Preview langes handbook of chemistry, seventeenth edition by james speight (2016)

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LANGE'S HANDBOOK OF CHEMISTRY

LANGE'S

HANDBOOK OF CHEMISTRY

1976, no part ofthis publication may be reproduced or distributed in any form or by any means, or stored in a database or retrieval system, without the prior written permission of the publisher

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TERMSOFUSE

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THE WORK IS PROVIDED "AS IS." McGRAW-HILL EDUCATION AND ITS LICENSORS MAKE NO GUARANTEES

OR WARRANTIES AS TO THE ACCURACY, ADEQUACY OR COMPLETENESS OF OR RESULTS TO BE OBTAINED FROM USING THE WORK, INCLUDING ANY INFORMATION THAT CAN BE ACCESSED THROUGH THE WORK VIA HYPERLINK OR OTHERWISE, AND EXPRESSLY DISCLAIM ANY WARRANTY, EXPRESS OR IMPLIED, INCLUD-ING BUT NOT LIMITED TO IMPLIED WARRANTIES OF MERCHANTABILITY OR FITNESS FOR A PARTICULAR PURPOSE McGraw-Hill Education and its licensors do not warrant or guarantee that the functions contained in the work will

meet your requirements or that its operation will be uninterrupted or error free Neither McGraw-Hill Education nor its licensors shall be liable to you or anyone else for any inaccuracy, error or omission, regardless of cause, in the work or for any damages resulting therefrom McGraw-Hill Education has no responsibility for the content of any information accessed through the work Under no circumstances shall McGraw-Hill Education and/or its licensors be liable for any indirect, incidental, special, punitive, consequential or similar damages that result from the use of or inability to use the work, even if any of them has been advised of the possibility of such damages This limitation of liability shall apply to any claim or cause whatsoever whether such claim or cause arises in contract, tort or otherwise

Dr James G Speight, CChem FRSC, FCIC, FACS, earned his B.Sc and Ph.D degrees (in chemistry) from the University of Manchester, England He also holds

a D.Sc (in geological sciences) from VINIGRI, St Petersburg, Russia, and a Ph.D (in petroleum engineering) from Dubna International University, Moscow, Russia

Dr Speight has more than 45 years of experience in areas associated with (1) the properties, recovery, and refining of reservoir :fluids, conventional petro-leum, heavy oil and tar sands bitumen; (2) the properties and refining of natural gas and gaseous fuels; and (3) the properties and refining of biomass, biofuels, and biogas, and the generation of bioenergy His work has also focused on safety issues, environmental effects, and remediation associated with the production and use of fuels and biofuels Dr Speight is the author of more than 65 books

on petroleum science, petroleum engineering, biomass and biofuels, and ronmental sciences

envi-He was elected to the Russian Academy of Sciences in 1996 and awarded the Gold Medal of Honor that same year for outstanding contributions to the field of petroleum sciences Dr Speight has also received the Scientists without Borders Medal of Honor from the Russian Academy of Sciences In 2001, the Academy awarded him the Einstein Medal for outstanding contributions and service in the field of geological sciences

CONTENTS

For the detailed contents of any section, consult the first page of that section See also the alphabetical index in the back of this Handbook

Preface to the Seventeenth Edition ix

Preface to the Sixteenth Edition xi

Preface to the First Edition x111

Section 1 Inorganic Chemistry

Section 2 Organic Chemistry

Section 3 Naturally Occurring Chemicals and Chemical Sources

PREFACE TO THE SEVENTEENTH EDITION

lbis new edition continues the tradition of previous editions by being a one-volume source of tual information for professional chemists, technicians, and students The aim of Lange's Handbook

fac-of Chemistry is to provide sufficient data to satisfy the general needs of those working in the field of chemistry without their having to consult a multitude of scattered and diverse reference sources The book is divided into three main sections on inorganic chemistry, organic chemistry, and naturally occurring chemicals and chemical sources

Section 1, Inorganic Chemistry, contains information relevant to the properties and behavior of elements and compounds The data for each element and compound include (where available) name, naturally occurring isotopes, structural formula, formula weight, density, refractive index, melting point, and solubility in water

Section 2, Organic Chemistry, contains the descriptive properties of approximately 5000 organic compounds Entries are listed alphabetically to the extent possible, and the data for each compound include (where available) name, structural formula, formula weight, density, refractive index, melt-ing point, boiling point, flash point, and solubility in water and various common organic solvents Alternative names, as well as trivial names of long-standing usage, are listed as well

