silver (Ag,Au)Te 3 (if Ag : Au ==1:1) Te, 55.8 ; Au, 28.5 ; 
 Ag, 15.7=100. Color and streak, steel-gray to silver-white, 
 and sometimes nearly brass-yellow. H. 1.5-2. G. 7.99-8.33. 
 Monoclinic. Called graphic because of a resemblance in the 
 arrangement of the crystals to written characters. Found in 
 California and Colorado.* In an open glass tube yields a white 
 sublimate, which, when played upon by the flame, fuses to 
 transparent drops. On coal fuses to a dark-gray globule, de- 
 positing at the same time a white coating, which in the R. F. 
 disappears, tinging the flame bluish-green. Soluble in aqua 
 regia, leaving a residue of chloride of silver. The solution 
 gives a white precipitate with water. 
 
 Nagyagite, or foliated tellurium, is a telluride of lead contain- 
 ing 9 to 13 per cent, of gold. (See Lead Ores.) 
 
 Petzite is a telluride of silver containing gold ; a specimen 
 from Golden Rule Mine, Colorado, contained, according to 
 Genth, 25.60 per cent. (See Silver Ores.) 
 
 NATIVE PLATINUM (Ft) Color and streak, pale or dark 
 steel-gray. Lustre, metallic, shining like silver. Ductile and 
 malleable. H. 4-4.5. G. 16-19. Isometric. Often slightly 
 magnetic, and some masses will take up iron filings. Usually 
 in flattened or angular grains or irregular masses. 
 
 Composition : Flatinum is generally combined with more or 
 less of the rare metals iridium, rhodium, palladium, and 
 osmium besides copper and iron, jyhich give it a darker color 
 than belongs to the pure metal. A Russian specimen afforded 
 Pt, 78.9; Ir, 5.0; Os and Ir, 1.9; Rh, 0.9; Pel, 0.3; Cu, 
 0.7; Fe. 11.0 = 98.75. 
 
 * Consult James D. Dana's Manual of Mineralogy and Lithology, 
 3d ed. New York, 18S1, p. 10!). 
 
OIJKS OK IROX. 343 
 
 It is one of the most infusible substances known. It is 
 wholly unaltered before the blowpipe or by fluxes. Soluble only 
 in heated aqua regia. The solution gives a yellow granular 
 precipitate with chloride of potassium. Platinum fuses readily 
 before the oxy-hydrogen blowpipe; 
 
 Platin-irldinm Grains of iridium have been found in 
 Russia, consisting of 76.8 iridium, and 19.64 platinum, with 
 some palladium and copper. A specimen from Brazil con- 
 tained 27.8 iridium, 55.5 Pt, and 6.9 Rh. 
 
 Osmium (iridium, iridosrnine}, A compound of Ir and Os 
 from the platinum mines of Russia, South America, the East 
 Indies, and California. The crystals are pale steel-gray hexa- 
 gonal prisms, usually found in flat grains. II. 6.7. G. 19.5- 
 21. Hexagonal. Slightly malleable. 
 
 Composition variable. One variety, called newjanskite, 
 contains Ir, 46.8; Os, 49.3; Rh, 3.2; Fe, 0.7. Another, 
 sisserskite^ Ir, 25.1 ; Os, 74.9. The grains are distinguished 
 from those of platinum by their superior hardness. Iridosmine 
 is common in the gold of Northern California, and injures 
 its quality for jewelry. 
 
 B. B. infusible. When heated with nitre in a glass tube the 
 characteristic osmium odor is produced. The fused mass is 
 soluble in water; the solution gives, on addition of nitric acid, 
 a green precipitate. Not visibly affected by any acid. 
 
 Palladium Color, steel-gray, inclining to silver-white. 
 
 Ductile and malleable. H. 4.5-5. G. lT.3-12.2. Isometric. 
 
 Consists of Pd with some Pt and Ir. 
 
 Fuses with sulphur, but not alone. In hardness it is equal 
 to fine steel. 
 
 Selenpalladite or allopalladium is native pa'.ladium in hexa- 
 gonal tables from the Hartz Mountains. 
 
 Torpezite is gold containing about 10 per cent, of palladium. 
 
 Ores of Iron. 
 
 Iron occurs native, and alloyed with variable quantities of 
 nickel in meteoric iron. Its ores arc very widely disseminated. 
 
344 MINERALOGY SIMPLIFIED. 
 
 The iron carbonate is one of the most abundant and valuable 
 ores. The spec. grav. of the ordinary workable ores seldom 
 exceeds o. They are of difficult fusibility before the blowpipe, 
 and nearly all minerals containing iron are attracted by the 
 magnet, either before or after heating. 
 
 NATIVE IRON. Color and streak, iron-gray. Fracture, 
 hackly. Malleable and ductile. H. 4.5. G. 7.3-7.8. Acts 
 strongly on the magnet. It occurs usually massive, dissemi- 
 nated in igneous rocks in grains, or is found in very large 
 masses weighing over a tori (meteoric). 
 
 MKTEORIC IRON. It contains from 1 to 20 per cent, of 
 nickel, with traces of Co, Cu, Mn, Sn, Cr, P, S, Cl, C. 
 
 Color, iron-gray. Lustre, metallic. It possesses often a 
 very broad crystalline structure, long lines and triangular 
 figures being developed by putting nitric acid on a polished 
 surface. Nodules of troilite (FeS) and schreibersite (FeP) 
 are common constituents of iron meteorites. Meteoric iron 
 may be worked like ordinary malleable iron. The nickel 
 diminishes the tendency to rust. 
 
 To detect the presence of the other heavy metals, the assay- 
 piece must be dissolved in aqua regia, the liquid mixed with 
 an excess of ammonia, filtered, and the ammoniacal filtrate 
 precipitated with sulphide of ammonium (NH 4 ) a S. The pre- 
 cipitate consists of sulphides of nickel, cobalt, manganese, and 
 copper, which may be collected on a filter, and treated with 
 borax on coal in the reduction flame until all volatile substances 
 are expelled, the remaining mass powdered in an agate mortar, 
 the powder well calcined, and the calcined mass treated with 
 borax on coal in the O. F. If Co is the only coloring metal 
 present, the bead will exhibit a pure blue color, a small quan- 
 tity of iron will make the glass appear green while hot, but 
 blue when cold. Cu and Ni, when present to some extent, 
 will interfere with the blue cobalt color. The bead in this 
 case exposed to the R. F. until it appears transparent, and 
 flows quietly. The oxides of copper and nickel are by this 
 
OHKS OF IKON. M I.") 
 
 menus reduced, and the pure color of cobalt or that of cobalt 
 mixed with iron becomes distinct. 
 
 Limonite (brown hematite) Color, dark brown and black 
 to ochre-yellow ; streak, yellowish-brown to dull yellow. Lus- 
 tre, sometimes submetallic, often dull and earthy. H. 5-5.5. 
 G. 3.6-4. Usually massive and often in mammillary or sta- 
 lactitic forms. 
 
 The following are the principal varieties : 
 
 Brown lematite The botryoidal, stalactitic, and associated 
 compact forms. 
 
 Brown ochre, yellow ochre Earthy ochreous varieties of 
 
 a brown or yellow color. 
 
 Brown and yellow clay ironstone Impure ore, hard and 
 
 compact, of a brown or yellow color. 
 
 P.og iron ore A loose, earthy ore of a brownish-black 
 color, occuring in low grounds. 
 
 Composition : *WI 6 ( == 2Pe0 3 -f 2H 2 0) = Fe 2 3 . 85.6, H 2 14.4 
 = 100 ; or it is a hydrous iron sesqiiioxide, containing, when 
 pure, about two-thirds its weight of pure iron. 
 
 "B. B. blackens and becomes magnetic ; with borax in the 
 outer flame, a yellow glass. In a matrass yields water, and 
 red scsquioxide remains ; the clayey varieties treated with salt 
 of phosphorus gives a cloud of undissolved SiO 2 ; treated with 
 soda and nitre on platinum-foil, the manganese reaction is 
 almost always obtained. 
 
 Bog ores usually obtain much P, from organic sources. 
 
 Gothite (pyrosiderite, Lepidokrokit), is another iron hy- 
 drate, often in prismatic crystals, as well as fibrous and mas- 
 sive, of the formula Fe0 4 H. 2 (= Fe0 3 + H 2 0), and G. 4:0-4.4. Or- 
 thorhombic. 
 
 Turgite has the formula, *V/) 7 II 2 = 2Fe0 3 -f H 2 0. H. 5-6. G. 
 3.5-4. Xanthosiderite and limnite are other related hydrates. 
 
 Hematite (ipecHlat iron, iron sesqui oxide) Color, dark, 
 steel-gray or iron-black, and often when crystallixiul having a 
 highly splendent lustre (from Elba, St. ( Jothard, etc.) ; streak, 
 powder cherry-red to brown. II. 5.5-0.5 (of crystals) G. 
 
840 MINERALOGY SIMPLIFIED. 
 
 4.5-5.3. Hexagonal varieties : Crystallizes in complex modi- 
 fications of a rhombohedron ; also, massive, granular, or mica- 
 ceous. 
 
 Specular iron. Having a perfectly metallic lustre. 
 
 Micaceous iron Structure foliated. 
 
 Red hematite. Submetallic, or non-metallic, and of a 
 brownish-red color. 
 
 Red ochre Soft and earthy, and often containing clay. 
 
 Red chalk More firm and compact than red ochre, and of 
 a fine texture. 
 
 Jaspery clay-iron. A hard, impure, silicious clayey ore, 
 having a brownish-red, jaspery look and compactness. 
 
 Clay ironstone The same as the last ; the color and ap- 
 pearance less like jasper. But this is one variety only of what 
 is called clay iron, " clay ironstone,'/ a name including also a 
 related variety of siderite and limonite. 
 
 Lenticular argillaceous ore A red ore, consisting of small, 
 flattened grains. 
 
 Martite is a hematite in octahedrons, derived, it is supposed, 
 from the oxidation of magnetite. 
 
 Composition : Fe0 3 = 0, 30 ; Fe, 70 = 100. 
 
 B. B. Infusible alone. Heated in the inner flame it be- 
 comes strongly magnetic, and gives the usual indications of 
 iron with the fluxes. It dissolves in HC1. Contains some- 
 times chromium and titanium. 
 
 Diff. The red streak and the magnetism produced in the 
 R. F. distinguish hematite (blood-stone) from all other ores. 
 
 Magnetite (magnetic iron ore). Color, iron-black ; streak, 
 black. Brittle. H. 5.5-6.5. G. 5.0-5.1. Isometric. Strongly 
 attracted by the magnet, and sometimes showing polarity. 
 Often in octahedrons and dodecahedrons, also granularly mas- 
 sive. 
 
 Composition : Fee0 4 = FeO -f Fe0 3 = 0, 27.6 ; Fe, 72.4 = 100. 
 
 B. B. infusible, and gives the usual reactions of iron with 
 the fluxes, e. g., with borax in the outer flame, a yellow glass. 
 
 DifF. The black streak and strong magnetism distinguish it 
 
ORES OF IKON. 347 
 
 from other species. It constitutes what are called loadstones, 
 or native magnets. 
 
 Pyrite (iron pyrites, iron bisulphide). Color, bronze-yel- 
 low ; streak, brownish-black. Lustre of crystals often splen- 
 dent metallic. Brittle. H. 6-G.5. G. 4-8.5, being hard 
 enough to strike fire with steel. G. 4.8-5.1. Isometric. 
 Usually in cubes, the strice of one face at right angles with 
 those of the adjoining faces. 
 
 Composition : FeS 2 = S, 53.3 ; Fe, 46.7 -f 100. Pyrite often 
 contains a minute quantity of gold. 
 
 B. B. on charcoal gives off sulphur, and ultimately affords a 
 globule attractable by the magnet. 
 
 Heated in a closed tube, it usually evolves SH 2 , and yields a 
 sublimate of S ; the residue is attracted by the magnet. But 
 slightly affected by HC1 ; HNO 3 dissolves it, leaving a residue 
 of S. 
 
 Marcasite (white iron pyrites') Color, usually light bronze- 
 yellow, sometimes inclined to green or gray. H. 6-6.5. G. 
 4.6-4.85. Trimetric. Occurs frequently in radiated masses. 
 Very liable to decomposition. 
 
 Composition, FeS 3 . 
 
 B. B. like the preceding. 
 
 Pyrrhotite (magnetic pyrites, iron sulphide). Color, be- 
 tween bronze-yellow and copper-red ; streak, dark grayish- 
 black. Brittle. H. 3.5-4.5. G. 4.4-4.65. Hexagonal. 
 slightly attracted by the magnet. 
 
 Composition : Fe ? S 8 = S, 39.5 ; Fe, 00.5. Contains sometimes 
 from 3 to 5 per cent, of nickel. 
 
 B. B. on charcoal in the O. F. converted into red oxide of 
 iron. In the R. F. it fuses and glows, and yields a black glo- 
 bule which is magnetic, and has a yellow color on a surface of 
 fracture. 
 
 Heated in a matrass, it remains unchanged; in the open 
 tube, evolves SO a , but yields no sublimate. 
 
 Soluble in IIC1, exceping the S, with evolution of IT 2 S. . 
 
 Ditf. From common iron pyrites, which it n.-si-mbh:s, it is 
 
348 - MINERALOGY SIMPLIFIED. 
 
 distinguished by its inferior hardness and its magnetic quality; 
 and from chalcopyrite or copper pyrites, by its paleness of 
 color. 
 
 Arsenopyrite (.mispickety Color, silver-white. Streak, 
 
 dark grayish-black. Lustre, shining. Brittle. H. 5.5-6. G. 
 6.3. Trimetric. Occurs in rhombic prisms and also massive. 
 
 Composition: FeAsS = As, 46.0 ; S, 19.6 ; Fe, 34.4 = 100. 
 
 Danaite, a cobaltic variety found in New Hampshire, con- 
 sists of As, 41.4 ; S, 17.8 ; Fe, 32.9 ; Co, 6.5. 
 
 B. B. affords fumes of As and a globule of iron sulphide, 
 which is attracted by the magnet. 
 
 Heated in a matrass, yields first a red sublimate of arsenic 
 sulphide, and afterwards a black crystalline one of metallic As. 
 Gives fire with a steel and emits a garlic odor. 
 
 Soluble in HNO 3 and aqua regia, leaving a residue of S, and 
 As 2 O 6 , which dissolve by continued digestion. 
 
 Diff. Resembles arsenical cobalt, but is much harder and 
 yields a magnetic globule, and does not afford the cobalt reac- 
 tion with fluxes. 
 
 Scorodite. Color, pale leek-green or liver-brown. Streak, 
 uncolored. Lustre, vitreous. H. 3.5-4. G. 3.1-3.3. Tri- 
 metric. Crystallizes in rhombic prisms. 
 
 Composition : PeAs,0 8 -f- 4Aq. A hydrous arsenate of iron, 
 containing As 2 O., 49.8 ; Fe a O 8 , 34.6 ; H 2 0, 15.6 = 100. 
 
 B. B. fuses easily, coloring the flaiie blue, P 2 O 5 . On char- 
 coal gives arsenical fumes, and with soda a black magnetic 
 scoria. With the fluxes reacts for iron. 
 
 In a matrass, yields pure water and turns yellow. 
 
 Not affected by HNO 3 ; forms a brown solution with HC1. 
 
 Iron sinter is an amorphous form of the same mineral. 
 
 Menaccanite (titaniferoas iron, ilmenite, titanic iron, wash- 
 ingtonite) Color, iron-black. Streak, submetallic. Lustre, 
 metallic or submetallic. H. 5.6. G. 4.5-5. Hexagonal. Acts 
 slightly on the magnetic -needle. 
 
 Composition: (Ti,Fe) 2 O 3 , or Ti0 3 and Fe a O 3 in variable 
 
ORES OF IRON. 349 
 
 proportions. It is a hematite, in which a part of the iron is 
 replaced by Ti. 
 
 B. B. alone infusible. With borax and salt of phosphorus in 
 O. F., gives the reactions of pure oxide of iron ; but the salt, of 
 phosphorus bead, when treated with the R. F., assumes a 
 brownish-red color, the intensity of which depends upon the 
 amount of TiO 3 present ; this glass, when treated with tin on 
 charcoal, turns violet. 
 
 Diff. It resembles specular iron, but gives no red powder. 
 
 It is of no value in the arts, and forms a deleterious consti- 
 tuent of many iron ores. 
 
 Siderite (spathic iron, iron carbonate) Color, light-gray- 
 ish to brown ; often dark brownish-red ; crystallizes in rhom- 
 bohedrons with distinct cleavage. Usually massive. H. 3-4.5. 
 G. 3.7-3.9. Hexagonal. Streak, uncolored. 
 
 Composition: FeO 3 C = C0 2 , 37.9 ; FeO, 62.1=100. Con- 
 tains frequently some manganese oxide or magnesia, and lime 
 replacing part of the iron protoxide. 
 
 B. B. it blackens and becomes magnetic ; but alone it is 
 infusible. With borax and salt of phosphorus it gives the 
 pure iron reactions, and with soda and a little nitre sometimes 
 the green manganese reaction. It dissolves in heated HC1 
 with effervescence. 
 
 Diff. This mineral, called spathic iron, because it has the 
 aspect of a spar, cleaves like calcite and dolomite, but it has a 
 much higher spec, gravity. Heated in a close glass tube, it 
 gives off CO 2 and becomes magnetic, which distinguishes it 
 from other iron ores. 
 
 Melanterite (copperas, green vitriol] Color, greenish to 
 white. Lustre, vitreous. Taste, astringent and metallic. Be- 
 comes yellowish (oxidizes) when exposed to the air. H. 2. 
 G. 1.83. Monoclinic. 
 
 Composition : FeO 4 S -f 7Aq = SO 3 , 28.8 ; FeO, 25.9, 11,0 
 45.2 = 100. 
 
 U. B. becomes magnetic, yields glass with borax. 
 30 
 
350 MINERALOGY SIMPLIFIED. 
 
 In a matrass gives off SO 2 and H 2 O, which shows acid reac- 
 tion. Strongly heated, only Fe 2 O 3 remains. Soluble in water. 
 
 Vivianite {hydrous iron phosphate) Color, deep blue to 
 green. Streak, bluish. Lustre, pearly. H. 1.5-2. G. 
 2.66. Monoclinic. Crystallized, or in reniform and globular 
 masses. 
 
 Composition: Fe 3 O 8 P 2 + 8Aq = P 2 O 5 , 28.3; FeO, 43.0; 
 H 2 O, 28.7 = 100. 
 
 B. B. fuses easily to a magnetic globule, coloring the outer 
 flame greenish-blue (P 2 O 5 ). In the forceps the coloring becomes 
 very perceptible. In a matrass, swells and gives pure water. 
 Easily soluble in HC1 and HN0 3 . A solution of HKO 
 blackens it. 
 
 Franklinite Color, iron-black. Streak, dark reddish- 
 brown. Brittle. H. 5.5-6.5. G. 4'.85-5.1. Isometric. Usu- 
 ally attracted by the magnet. In octahedral and dodeeahedral 
 crystals. Also coarse, granular, massive. 
 
 Composition : General formula like that of magnetite, R B0 4 , 
 but having zinc and manganese replacing part of the iron, as 
 indicated in the formula (Fe,Zn,Mn) (3?e,Mn)0 4 . A common 
 variety corresponds to Fe 2 O 3 , 67.6 ; FeO, 5.8 ; ZnO, 6.9 ; MnO, 
 9.7 = 100. 
 
 B. B. with soda on charcoal, a zinc coating is obtained. A 
 soda bead in^the outer flame is colored green by manganese. 
 The addition of a little saltpetre and soda to the powdered min- 
 eral, and heating the mixture on platinum foil over a Bunsen 
 burner, facilitates the production of a green mass. Soluble in 
 HC1, with evolution of a little chlorine. 
 
 Diff. Resembles magnetic iron, but is of a more decided 
 black color, and the streak is a reddish-brown. Found abun- 
 dantly in New Jersey. 
 
 Ores of Lead. 
 
 NATIVE LEAD A rare mineral, occurring in thin lamina? 
 or globules. G. 11.35. 
 
 Galenite (galena, lead sulphide). Color and streak, lead- 
 
ORES OF LEAD. 3 5 1 
 
 graj . Lustre, shining metallic. Fragile. II. '2. it. G. 7.V5-7.7. 
 Isometric. Cleavage, cubic, and easily obtained. 
 
 Composition : PbS = S, 13.4; Pb, 86.6 = 100. Often con- 
 tains some silver sulphide, and at times zinc sulphide. 
 
 B. B. on charcoal, it decrepitates, unless heated with cau- 
 tion, and fuses, giving off sulphur, coats the coal yellow, and 
 finally yields a globule of lead. It dissolves with difficulty in 
 boiling HC1 with evolution of H 2 S. . Concentrated HNO 3 dis- 
 solves it with evolution of red nitrous acid vapor. 
 
 Biff. Galena resembles some silver and copper ores in color, 
 but its cubical cleavage, or granular structure when massive, 
 will distinguish it. Its reactions B. B. show it to be a lead 
 ore, and a sulphide. 
 
 The lead of commerce is obtained from this ore. It is also 
 employed in glazing common stoneware. 
 
 Ilournonite (R'ddelerz, Germ., wheel ore). Color and streak*, 
 steel-gray. Lustre, metallic. Brittle. H. 2.5-3. G. 5.7-0.1). 
 Trimetric. Occurs crystallized and massive, granular, compact. 
 
 Composition : Variable, CuPbSbS 3 . Ramrnelsb. (or 3RS -j- 
 Sb 8 S 3 , with'SRS. = 2PbS4-Cu a S) = S, 19.6; Sb, 25.0; Pb, 
 42.4; Cu, 13.0= 100. 
 
 In the closed tube decrepitates, and gives a dark-red subli- 
 mate. In the open tube, gives sulphurous acid, and a white 
 sublimate of antimonous oxide. B. B. on charcoal fuses easily, 
 and at first coats the coal white, from antimonious oxide ; con- 
 tinued blowing gives a yellow coating of lead oxide ; the resi- 
 due, treated with soda in R. F., gives a globule of copper. 
 
 Decomposed by nitric acid, affording a blue solution, and 
 leaving a residue of sulphur, and a white powder, containing 
 antimony and lead. 
 
 The following antimonial and arsenical sulphides of lead 
 behave B. B. in a similar' manner. 
 
 These ores include : surtorite, zinkenite, p1nyionite, janu'- 
 stmiti'i dtifrenoysite, bon,/itnf/crifi\ ko/ic/fifc, nn'n.cf//iiin'fc^ </<- 
 rro/t/fc; also, hnujniiirditc^ and freteslebeuifi 1 , in which silvrr 
 
352 MINERALOGY SIMPLIFIED. 
 
 is present, and stylolypite .and ct\kemite 9 in which copper is 
 present. 
 
 Those minerals in which a part of the SbS 3 is substituted by 
 As$ 3 , afford on charcoal arsenical vapors, and in the open 
 tube a crystalline sublimate. 
 
 Cerussite (white lead ore, lead carbonate) Color, white, 
 yellow, or gray. Lustre, adamantine. H. 3-3.5. G. 6.46- 
 6.48. Trimetric. Occurs in modified right rhombic prisms ; 
 also massive, rarely fibrous. 
 
 Composition ; PbO 3 C = CO 2 , 16.5 ; PbO, 83.5 = 100. 
 
 B. B. decrepitates, fuses, and, by careful blowing, affords on 
 charcoal a globule of lead. Treated with fluxes, dissolves with 
 effervescence, and gives the reactions of pure lead oxide. Dis- 
 solves readily with effervescence in dilute HNO 3 ; with HC1 
 leaves a white residue of lead chloride ; dissolves in a solution 
 of KHO. Associated usually with galena. 
 
 Anglesite (lead sulphate). Color, white, or slightly gray 
 or green. Lustre, adamantine. H. 2.75-3. G. 6.1-6.4. Tri- 
 metric. Occurs in rhombic prisms, and other forms ; often in 
 laminar masses. 
 
 Composition : PbSO 4 , affording about 73 per cent, of oxide 
 of lead. 
 
 B. B. fuses in the flame of a candle, and on coal yields lead 
 with soda. The soda is absorbed by the coal, and shows on 
 silver-foil, or a coin, a strony sulphur reaction. With great 
 difficulty dissolved by acids. The powdered mineral is soluble 
 in caustic potassa solution. 
 
 Minium (oxide of lead, Mennige, Germ.). Pulverulent. 
 Color, bright red tinged with yellow. G. 4.6. 
 
 Composition-: Pb 3 O 4 PbO 2 -|- 2PbO. Usually associated with 
 galena. 
 
 B. B. affords globules of lead in R. F. With HC1 evolves 
 chlorine, and is converted into lead chloride. 
 
 Massicot (plumbic ochre, Bleiglatte, Germ.) Color, yellow. 
 
 Composed of lead protoxide, PbO; but generally impure. 
 
 B. B. behaves like oxide of lead. 
 
ORES OF LEAD. ;}."i;i 
 
 Phunbogummite (fileigtrmmi), Contains Al 8 O s ,Pb,H 2 O, 
 P 2 O 5 , in globular forms, having a lustre like gum arabic, and a 
 yellowish or reddish-brown color. H. 4-4.5. G. 6.3-6.4. 
 
 Crocoite (crocoisite, lead ckromate, Rothbleierz, Germ.) 
 
 Color, bright red; streak, orange-yellow. H. 2.5-3. G. 5.9-61. 
 Monoclinic. Occurs in oblique rhombic prisms and massive. 
 
 Composition : PbO 4 Cr= CrO,, 31.1 ; PbO, 68.9 = 100. 
 
 B. B. fuses at 1.5, and on coal is reduced to metallic lead 
 with deflagration, leaving a residue of chromic oxide, and giv- 
 ing a lead coating. With salt of phosphorus gives an emerald- 
 green bead in both flames. Heated in a matrass, decrepitates, 
 blackens, but recovers its original color on cooling. Fused 
 with potassium bisulphate in the platinum spoon, forms a dark 
 violet mass, which on solidifying becomes reddish, and when 
 cold, greenish-white, thus differing from vanadanite, which on 
 similar treatment gives a yellow mass. (Plattner.) 
 
 VAUQUELINITE. A lead and copper chromate, of a very dark green 
 or pearly-black color, occurring usually in minute, irregularly aggre- 
 gated crystals; also, reniform and massive. H. 2.5-3. G. 5.5-5.8. 
 Monoclinic. 
 
 Composition : Pb 2 CuO 2 9 . The formula requires : Cr0 3 , 27.6 ; PbO, 
 61.5; CuO, 10.9=100. 
 
 B. B. on coal slightly iiituinesces, and fuses to a gray submetallic 
 globule, yielding at the same time small globules of metal. With 
 borax or salt of phosphorus affords a green transparent glass in the 
 outer flame, which in the inner, after cooling, is red to black, accord- 
 ing to the amount of mineral in the assay ; the red color is more dis- 
 tinct with tin. Partly soluble in HN0 3 to a dark green liquid; the 
 residue is yellow. 
 
 Slolzite or lead tungstate. In square octahedrons or prisms. Color, 
 given, gray, brown, or red. Lustre, resinous. H. 2.5-3. G. 7.9-8. ]. 
 
 Composition : PbW0 4 = W0 3 , 51 ; PbO, 49 = 100. 
 
 \Viilfanite (lead molyhdate, Gelbbleierz, Germ.) In dull yellow 
 octahedral crystals, and also massive. Lustre, resinous or adaman- 
 tine. H. 2.75-3. G. 6.03-7.01. Dimetric; brittle. 
 
 Composition : PbM0 4 = M0 3 , 38.5 ; PbO, 61.5 = 100. Some varieties 
 contain chromium. 
 
 B. B. decrepitates and fuses below 2 ; with borax in 0. F. gives a 
 colorless glass, in R. F. it becomes opaque. Mack, or dirty green, with 
 
 30* 
 
354 MINERALOGY SIMPLIFIED. 
 
 black flakes. With salt of phosphorus in 0. F. gives a yellowish- 
 green glass, which in R. F. becomes dark green. With soda on char- 
 coal yields metallic lead. Decomposed on evaporation with HC1, with 
 the formation of PbCl and Mo0 3 ; on moistening the residue with 
 water, and adding metallic zinc, it gives an intense blue color, which 
 does not fade on dilution of the liquid. 
 
 'Lanarkite, PbSO 4 -f PbO. The formula requires PbSO 4 , 
 
 57.6; PbO, 42.4 = 100. H. 2-2.5. G. 6.3 Color, pale 
 
 yellow. Monoclinic. 
 
 LeadhiWte, PbS0 4 -f 3PbCO 3 = PbSO 4 , 27.45; PbC0 3 , 
 72. 55 = 100. Recent analyses show the presence of some 
 water. H. 2.5. G. 6.26-6.44. Orthorhombic. Lustre, pearly. 
 Color, white, passing into yellow, green, or gray. Streak, 
 uncolored. 
 
 B. B. intumesces, fuses at 1.5. and turns yellow, but white 
 on cooling. Easily reduced on charcoal. With soda affords 
 the reaction for sulphuric acid. Dissolves in HNO 3 with 
 effervescence, leaving a white residue of lead sulphate. 
 
 Fhosgemte, or corneous lead. PbC0 3 -f PbCl 2 73.8, Pb. 
 H. 2.75-4. G. 6-6.31. Dimetric. Occurring in whitish 
 adamantine crystals. Streak, white. 
 
 B. B. fuses readily, emits acid vapors, becomes reduced to 
 metallic lead, and gives a white coating of PbCl 2 , and a yellow 
 one of Pb0 2 . With salt of phosphorus and copper oxide gives 
 the chlorine reaction. 
 
 Soluble in HNO 3 with effervescence. 
 
 Pyromorphite (lead phosphate] Color, bright green to 
 
 brown ; sometimes fine orange-yellow, owing to an intermixture 
 with chromate of lead. Streak, white, or nearly so. Lustre, 
 resinous. Nearly transparent. Brittle. H. 3.5-4. G. 6.5-7.1. 
 Hexagonal. In hexagonal prisms, also in globular masses. 
 
 Composition: Analogous to apatite, Pb s O 8 P a -f- ^PbCl 2 = 
 PO 5 , 15.71 ; PbO, 82.27 ; Cl, 2.62 = 100.60. Some varieties 
 contain As, replacing part of the P, and others, calcium replac- 
 ing the lead. 
 
 B. B. in the forceps fuses easily at 1.5, coloring the flarne 
 
ORES OF MANGANESE. 3>5 
 
 bluish-green ; on charcoal fuses without reduction to a globule, 
 which on cooling assumes a crystalline polyhedral form, while 
 the coal is coated white from the chloride, and nearer to the 
 assay, yellow from lead oxide. With soda on coal yields me- 
 tallic lead ; some varieties contain As and give, on charcoal, 
 in the R. F. the odor of garlic. With salt of phosphorus, 
 previously saturated with CuO, gives an azure-blue color to 
 the flame when treated in O. F. (chlorine). In a closed tube 
 gives a white sublimate of PbCl 2 . 
 
 Soluble in HNO 3 and a solution of KHO. 
 
 Minerals containing lead : clausthalite, mendipite, caledo- 
 riite, mimetite, vanadinite, melanochroite, stolzite, etc. 
 
 Ores of Manganese. 
 
 Pyrolusite (black oxide of manganese, manganese dioxide). 
 Color, iron-black. Streak, black, non-metallic. H. 2-2.5. 
 G. 4.8. Trimetric. In small modified rectangular prisms, or 
 in globular masses. 
 
 Composition : MnO 2 = Mn, 63.2 ; O, 36.8 = 100. 
 
 B. B. with borax affords a deep amethystine color while hot, 
 which becomes red-brown on cooling. In a matrass yields 
 little or no water; when heated to redness, oxygen is evolved. 
 
 Differs from psilomelane- by its inferior hardness, and from 
 iron ores by the violet glass with borax ; gives frequently 
 indications of iron. 
 
 Soluble in HC1 with evolution of Cl. 
 
 Hausmannite, Mn 3 4 = 2MnO, Mn0 2 , when pure, contains 72.1 per 
 cent, of manganese. Color, brownish-black. Streak, chestnut-brown. 
 H. 5-5.5. G. 4.7. Dimetric. 
 
 B. B. and to 1IC1 behaves like the preceding ore. 
 
 Braunite, 2(2MnO,Mn0 2 ) -\- MnO 2 ,Si0 2 , An oxide of manganese, con? 
 taining 69 per cent, of Mn when pure. Color and streak, dark brown- 
 ish-black. Lustre, submetallic. Occurs in square octahedrons ami 
 massive. H. 6-6.5. G. 4.8. Dimetric. 
 
 B. B. like pyrolusite dissolves in HC1, giving off chlorine, leaving 
 
'))<) MINERALOGY SIMPLIFIED. 
 
 Munganite. A hydrous oxide of manganese. Occurs massive and 
 in rhombic prisms. Color, steel -black to iron -black H. 4-4.5. GL 
 4.3-4.4. Trimetric. Columnar, often stalactitic. Lustre, subme- 
 metallic. Color, steel-gray. Streak, reddish-brown, opaque. Frac- 
 ture, uneven. 
 
 In the closed tube yields water ; otherwise similar to braunite. 
 
 .' 
 
 Psilomelane Color, black or greenish-black. Streak, red- 
 dish or brownish-black, shining. H. 56. G. 44.4. Massive 
 and botryoidal. 
 
 Composition : Doubtful. Essentially MnO 2 , with some BaO 
 or K 2 O and H 2 O. H. 5.G. G. 3.7-4.3. Massive. Color, 
 iron-black to steel-gray. 
 
 B. B. like pyrolusite, except that it affords water. 
 Wad (bog manganese). Color and streak, black or brown- 
 ish-black. Lustre, dull, earthy. H. 1-6. G. 3-4. Soils the 
 fingers. Massive, reniform, or earthy. 
 
 Composition : Consists of manganese dioxide, in varying 
 proportions, from 30 to 70 per cent, mechanically mixed with 
 more or less of iron sesquioxide, 10 to 25 per cent, of water, 
 and often several per cent, of oxide of cobalt or copper. 
 
 In a matrass yields water abundantly, and affords a violet 
 glass with borax. There are several varieties. 
 
 Lampadite, or cupreous manganese, constitutes a wad, con- 
 taining 4 to 18 per cent, of copper oxide. 
 
 B. B., when treated with soda and borax on charcoal, affords 
 a globule of metallic copper. 
 
 JRhodochrosite (manganese carbonate dialogite, Mangaspath). 
 Color, rose-red. Streak, white. H. 3.5-4.5. G. 3.4-3.7. 
 Hexagonal. Like calcite in having three easy cleavages, and 
 in lustre. 
 
 Composition : MnO 3 C = CO 2 , 38.6 ; MnO, 61 .4 = 100. Part 
 of the Mn often replaced by Ca,Mg, or Fe. 
 
 B. B. changes color to gray, brown, black, and decrepitates 
 strongly, but is infusible. With salt of phosphorus and borax 
 in O. F. gives an amethystine colored bead ; in R. F. becomes 
 colorless. "With soda and saltpetre on platinum foil yields a 
 
ORES OF MERCURY. 3;>7 
 
 Heated with IIC1 dissolves with effervescence. 
 
 Rhodonite Usually massive. Color, light brownish-red, 
 flesh-red, sometimes greenish or yellowish when impure ; or 
 black on the surface from exposure. Streak, uncolored. II. 
 5.5-6.5. G. 3.4-3.7. Triclinic. Usually massive. 
 
 Composition : Var. MnSiO 3 = SiO 2 , 45.9; MnO, 54.1 = 100. 
 When heated becomes dark-brown, and gives to borax a deep 
 violet while hot, and reddish-brown when cold. 
 
 Resembles red feldspar, but differs in specific gravity, black- 
 ening on exposure, and coloring the borax bead. 
 
 FranMinite (Fe,ZnMn) (FeMn) O 4 . (See Ores of Iron.) 
 This, and other iron ores containing manganese, are used for 
 making " spiegdeisen" 
 
 Minerals containing manganese : wolframite, alabandite, 
 hauerite, chalcophanite, lithiopholite, triphillite, triplite, dick- 
 insonite, reddingite, fairfieldite, triploidite, etc. 
 
 Ores of Mercury. 
 
 
 
 NATIVE MERCURY. Hg. Occurs in fluid globules scat- 
 tered .through the gangue. Color, tin-white. G. 13.56. Be- 
 comes solid and crystallizes at 39 F. (--39.40 C.). 
 
 Heated in a matrass, it volatilizes, condensing in the neck 
 of the matrass in minute globules. Dissolves readily in HNO 3 . 
 Hg is used for the extraction of gold and silver ores. 
 