Section 3, Naturally Occurring Chemicals and Chemical Sources, is new, and offers the reader details of the behavior and properties of the various fossil fuels (coal, crude oil, natural gas, tar sands, and oil shale) as well as details of the behavior and properties of biomass, biofuels, and minerals 1\vo additional sections filled with useful information are available online at www.mhprofessional com!Langes The first, Spectroscopy, includes ultraviolet-visible spectroscopy, fluorescence, infra-red and Raman spectroscopy, and X-ray spectrometry Detection limits are listed for the elements when using flame emission, flame atomic absorption, electrothermal atomic absorption, argon induction-coupled plasma, and flame atomic fluorescence Nuclear magnetic resonance embraces tables for the nuclear properties of the elements, proton chemical shifts and coupling constants, and

The second section, General Information and Conversion Tables, contains the general information and conversion tables required by the chemist

Working professionals will find this Handbook appropriate for their needs It is oriented toward scientists, engineers, or technologists who are employed by consultants, public works agencies, industry, regulatory agencies, universities, or equipment manufacturers, as well as planners, corpo-rate managers, architects, elected officials, lawyers, students, or others seeking insight into the properties and behavior of chemicals

It is hoped that users of this Handbook will continue to offer suggestions of material that might

be included in, or even excluded from, future editions and call attention to errors Such tions should be directed to the editor either directly or through the publisher, McGraw-Hill Education

communica-Dr James G Speight Laramie, "Yoming JamesSp8@aol.com

ix

PREFACE TO THE SIXTEENTH EDITION

This Sixteenth Edition of Lange's Handbook of Chemistry takes on a new format under a new editor

Nevertheless, the Handbook remains the one-volume source of factual information for chemists and chemical engineers, both professionals and students The aim of the Handbook remains to provide sufficient data to satisfy the general needs of the user without recourse to other reference sources The many tables of numerical data that have been compiled, as well as additional tables, will provide the user with a valuable time-saver

The new format involves division of the Handbook into four major sections, instead of the

11 sections that were part of previous editions Section 1, Inorganic Chemistry, contains a group of tables relating to the physical properties of the elements (including recently discovered elements) and several thousand compounds Likewise, Sec 2, Organic Chemistry, contains a group of tables relat- ing to the physical properties of the elements and several thousand compounds Following these two sections, Sec 3, Spectroscopy, presents the user with the fundamentals of the various spectroscopic techniques This section also contains tables that are relevant to the spectroscopic properties of elements, inorganic compounds, and organic compounds Section 4, General Information and Conversion Tables, contains all of the general information and conversion tables that were previously found in different sections of the Handbook

In Sees 1 and 2, the data for each compound include (where available) name, structural formula, formula weight, density, refractive index, melting point, boiling point, flash point, dielectric constant, dipole moment, solubility (if known) in water and relevant organic solvents, thermal conductivity, and electrical conductivity The presentation of alternative names, as well

as trivial names of long-standing use, has been retained Section 2 also contains expanded mation relating to the names and properties of condensed polynuclear aromatic compounds Enthalpies and Gibbs Energies of Formation, Entropies, and Heat Capacities of Organic and Inorganic Compounds, and Heats of Melting, Vaporization and Sublimation and Specific Heat at Various Temperatures, are also presented in Sees 1 and 2 for organic and inorganic compounds, as well as information on the critical properties (critical temperature, critical pressure, and critical volume)

infor-AB in the previous edition, Sec 3, Spectroscopy, retains subsections on infrared spectroscopy, Raman spectroscopy, fluorescence spectroscopy, mass spectrometry, and X-ray spectrometry The section on practical laboratory information (now Sec 4) has been retained as it offers valuable infor- mation and procedures for laboratory methods

AB stated in the prefaces of earlier editions, every effort has been made to select the most useful and reliable information and to record it with accuracy It is hoped that users of this Handbook will continue to offer suggestions of material that might be included in, or even excluded from, future editions and call attention to errors These communications should be directed to the editor through the publisher, McGraw-Hill