 Native amalgam is a compound of silver and mercury. H. 
 3-3.5. G. 13.5-14. Isometric. The compounds AgHg= Ag, 
 35.1 ; Hg, 64.9, or Ag 2 Hg 3 = Ag, 26.5 ; Hg, 73.5, are included. 
 Another from Chili having the formula Ag 12 Hg, and con- 
 taining 86.6 per cent, of silver, has been called arguerite ; and 
 still another Ag ls Hg, kongsbergite. 
 
 All the ores of mercury are completely volatile, excepting 
 when Ag and Cu are present. In a matrass boils, gives a sub- 
 limate of metallic Ilg, and leaves a spongy residue of Ag, 
 which, on charcoal, fuses readily to a globule. Dissolves 
 readily in nitric acid. 
 
- 358 MINERALOGY SIMPLIFIED. 
 
 Gerargyrite (calomel, hornsilver), occurs usually in dis- 
 tinct crystals or crystalline coats of a pearl-gray color, and resin- 
 ous adamantine lustre. H. 1-1.5. G. 5.5. Dimetric. 
 
 Composition : HgCl. 
 
 In a matrass yields a white sublimate of HgCl. In a closed 
 tube, with bisulphate of potassium, gives off vapors of HC1, fuses 
 to a pale hyacinth-red globule, becomes yellow when cold. 
 Not affected by HNO 3 . Dissolved by aqua regia. With a 
 solution of KHO, becomes black. 
 
 Cinnabar (mercury sulphide) Color, bright red to brown- 
 ish-red, and brownish-black. Streak, scarlet-red. Occurs in 
 small tabular orsix-sided crystals. Also massive. Lustre, unme- 
 tallic; of crystals, adamantine. H. 2-2.5. G. 8.5-9. Hexagonal. 
 
 Composition : HgS 2 =S, 13.8 ; Hg, 86.2. It contains often 
 impurities. Carbon and clay are* found in the liver ore, or 
 hepatic cinnabar, which has a brownish color and streak. The 
 pure variety volatilizes entirely before the blowpipe, which fact 
 distinguishes it from red oxide of iron or chromate of lead ; 
 from realgar it differs by giving off no alliaceous fumes (As). 
 Mixed with soda and heated in a matrass, affords globules of 
 Hg. In an open tube it is partially decomposed into metallic 
 Hg and S0 2 . 
 
 HNO 3 and HC1 have no visible effect on it. Aqua regia 
 dissolves it, part of the sulphur being precipitated. Insoluble 
 in KHO. 
 
 Metacinnabarite, has the same composition as cinnabar, but 
 differs in crystallization ; it is from Redington Mine, Lake 
 County, California. 
 
 Guadalcazarite, of Mexico, is-HgS, in which a little of the 
 sulphur is replaced by selenium. 
 
 Mercury iodide A reddish-brown ore from Mexico. 
 
 .Tiemannite. A dark steel-gray mercury selenide, from the 
 Hartz and California. 
 
 Coloradoite A grayish-black mercury telluride, with G. 
 8.G27, from Colorado. (Genth.) 
 
 . A mercurous tellurate, HgO 4 Te, from Colorado. 
 
ORES OF NICKEL. 359 
 
 Ores of Nickel. 
 
 NICCOLITE, COPPER NICKEL, ARSENICAL NICKEL Color, 
 pale, copper-red ; streak, pale brownish-red. Lustre, metallic. 
 Brittle. H. 5-5.5. G. 7.3-7.7. Hexagonal ; usually massive. 
 
 Composition : . Ni As = Ni, 44 ; As, 56 = 100. Sometimes a 
 part of the arsenic is replaced by Sb. 
 
 B. B. gives off arsenical fumes, and fuses to a pale globule, 
 which darkens on exposure. In an open tube yields a copious 
 sublimate of As 2 O 3 , and the assay piece assumes a yellowish- 
 green color, and crumbles to pieces. Dissolves almost entirely 
 in HNO 3 ; the solution has a green color ; on cooling As 2 O 3 
 separates. Dissolves readily in aqua regia. 
 
 Breithaiiptite or antimonial nickel. Composition : NiSb 
 = Sb, 67.8 ; Ni, 32.2 = 100. It has a pale copper-red color, 
 inclining to violet. H. 5.5-6. G. 7.54. Crystals hexagonal. 
 
 B. B. after long heating on charcoal it yields a magnetic 
 globule. Fuses with difficulty. In an open tube it gives no 
 sulphur reaction. HC1 acts but little on it, but aqua regia dis- 
 solves it completely. 
 
 Gersdorffite Nickel glance ; a nickel arserio-sulphi.de ; Ni 
 
 S a -f NiAs' = NiAsS = As, 45.5; S, 19.4; Ni, 35.1, but vary- 
 ing much in composition. Color, sulphur-white to steel-gray. 
 II. 5.5. G. 5.6-6.9. Isometric. In a matrass decrepitates 
 violently, yelding a yellowish-brown As 2 S 3 . In an open tube 
 evolves As 2 O. and SO,. Partly dissolved by HNO 3 , while S and 
 As 2 O 3 are precipitated. Aqua regia dissolves it to an apple- 
 green solution, which an excess of NH 3 turns sapphire-blue. 
 
 Ullmannite (nickel stibine, nickdiferous gray antimony) 
 Composition : NiSbS. An antimonial nickel sulphide, con- 
 taining 25 to 28 per cent, of nickel. 
 
 Color, steel-gray, inclining to silver-white. In cubical crys- 
 tals also massive. H. 5-5.5. G. 6.45. Isometric. 
 
 B. B. on charcoal in R. F. fuses to a globule, and yields a 
 white coat of SbO 8 , sometimes emits the odor of As. The 
 melting globule treated with borax frequently gives. the 
 
360 MINERALOGY SIMPLIFIED. 
 
 tion of Fe and Co, besides those of Ni. Concentrated IINO 3 
 acts violently on it, S and Sb 2 O 3 being precipitated. Aqua 
 regia dissolves it, excepting some S, to a green liquid. 
 
 Grunanite (bismuth-nickel) A sulphide containing 31 to 
 38.5 per cent, of S, 10 to 14 per cent, of Bi, and 22 to 40.7 
 per cent, of Ni. Contains also Cu and Fe. 
 
 Color, light steel-gray to silver-white. Often tarnished 
 yellowish. H. 4.5. G. 5.13. 
 
 Millerite (capillary pyrites, nickel sulphide) Color, brass- 
 yellow. Lustre, metallic. Streak, bright. Occurs usually in 
 capillary- or needle-like crystallizations, sometimes like wool. 
 Brittle. H. 3-3.5. G. 4.6-5.65. Hexagonal. 
 
 Composition: NiS=S, 35.6; Ni, 64.4= 100. 
 
 B. B. on charcoal fuses to a globule, and, after roasting, 
 gives, with borax and salt of phosphorus, a violet bead in O. F. 
 which in R. F. becomes gray from reduced metallic nickel. 
 
 In the open tube affords fumes of SO 2 . It is but little 
 affected by concentrated HNO 3 , but aqua regia dissolves it 
 entirely. 
 
 Zaratite (emerald nickel). Color, bright green. Lustre, 
 vitreous. Usually forms incrustations. H. 3-3.25. G. 2.5- 
 2.7. 
 
 Composition : Ni 3 C0 6 -f 6Aq. It is a hydrous nickel car- 
 bonate. 
 
 B. B. infusible alone. Dissolves with effervescence in borax 
 and salt of phosphorus, exhibiting the characteristic nickel 
 reactions. In a matrass loses at 212 F. a large amount of 
 water and blackens. Dissolves readily in heated dilute HNO 3 
 with effervescence (CO 2 ). 
 
 Annabergite (nickel ochre, nickel arsenate). Composition : 
 Ni 3 As 2 O 8 + 8Aq = As 2 5 , 38.6 ; NiO, 37.2 ; H 2 O, 24.2 = 100. 
 Soft, earthy. 
 
 Color, apple-green. 
 
 B. B. on charcoal in R. F. fuses with emission of arsenical 
 vapor to a blackish -gray globule. When treated with borax 
 
ORES OF SILVER. 3d 
 
 the globule gives tlie reactions of nickel, sometimes also those 
 of iron and cobalt. Soluble in acids. 
 
 Morenosite A nickel vitriol, NiO 4 S -{- 7Aq, having an 
 
 apple-green to greenish-white color. 
 
 Lindackerite, hydrous nickel copper arsenate. 
 
 Remingtonite A hydrous nickel carbonate, rose-colored, 
 
 from Maryland. 
 
 Genthite (nickel silicates'), H 4 (Ni,Mg) 4 Si 3 O, 2 , is a hydrous 
 magnesium and nickel silicate, of a pale apple-green color, 
 yielding in one analysis 80 per cent, of nickel oxide. II. 3.4. 
 G. 2.4. Amorphous. 
 
 Rottisite is similar. 
 
 Primelite is an impure apple-green silicate, affording in one 
 case 15.6 per cent, of NiO. 
 
 Alipite is similar ; so, also, garnierite .(and naumeite) from 
 New Caledonia, and worked there for nickel. 
 
 . Ores of Silver. 
 
 Silver occurs native and alloyed with gold, or sometimes 
 with platinum ; also combined with arsenic, sulphur, tellurium, 
 antimony, bismuth, chlorine, bromine, iodine ; but never as an 
 oxide, carbonate, sulphate, or phosphate. 
 
 NATIVE SILVER Color and streak, silver-white and shin- 
 ing. Often black externally from tarnish ; ductile and malle- 
 able. H. 2.5-3. G. 10-11. Isometric. Occurs usually 
 in filiform and arborescent shapes, sometimes in lamina? and 
 massive. 
 
 Composition : Native silver is usually an alloy of silver and 
 copper, the latter amounting often to 10 per cent. Also 
 alloyed with gold, as stated under that metal. 
 
 B. B. on charcoal fuses easily to a globule of a silver- white 
 
 color. Dissolves in HNO 3 , from which it is precipitated as 
 
 chloride by HC1 ; the precipitate is soluble in NH 3 . A bright 
 
 plate of copper, immersed in the nitric-acid solution, becomes 
 
 31 
 
362 MINERALOGY SIMPLIFIED. 
 
 coated with silver. Native amalgam is a compound of mer- 
 cury and silver. (See Mercury Ores.) 
 
 Argentite (silver glance, sulphide of silver) Color and 
 streak, blackish, lead-gray. Streak, shining. Very sectile. 
 H. 2-2. f). G. 7.19-7.4. Isometric. In dodecahedrons. 
 Also reticulated and massive. Cuts like lead (distinction 
 from minerals of the same color). 
 
 Composition : When pure, Ag,S = S, 12.9; Ag, 87.1. 
 
 B. B. on charcoal in O. F. intumesces, evolves SO 2 , and 
 finally yields a globule of metallic Ag. Soluble in dilute 
 IINO 3 , leaving a residue of sulphur. The solution, when 
 treated with HC1 affords a heavy white precipitate of AgCl, 
 which is redissolved by an excess of ammonia. 
 
 Acanthite Ag 2 S. Trimetric. Differs only in crystalline 
 
 form from the preceding. 
 
 Daleminzite is another silver sulphide from near Freiberg. 
 
 Stromeyerite A steel-gray sulphide of silver and copper. 
 
 Ag 2 S + Cu 2 S =8,15.7; Ag, 53.1; Cu, 31.2 = 100. G. 6.26. 
 
 B. B. it fuses, and gives in the open tube SO 2 , but a silver 
 globule is not obtained, except by cupellation with lead. 
 
 Sternberffite.^-Age. 2 $ s . A sulphide of silver and iron, 
 containing 33 per cent, of silver. 
 
 Color, pinchbeck-brown. Streak, black. The ore is foliated, 
 and leaves a tracing on paper like graphite. 
 
 B. B. partially reduced to Ag. Partly soluble in HNO 3 . 
 The solution yields with HC1 a heavy precipitate of AgCl. 
 
 Naumannite. A selenide of silver and lead in iron-black 
 cubes and massive. G. 8. Contains 73 per cent, of silver. 
 
 B. B. fuses easily in O. F ; quietly in R. F., with intumes- 
 cence. With borax yields a pure silver globule. 
 
 Cerargyrite (hornsilver, silver chloride). Color, gray, pass- 
 ing into green and blue. Looks somewhat like horn or wax, 
 and cuts like it. H. 1-1.5. G. 5.5. Isometric. Lustre, 
 resinous. Streak, shining. Extensively worked in the mines 
 of South America and Mexico. 
 
OKKS OF SILVEU. 303 
 
 Composition : AgCl Cl, 24.7 ; Ag, 75.3 100. Fuses in 
 the flame of a candle, and emits acrid fumes. 
 
 B. B. on charcoal affords readily a silver globule. The sur- 
 face of a plate of iron rubbed with it is silvered. Mixed with 
 oxide of copper, and heated on charcoal in R. F., chloride of 
 copper is formed, which colors the flame azure blue. Insoluble 
 in H 2 O and HN0 3 , but soluble in NH 3 . Partially decomposed 
 by a boiling solution of caustic potash. 
 
 Embolite. A chloro-brornide of silver, resembling the horn- 
 silver. 
 
 Color, asparagus- to olive-green. Lustre, adamantine. H. 
 1-1.5. G. 5.3-5.8. Isometric. Malleable and sectile. 
 
 Composition : Ag(Cl,Br) AgCl, 51 ; AgBr, 40. 
 
 B. B. fused with oxide of copper on charcoal in R. F. colors 
 the O. F. greenish, then blue. With soda on charcoal reduced 
 to metallic silver. Heated in a closed tube with bisulphate of 
 potassium gives off bromine vapors, fuses to an intense garnet- 
 red globule, becoming yellow when cold. 
 
 Bromyrite (bromic silver) -Color, yellowish-green or green. 
 Lustre, splendent. H. 2-3- G. 5.8-6. Isometric. 
 
 Composition: AgBr = Br, 42.6 ; Ag, 57.4 = 100. 
 
 B. B. behaves like the preceding. 
 
 Jodyrite Silver iodide. Agl == I, 54.0 ; Ag, 4G.O = 100. 
 
 Color, bright yellow. Lustre, adamantine. H. 1.5. G. 5.7. 
 Hexagonal. 
 
 B. B. on charcoal fuses readily, colors the flame purple-red, 
 and affords a globule of silver. In a closed tube, with bisul- 
 phate of potassium, gives off iodine vapors, fuses to a very 
 dark, almost black, globule. 
 
 Tocornalite A silver and mercury iodide from Chili. 
 
 Amorphous. 
 
 Color, pale yellow. 
 
 Hessite A telluride of silver, Ag 2 Te = Te, 37.2 ; Ag, 62.8 
 
 = 100. 
 
 Color, between lead-gray and steel-gray. Sectile. G. 8.3- 
 8.C,. Malleable. 
 
364 MINERALOGY SIMPLIFIED. 
 
 B. B. in the open tube a faint sublimate of tellurious acid ; 
 on charcoal with soda a silver globule. "In HNO 3 dissolves 
 entirely. 
 
 Petzite is a hessite with the silver replaced in part by gold, 
 (Ag,Au) a Te. G. 8.7-9.4. Between steel-gray to iron-black. 
 Streak, same. One variety yielded Genth : Te, 32. G8 ; Ag, 
 41.86; Au, 25.60 = 100.14. Occurs in Colorado, Utah, etc., 
 witli hessite. 
 
 Tapaltite is a telluride of bismuth and silver. 
 
 Sylvanite (graphite tellurium) A telluride of gold and 
 silver. (See Gold Ores.) 
 
 Eucairite, (Cu,Ag) 2 Se A selenide of silver and copper, 
 containing 4245 per cent, of Ag. 
 
 Color, silver-white to lead-gray. Easily cut with the knife. 
 
 Solution in HNO 3 yields with HC1 a heavy precipitate of 
 AgCl. 
 
 J)yscrasite (antimonial silver) consists simply of Ag and 
 Sb = Ag 4 Sb = Ag, 78; Sb, 22 = 100. Color, nearly tin- white. 
 G. 9.4-9.8. Trimetric. 
 
 B. B. affords furnes of Sb, leaving finally a globule of Ag. 
 Dissolves in HNO 3 , leaving a residue of Sb 2 O 8 . 
 
 Pyrargyrit'e (ruby silver, da jfc-red silver ore) Color, black 
 
 to dark cochineal-red. Streak, cochineal-red. Lustre, splen- 
 dent, metallic, adamantine. H. 2-2.5. G. 5.7-5.9. Hexago- 
 nal. 
 
 Composition : Ag 8 S 8 Sb(= 3Ag. 2 S -f Sb a S 3 ) = S, 17.7 ; Sb, 
 22.5; Ag, 59.8 = 100. Crystallizes in hexagonal prisms. 
 
 B. B. fus^s very easily ; on charcoal a white deposit of SbO 3 
 is deposited, and, mixed with soda in R. F., a globule of Ag 
 is obtained. In an open tube gives antimony fumes, and SO 2 , 
 reddening blue litmus paper. In a matrass fuses easily, yield- 
 ing by continued heating a sublimate of SbS 3 . 
 
 Proustite (light-red silver ore). Resembles the preceding 
 ore. It contains arsenic in place of much or all of the antimony. 
 H. 2-2.5. G. 5.4-5.56. Hexagonal. 
 
ORES OF SILVER. 305 
 
 Composition : Ag s $ s As = S 10.4, A* 15.1, Ag 05.5 = 100. 
 
 B. B. gives off garlic odors. 
 
 Stephanite (brittle silver ore, black silver) Color and 
 streak, iron-black. H. 2-2.5. G. 6.27. Trimetric. Crys- 
 tallized and massive. 
 
 Composition : Ag 5 S 4 Sb(==5Ag 1 S + Sh a S JI ) = S 16.2, Sb 15.3, 
 Ag 68.5. 
 
 B. B. it gives an odor of SO 2 , and also fumes of antimony, 
 and yields a dark, metallic globule, from which silver may be 
 obtained by the addition of soda. Soluble in dilute nitric acid, 
 and the solution indicates the presence of silver by silvering a 
 plate of copper. 
 
 Polybasite Composition : Ag fl Sh 6 (or 9Ag 2 S + Sb,S 3 ), 75.5 
 Ag. Is near stephanite in color, spec, grav., and composition. 
 It crystallizes usually in tabular, hexagonal prisms. H. 2-3. 
 G. 6.214. Trimetric. In the open tube fuses, gives sulphu- 
 rous and antimonial fumes. 
 
 B. B. fuses with spirting to a globule, gives off S (sometimes 
 As), and coats the coal with SbO 3 . Long-continued blowing 
 yields a metallic globule, which, with salt of phosphorus, reacts 
 for copper, and, cupelled with lead, gives pure silver. Decom- 
 posed by HNO 3 . 
 
 Miargyrite. Composition : AgSbS 2 . Is an antimonial 
 silver sulphide, containing but 36.5 per cent, of silver, and 
 having a dark, cherry-red streak, while its color is iron-black. 
 H. 2.5. G. 5.2. Monoclinic. 
 
 B. B. on charcoal gives off fumes of Sb, and an odor of 
 SO 2 ; and in the O. F. a globule is left, which finally yields a 
 button of pure silver. A mixture of borax and soda facilitates 
 the formation of a malleable silver-bead. 
 
 Brongniardite Composition : Ag s PbSb a S s (or PbS -f Ag, 
 
 S + Sb.^). Contains about 25 per cent, of silver. 
 
 Color, black-gray. H. 3. G. 5.0. Isometric. Occurs in 
 octahedrons and massive. 
 
 B. B. gives S reaction. The nitric acid solution yields with 
 H a SO 4 a precipitate of sulphate of lead. 
 
 31* 
 
366 MINERALOGY SIMPLIFIED. 
 
 Polyargyrite Composition: 12Ag. 2 $ -f- Sb 2 S 8 . Isometric. 
 
 Cleavage, cubic. Malleable. Resembles polybasite in compo- 
 sition and behavior. Wolfach, Baden. 
 
 Freieslebenite (Schilfglaserz, Germ.) Composition: (Pb, 
 
 Ag) 5 Sb 2 S n = S, 18.8; Sb, 26.9; Pb, 30.5; Ag, 23.8 = 100. 
 
 Color and streak, steel-gray. Lustre, metallic. H. 2-2.5. 
 G. 6-6.4. Monoclinic, yields easily to the knife*, and is rather 
 brittle. In an open tube gives sulphurous and antimonial 
 fumes, the latter condensing as a white sublimate. 
 
 B. B. on charcoal fuses easily, giving a coating of white 
 antimonious oxide on the outer edge, and near the assay, a 
 yellow one from oxide of lead. Continued blowing leaves a 
 globule of silver. 
 
 Pyrostilpnite, (Feuerblende, Germ.) In delicate crystals. 
 Color, hyacinth-red. Contains 62^.3 per cent, of silver ; also 
 sulphur and antimony. 
 
 Ores of Tin. 
 
 CASSITERITE, TIN ORE, TIN OXIDE. Color, brown, or 
 black ; streak, pale gray to brownish. Lustre, adamantine (of 
 crystals). H. 6.7. G. 6.4-7.1. Dimetric. In square prisms 
 and octahedrons ; often twinned ; also massive, in grains and 
 rolled pebbles (Stream tin). 
 
 Composition : SnO 2 = O, 21.33 ; Sn, 78.67 = 100 ; often con- 
 tains a little iron and sometimes tantalum. 
 
 B. B. alone infusible. On charcoal, with soda, affords a 
 globule of tin. Insoluble in acids. Fused with HKO yields a 
 mass which is mostly soluble in water. 
 
 Stannite (tin pyrites) (Cu,Sn,Fe,Zn)S. A sulphide con- 
 taining 26 per cent, of tin. Color, steel-gray. Lustre, metallic. 
 Occurs usually massive. H. 4, G. 4.3-4.5. Probably di- 
 metric and hernihedral. In an open glass tube yields S0 3 and 
 SnO 2 , which collect close to the assay-piece, and which cannot 
 be volatilized by heat. 
 
ORES OF ZINC. 3G7 
 
 B. B. on charcoal, in R. F. fuses to a black scoriaceous 
 globule ; in O. F. gives off SO 2 , and becomes covered with 
 8nO 2 . When well calcined by the alternate application of the 
 O. F. and R. F., gives with borax the indications of ,Fe and Cu. 
 Soluble in nitric acid to a blue solution, while a mixture of S 
 and SnO remains undissolved. 
 
 Ores of Zinc. 
 
 ZIXCITE, RED ZINC ORE, RED ZINC OXIDE Color, deep 
 or bright red ; streak, orange-yellow. Lustre, brilliant. H. 
 4-4.5. G. 5.4-5.7. Hexagonal. Of distinctly foliated structure. 
 
 Composition : ZnO = O, 19.7; Zn, 80.3 = 100. 
 
 B. B. infusible alone, but yields a yellow transparent glass 
 with borax ; sometimes the manganese reaction in O. F. with 
 borax. On charcoal, a coating of ZnO. 
 
 Dissolves in HNO 3 without effervescence. Occurs with 
 Franklinite at Mine Hill and Sterling Hill, Sussex -County, 
 N. J. 
 
 Sphalerite (blende, zinc sulphide) Color, waxy-yellow 
 
 to black ; streak, white to reddish-brown. Lustre, resinous. 
 Brittle. H. 3.5-4. G. 3.9-4.2. Isometric. Crystallizes in 
 dodecahedrons. 
 
 Composition : ZnS = S, 33 ; Zn, 67 = 100. Contains fre- 
 quently a portion of FeS when dark colored ; often also 1 to 2 
 per cent, of CdS (especially the red variety). This ore is 
 the blackjack of miners. 
 
 B. B. alone infusible. On charcoal in R. F. a feeble dark 
 coat of CdO is usually obtained, which is followed by a coat 
 of pure ZnO. With soda on coal it is easily reduced, and the 
 characteristic zinc flame frequently observed. Fe 'is detected 
 by calcining the mineral in O. F. and treating the residue with 
 borax. 
 
 Strongly heated in an open tube SO 2 is evolved, and the 
 color of the calcined assay is white, yellowish, or brownish," 
 according to the amount of FcS. 
 
368 MINERALOGY SIMPLIFIED. 
 
 The pulverized mineral dissolves in HNO 3 , emitting H >2 8. 
 
 Smith sonite (carbonate of zinc") Color, impure white, 
 
 green or brown. Streak, uncoloreil. Lustre, vitreous or 
 pearly. H. 5. G. 4.3-4.45. Brittle. Hexagonal. Often reni- 
 ibrm and stalactitic. 
 
 Composition: ZnO 3 C = C0 2 , 35.2; ZnO, 64.8 (four-fifths of 
 which is pure zinc) = 100. Often contains Cd. 
 
 B. B. infusible alone, but CO 2 and ZnO are finally vaporized. 
 Negatively electric by friction. 
 
 Mixed with soda and exposed to the R. F. it is decomposed 
 and white ZnO deposited on the coal. The coating is at first 
 dark -yellow, or reddish, when Cd is present. It dissolves 
 readily in acids with effervescence ; also in a solution of KHO. 
 
 Calcimine (hydrous zinc silicate, Galmei). Color, whitish 
 or white, bluish, greenish, or brownish. Streak, uncolored. 
 Lustre, vitreous or subnacreous. Brittle. H. 4.5-5. G. 3.16- 
 3.9. Orthorhombic. Pyro-electric. The smallest fragment 
 heated attracts light substances. In its physical characters it 
 resembles the preceding ore. 
 
 Composition: Zn 2 O 4 Si-f Aq = SiO , 25.0; ZnO, 67.5; H 2 O, 
 7.5 = 100. 
 
 B. B. alone almost infusible. Forms a clear glass with borax. 
 In heated F^SO^ it dissolves, and the solution gelatinizes on 
 cooling. Partly dissolved by solution of HKO. 
 
 Willemite (zinc silicate, troostite) Color, whitish, greenish- 
 yellow, apple-green, flesh-red, yellowish-brown. Streak, un- 
 colored. Brittle. H. 5.5. G. 3.89-4.18. Hexagonal. 
 
 Composition: Zn0 3 Si = SiO 2 , 27.1 ; ZnO, 72.9 == 100. 
 
 B. B. fuses with difficulty to an enamel; on charcoal with 
 soda yields a coating which is yellow while hot, and white on 
 cooling, and which, moistened with cobalt solution and treated 
 in O. F., is colored bright green. Gelatinizes with HCL 
 
 The zincite, willemite, and franklinite (the latter described 
 under iron ores), of Frankline, N. J., are together worked as 
 a zinc ore, and both zinc and zinc oxide are produced. 
 
APPENDIX. 
 
 Carbonaceous Compounds. 
 
 Grnplilte (plumbago, C.) consists essentially of pure carbon ; 
 most specimens contain iron, the quantities of which vary 
 from a mere trace up to 5 per cent. Hexagonal. In flat six- 
 sided prisms or tables. Lustre, metallic. Color, iron-black 
 to dark steel-gray. Thin laminae, flexible. H. 1-2. G. 2.25- 
 2.27. Soils paper, and feels greasy. The finest and most 
 valuable mineral is used for lead pencils. At a high tempera- 
 ture it burns in the air without flame or smoke, leaving usually 
 some red oxide of iron behind. 
 
 B. B. infusible, both alone and with reagents ; not acted 
 upon by acids ; i'used with nitre in a platinum spoon, defla- 
 grates, converting the reagent into potassium carbonate, which 
 effervesces with acids. 
 
 Anthracite Anthracite (called also glance coal, and stone 
 coal) has a high lustre, and is often iridescent ; fracture con- 
 choidal. H. 2.25. G. 1.3-1.8. 
 
 Composition : It usually contains 80 to 83 per cent, of car- 
 bon, with 4 to 7 of volatile matter ; the rest consisting of earthy 
 impurities, which consist of SiO^Al./),, and Fe s O 3 . Burns 
 with a feeble blue flame. In a matrass, gives usually a little 
 water, but no empyreumatic oil. Does not color a boiling 
 solution of caustic potash. 
 
 Bituminous Coal C,H,O, in variable proportions. Bitu- 
 minous coal varies much in the amount of oil, coal-tar, or gas 
 it yields when heated ; and there is a gradual passage in its 
 varieties through semi-anthracite to anthracite. It is of a 
 
370 APPENDIX. 
 
 black color, with the powder black, but it is softer than anthra- 
 cite. G. 1.2-1.5. The volatile bituminous matter contains 
 from 76 to 90 per cent, of carbon. The earthy impurities 
 consist principally of SiO 2 , A1 2 O 3 , and CaO. 
 
 The following tabulation, from Wagner's Technology, exhibits 
 at a glance the successive stages and nature of this conver- 
 sion : 
 
 
 Carbon. 
 
 Hydrogen. 
 
 Oxygen. 
 
 Wood 
 
 . 52.65 
 
 5.25 
 
 42.10 
 
 Peat. 
 
 . 60.44 
 
 5.96 
 
 33.60 
 
 Lignite . . . 
 
 . 66.96 
 
 5.27 
 
 27.76 
 
 Earthy brown coal . 
 
 . 74.20 
 
 5.89 
 
 19.90 
 
 Coal (secondary) 
 
 . 76.18 
 
 5.64 
 
 18.07 
 
 Coal (older) 
 
 . 90.50 
 
 5.05 
 
 4.40 
 
 Anthracite 
 
 . 92.85 
 
 3.96 
 
 3.19 
 
 In a matrass some varieties of bituminous coal soften and 
 cake (coking coal), while others are entirely infusible ; all 
 varieties are decomposed, evolve combustible gases and empy- 
 reumatic oils, and leave a porous residue of more or less metallic 
 lustre (coke), which behaves like anthracite. 'On platinum 
 foil burns with a luminous flame and emission of smoke, leaving 
 an earthy residue. Boiled with a solution of caustic potash or 
 with etlier imparts to these solvents no color, or only a pale 
 yellow. 
 
 Brown Coal Composition nearly the same as that of bitu- 
 minous coal, but the organic constituents contain only from GO 
 to 7o per cent, of carbon. In physical properties bears some- 
 times a close resemblance to the preceding. Some varieties 
 show distinctly the texture of wood (lignite). 
 
 In a matrass infusible, but some varieties soften ; evolves 
 combustible gases, empyreumatic oils, water of acid reaction, 
 and a peculiar, disagreeable odor, leaving a residue which con- 
 sists of carbon and a considerable amount of ash. On platinum 
 foil burns with a smoky flame and emission of a peculiar odor. 
 Boiled with a solution of caustic potash colors the liquid brown. 
 
 Asphaltum C,H,O in variable proportions, with about 
 
CARBONACEOUS COMPOUNDS. 371 
 
 75 per cent, of carbon. G. 1-1.8. Of black or brownish-black 
 color and bituminous odor, is amorphous and pitch-like. Fuses 
 at about 100 C., and burns with a bright flame and emission 
 of a thick smoke, leaving little ash, which consists essentially 
 of SiO 2 , A1O 3 , and FeO 3 . 
 
 In a matrass gives empyreumatic oil, some ammoniacal 
 water, combustible gases, and leaves a carbonaceous residue. 
 Treated with boiling ether colors the solvent wine-red to 
 brownish-red (distinction from bituminous coal) ; when treated 
 with a. boiling solution of caustic potash it does not color the 
 liquid, or at the most imparts to it a pale-yellow color (distinc- 
 tion from brown coal). 
 
 Albertite Coal-like in hardness. Color, jet-black, but 
 
 slightly soluble in camphene. and only imperfectly fusing when 
 heated, but having the lustre of asphaltum, and softens a little 
 in boiling water. H. 1-2. G. 1.097. 
 
 Fills fissures in the subcarboniferous rocks near Hillsborough, 
 Nova Scotia, and supposed to have been derived from the 
 hydrocarbon of the adjoining rock, and to have been oxidized 
 at the time it was formed, and filled the fissures (J. D. Dana). 
 
 GraTiamit'e. From West Virginia. Forms a related mate- 
 rial. H. 2. G. 1.145. 
 
 Color, pitchy-black. Soluble mostly in camphene, but melts 
 only imperfectly. An analysis afforded carbon, 70.45 ; hydrogen, 
 7.82; oxygen (with traces of nitrogen), 13.46; ash, 2.26 
 100. 
 
 Amber (Bernstein, Germ.) Composition, C,H,O. Forms 
 irregular masses. 
 
 Color, yellow, sometimes brownish or whitish. Lustre, 
 resinous. Transparent to translucent. H. 2-2.5. G. 1.18. 
 Electric by friction. It consists mainly (85 to 90 per rent.) 
 of a resin, insoluble in all solvents, called succinite, and two 
 other resins soluble in alcohol and ether an ethereal oil and 
 succinic acid (2^ to 6 per cent.). Amber fuses with diffi- 
 culty in the matrass, yielding water, empyreumatic oil, gases, 
 succinic acid, and a residue of amber-resin. It burns with 
 
372 APPENDIX. 
 
 a yellow flame, emitting an agreeable odor, leaving behind a 
 black, shining, carbonaceous substance. 
 
 Elaterite (mineral caoutchouc, elastic bitumen) contains C 
 and H. Found in soft flexible masses, hence its name. 
 Color, brownish-black ; sub-translucent. G. 0.91.25. 
 
 Composition : C, 85.5 ; H, 13.3-98.8. Burns in the flame of 
 a candle with a yellow flame and bituminous odor. 
 
 Retinite or retinasphalt It is found in brown coal, and 
 constitutes a fossil resin, which has a yellow color, is fusible 
 and inflammable, and largely soluble in alcohol. 
 
 Hatchettine, similar to the last named, is met with in mineral 
 coal-beds at Merthr Tydail, and near Loch Fyne in Scotland. 
 
 Ozocerite is like wax or spermaceti in consistence. G. 0.85 
 -90. Color, white, yellowish-brown. Soluble in ether. It 
 feels greasy, and fuses at 132 to 145 Fah. It has been ob- 
 tained by destructive distillation from mineral coal, peat, petro- 
 leum, etc. 
 
 Petroleum.* 
 
 Mineral oils of density from O.GO-0.85. Soluble in benzine 
 or camphene. Consists of many liquids of the naphtha and 
 etJiylene series. The composition of the naphtha, or marsh-gas 
 series, is expressed by the general formula C n -|-H 2n _(_ 2 , of which 
 methane, or marsh-gas, CH 4 is the first or lowest member; 
 and that of the ethylene (olefiant gas) series by the formula 
 C n H 2n = C, 85.71 ; H, 14.29 = 100. It occurs in rocks of all 
 ages from the lower silurian to the 'most recent ones, and has 
 been formed through the decomposition of animal or vegeta- 
 ble substances, or both. 
 
 Petroleum is obtained chiefly at the present time from more 
 or less deeply-seated, subterranenean chambers, or cavities, 
 among the rock-strata, only reached by boring. Being under 
 
 * See Coal Oil and Petroleum. Their Origin, History, Geology, and 
 Chemistry, by Henri Erni. Philadelphia, 1865, published by Henry 
 Carey Baird. 
 
PETROLEUM. 373 
 
 pressure of the gas, associated with it, and, in many cases, that 
 of water also, it rises to the surface in boring, and sometimes 
 makes a " spouting" well. The mineral oil of the rocks has 
 been formed through the decomposition of animal or vegeta- 
 ble substances. From the nature of the rocks, which most 
 abound in the species of hydrocarbons that yield oil, it is evi- 
 dent that .the rock material was in the state of a fine mud ; that 
 through this mud much vegetable or animal matter was dis- 
 tributed, almost in the condition of an emulsion ; that the stra- 
 tum of this mud becoming afterwards overlaid by other strata, 
 the decomposition of vegetable or animal matter went forward 
 without the presence of atmospheric air, or with very little of 
 it. Under such circumstances either vegetable material or 
 animal oils might be converted, as chemists have shown, into 
 mineral oil. Dry wood consisting approximately (excluding 
 the ash and nitrogen^ of 6 atoms of carbon to 9 of hydrogen, 
 and 4 of oxygen. If now all the oxygen of the wood combines 
 with a part of the carbon to form carbonic acid, and this 2C0 2 , 
 thus made, is removed, there will be left C 4 H 8 ; twice this, 
 C 8 H ]g , is the formula of a compound of the marsh gas, or 
 naphtha series. Again, animal oils, by decomposition under 
 similar circumstances, produce like results. Removing from 
 oleic acid its oxygen, O 2 , and 1 of carbon, together equivalent 
 to 1 of carbonic acid, there is left C 17 H 3i , which is an oil of the 
 ethylene series. (J. D. Dana.) 
 
 Mendelejeff (Baird's Annual of 1878, p. 146) has proposed 
 a new hypothesis of the origin of petroleum. Starting with 
 the nebular hypothesis, the author regards the interior of the 
 earth as metallic, doubtless composed largely of iron, and car- 
 bides of iron. Through rents made by earthquakes, water 
 gained access to these bodies at a high temperature and under 
 great pressure ; and by their mutual chemical action metallic 
 oxides and saturated hydro-carbons resulted. These latter, 
 carried by watery vapor, have spread themselves through the 
 overlying rocks. Pie gives various geological and chemical 
 facts which go to sustain his hypothesis. 
 32 
 
374 
 
 APPENDIX. 
 