Dr James G Speight U:lramie, "Yoming

xi

PREFACE TO THE FIRST EDITION

This book is the result of a number of years' experience in the compiling and editing of data useful

to chemists In it an effort has been made to select material to meet the needs of chemists who cannot command the unlimited time available to the research specialist, or who lack the facilities of a large technical library which so often is not conveniently located at many manufacturing centers If the information contained herein serves this purpose, the compiler will feel that he has accomplished a worthy task Even the worker with the facilities of a comprehensive library may find this volume of value as a time-saver because of the many tables of numerical data which have been especially com-puted for this purpose

Every effort has been made to select the most reliable information and to record it with accuracy Many years of occupation with this type of work bring a realization of the opportunities for the occurrence of errors, and while every endeavor has been made to prevent them, yet it would be remarkable if the attempts towards this end had always been successful In this connection it is desired to express appreciation to those who in the past have called attention to errors, and it will be appreciated if this be done again with the present compilation for the publishers have given their assurance that no expense will be spared in making the necessary changes in subsequent printings

It has been aimed to produce a compilation complete within the limits set by the economy of available space One difficulty always at hand to the compiler of such a book is that he must decide what data are to be excluded in order to keep the volume from becoming nnwieldy because of its size He can hardly be expected to have an expert's knowledge of all branches of the science nor the intuition necessary to decide in all cases which particular value to record, especially when many differing values are given in the literature for the same constant If the expert in a particular field will judge the usefulness of this book by the data which it supplies to him from fields other than his specialty and not by the lack of highly specialized information in which only he and his co-workers are interested (and with which he is familiar and for which he would never have occa-sion to consult this compilation), then an estimate of its value to him will be apparent However,

if such specialists will call attention to missing data with which they are familiar and which they believe others less specialized will also need, then works of this type can be improved in succeed-ing editions

Many of the gaps in this volume are caused by the lack of such information in the literature It is hoped that to one of the most important classes of workers in chemistry, namely the teachers, the book will be of value not only as an aid in answering the most varied questions with which they are confronted by interested students, but also as an inspiration through what it suggests by the gaps and inconsistencies, challenging as they do the incentive to engage in the creative and experimental work necessary to supply the missing information

While the principal value of the book is for the professional chemist or student of chemistry,

it should also be of value to many people not especially educated as chemists Workers in the natural sciences physicists, mineralogists, biologists, pharmacists, engineers, patent attorneys, and librarians are often called upon to solve problems dealing with the properties of chemical products or materials of construction For such needs this compilation supplies helpful information and will serve not only as an economical substitute for the costly accumulation of a large library of monographs on specialized subjects, but also as a means of conserving the time required to search

xiii

for information so widely scattered throughout the literature For this reason especial care has been taken in compiling a comprehensive index and in furnishing cross references with many of the tables

It is hoped that this book will be of the same usefulness to the worker in science as is the

diction-ary to the worker in literature, and that its resting place will be on the desk rather than on the bookshelf

N.A Lange Cleveland, Ohio May2, 1934

LANGE'S HANDBOOK OF CHEMISTRY

1.1.8 Salts and Funetional Derivatives of Acids

Tabla 1.1 Trivial Names for Acids

1.1.7 Coordination Compounds

1.1.8 Addition Compounds

1.1.9 Synonyms and Mineral Names

Table 1.2 Synonyms and Mineral Names

1.1.10 Classification of Inorganic Substances

1.2 PHYSICAL PROPERTIES OF INORGANIC COMPOUNDS

1.2.1 Density

1.2.2 Malting Point (Freezing Temperature)

1.2.3 Boiling Point

1.2.4 Rafraetiva Index

Table 1.3 Physical Constants of Inorganic Compounds

Tabla 1.4 Color, Crystal Symmetry, and Refractive Index of

Inorganic Compounds Table 1.5 Refractive Index of Minerals

Tabla Ui Properties of Molten Salts

Table 1.7 Triple Points ofVarious Materials

Tabla 1.8 Density of Mercury and Water

Tabla 1.9 Specific Gravity of Air at Various Temperatures

Table 1.10 Boiling Points of Water

Tabla 1.11 Boiling Points ofWatar

Table 1.12 Refractive Index, Viscosity, Dielectric Constant, and

SurfacaTansion ofWater atVariousTamparaturas Tabla 1.13 Compressibility of Water

Table 1.14 Flammability Limits of Inorganic Compounds in Air

Tabla 1.15 Cyanide Compounds (Inorganic)