 The petroleum, as obtained by boring, originally contains 
 several gaseous carbo-hydrogens, viz., methane, CII 4 ; propane, 
 C 3 H g ; and butane (quartane) : as fluids are present, pentane, 
 C 5 H 12 ; hexane, C 6 H U ; heptane, C 7 H 16 ; octane, C g H 18 ; nonane, 
 C 9 H 20 ; and further, tridecane, C 13 H 28 ; quatuordecane, C U II 30 ; 
 quindecane, C 15 H 32 . The higher members of the methane 
 series, the paraffines* proper, containing 20 or more atoms 
 of C, have the consistency of butter, or are more or less 
 crystalline solids. In many kinds of petroleum they exist in 
 a state of solution, and may be separated by distilling off the 
 more volatile portions. Solid paraffine is a colorless, crystal- 
 line, fatty substance, probably consisting of a mixture, of seve- 
 ral of the higher members of the series, C n -{- H 2n + 2 . 
 
 Alfred Allen has furnished the following table serving for 
 the distinction of petroleum benzine or naptha from the coal- 
 tar naptha or " benzol" : 
 
 PETROLEUM BENZINE. 
 
 1. Consists of heptane (C 7 Hi 6 ) 
 to the amount of about 50 per 
 cent, and its homologues. 
 
 2. Heptane contains 84 per 
 cent. C. 
 
 3. Begins to boil at 140O-17QO 
 Fah. 
 
 4. Specific gravity about 0.69- 
 0.72. 
 
 5. Has the odor of petroleum. 
 
 6. Dissolves iodine, forming a 
 rasberry-red solution. 
 
 COAL-TAR NAPHTA, OR BENZOLE. 
 
 1. Consists of benzole (C 6 H 6 ), 
 and its homologues. 
 
 2. Benzole contains 92.3 per 
 cent. C. 
 
 3. Begins to boil at 176 Fall. 
 
 4. Specific gravity about 0.88. 
 
 5. Has the odor of coal-tar. 
 
 6. Dissolves iodine, forming a 
 purple-red solution (similar to 
 the aqueous solution of potassium 
 permanganate). 
 
 * From parum affinis, indicating their chemical indifference. The 
 name paraffine has long been applied to the solid compounds of the 
 series, on account of this character; and many of the liquid com- 
 pounds of the same series are known commercially as paraffine oils. 
 It is convenient, therefore, to employ the term paraffine as a generic 
 name for the whole series. 
 
NITROGEN IN ORGANIC COMPOUNDS. 
 
 375 
 
 PETROLEUM BENZINE. 
 
 7. Dissolves (even after some 
 time) only very little pitch of pit 
 coal, the solution being scarcely 
 colored. 
 
 8. Does not mix with carbolic 
 acid, even when previously fused. 
 
 9. Soluble at a common tem- 
 perature in a mixture of 2 volumes 
 of absolute (100 percent.) alcohol 
 or in 4 to 5 volumes of methylic 
 (wood spirit), spec. grav. 0.828. 
 
 10. When heated with 4 vols. 
 of nitric acid (spec. grav. 1.45) 
 the acid assumes a brown color, 
 while the oil swims on the top 
 of it. 
 
 COAL-TAR NAPHTHA, ou BENZOLE. 
 
 7. Dissolves coal-tar pitch free- 
 ly, forming a dark-brown liquid. 
 
 8. Mixes in all proportions 
 with pure carbolic acid. 
 
 9. With anhydrous alcohol 
 miscible in all proportions. 
 Forms with an equal volume of 
 methylic alcohol (sp. grav. 0.828) 
 a homogeneous liquid. 
 
 10. Readily miscible with 4 
 volumes of nitric acid (sp. grav. 
 1.45) with evolution of heat and 
 formation of a dark-brown color. 
 A portion of the nitro-benzol 
 thus produced may, when cold, 
 separate as a distinct layer. 
 
 Experiment 10 serves to separate petroleum-benzine from 
 light coal-tar oils. The mixture of the oils is treated in a 
 narrow bolt-head, with attached cpndenser, with nitric acid 
 (spec. grav. 1.45). After the reaction has almost ceased, the 
 liquid is poured into a narrow, graduated tube. The bulk of 
 the upper layer read off gives approximately the quantity of 
 petroleum benzine. The nitro-benzol produced from the coal- 
 tar naphtha remains dissolved in the nitric acid. If a great 
 deal of benzol is present, whereby the nitric acid is incapable 
 to dissolve at all, an independent layer of a deep brown color 
 collects beneath the petroleum benzine. 
 
 Detection of Small Quantities of Nitrogen in 
 Organic Compounds. 
 
 The detection is based upon the reaction of metallic potas- 
 sium, which, when heated with any nitrogenous organic com- 
 pound, forms cyanide of potassium. 
 
 A piece of K is placed at the bottom of a narrow test-tube, 
 
0/0 APPENDIX. 
 
 ami covered with the substance to be examined ; llie mixture 
 is then heated to redness till the excess of K is volatilized, the 
 residue dissolved in water ; the solution precipitated by ferroso- 
 i'erric salt, e. g., a solution of copperas (oxidized by standing 
 in the air), and mixed with excess of HC1, which, if cyan-ide 
 of potassium has been formed, leaves a. residue of Prussian 
 blue. Substances not containing nitrogen likewise give this 
 reaction if they contain nitre or nitrous acid.. Hydrate or 
 carbonate of potassium, instead of potassium, does not give so 
 delicate an indication of nitrogen.* 
 
 r? 
 
 * Lassaigne, J. Chim. nied., 19, 201 ; also, Jour. j>r. Chem., 20, 
 p. 143; also, Gmelin's Handbook. of Chem., vol. vii. 147, 153. 
 
INDEX. 
 
 Absolite, 314 
 
 Absorption-spectrum, 163 
 Acanthite, 243 
 Acetic acid, 116 
 
 detection of, 100 
 
 Acid potassium sulphate, examina- 
 tion with, 99-101 
 salts, 32, 33 
 Acids, division of, 29 
 hydrogen, 29, 30 
 hydroxyl, 29, 30 
 oxygen, 29, 30 
 properties of, 28 
 sulphur, 29, 30 
 testing, 107, 108 
 Acmite, 275 
 Adamite, 283 
 ^Eschynite, 255, 324 
 Agalmatolite, 306 
 Agate mo_rtar, 39 
 Aikinite, 245 
 Alabandine, 252, 285 
 Alabandite, 244, 285 
 Alberti te, 371 
 Albite. 301 
 Algodonite, 233 
 Alkalies, testing, 108, 109 
 Alkaline carbonates, action of 
 . cobalt, 159 
 
 deportment of, with the 
 alkaline earths, 174, 175 
 earths, chlorides and nitrates 
 
 of, solubility, 174 
 deportment of the alkaline 
 carbonates with, 174, 175 
 examination of, 110 
 metals of the, 173 
 sulphates of the, 203 
 metals, the new, 130 
 Allanite, 250, 273, 277 
 Allochroite, 274, 275 
 Alloclasite, 234 
 Allophanc, 305 
 Almandite, 275 
 Altaite, 238 
 
 Alumian, 306 
 
 Alumina, detecting, 139, 140 
 
 phosphate of. precipitation of, 
 140 
 
 salts, detecting, 139, 140 
 Aluminite, 303 
 
 Aluminium plate, as a support in 
 blowpipe analysis, 76 
 
 subphosphate of, 304 
 
 sulphate of, 303 
 Alum-stone, 303 
 Alunite, 303 
 Amalgam, native, 357 
 Amalgams, 177, 178 
 Amber, 371, 372 
 Amblygonite, 285 
 Amethyst, 325, 326 
 Amianthus, 300 
 Ammonia, 68, 116 
 
 action of, on cobalt, 159 
 
 on manganous salt, 176, 177 
 Ammonia-alum, 283, 303 
 Ammonia, detecting, 140, 141 
 
 hydrate, 68 
 Ammonic carbonate-, 68 
 
 chloride, 68 . 
 Ammonium chloride, 256 
 
 sulphide, 116 
 
 sulphydrate, 116 
 Amphibole, 275, 299 
 Amphithalite, 304 
 Analcite, 290 
 
 Analysis, humid, and the blowpipe, 
 determination of minerals by, 
 207-31 )S 
 
 Andalusite, 307 
 Anglesite, 2(52 
 Anhydrite, 280, 281 
 Annabergfte, 2is 
 Anorthite, 293 
 Anthophylliti', 3i_>3 
 Anthosidcrite, 31:.! 
 Anthracite, 361) 
 Antigorite, 380 
 Antimonfahlerz, 240, 241 
 
 32* 
 
INDEX. 
 
 Antimonial nickel, 243 
 silver, 241 
 sulphuret of lead and copper, 
 
 240 
 
 Antimoniates, 143, 144 
 Antimonic acid, 143 
 Antimonite, 240 
 Antimony, 121 
 
 and arsenic, distinguishing, 
 
 145, 146 
 
 and lead, sulphides of, treat- 
 ment of, 142 
 sulphuret of, 240 
 characteristics of, 142-144 
 combined with copper, separa- 
 tion of, 141 
 with lead and bismuth, 
 
 detection of, 141 
 compounds of, Plattner's treat- 
 ment of, 142 
 detecting, 141-144 
 from tin, separation of, 194 
 fusion point of, 142 
 glance, 240 
 
 mirror, characteristics of, 146 
 native, 236 
 ores of, 331, 332 
 oxide of, 256 
 red, 256 
 spots, characteristics of, 145, 
 
 146 
 
 sulphide of, 142 
 sulphuret of, 240 
 tin, and copper, oxides of, 
 
 treatment of, 142 
 Anvil, 39 
 Apatite. 285, 315 
 Aphthitalite, 278 
 Apophyllite, 290 
 Apparatus and manipulations in 
 
 the laboratory, 38-58 
 and method employed for sub- 
 mitting test substances to the 
 flame, 112-114 
 for Marsh's tests, 147 
 for observations of flame colora- 
 tions, 105 
 
 Aqua regia, 67, 116 
 Aragonite, 310 
 Arfvedsonite, 275 
 Argand burner, 54 
 Argentic nitrate, 68 
 'Argentite, 231 
 Arkansite, 253, 282, 324 
 Arsenate of calcium, 281 
 Arsenic, 121, 144-150 
 
 and antimony, distinguisluiii}-. 
 145, 146 
 
 Arsenic, characteristics of, 144 
 
 distil phide, 256 
 
 in minerals containing no sul- 
 phur, test for, 148-150 
 
 mirror, characteristics of, 146 
 
 native, 232 
 
 ores of, 332, 333 
 
 Reinech's test for, 150 
 
 spots, characteristics of, 145, 
 146 
 
 sulphide of, 142 
 
 trisulphide, 256 
 
 white, 256 
 Arsenicum, 144-150 
 Arseniosiderite, 269 
 Arsenio-sulphuret of iron, 235, 236 
 Arsenious acid, 256 
 
 small traces of, detection 
 of, 149 
 
 and arsenic acids, examination 
 
 of, 149 
 reduction of, 144, 145 
 
 hydride, decomposition of, 145 
 
 gas, 145 
 Arsenite, 256 
 Arsenomelane, 232 
 Arsenopyrite, 235, 236, 252 
 Asb'estos, blue, 275 
 
 fibres of, 114 
 Asperolite, 316 
 Asphaltum, 370, 371 
 Assay, supports for, 75-78 
 
 tubes for arsenic, 149-150 
 Assays, small, phenomena to be 
 
 considered in, 117 
 Astrophyllite, 274 
 Atacamite, 2(55 
 Atlasite, 265, 267 
 
 Atmospheres, solar and stellar, 137 
 Atomicity of elements, 32-35 
 Atomic weights of the elements, 
 
 table of, 36-38 
 Atoms, linking of, 34 
 
 terms applied to various, .'>: 
 Augite, 275, 299 
 Aurichalchite, 266 
 Aurotellurite, 239 
 Automaton blowpipe, 84 
 
 hand blowpipe, 84, 85 
 Autunite,-286 
 
 Auxiliary apparatus and manipula- 
 tions in the laboratory, 38-58 
 Avogadro's law, 27 
 Axinite, 298 
 Azurite, 266 
 
 Babingtonite, 275 
 Baric chloride, 69 
 
INDEX. 
 
 379 
 
 B.irir nitrate, 68 
 
 Barite, 2S1 
 
 Barium, examination of, 110 
 
 flame, spectrum of, 129 
 
 spectrum lines of, 138 
 
 sulphate of, 281 
 Barnhardtite, 245 
 Barsowite, 289 
 
 Baryta, characteristics of, 150 
 Baryto-calcite, 311 
 Bases, 30, 31 
 
 oxygen, 30, 31 
 Basic hydroxides, 31 
 
 salts, 32, 33 
 Bastite, 318 
 Bastnasite, 316 
 Bauxite, 323 
 Beakers, the, 41, 43 
 Behavior of the elements at high 
 temperatures, 112-114 
 
 of the most important ores be- 
 fore the blowpipe and with 
 solvents, 330-368 
 Bellows, double, for hand use, 83 
 Belonite, 245 
 Bending and closing glass tubes, 
 
 56-58 
 
 Benzine, 374, 375 
 Benzole, 374, 375 
 Beraunite, 272 
 Berlinite, 304 
 Berthierite, 243 
 Beryl, 164; 326 
 BerzeHanite, 237 
 
 Berzelius and Plattner's lamp, 78, 79 
 Berzelius's test for bromine, 153 
 
 for small traces of urscui- 
 
 ous acid, 149 
 Beyrichite, 247 
 Biborate of sodium, 279 
 Biliary theory of chemistry, 25 
 Bindheimite, 260 
 Binnite, :1'.\:>' 
 
 Biotite, 296, 321, 322 *<^"\ 
 Bismuth, 121, 150, 151, 234, 235, 
 248, 249 
 
 acicular, 245 
 
 and tin, separation of, 193 
 
 characteristics of, 150, 151 
 
 nickel, 245 
 
 ores of, 333, 334 
 
 oxide of, 283 
 
 selenideof, 2:5(5 
 
 silicate of, 276 
 
 telluret of, 2:59 
 Bismuthinite, :J4s 
 Bismuthous nitrate, 116 
 P.ismutite, 276 
 
 Bisulphuret of iron, 246 
 Bitumen, elastic, 372 
 Bituminous coal, 369, 370 
 Black copper ore, 266 
 
 lead, 254 
 
 Blast-lamps, 81-86 
 Bloedite, 278 
 Blowers, foot, 55, 56 
 Blowing machine, 85 
 
 with the blowpipe, 71, 72 
 Blowpipe analysis and apparatus, 
 69-92 
 
 and humid analysis, determina- 
 tion of minerals by, 207-368 
 
 flame, 72-75 
 
 furnace, 54 
 
 lamps, 78-80 
 
 mouth, 69-71 
 
 reagents, 89-91 
 
 treatment of oxides with, 99 
 Blowpipes and blast-lamps, fixed, 
 
 81-86 
 Blue iron earth, 271 
 
 vitriol, 265 
 Bog iron ore, 312 
 Boltonite, 321 
 Bonds of attraction, 34 
 Boracic acid, 151, 153 
 Boracite, 281, 284 
 
 Borate of sodium, detection of, 152 
 Borax, 279 
 
 behavior of metallic oxides 
 with, 94 
 
 reactions of oxides with, 99 
 Boric acid, 151, 153, 284 
 
 compounds of, with an 
 
 alkali testing, 152 
 testing, 108 
 Borickite, 271 " 
 Bornite, 244 
 
 determination of, 222 
 Borocalcite, 279 
 Borosilicate of calcium, 286 
 Botryogen, 269 
 Boulangerite, 241 
 Bournonite, 241 
 Braunite, 251 
 Breithauptite, 243 
 Brewstrite, 291 
 Brochantite, 265, 266 
 Brogniardite, 242 
 Bromide, detection of, 
 Bromine, 116, 152, 153 
 
 detecting, 153 
 Brongniartine, 280, 281 
 Bronzite, :'.2:; 
 Brookiti', 255. 324 
 Knnvn coal, 370 
 
380 
 
 INDEX. 
 
 Brown hematite, 253 
 
 spar, 310 
 Brucite, 309, 310 
 Brushite, 288 
 Buch's hammer, 39 
 Bulb-tubes, 89 
 Bunsen and Kirchhoff, researches 
 
 of, 127, 134 
 burner, use of, 220 
 gas-burner, 81 
 holder, 113 
 
 Bunsen's burner, use of, in the 
 examination of flame colora- 
 tions, 104, 107 
 flame reactions, 111, 112 
 
 chemical reagents em- 
 ployed for, 115, 116 
 gas blowpipe and blast-lamp, 
 
 83, 84 
 
 gas-burner, 53, 54 
 gas-larnp, 111, 112 
 Buratite, 206 
 Burners, 52, 53, 54 
 
 Cacoxenite, 271 
 Cadmium, 121, 153, 154 
 
 detection of, 153, 154 
 
 sulphuret of, 313 
 
 treatment of, 153 
 Caesium, discovery of, 130 
 
 spectrum lines of, 133 
 Calamine, 301, 309 
 Calcite, 310 
 
 Calcium, anhydrous sulphate of, 
 280 
 
 carbonate of, 310 
 
 flame, spectrum of, 129 
 
 hydrated sulphate of, 280 
 
 phosphate of, 315 
 
 spectrum lines of, 133 
 Calomel, 178, 257 
 Cancrinite, 282 
 Carat, 329, 330 
 Carbon, 154, 155 
 
 compounds, 154, 155 
 
 dioxide, detection of, 101 
 
 group, 328, 330 
 
 monoxide, 154 
 
 detection of, 101 
 
 Carbonaceous compound, 369-372 
 Carbonate of ammonia, 68 
 
 of barium, 280 
 
 and calcium, 311 
 
 of calcium and sodium, 280 
 
 of lead, 261 
 
 of silver, 259, 260 
 
 of sodium, action of, on cobalt, 
 159 
 
 Carbonic dioxide, 154 
 
 test, 40 
 
 Carburet of iron, 254 
 Carmenite, 246 
 Carnallite, 27!) 
 Carpholite, 294 
 Carphosiderite, 270 
 Carrol lite, 246 
 Cassiterite, 254, 324, 325 
 Castor, 297 
 Catapleiite, 291 
 Caustic potash, 69 
 
 action of, on cobalt, 159 
 potassa, action of, on chro- 
 mium, 157 
 soda solution, 115 
 ! Cellestine, 281 
 ' Cerargyrite, 259 
 Cerite, 317 
 
 decomposition of, 155 
 Cerium, 155, 156 
 oxide of, 312 
 protoxide of, 156 
 Cerolite, 319, 322 
 Ceroxide, 156 
 Cerussite, 262 
 Cervautite, 311 
 Chabazite, 291 
 Chalcedony, 325, 326 
 Chalcocite', 246 
 Chalcodite, 273 
 Chalcolit, 267 
 Chalcophyllite, 264 
 Chalcopyrite, 244, 245 
 Chalcostibite, 242, 243 
 Charcoal borers, 75, 76 
 
 rod, reduction on the, 118 
 rods, 114 
 
 supports for assay, 75 
 Chemical affinity, 25 
 
 combination by volume, law of, 
 
 26,27 
 
 compounds, complex, detect- 
 ing certain elements in, 139- 
 202 
 
 law, fundamental, 26, 27 
 mixtures, testing, 107-111 
 notation, 25 
 philosophy 25-38 
 properties of minerals, 219 
 reagents for Bunsen's flame re- 
 action, 115, 116 
 solution, 220 
 system, changes of notation in, 
 
 28 
 new changes of notation in, 
 
 28 
 Chemically pure water, 59-62 
 
INDEX. 
 
 381 
 
 Chemistry, solar and stella, 134-137 
 
 theories of, 25-38 
 Chenevixite, 264 
 Childrenite, 248, 315 
 Chiolite, 282 
 Chloride of ammonia, 08 
 
 of ammonium, action of, on 
 man<ranous salt, 176 
 
 of barium, 69. i:>s 
 
 of copper, 265 
 
 of platinum, 68 
 
 Chlorides and nitrates of the alka- 
 line earths, solubility of, 174 
 
 detection of, 156 
 Chlorine, 100, 156, 157 
 Chlorite, 319, 322 
 Chloritoid, 1522 
 Chloropal,317, 318 
 Chlorospinel, 327, 328 
 Chodneffite, 282 
 Chondroarsenite, 283 
 Chonicrite, 290-292 
 Chromate of lead, 261 
 
 and copper, 262 
 
 Chromic acid, characteristics of, 158 
 detection of, 101 
 testing, 108 
 
 iron, 254. 
 
 oxide, detection of, 157 
 
 salts, detection of, 157 
 Chromite, 254 
 Chromium, 157-159 
 
 and vanadium, the same reac- 
 tions in, 157 
 
 compounds, 125 
 
 detection of, 97 
 
 ores of, 334, 335 
 
 oxide of, minerals containing 
 but little, treatment of, 157 
 
 recognition of, 116 
 
 sesquioxide of, 157 
 
 trioxide, detection of, 101 
 Chrondrodite, 320 
 Chrysoberyl, 308 
 Chrysocolla, 316, 317 
 Chrysotile, 318, 319, 320 
 Cimolite, 305 
 Cinnabar, 244, 257 
 Clarification or synopsis of the I 
 
 tables, key to, 226-228 
 Clausthalite, 237 
 Clinoclasite, :-C>4 
 Clintonite, 320 
 Cloanthite, 2:'.."> 
 Closed glass-tubes, reductions in, 
 
 118 
 
 Coal, successive stages and nature 
 of its conversion, 370 
 
 Coal-tar naphtha, 374, 375 
 Coals, 369, 370 
 
 Coating's or incrustations on porce- 
 lain, 118-120 
 Cobalt, 159, 160, 314 
 blue, 268 
 compounds, 122 
 ores of, 335, 336 
 oxides of, 159 
 peroxide of, 160 
 pyrites, 246 
 solution, colorations caused by, 
 
 103 
 
 examination with, 102, 103 
 Cobaltic oxide, 160 
 Cobaltus cobaltic hydrate, 159 
 hydroxide, 159 
 oxide, 159 
 
 salt, neutral solution of, treat- 
 ment of, 159 
 Cobellite, 241 
 Coeruleolactite, 304 
 Collyrite, 305 
 
 Colorations caused by cobalt solu- 
 tion, 103 
 Color of minerals, observations of, 
 
 210 
 Colored flames, flame reactions, and 
 
 spectrum analysis, 103-139 
 Colors in flame colorations, table 
 
 of, 104, 105 
 
 of flames, detection of sub- 
 stances by, 127 
 Columbite, 254, 255 
 Columbium, 160 
 pentoxide, 97 
 
 detection of, 101 
 Combination by volume, chemical 
 
 law of, 26, 27 
 
 Complex chemical compounds, 
 detecting certain elements in, 
 139-202 
 
 Compounds, detection of, 375, 376 
 Comptonite, 287 
 Conichalcite, 264 
 Continuous spectrum, 128, 163 
 Cookeite, 21)6 
 Copiapite, 270 
 Copper, 160-162 
 
 and bismuth, sulphuret of, 
 
 244 
 
 and iron, sulphuret of, 244 
 and lead, selehieuret of, 237 
 and tin, separation of, 193 
 anhydrous, carbonate of, 266 
 blue, carbonate of, 266 
 chloride of, 265 
 compounds. 1 _' [ 
 
382 
 
 INDEX. 
 
 Copper, compounds of oxides of, 
 263 
 
 detection of, 160, 161 
 
 examination of, 110, 111 
 
 gray, 242 
 
 preen, carbonate of, 266 
 
 metallic, 162 
 
 mica, 264 
 
 native, 231 
 
 nickel, 235 
 
 ore, black, 266 
 red, 249 
 
 ores of, 336-340 
 
 phosphate of, 267 
 
 prismatic arsenate of, 264 
 
 pyrites, 244 
 
 variegated, determination 
 of, 222 
 
 recognition of, 116 
 
 red oxide of, 266 
 
 selenieuret of, 237 N 
 
 sulphate of, 265 
 
 sulphuret of, 244 
 
 variegated, 244 
 Copperas, 269 
 Coquimbite, 270 
 Cordierite, 326 
 Corks, 50, 51 
 Cornwallite, 265 
 Corundum, 308 
 
 detecting, 139 
 Corynite, 235 
 Cotunnite, 257 
 Covellite, 265 
 Crednerite, 251 
 Crocidolite, 275 
 Crocoisite, 261 
 Crocoite, 261 
 Cronstedtite, 272 
 Crookesite, 237 
 Crucible tongs, 49, 50 
 Crucibles, 48, 49 
 
 supports for, 51-53 
 Cryolite, 281 
 Cryophyllite, 292 
 Crystallization, 217, 218 
 
 names used by different 
 
 authors, 218 
 systems of, 218 
 Cubanite, 244 
 Cupreine, 246 
 Cupric oxide, 161 
 Cuprite, 249, 266 
 Cuproplurnbite, 245, 246 
 Cuprous oxide, 161 
 Cutting pliers, 40, 89 
 Cyanic acid, detection of, 100 
 Cyanochalcite, 3L6, 317 
 
 | Dalton's contributions to chemistry, 
 26 
 
 Danatite, 287 
 
 Danburite, 295 
 
 Datolite, 286 
 
 Datolith', 286 
 
 Decantation and precipitation, 
 41-43 
 
 Dechenite, 261, 262 
 
 Decomposition by acids, 221, 222 
 of light, 128 
 
 Deflagration, 205 
 
 Delessite, 322 
 
 Deportment of the alkaline carbo- 
 nates with the alkaline earths, 
 174, 175 
 
 Descloizite, 263 
 
 Detecting certain elements in com- 
 plex chemical compounds, 139-202 
 
 Determination of minerals by ex- 
 periments with the blowpipe and 
 humid analysis, 207-368 
 i Determinative mineralogy, 207-368 
 
 Deweylite, 292 
 
 Diadochite, 271 
 j Diallage, 297 
 I Diallogite, 310, 311, 312 
 j Diamond, 328-330 
 
 steel mortar, 38 
 i Diamonds, valuation of, 329, 330 
 
 Diaspore, 305 
 
 Didymium, 162, 163 
 
 salts, solutions of, 163 
 
 Digenite, 246 
 I Diopside, 295, 299 
 
 Dioptase, 316 
 
 Dishes and crucibles, 48, 49 
 
 Disthene, 307 
 
 Disterrite, 307 
 
 Distilling apparatus for water, 
 59-62 
 
 Dolomite, 310 
 
 Dorneykite, 232, 233 
 
 Double salts, 33 
 
 Dualism, chemical. 25, 26 
 
 Dualistic theory, a discovery as to 
 salts which disposes of it, 32 
 
 Dufrenite, 271 
 
 Dufidnoywte, 232, 233 
 
 Dumas, discovery of substitution 
 by, 26 
 
 Durangite, 283 
 
 Dyaphorite, 242 
 
 Dyscrapsite, 241, 242 
 
 Dysulite, 328 
 
 Edelforsite, 302 
 Edingtonite, 286 
 
IXDKX. 
 
 383 
 
 Eh ntc, 2<jr 
 
 F.kel)crite, 29:! 
 Ekmannite, 273 
 Elastic bitumen, 372 
 Elaterite, 372 
 
 Electro-chemical theory of chemis- 
 try, 25, 2IJ 
 
 Elements at high temperature, be- 
 havior of, 112-114 
 ignition of, 117 
 atomic weights of, 36-38 
 in complex chemical com- 
 pounds, detecting, 139-202 
 which can be best recognized 
 from the reactions of their 
 compounds, 121-127 
 Emerald nickel, 312 
 Emery, 308 
 
 detecting, 139 
 Emerylite, 296 
 Emission of light, ascertaining, 
 
 117 
 
 Enargite, 232, 233 
 Epsomite, 278, 282 
 Epsom salt, 278 
 Erbium, 163 
 Erinite, 265 
 
 Erlenmeyer's argand burner, 54 
 Erubescite, 244 
 Erythrite, 268 
 Eucairite, 237 
 Euchroite, 265 
 Euclase, 164, 326 
 Eudialyte, 288 ' 
 Eukenite, 325 
 Eukolite, 293 
 Eulytite, 276 
 EuphyHite, 298 
 Euraltte, 273 
 Eusynchite, 262, 263 
 Evansite, 304 
 Evaporation, 46, 47 
 Examination, methods of, 117-120 
 of minerals with soda, 96-98 
 of the assay in the platinum 
 forceps for flame colorations, 
 103-105 
 
 with acid potassium sulphate 
 or concentrated sulphuric 
 acid, 99-101 
 
 with cobalt solution, 102, 103 
 with zinc and hydrofluoric acid, 
 after previous decomposition 
 (fusion) of the mineral, 101 
 Examinations of metals with sodium 
 
 thiosulphate, 98, Ji'. 
 Experiments in flame colorations, 
 105-107 
 
 Fats for lamps, 80 
 Fayalite, 249 
 Feldspars, 301 
 Ferberrite, 275 
 Ferric acid, 170 
 
 oxide, characteristics of, 
 
 168-170 
 Ferrocyanide of potassium, 116 
 
 action of, on manganous 
 
 salt, 177 
 action of, with ferrous salts, 
 
 168 
 
 Ferroilmenite, 254 
 
 Ferrous oxide, 167 
 
 salts, 167 
 
 action of, on chloride of 
 gold and nitrate of silver, 
 168 
 action of sulphydric acid 
 
 on, 167 
 action of various substances 
 
 on, 167, 168 
 Fibroferite, 270 
 File, triangular, 89 
 Filtering stands, 44 
 Filtration, 43-46 
 Fischerite, 304 
 Fixed blowpipes and blast-lamps, 
 
 Fauserite. 283 
 
 Flame blowpipe, 72-75 
 
 colorations, 103-105, 117 
 
 apparatus for, 105 
 coloring elements, spectrum 
 
 lines of, 133 
 
 reactions, reducible to metals, 
 yielding no incrustations, 
 121-124 
 
 Bunsen's, 111,112 
 elements recognized by, 120 
 general review of, 120-127 
 submitting test substance to 
 
 the, 112-114 
 Flames, colored, flame reactions, and 
 
 spectrum analysis, 103-139 
 detection of substances by the 
 
 colors of, 127 
 examination of, through a 
 
 prism, 127, 128 
 Flaming, 71, 72 
 Fletcher-Plattner blowpipe furnace, 
 
 54 
 
 Fletcher's blowpipe lamp, 79, 80 
 burners, 53, 54 
 chemical blowpipe, 82, 83 
 hot-blast blowpipe, 86 
 
 chemical blowpipe, 70, 71 
 new mouth blowpipe, 85 
 
384 
 
 INDEX. 
 
 Flintstone, 325, 326 
 
 Fluocerite, 316 
 
 Fluoride ol sodium and aluminium, 
 
 281 
 
 Fluorides, 164 
 Fluorine, 163, 164 
 Fluorite, 281 
 
 Flux most commonly used, 203 
 Fluxing and fusion, 203-206 
 
 for the analysis of the sulphates 
 of the alkaline earths, 203 
 
 how the term is applied, 203 
 Foot blowers, 55, 56 
 Forceps with platinum points, 88 
 Foster's lamp, 80 
 Franklinite, 251, 252 
 Frauenhofer lines, 134 
 Freiberg 1 hammer, 39 
 
 lamp, 78, 79 
 Freieslebenite, 242 
 French weights and measures, 
 
 223-226 
 Frenzelile, 236 
 Fuel lamps, 78-80 
 Fuming hydriodic acid, 115 
 Fusibility- from 1-5 or easily vola- 
 tilized, 232-251 
 
 of minerals, 209 
 
 scale of, 209 
 
 six grades of, 117 
 Fusion, how the term is applied, 203 
 
 and fluxing, 203-206 
 
 Gadolinite, 200, 201, 320 
 
 analysis of, 201 
 Gahnite, 327 
 Galena, 244 
 Galenite, 241, 244 
 
 Galls, tincture of, action of, on fer- 
 rous salts, 168 
 Garnet, 327 
 
 almandine, 275 
 Gas-bottle, 51 
 Gas-burner, Bunsen's, 81 
 Gases, colors and odors of different, 
 
 evolved, 100, 101 
 molecules of, in compound 
 
 bodies, law of, 26, 27 
 Gay-Lussac's contributions to chem- 
 istry ,-26, 27 
 law of combination by volume, 
 
 26,27 
 
 Gay-lussite, 280 
 Gearksutite, 282 
 Gehlenite, 289, 320 
 General review of flame reactions, 
 
 120-127 
 Genthite, 318 
 
 Geocronite, 241 
 Gerhardt's residues, 34, 35 
 
 system of chemical notation, 25 
 Gersdorffite, 235 
 Gibbsite, 304 
 Gillingite, 274 
 Gismondite, 287 
 Glaserite, 278 
 Glass-beads, fused, 118 
 Glasses for examinations of flame 
 
 colorations, 105, 106 
 Glass-tubes, bending and closing, 
 
 56-58 
 
 Glauber salt, 278 
 Glauberite, 280, 281 
 Glaucodot, 234 
 Glaucolite, 293 
 Glauconite, 275 
 Glucina, 164, 165 
 
 combinations in which it occurs, 
 
 164, 165 
 
 Goethite, 312, 313 
 Gold, 165, 166 
 
 compounds, 123 
 
 native, 230, 231 
 
 ores of, 341-343 
 
 testing, 116 
 
 Goldschmidt's test for bromine, 153 
 Goslarite, 283 
 Grahamite, 371 
 Graphic tellurium, 239 
 Graphite, 254, 369 
 Green earth, 275 
 Greenockite, 313 
 Grossularite, 294, 301 
 Guadalcazarite, 236, 237 
 Guanajuatite, 236 
 Guarinite, 300 
 Gvmnite, 319 
 Gypsum, 280. 281 
 
 Haematite, 249, 252 
 Halite, 279 
 Halloysite, 305 
 Halogens, 28 
 Hammers, 39 
 Hardness of minerals, 210 
 
 scale of, 210 
 Harmotome, 298 
 Hatchetin, 372 
 Hauerite, 244, 252 
 Hausmannite, 251 
 Hausmann's hammer, 39 
 Hauynite, 285, 287 
 Heating an assay on charcoal in the 
 
 blowpipe flame, 75, 76 
 Heavy spar, 281 
 Hebronitc, 286 
 
INDEX. 
 
 385 
 
 Hedenbergite, 209 
 Hedyphane, 260 
 
 Hclvite, 287 
 
 Hematite, 272, 312, 313 
 
 Herapath blowpipe, 81, 82 
 
 Hessite, 238 
 
 Heterogenite, 268 
 
 Hexagonal mica, 321 
 
 High temperatures, behavior of the 
 elements at, 112-114 
 
 Hipostilbite, 291 
 
 Homichline, 245 
 
 Hornblend, 299 
 black, 275 
 
 Hortonolite, 249, 273 
 
 Howlite, 295 
 
 Huascolite, 244, 246 
 
 Huggins, Mr., substances discov- 
 ered by, in the atmosphere of the 
 stars, 137 
 
 Humboldt, Alexander, contribu- 
 tions to chemistry, 26 
 
 Hureaulite, 270 
 
 Hutchinson's hammer, 39 
 
 Hyalophane, 301, 325 
 
 Hydraeids, 29 
 
 Hydrates and oxides of metals, 31 
 
 Hydric sulphide, (H-OO 
 detection of, 100 
 
 Hydroboracite, 284 
 
 Hydroborate of calcium and magne- 
 sium, 284 
 
 Hydrochleric acid and zinc, exami- 
 nation with, 101 
 detection of, 100 
 testing, 108 
 
 Hydrofluoric acid, 66, 67, 164 
 detection of, 100 
 
 Hydrogen acids, 29, 30 
 
 Hydro-hematite, 313 
 
 Hydromagnocalcite, 309 
 
 Hydrostatic balance, 211 
 
 Hydrotalcite, 312 
 
 Hydrous ammonium sulphate, 256, 
 
 257 
 
 phosphate of iron and manga- 
 nese, 270 
 
 Hydroxides, basic, :>1 
 
 Hydroxyl acids, 29, 30 
 
 Hydrozincite, 309 
 
 Hyposulphite of sodium, examina- 
 tions of metals with, 98, 99 
 
 Hystatite, 253 
 
 Ignition of the elements ut high 
 
 temperatures, 117 
 I les's reaction for boric acid, l.Y> 
 33 
 
 Illuminating gas, 81 
 Ilmenite, 253 
 
 Incrustations or coatings on porce- 
 lain, 118, 120 
 Indices of Valence, 34 
 Indium, 121 
 
 discovery of, 130 
 
 spectrum lines of, 133 
 Infusible or infusibility above 5, and 
 
 non-volatile, 251-255 
 Inorganic substances, tests of, 91, 92 
 Insolubility, 220 
 lodargyrite, 259 
 Iodide films, 120 
 
 of silver, 166 
 Iodides, 166 
 Iodine, 166 
 
 compound, test of, 153 
 
 detection of, 100 
 Iridium, 166, 167 
 
 compounds, 123 
 
 ores of, 341-343 
 Iridosimine, 255 
 Iron, 167, 170 
 
 and manganese, phosphate of, 
 270 
 
 and nickel, sulphuret of, 245 
 
 arsenio-sulphuret of, 235, 236 
 
 compounds, 121, 122 
 
 hydrated peroxide of, 274 
 
 lime garnet, 274 
 
 magnetic, 249, 252 
 
 ore, red, 249, 252, 272 
 
 ores of, 343-350 
 
 oxides of, 167 
 
 peroxide of, 272 
 
 pyrites, 246 
 
 recognition of, 116 
 
 sesquioxide of, 168-170 
 
 spar, 310 
 
 specular, 272 
 
 vitriol, 269 
 Isoclasite, 285 
 Isometric iron pyrites, 247 
 Ittnerite, 287 
 
 Jacobsite, 252 
 
 Jalpaite, 243 
 
 Jamcsonite, 240 
 
 Jargons, 202 
 
 Jarosite, 270 
 
 Jasper, 325, 326 
 
 Jefferisite, 291 
 
 Jefferson i to, 299 
 
 Jolly's spring balance, 214-21(5 
 
 .lully!.-, 290 
 
 Jordanite, 232 
 
386 
 
 INDEX. 
 