Table 1.16 Subdivision of Main Energy Levels

Tabla 1.17 Chemical Symbols, Atomic Numbers, and Eleetron

Arrangements of the Elements Table 1.18 Atomic Numbers, Periods, and Groups of the Elements

(The Periodic Table) Table 1.19 Atomic Weights of the Elements

Tabla 1.20 Physical Properties of the Elements

Tabla 1.21 Conductivity and Resistivity of the Elements

Table 1.22 Work Functions of the Elements

Tabla 1.23 Relative Abundances of Naturally Occurring Isotopes

Table 1.24 Radioactivity of the Elements (Neptunium Series)

Tabla 1.25 Radioactivity of the Elements (Thorium Series)

Table 1.26 Radioactivity of the Elements (Actinium Series)

Table 1.27 Radioactivity of the Elements (Uranium Series) 149 Tabla 1.28 Electronic Configuration of the Elements 150

Tabla 1.30 Ionization Energy of Molecular and Radical Species 157

Tabla1.31 ElectronagativityValues of the Elements 161

Tabla1.32 Electron Affinities of Elements, Molecules, and Radicals 162

Tabla 1.41 Dipole Moments and Dielectric Constants 189

Table 1.42 Spatial Orientation of Common Hybrid Bonds 191

Table 1.46 Vapor Pressures of Selected Elements at DifferentTemperatures 217 Table 1.47 Vapor Pressures of Inorganic Compounds up to 1 Atmosphere 219 Tabla 1.48 Vapor Pressures of Various Inorganic Compounds 228

Tabla 1.50 Vapor Pressure of lea in Millimeters of Mercury 238 Table 1.51 Vapor Pressure of Liquid Ammonia, NH3 239

Tabla 1.54 Viscosity and Surface Tension of Inorganic Substances 242

Tabla 1.56 Thermal Conductivity of Various Solids 248

Table 1.58 Enthalpies and Gibbs Energies of Formation, Entropies, and

Heat Capacities of the Elements and Inorganic Compounds 253 Table 1.59 Heats of Fusion, Vaporization, and Sublimation and

Specific Heat at Various Temperatures of the Elements and

Tabla 1.60 Individual Activity Coefficients of Ions in Water at 25•c 316

Table 1.61 Constants of the Debye-Hi.ickel Equation from 0 to 1oo-c 316 Tabla 1.82 Individual Ionic Activity Coefficients at Higher Ionic Strengths

1.17.1 Standards for pH Measurement of Blood and Biological Madia 317

Table 1.63 National Bureau of Standards (U.S.) Reference pH

Table 1.64 Compositions of Standard pH Buffer Solutions

Tabla 1.65 Composition and pH Values of Butler Solutions 8.107 320 Table 1.66 Standard Reference Values pH for the Measurement

of Acidity in 50 Weight Percent Methanol-Water 322 Table 1.67 pH Values for Buffer Solutions in Alcohol-Water Solvents

Table 1.68 pH Values of Biological and Other Buffers for Control Purposes 324

Table 1.70 Solubility of Inorganic Compounds and Metal Salts of

Organic Acids in Water at Various Temperatures 332 Table 1.71 Dissociation Constants of Inorganic Acids 346

Tabla 1.77 Cumulative Formation Constants for Metal Complexes

Table 1.78 Cumulative Formation Constants for Metal Complexes with

Tabla 1.85 Potentials of Reference Electrodes (in Volts) at 25•c for

Tabla 1.87 Limiting Equivalent Ionic Conductances in Aqueous Solutions 423 Table 1.88 Standard Solutions for Calibrating Conductivity Vessels 426 Tabla 1.89 Equivalent Conductivities of Electrolytes in Aqueous Solutions

Tabla 1.90 Conductivity ofVery Pure Water at Various Temperatures and the

Equivalent Conductances of Hydrogen and Hydroxyl Ions 432

1.1 NOMENCLATURE OF INORGANIC COMPOUNDS

The following synopsis of rules for naming inorganic compounds and the examples given in tion are not intended to cover all the possible cases

explana-Generally, there are two types of inorganic compounds that can be formed: ionic compounds and molecular compounds

Compounds consisting of a metal and nonmetal are commonly known as ionic compounds, where the compound name has an ending of -ide Cations have positive charges while anions have negative charges The net charge of any ionic compound must be zero, which also means it must be electri-cally neutral For example, one Na+ is paired with one cr, and one Ca2+ is paired with two Br- The rules of nomenclature state that (1) the cation (metal) is always named first with its name unchanged, and (2) the anion (nonmetal) is written after the cation, modified to end in -ide