 Kainite, 283 
 
 Kammererite, 319 
 
 Kaolin, 305 
 
 Kaolinite, 278, 305 
 
 Kassiterite, 309 
 
 Keramohalite, 283 
 
 Kermesite, 256 
 
 Key to the general classification or 
 
 synopsis of the tables, 226-228 
 Kieserite, 278, 282 
 Kilbrickenite, 241 
 Kjerulflne, 285 
 Klaprothite, 246 
 Klipsteinite, 250, 289 
 Kuebelite, 274 
 Kreittonite, 326 
 
 Labradorite. 293, 294, 301 -^ 
 Lamp, alcohol ,- 79, 80 
 Lamps, fuel, 78-80 
 Lanarkite, 261 
 Langite, 266 
 Lapis-lazuli, 288, 292 
 Larderellite, 284 
 Lasurstein, 288, 292 
 Laumontite, 286 
 Laxmannite, 263 
 Lazulite, 306 
 Lead, 121, 170, 171 
 
 and antimony, sulphides of, 
 treatment of, 142 
 
 and copper, seleuiuret of, 237 
 
 arsenate, 260 
 
 and chloride of, 260 
 
 carbonate of, 261 
 
 chloride of, 257 
 
 cuprous, sulphate of, 261 
 
 molybdate of, 262 
 
 native, 231 
 
 ores of, 350-355 
 
 sesqui-chromate of, 261 
 
 sulphate of, 262 
 
 superoxide of, 250 
 
 tungstate of, 262 
 Leadhillite, 262 
 Lehrbachite, 236 
 Lepidolite, 276, 296 
 Lepidomelane, 274, 276, 277 
 Leuchtenbergite, 322 
 Leucite, 308,^321 
 Leucophanite, 297 
 Libethenite, 267 
 Lievrite, 250, 273 
 Light, compound nature of, 128 
 
 decomposition of, 128 
 
 refraction of, 128 
 
 refrangibility of, 129 
 
 white, composition of, 128, 129 
 
 Lime, 171, 172 
 
 harmotome, 287 
 Lime-alumina-garnet, 294 
 Limonite, 253, 312 
 Limonites, 274 
 Linking of atoms, 34 
 Linnarite, 261 
 Liquor ammonise, 68 
 Liroconite, 264 
 Lithia, 172, 173, 270 
 
 tourmaline, 308 
 Lithionite, 276 
 Lithiophorite, 251, 311 
 Lithium compounds, spectrum 
 analysis of, 130 
 
 flame, spectrum of, 129 
 
 salts of, 172, 173 
 
 spectrum lines of, 133 
 
 testing, 109 
 
 Litmus paper, preparation of, 63 
 Lolingite, 252 
 Lbweite, 278 
 Ludwigite, 269, 311 
 Lunar caustic, 68 
 Luneburgite, 285 
 Lunnite, 267 
 
 Lustre, minerals without metallic, 
 256, 257 
 
 of minerals, 209 
 
 of the mineral, noting the, 208 
 
 Magnesia, 173-175 
 
 characteristics of, 173 
 
 hydrate of, 309 
 Magnesite, 310 
 Magnesium, 310, 327 
 
 borate of, 284 
 
 hydrated silicate of, 319 
 
 pyrophosphate of, 175 
 
 sulphate of, 278 
 Magnetic iron, 249, 252 
 
 needle, 89 
 
 pyrites, 247 
 Magnetite, 249, 252 
 Magnets, 40, 89 
 Magnifying glass, 40 
 Magnoferrite, 253 
 Malachite, 266, 295, 297 
 Malgonite, 230 
 Malleable metals and mercury, 
 
 230-232 
 Manganese, 175-177, 249, 314 
 
 black silicate of, 250 
 
 carbonate of, 311 
 
 characteristics of, 175, 176 
 
 compounds, 126 
 
 detection of, 97 
 
 dioxide, 176 
 
IXDKX. 
 
 387 
 
 Manganese, ores of, 355-357 
 
 oxide of, 25:>, 2*3 
 
 peroxide of, 252 
 
 recognition of, 116 
 Manganic acid. 17(5 
 
 oxide, 176,' 177 
 Manganite, 251, 252 
 Man.ganous oxide, 175 
 Manipulations in the laboratory, 
 
 38-58 
 
 Marcasite, 247 
 Margarite, 296 
 Margarodite, 322 
 Marmatite, 313 
 Mannol itc, 319 
 Marsh's test apparatus, 147 
 Mascagnite, 25(5, 257 
 Measuring the spectrum, 1"8, 139 
 Meerschaum, 290, 292, 318 
 Megabasite, 276 
 Meionite, 289 
 Melaconite, 2fi6 
 Melanocroite, 261 
 Melanterite, 269, 270 
 Melilite, 289 
 Meionite, 238 
 Menaccannite, 253 
 Mendelejeff, D. J., investigations of, 
 
 in regard to uranium, 198 
 Meneghinite, 241 
 Mercuric cyanide, 116 
 
 oxide, 178 
 Mercurous chloride, 257 
 
 chlorides, 178 
 
 compounds, 177 
 
 salts, 178 
 Mercury, 121 
 
 metallic, 178 
 
 native, 231, 232 
 
 ores of, 357, 358 
 
 selenide of, 236 
 
 sulphuret of, 257 
 Mesitine, 311 
 Mesitite, 311, 312 
 Mesolite, 287 
 Metaeinnabarite, 248 
 Metallic films or incrustations, sepa- 
 ration of, 119 
 
 lustre, minerals with, 226-229, 
 
 230-255 
 
 minerals without, 227-229, 
 256, 257 
 
 matters, elimination of, 97 
 
 oxides, reduction of, 97 
 
 with borax, behavior of, 94 
 with salt of phosphorus, 
 95 
 
 sulphides, 127 
 
 Metals, examinations of, with 
 
 sodium thiosulphate, 98, 99 
 hydrates and oxides on, 31 
 native, malleable, and mercury, 
 
 230-232 
 
 Metantimonic acid, 143 
 Metastanic acid, 193 
 Metatungstic acid, 196, 197 
 Metaxite, 319 
 
 Methods of examination, 117-120 
 Miarygyrite, 242 
 Mica, 307 
 Micas, 321 
 
 Miller, Prof. W. A., substances dis- 
 covered by, in the atmosphere of 
 the stars, 137 
 Millerite, 246, 247, 248 
 Mimetisite, 260 
 Mineral caoutchouc, 372 
 Mineralogy, determinative, 207-368 
 Minerals, altered reactions of im- 
 pure, 217 
 containing oxide of chromium, 
 
 treatment of, 157 
 determination of, with experi- 
 ments with the blowpipe and 
 humid analysis, 207-368 
 easily volatile or combustible, 
 
 256, 257 
 examination of, with soda, 
 
 96-98 
 
 grouping for testing, 219 
 infusible or fusible above 5, 
 
 303-328 
 
 preparation of, for the blow- 
 pipe, 38-40 
 
 species selected for the study 
 of determinative mineralogy, 
 222, 223 
 
 tables of, introduction to, 207 
 which fuse easily and volatilize 
 only partially or not at all, 
 258-302 
 with metallic lustre, 226, 27, 
 
 280-255 
 without metallic lustre, 227- 
 
 229, 256, 257 
 Minium, 261 
 Mispiekel, L.':'.:>, 236 
 Mock diamonds, 330 
 Mohr's hydrostatic balance., 211 
 Molecules of compound bodir.--, law 
 
 of, 26, 27 
 
 Molybdate of ammonia, 6S 
 Molybdenite, 254 
 Molybdenum, 17S-1SO 
 compounds, 124 
 recognition of, 116 
 
388 
 
 INDEX. 
 
 Molybdie acid testing los 
 trioxidc, detection of, 101 
 
 Molybdite, 276 
 
 Monazite, 315 
 
 Monradite, 320 
 
 Monticellite, 321 
 
 Monzonite, 302 
 
 Mordenite, 292 
 
 Morenosite, 269 
 
 Mortar, agate, 39 
 diamond steel, 38 
 
 Mosandrite, 291 
 
 Mouth blowpipe, G9-71 
 
 Muellerite, 239 
 
 Muriatic acid, 67 
 
 Muscovite, 296, 307, 321 
 
 Myeline, 306 
 
 Myrabalite, 278 
 
 Myrgyrite, 259 
 
 Mysorine, 266 
 
 Nadorite, 260 
 Nagyagite. 239 
 Naphtha, 374, 375 
 Native malleable metals and mer- 
 cury, 230-232 
 Natokite, 265 
 Natrolite, 286 
 Naumannite, 237 
 Needle spar, 310 
 Nernalite, 310 
 Neolite, 320 
 Nephelite, 288 
 Nephrite; 300 
 Nessler's test, 140 
 Neutral salts, 32 
 New or unitary system of chemistry, 
 
 25-38 
 Newton, Sir Isaac, experiment of, 
 
 on light, 128, 129 
 Niccolite, 235 
 Nickel, 180, 181, 234 
 
 compounds, 122 
 
 emerald, 312 
 
 ores of, 359-361 
 
 to detect, with cobalt, 160 
 
 vitriol, 269 
 Nickelbluethe, 268 
 Nickeliferous gray antimony, 243 
 Nickeline, 235, 243 
 Niobian compounds, 125 
 Niobite, 254 
 Niobium, 160 
 Nippers, 40 
 Nitrate of baryta, 68 
 
 of potassium, 277 . 
 
 of silver, 68 
 
 solution, 115 
 
 Nitrate of sodium, 277 
 Nitrates, 181,182 
 
 and chlorides of the alkaline 
 
 earths, solubility of, 174 
 Nitratine, 277 
 Nitric acid, 67, 116, 181, 182 
 
 testing, 107, 108 
 Nitrogen tetroxide fumes, detection 
 
 of, 100 
 
 Nitrous acid, testing, 107, 108 
 Nohlite, 297 
 Normal salts, 32 
 Nosite, 288 
 Notation, changes of, in the new 
 
 chemical system, 28 
 Nuttallite, 293 
 
 Oblique mica, 321 
 
 Obsidian, 302 
 
 Ochre, brown, 312 
 
 Octahedrite, 324 
 
 Okenite, 287, 290 
 
 Oligoclase, 301 
 
 Olive oil, 78 
 
 Olivenite, 264 
 
 Opal, 325 
 
 Optical investigation of minerals, 
 
 217 
 
 Ore, and what it is, 330 
 Ores, behavior of, before the blow- 
 pipe and with solvents, 330- 
 368 
 
 of antimony, 331, 332 
 
 of arsenic, 332, 333 
 
 of bismuth, 333, 334 
 
 of chromium, 334, 335 
 
 of cobalt, 335, 336 
 
 of copper, 336-340 
 
 of gold, platinum, iridium, and 
 palladium, 341-343 
 
 of iridium, 341-343 
 
 of iron, 243-350 
 
 of lead. 350-355 
 
 of manganese, 355-357 
 
 of mercury, 357, 358 
 
 of nickel, 359-361 
 
 of palladium, 341-343 
 
 of silver, 361-366 
 
 of tin, 366, 367 
 
 of zinc, 367, 368 
 Organic acids, detection of, 101 
 Orpiment, 256 
 Orthite, 200 
 Orthoclase, 301, 325 
 Ortho- rhombic iron pyrite, 247 
 Osmium compounds, 123 
 Oxacids, 29 
 Oxalate of ammonium, 69, 280 
 
INDEX. 
 
 389 
 
 Oxalate of calcium, 280 | Pharmacosiderite, 208 
 
 Oxidation and reduction of sub- Phenacite, 326 
 
 stances, 118 
 
 Oxide incrustations, 119 
 Oxides and hydrates of metals, 31 
 
 behavior of, treated before the 
 
 Phenakite, 164 
 Phillipsite, 287 
 Philosophy, chemical, 25-38 
 
 Phlogopite, 322 
 
 blowpipe with sodium thio- Phoenicochroite, 261 
 sulphate, 99 | Pholerite, 305 
 
 metallic, behavior of, with I Phosphate of alumina, precipitation 
 . borax, 94 of, 140 
 
 of ammonium-magnesium, 281 
 of iron and manganese, 270 
 of soda, 68 
 of sodium, 175 
 
 with salt of phospho- 
 rus, 95 
 
 reduction of, 97 
 reactions of, with borax, 99 
 
 with general reagents, 93- 
 
 103 
 
 Oxygen, 181, 183 
 acids, 29 
 bases, 30, 31 
 Ozocerite, 373 
 
 Pachnolite, 282 
 Palagonite, 273 
 Palladium, 182, 183, 231 
 
 compounds, 122 
 
 detection of, 116 
 
 occurrence of, 182 
 
 ores of, 341-343 
 Paper for filtering, 43, 44 
 Parisite, 312 
 Pastreite, 270 
 Patience in the study of determina- 
 
 tive mineralogy, 222 
 
 Pearlstone, 302" 
 
 Pectolite, 290, 292 
 
 Peganite, 304 
 
 Peligot, views of, in regard to ura- 
 nium, 198 
 
 Pencatite, 310 
 
 Pennitite, 319, 322 
 
 Pentaldite, 245 
 
 Percylite, 2(55 
 
 Permanent gases, spectra of, 131, 
 132 
 
 Permanganic acid, 176 
 
 Permangate salt, 176 
 
 Perofskite, 254, 255, 324 
 
 Peroxide of tin, :;2l' 
 
 Petalite, 296 
 
 Petroleum, 372-375 
 benzine, 374, 375 
 composition of, 372, 374 
 MendelejefTs theory of the 
 
 origin of, 373 
 where obtained, 372, 373 
 
 Pettkoite, 26!) 
 
 Petzite. 2:ii) 
 
 Pluirmacolite, 281 
 
 Phosphates, 183 
 Phosphochalcite, 267 
 Phosphochromite, 263 
 Phospho-molybdate of ammonium, 
 
 263 
 Phosphoric acid, 68 
 
 or phosphates, 183 
 
 testing, 108 
 Phosphorus compounds, 126 
 
 salt of, behavior of metallic 
 
 oxides with, 95 
 
 Physical properties of minerals, 209 
 Picromerite, 273, 282 
 Picrosmine, 319 
 Piedmontite, 295 
 Pisanite, 266 
 Pissophanite, 303 
 Pistacite, 301 
 
 Pitchstone, 302 
 Pitticite, 208 
 Plagionite, 241 
 Platinum, 183, 184 
 
 action of different substances 
 
 on, 205, 206 
 apparatus, 48, 49 
 
 and appliances, 87, 88 
 care required in handling, 
 
 205 
 
 compounds, 123 
 crucibles, dishes, etc., 48, 49 
 
 repairing, 206 
 native, 231 
 ores of, 341-343 
 spoons, 87 
 
 substances by which it is attack- 
 ed or not attacked, 205, 206 
 testing, llii 
 vessels, use and preservation 
 
 of, 205, 206 
 wire, 87, 114 
 Plattner's blowpipe, 70 
 
 treatment of compounds of 
 
 antimony, 142 
 PlattiH'i-itr, :.'.->6 
 33* 
 
390 
 
 INDEX. 
 