The transition metals may form more than one ion, thus it is needs to be specified which lar ion we are talking about This is indicated by assigning a Roman numeral after the metal, which denotes the charge and the oxidation state of the transition metal ion For example, iron can form two common ions: Fe2+ and Fe3+ To distinguish between the two, Fe2+ is named iron (II) and F~ is named iron (Ill)

particu-However, some of the charges on transition metals have specific Latin names Just like the other nomenclature rules, the ion of the transition metal that has the lower charge has the Latin name ending with -ous and the one with the higher charge has a Latin name ending with -ic

Several exceptions apply to the Roman numeral assignment: aluminum, zinc, and silver Although they belong to the transition metal category, these metals do not have Roman numerals written after their names because these metals only exist in one ion Instead of using Roman numerals, the differ-ent ions can also be presented in plain words The metal is changed to end in -ous or -ic

Although HF can be named hydrogen fluoride, it is given a different name for emphasis that it is an acid-a substance that dissociates into hydrogen ions (H') and anions in water A quick way to identify acids is to see if there is an H (denoting hydrogen) in front of the molecular formula of the compound

To name acids, the prefix hydro- is placed in front of the nonmetal modified to end with -ic The state

of acids is aqueous (aq) because acids are found in water Some common binary acids include:

HF (g) (hydrogen fluoride)~ HF (aq) (hydrofluoric acid) HBr (g) (hydrogen bromide)~ HBr (aq) (hydrobromic acid) HCl (g) (hydrogen chloride)~ HCl (aq) (hydrochloric acid)

H2S (g) (hydrogen sulfide)~ H2S (aq) (hydrosulfuric acid) Polyatomic ions (meaning two or more atoms) are joined together by covalent bonds Although there may be an element with positive charge like W, it is not joined with another element with an ionic bond This occurs because if the atoms formed an ionic bond, then it would have already become a compound, thus not needing to gain or lose any electrons Polyatomic anions have negative charges while polyatomic cations have positive charges To correctly specify how many oxygen atoms are in the ion, prefixes and suffixes are used

Cations and AniODB

+1 Charge Hydrogen: W

Calcium: Ca2+

Strontium: s~

Barium: Ba2+

-1 Charge Hydride: I r Fluoride: p-Chloride: a-Bromide: Br-Iodide: :r-

-2Charge -3 Charge -4Charge Oxide: o~ Nitride: N~ Carbide: C""" Sulfide: S2- Phosphide: p>-

Transition Metals and Metal Cations

+1 Charge Copper(I): eu+

Silver: Ag+

1.1.1 Writing Fonnulas

+2Charge Copper(ll): Cu2+

cor cia-

ClOi Cl03 Cl04

CIOt

CrzDt

c~

011 NOi N03

CzOt

Mn04 POt

sor sot sCN-

szor

+4Charge

Lead(IV): Pb4+

Tin(IV): Sn4+

1.1.1.1 Mass Number, Atomic Number, Number of Atoms, and Ionic Charge The mass

number, atomic number, nwnber of atoms, and ionic charge of an element are indicated by means of four indices placed around the symbol:

mass number atomic number SYMBOL ionic charge

number of atoms

Ionic charge should be indicated by an Arabic supei8Cript numeral preceding the plus or minus sign: Mg2+, POl-

1.1.1.2 Pllleement of Aloms in a Fonnu/4 The electropositive constituent (cation) is placed first

in a formula If the compound contains more than one electropositive or more than one tive constituent, the sequence within each class should be in alphabetical order of their symbols The alphabetical order may be different in formulas and names; for example, NaNH,.HP04, ammonium sodium hydrogen phosphate

electronega-Acids are treated as hydrogen salts Hydrogen is cited last among the cations

When there are several types of ligands, anionic ligands are cited before the neutral ligands

1.1.1.3 Binary Compounds between NonmetlJls For binary compounds between nonmetals, that constituent should be placed first which appears earlier in the sequence:

Rn, Xe, Kr, Ar, Ne, He, B, Si, C, Sb, AB, P, N, H, Te, Se, S, At, I, Br, Cl, 0, F Examples: ABC13, SbH3, H3 Te, BrF3, OF2, and N4S4•

1.1.1.4 Chain Compounds For chain compounds containing three or more elements, the sequence should be in accordance with the order in which the atoms are actually bound in the mole-cule orion

Examples: SCW (thiocyanate), HSCN (hydrogen thiocyanate or thiocyanic acid), HNCO (hydrogen

isocyanate), HONC (hydrogen fulminate), and HPH202 (hydrogen phosphinate)

1.1.1.5 Use of Centered Period A centered period is used to denote water of hydration, other solvates, and addition compounds; for example, CuS04 · 5H20, copper(II) sulfate 5-water (or pentahydrate)

1.1.1.6 Free Rtulicals In the formula of a polyatomic radical an unpaired electron(s) is (are) indicated by a dot placed as a right superscript to the parentheses (or square bracket for coordination compounds) In radical ions the dot precedes the charge In structural formulas, the dot may be placed to indicate the location of the unpaired electron(s)

Examples: S2Cl2, S8, N204, and ~206; not SCI, S, N02, and H;zP03•

1.1.1.9 Structurtd Formula and Prefixes In the structural formula the sequence and spatial arrangement of the atoms in a molecule are indicated

Examples: NaO(O=C)H (sodium formate), Cl -S S -Cl (disulfur dichloride)

Structural prefixes should be italicized and connected with the chemical formula by a hyphen: cis-,

trans-, anti-, syn-, cyclo-, catena-, o-or ortho-, m-or meta-, p-or para-, sec-(secondary),

tert-(tertiary), v-(vicinal), meso-, as-for asymmetrical, and s-for symmetrical

The sign of optical rotation is placed in parentheses, (+)for dextrorotary,(-) for levorotary, and (±) for racemic, and placed before the formula The wavelength (in nanometers is indicated by a right subscript; unless indicated otherwise, it refers to the sodium D-line

The italicized symbols d-(for deuterium) and t-(for tritium) are placed after the formula and nected to it by a hyphen The number of deuterium or tritium atoms is indicated by a subscript to the symbol

con-Examples:

1.1.2 Naming Compounds

cis-[PtCl2(NH3)i]

di-tert-butyl sulfate methan-ol-d

methan-~-ol (+)ss9 [Co(en)3]Cl2

Table 1.3 Wolfram is preferred to tungsten but the latter is used in the United States In forming a complete name of a compound, the name of the electropositive constituent is left unmodified except when it is necessary to indicate the valency (see oxidation number and charge number, formerly the Stock and Ewens-Bassett systems) The order of citation follows the alphabetic listing of the names

of the cations followed by the alphabetical listing of the anions and ligands The alphabetical citation

is maintained regardless of the number of each ligand

obtained from the element name with its ending (-en, -ese, -ic, -ine, -ium, -ogen -on, -oru.s, -urn, -ur, -y, or -ygen) replaced by -ide The elements bismuth, cobalt, nickel, zinc, and the noble gases are used unchanged with the ending -ide Homopolyatomic ligands will carry the appropriate prefix A few Latin names are used with affixes: cupr- (copper), aur- (gold), ferr- (iron), plumb- (lead), argent-(silver), and stann- (tin)

For binary compounds, the name of the element standing later in the sequence in Sec 1.1.1.3 is modified to end in -ide Elements other than those in the sequence of Sec 1.1.1.3 are taken in the reverse order of the following sequence, and the name of the element occurring last is modified to end in -ide; e.g., calcium stannide

ELEMENT SEQUENCE

1.1.2.3 Stoichiometric Proportions The stoichiometric proportions of the constituents in a formula may be denoted by Greek numerical prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, acta-, nona- (Latin), deca-, undeca- (Latin), dodeca-, , icosa- (20), henicosa- (21), , triconta-(30), tetraconta- (40), , hecta- (100), and so on, preceding without a hyphen the names of the elements to which they refer The prefix mono can usually be omitted; occasionally hemi- (1/2) and sesqui-(3/2) are used No elisions are made when using numerical prefixes except in the case of icosa- when the letter "i" is elided in docosa- and tricosa- Beyond 10, prefixes may be replaced by Arabic numerals

When it is required to indicate the number of entire groups of atoms, the multiplicative numerals bis-, tris-, tetrak:is-, pentak:is-, and so on are used (i.e., -kis is added starting from tetra-) The entity

to which they refer is placed in parentheses

Examples: Ca[PF61z, calcium bis(hexafluorophosphate); and (CIDH21) 3PO•, tris(decyl) phosphate instead of tridecyl which is (C13H2r-)