 Pleonaste, 327 
 Pliers, 40 
 Plumbago, 369 
 Plumbic acetate, 116 
 Plumbogummite, 304 
 Plumbo-resinite, 304 
 Polybasite, 232 
 Polycraee, 255, 315 
 Polyhalite, 280, 281 
 Poly lite, 299 
 Polytelite, 241 
 
 Porcelain dishes and crucibles, 48 
 earth, 305 
 lamp plate, 112 
 spar, 293 
 supporters, 76 
 Porcellanite, 293 
 Potash alum, 278, 303 
 Potassa, action of cobalt on, 159 
 Potassium, 184 
 
 and aluminium, sulphate of, 
 
 278 
 
 cyanide, 96 
 
 flame, spectrum of, 129 
 nitrate of, 277 
 oxalate, 96 
 
 spectrum lines of, 133 
 sulphate, examination with, 99- 
 
 101 
 
 sulphates of, 278 
 testing, 108, 109 
 Prasine, 267 
 
 Precipitates, washing, 45, 46 
 Precipitation and decantation, 41-43 
 Predazzite, 310 
 Prehnite, 291, 292 
 Preliminary tests of inorganic solid 
 
 substances, 91, 92 
 Preparation of reagents required for 
 
 analysis in the wet way, 59-69 
 Prism, examination of flames 
 
 through a, 127, 128 
 Prismatic arsenate of copper, 264 
 Protoxide of cerium, 156 
 Pseudomalachite, 267 
 Psilomelane, 250, 252, 314 
 Pucherite, 276 
 Pulverization, 38-40 
 Pumice, 302 
 Pycrophyll, 319 
 Pyrargyrite, 242, 258 
 Pyrites, 246, 247 
 
 copper, variegated, determina- 
 tion of, 222 
 Pyrochlore, 325 
 Pyrochroite, 309, 314 
 Pyro-electricity, 216 
 Pyrolusite, 176, 252 
 
 Pyromeline, 269 
 
 Pyromorphite, 260 
 
 Pyrope, 301 
 
 Pyrophosphate of magnesium, 175 
 
 Pyrophyllite, 295, 307, 322 
 
 Pyrosclerite, 290 
 
 Pyrosmalite, 274 
 
 Pyrostibite, 256 
 
 Pyroxene, 295, 297, 298 
 
 Pyrrothite, 247 
 
 Quantivalence, 25, 31 
 
 of elements, how expressed, 34 
 valence, or atomicity of ele- 
 ments, 33-35 
 
 Quartz, 325, 326 
 
 Quicksilver, horn, 257 
 
 Rabdionite, 249, 269 
 Racks and test-tubes, 40, 41 
 Raimondite, 270 
 Ralstonite, 303 
 Raphanosmite, 237 
 Reactions, altered, of impure mine- 
 rals, 217 
 
 of oxides with general reagents, 
 
 93-103 
 Reagents, 115, 116 
 
 for analysis in the wet way, 
 
 preparation of, 39-69 
 Realgar, 256 
 Red iron ore, 249, 252 
 vitriol, 269 
 
 rays, refrangibility of, 129 
 Redonite, 304 
 Reduction of substances, 118 
 
 on the charcoal rod, 118 
 Reductions in closed-glass tubes, 
 
 118 
 
 Refraction of light, 128 
 Refrangibility of light, 129 
 Reinsch's test for arsenic, 150 
 Residues, Gerhardt's, 34, 35 
 Retinasphalt, 372 
 Retinite, 372 
 Retort stand, 45 
 Rhodium, 184, 185 
 
 compounds, 123 
 Rhodonite, 276, 294 
 Richmondite, 304 
 Richterite, 295, 300 
 Rionite, 232, 233 
 Ripidolite, 319, 322 
 Rock crystals, 325, 326 
 Roemerite, 270 
 Ropperite, 249, 274, 321 
 Ross, Col. Wm. A., 76, 77 
 
INDEX. 
 
 391 
 
 Rottisitc, '517 
 Rubellite, 308 
 Rubidium, 184, 185 
 
 discovery of, 130 
 
 spectrum lines of, 133 
 Ruby, detecting:, 130 
 
 silver ore, 242 
 Ruthenium, 185 
 Rutile, 195, 254, 255, 324, 325 
 
 Sal-ammoniac, 63, 256 
 Salt, 68 
 
 common, 279 
 Saltpetre, 277 
 Salts, 28, 29, 32, 33 
 
 normal, acid and basic, 299 
 Samarskite, 250, 279 
 Samoite, 305 
 Sand-bath, 51 
 Sapphire, 308 
 
 detecting-, 139 
 Sarcopsrde, 271 
 Sassolite, 284 
 Saynite, 245 
 Scales of thermometers, relations 
 
 of, 224-226 
 Scapolite, 293 
 Scheelite, 295, 324 
 Schorlomite, 293 
 Scolecite, 2S6 
 Scorodite, 208 
 Selbite, 254, 260 
 Selenide of bismuth, 236 
 
 of mercury, 236 
 
 and lead, 236 
 Selenium, 121 
 
 and seleniurets, 185 
 
 detection of, 97 
 Seleniuret of copper, 237 
 and lead, 237 
 
 of silver and copper, 237 
 Senarmontite, 256 
 Separation of As, Sb, Sn, 194 
 Sepiolite, 290, 292 
 Serpentine, 296, 318, 319, 320 
 Sesquicarbonate of sodium, 1277 
 Sesquioxide of chromium, 157 
 Seybertite, 307 
 Siderite, 270, 310, 311, ;;l:3 
 Sideroschisolite, 272 
 Siegenite, 246 
 Silica, 185, 186 
 Silicate of bismuth, 276 
 Silicates, fusing, 203, 204 
 
 reaction of, 277 
 Silicic compounds, 126 
 
 oxide 96 
 Silicium, 185, 186 
 
 Silicon, 185, 186 
 Sillirnanite, 308 
 Silver, 186-188 
 
 and copper, seleniuret of, 237 
 sulphuret of, 244 
 
 and iron, sulphuret of, 247 
 
 antimonial, 241 
 
 compounds, 123 
 
 iodide of, 166 
 
 native, 230 
 
 ore, ruby, 242 
 
 ores, 258, 259, 361-365 
 
 sulphuret of, 243 
 Silverglance, 243 
 Simonyite, 278 
 Siphon, 42 
 Skutterudite, 233 
 Smaltite, 233, 234 
 Smithsonite, 309 
 Soapstone, 321 
 Soda, action of, on chromium, 157 
 
 examination of minerals with, 
 96-98 
 
 nitre. 277 
 Sodalite/288 
 Sodic phosphate, 68 
 Sodium, 188 
 
 biborate of, 279 
 
 carbonate, 277 
 
 chloride of, 279 
 
 flame, spectrum of, 129 
 
 nitrate of, 277 
 
 phosphate of, 175 
 
 spectrum lines of, 133 
 
 sulphates of, 278 
 
 testing, 109 
 
 thiosulphate, behavior of oxides 
 
 with, 99 
 
 examinations of metals 
 : with, 98, 99 
 
 Solar and stellar chemistry, 134-137 
 the foundations of, laid 
 by Bunsen and Kirch- 
 hoff, 134 
 Solubility, absolute, 220 
 
 degrees of, 220 
 
 Solution and carbonic dioxide test 
 40,41 
 
 and solvents, 220 
 
 chemical, 220 
 Sordawalite, 292, 297 
 Spaerite, 304 
 Spaniolite, 242 
 Spark spectra, 131 
 Spars, 310, 311 
 Spathic iron, 270 
 a holder, 46 
 
 platinum, 45, 46 
 
392 
 
 INDEX. 
 
 Special methods for detecting cer- 
 tain elements, or some of their 
 combinations when present in 
 complex chemical compounds, 
 139-202 
 
 Species, mineral, for the study of de- 
 terminative mineralogy, 222, 223 
 Specific gravity, determination of, 
 
 211-216 
 Spectra of different flames, 129 
 
 of the flames of different salts, 
 
 129 
 
 of the moon and planets, 134 
 of permanent gases, 131, 132 
 spark, 131 
 
 Spectroscope, 137-139 
 Spectrum, 128 
 
 absorption, 163 
 analysis, 127-139 
 
 advantages of, 129, 130 
 Bunsen and Kirchhoff re- 
 searches in, 127, 134 
 flame reactions, and colored 
 
 flames, 103-139 
 principles of, 127-131 
 bright lines of the, 129 
 colors of the, 128 
 continuous, 128, 163 
 lines of the most important 
 
 flame coloring elements, 133 
 measuring the. 138, 139 
 Specular iron, 249, 252, 313 
 Spessartite, 294 . 
 Sphalerite, 253, 313 
 Sphenoclase, 302 
 Spinel, 308, 327 
 Spodumene, 296, 297 
 Spoons, platinum, 87 
 Spring balance, 214-216 
 Staffelite, 280 
 Stannic acid, 193 
 
 oxide, 193 
 Stannine, 244, 246 
 Stannous chloride, 115, 178 
 
 salts, 193 
 Star, Aldebaran, constituents of, 
 
 137 
 Stars, atmosphere of the, 134, 137 
 
 the spectra of the, 137 
 Stassfurthite, 284 
 Staurotite, 326 
 Stearine candles, 78 
 Stellar and solar chemistry, 134-137 
 Stephanite, 241 
 Sternbergite, 247 
 Stibnite,'240 
 Stilbite, 291, 292 
 Stolzite, 262 
 
 Strassfurtite, 281 
 Streak of a mineral, 211 
 Stroganowite, 293 
 Stromeyerite, 244, 246 
 Strontia, 150 
 Strontianite, 280, 310 
 Strontium, 189 
 
 examination of, 110 
 flame, spectrum of, 129 
 spectrum lines of, 133 
 sulphate of, 281 
 Struvite, 283 
 Stylotypite, 241 
 Substitution, discovery of, by 
 
 Dumas, 26 
 
 theory of chemistry, 25-38 
 Sulphate of barium, 281 
 of baryta, 150 
 of magnesium, 278 
 of potassium, calcium, and 
 
 magnesium, 280 
 of strontium, 281 
 
 separation of, from sul- 
 phate of calcium, 174 
 Sulphates of barium, strontium, and 
 calcium, fusing with carbon- 
 ate of potassium or sodium, 
 174 
 
 of calcium, 280 
 of potassium, 278 
 of sodium, 278 
 of the alkaline earths, analysis 
 
 of, 203 
 
 Sulphide, hydric, 64-66 
 incrustations, 120 
 of ammonium, 66 
 
 action of, on ferric salts, 
 
 168 
 
 on manganous salts, 176 
 Sulphides containing tin, 192 
 
 of arsenic and antimony, 142 
 of lead and antimony, treat- 
 ment of, 142 
 Sulphur, 189-191 
 acids, 29, 30 
 compounds. 127 
 detection of, 97 
 dioxide, detection of, 100 
 native, 256 
 
 Sulphuret of antimony, 240 
 and lead, 240 
 and silver, 242 
 of bismuth, 248 
 of copper and antimony, 242 
 of iron and nickel, 245 
 of lead, 244 
 of silver, 231, 243 
 and iron. 247 
 
INDEX. 
 
 393 
 
 Sulplmrct of tin, 244 
 Sulphuretted hydrogen, ()4-(i(; 
 Sulphuric acid, 68 
 
 concentrated, examination 
 with, 99-101 
 
 testing-, 108 
 Sulphydric acid, action on manga- 
 
 nous salt, 176 
 Supports for crucibles, 51-53 
 
 for the assay, 75-78 
 Susannite, 263 
 Sussexite, 269, 284., 311 
 Svanbergite, 306 
 Sylvanite, 239 
 Syngenite, 281 
 
 Table of atomic weights of elements 
 according to the new system, 
 36-38 
 
 of volatile elements which can 
 be reduced 'as films or coat- 
 ings on porcelain, arranged 
 according to their reactions, 
 121 
 Tables of minerals, introduction to, 
 
 207 
 
 Tabular arrangement showing the 
 behavior of oxides when treated 
 before the blowpipe, with sodium 
 thiosulphate, together with their 
 reactions with borax. 99 
 Tachhydrite, 278 
 Tachylite, 289, 292 
 Tagilite, 267 
 Talc, 321 
 Tallingite, 265 
 Tantalite, 255 
 Tantalum, 191 
 
 compounds, 125 
 pentoxide, 97 
 Tavistockite, 304 
 Telluret of bismuth, 239 
 
 of gold and lead, 239 
 Tellurium, 121, 191, 192 
 
 compounds, detection of, 97 
 
 native, 238 
 
 ores of, division of, into groups, 
 
 238 
 Test, carbonic dioxide, 40 
 
 for arsenic in minerals contain- 
 ing no sulphur, 148-150 
 operations, 116 
 papers, preparation of, 63 
 substances, apparatus, and me- 
 thod employed for submit- 
 ting, to the flame, 112-114 
 Test-tube holder, 41 
 Test-tubes and racks, 40, 41 
 
 Testing and classifying minerals, 
 preliminary proceedings for, 
 219 
 
 chemical mixtures, 107-111 
 for water, 220, 221 
 of water, 62, 63 
 Tetradymite, 239 
 Tetrahedrite, 241,246 
 Thallium, 121 
 
 discovery of, 130 
 spectrum lines of, 133 
 Thenardite, 278 
 Theories of chemistry, 25-38 
 Thermometers, scales of, relations 
 
 of, 224-226 
 Thermonatrite, 277 
 Thermophyllite, 296 
 Thomsenolite, 282 
 Thorite, 317 
 Thraulite, 318 
 j Thuringite, 272 
 i Tiemannite, 236 
 : Tin, 192-1 94 
 
 and copper, separation of, 193 
 
 compounds, 124 
 
 dissolving of, 192 
 
 from antimony, separation of, 
 
 194 
 from bismuth, separation of, 
 
 193 
 
 ores of, 366, 367 
 pyrites, 244 
 recognition of, 116 
 Tinkal, 285 
 Tinstone, 324 
 Titanic acid, 324 
 
 native, 195 
 iron, 253 
 Titanite, 300 
 Titanium, 195 
 
 dioxide, 96, 97 
 
 detection of, 101 
 compounds, 125 
 treatment of, 195 
 ! Tongs, crucible, 49, 50 
 Topaz, 308, 327 
 Torbernite, 267 
 Tourmaline, 275, 298 
 Tremolite, 299, 300 
 Tridymite, 326 
 | Triphylite, 271 
 Triplite, 270, 271 
 Tripods, 47 
 Tio<rerite, 283 
 Troll eite, 304 
 Trona, 277 
 i Tscheff kinite, 293 
 i Tschermigite, 2.s:5 
 
394 
 
 INDEX. 
 
 Tubes, bending- and closing glass, 
 56-58 
 
 closed, 88, 89 
 
 of hard glass free from lead, 88 
 
 of thin glass, 114 
 Tungstate of calcium, 295, 324 
 
 of iron and manganese, 249 
 Tungstates, 196 
 Tungsten, 195-197 
 
 characteristics of, 195, 196 
 
 compounds, 125 
 
 dichloride, 197 
 
 hexachloride, 197 
 
 pentachloride, 197 
 
 tetrachloride, 197 
 
 treatment of, 196 
 
 with chlorine, 197 
 
 trioxide, 96, 97 
 
 detection of, 101 
 Tungstic acid, 196, 323 
 Tungstite, 323 . 
 Turgite, 313 
 
 Turmeric paper, preparation of, 63 
 Turquois, 314 
 Tyrolite, 264 
 
 Ulexite, 279 
 
 Ullmaunite, 243 
 
 Ultramarine, 288 
 
 Unitary system of chemistry, 25-38 
 
 Uranates, 199 
 
 Uranic nitrate, 198 
 
 sulphate, 198 
 
 trioxide, 198 
 Uranium, 197-199 
 
 atomic weight of, 198 
 
 behavior of, with different sul- 
 phides, 198, 199 
 
 compounds, 126 
 
 recognition of, 116 
 
 tetrachloride, 198 
 Uranus chloride, 198 
 
 dioxide, 198 
 Urinite, 255, 286, 314 
 Uwarowite, 327 
 
 Valence, 33, 35 
 
 varying in the same element, 34 
 Valentinite, 256 
 Vanadinite, 262 
 Vanadium, 199, 200 
 
 characteristics of, 199, 200 
 
 compounds, 125 
 
 pentoxide, 97 
 
 detection of, 101 
 
 recognition of, 116 
 Varying valence in the same ele- 
 ment, 34 
 
 Vauquclinite, 262, 263 
 Vermiculite, 291 
 Vesuvianite, 301 
 
 Violet rays, refrangibility of. 129 
 Vitriol, blue, 265 
 
 iron, 269 
 Vivianite, 271 
 Voigtite, 273 
 Volatile acids, detection of, 99-101 
 
 elements which can be reduced 
 as films or coatings on porce- 
 lain, 121 
 
 Volatility, determination of, 117 
 Volborthite, 267 
 Voltaite, 270 
 
 Wad, 314 
 
 Wagnerite, 285 
 
 Walpurgite, 283 
 
 Warvvickite, 323 
 
 Wash-bottle for precipitates, 45 
 
 Washing precipitates, 45, 46 
 
 Watch-glasses, 89 
 
 Water, 67 
 
 Water-bath, 46, 47 
 
 Water, chemically pure, 59-62 
 
 determination of, 220, 221 
 
 testing of, 62, 63 
 Wavel lite, 304 
 
 Weights and measures, 223-226 
 Wernerite, 293 
 Westanite, 307 
 
 Wet reagents generally, 67-69 
 Whitneyite, 233 
 
 test for, 148 
 Willemite, 306, 309 
 Wilsonite, 297 
 Wire gauze, 51 
 
 platinum, 87 
 Witherite, 280 
 Wittichite, 244, 245, 246 
 Wbhlerite, 293 
 
 Wolchonskoite, 317, 318, 323 
 Wolfachite, 235 
 Wolfram, 249, 275 
 
 decomposition of, 197 
 Wolframite, 249, 275 
 Wolframium, 19.5-197 
 
 compounds, 125 
 Wollastonite, 288, 302 
 Wulfenite, 262 
 
 Xanthoconite, 258, 59 
 Xanthophyllite, 305 
 Xenotime, 325 
 Xonaltite, 290, 317 
 Xylotile, 274, 318 
 
INDEX. 
 
 395 
 
 Yttria, reactions of, 200, 201 
 Yttrium, 200, 201 
 
 phosphate of, 325 
 Yttrocerite, 311, 316 
 Yttrotantalite, 200 
 Yttrotitanite, 300 
 
 Zaratite, 312 
 Zepharovichite, 304 
 Zinc, 121, 201 
 
 and hydrochloric acid, exami- 
 nation with, 101 
 behavior of, with different sub- 
 stances, 201 
 ores, 314, 367, 368 
 silicate of, 306 
 
 Zinc spinel, 327 
 
 sulphate of, 28o 
 
 sulphurets of, 313 
 
 vitriol, 309 
 
 Zincblende, 253, 309, 313 
 Zincite, 314 
 Zinkenite, 240, 241 
 Zippeite, 314 
 j Zirconia, 202 
 
 behavior of, with different sub- 
 stances, 202 
 Zirconite, 326 
 
 Zirconium salts, reactions of, 202 
 Zircons, 202 
 Zoisite, 301 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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HENRY CAREY BAIRD & OX'S CATALOGUE. 
 
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HENRY CARE* bAi*o> b: CO .o CATALOGUE,. n 
 
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ra HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 13 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 15 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 17 
 
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i8 HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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HENRY CAREY BAIRD & CO."S CATALOGUE. 19 
 
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xo HENRY CAREY BA1RD CO.'S CATALOGUE 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 21 
 
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22 HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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HENRY CAREY BA1RD & CO.'S CATALOGUE. 3 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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HENRY CAREY LAIRD & CO.'S CATALOGUE. 25 
 
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26 HENRY CAREY BAIRo & CO.'S CATALOGUE. 
 
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HENRV CAREY BAIRB & CO.'S CATALOGUE. 
 
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38 HENRY CAREY BAIRD & CO.'S CATALOGUE., 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE. 29 
 
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HENRY CAREY BAIRD & CO.'S CATALOGUE, 31 
 
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32 HENRY CAREY BAIRD & CO.'S CATALOGUE. 
 
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