Composite numeral prefixes are built up by citing units first, then tens, then hundreds, and so on For example, 43 is written tritetraconta- (or tritetracontak:is-)

In indexing it may be convenient to italicize a numerical prefix at the beginning of the name and connect it to the rest of the name with a hyphen; e.g., di-nitrogen pentaoxide (indexed under the letter ''n")

1.1.2.4 Oxidtzlion ami Charge Numbers The oxidation number (Stock system) of an element is indicated by a Roman numeral placed in parentheses immediately following the name of the ele-ment For zero, the cipher 0 is used When used in conjunction with symbols, the Roman numeral may be placed above and to the right The clwrge number of an ion (Ewens-Bassett system) rather than the oxidation state is indicated by an Arabic numeral followed by the sign of the charge cited and is placed in parentheses immediately following the name of the ion

Examples: P205, diphosphorus pentaoxide or phosphorus(V) oxide; Hg~ mercury(!) ion or cury (2+) ion; ~[Fe(CN)()], potassium hexacyanoferrate(ll) or potassium hexacyanoferrate(4-);

dimer-WzPbrvo., dilead(ll) lead(IV) oxide or trilead tetraoxide

Where it is not feasible to define an oxidation state for each individual member of a group, the overall oxidation level of the group is defined by a formal ionic charge to avoid the use of fractional oxidation states; for example, 02

1.1.2.5 Colkctive Names Collective names include:

Halogens (F, Cl, Br, I, At) Chalcogens (0, S, Se, Te, Po) Alkali metals (Li, Na, K, Rb, Cs, Fr) Alkaline-earth metals (Ca, Sr, Ba, Ra) Lanthanoids or lanthanides (La to Lu) Rare-earth metals (Sc, Y, and La to Lu inclusive) Actinoids or actinides (Ac to Lr, those whose 5! shell is being filled) Noble gases (He to Rn)

A transition element is an element whose atom has an incomplete d subshell, or which gives rise

to a cation or cations with an incomplete d subshell

1.1.2.6 Isotopically Labeled Compounds The hydrogen isotopes are given special names:

1H (protium), 2H or D (deuterium), and~ or T (tritium) The superscript designation is preferred because D and T disturb the alphabetical ordering in formulas

Other isotopes are designated by mass numbers: 1~ (boron-10)

Isotopically labeled compounds may be described by inserting the italic symbol of the isotope in brackets into the name of the compound; for exam~le, H3U is hydrogen chloride[36Cl] or hydrogen chloride-36, and ~38Cl is hydrogen eH] chloride[ 8Cl] orhydrogen-2 chloride-38

1.1.2.7 Allotropes Systematic names for gaseous and liquid modifications of elements are times needed Allotropic modifications of an element bear the name of the atom together with the descriptor to specify the modification The following are a few common examples:

some-Symbol nivial name

Atomic hydrogen

(Common oxygen)

Ozone White phosphorus a-Sulfur, ,8-Sulfur ,u-Sulfur (plastic sulfur)

Systematic name

Monohydrogen

Dioxygen Trioxygen Tetraphosphorus Octasulfur Polysulfur

Trivial (customary) names are used for the amorphous modification of an element

1.1.2.8 Heteroatomic aiUJ Other Anions A few heteroatomic anions have names ending in -ide These are

eN, cyanide ion -NH -NH2, hydrazide ion

Added to these anions are

Examples: B2~, diborane; B1ofl14, decaborane (14); B1ofl16, decaborane (16); P2~, diphosphane;

Sn2~, distannane; H2S~, diselane; H2T~ ditellane; H2S5 , pentasulfane; and pb~, plumbane

1.1.2.10 Neutral Rtulicals Certain neutral radicals have special names ending in -yl:

Radicals analogous to the above containing other chalcogens in place of oxygen are named by adding the prefixes thio-, seleno-, and so on; for example, PS, thiophosphoryl; CS, thiocarbonyl

1Similarly for the other halogens

2

1.1.3 Cations

1.1.4 Anions

example, Feu, iron(ll) ion; Fe3+, iron(Ill) ion

This principle also applies to polyatomic cations corresponding to radicals with special names ending in -yl (Sec 1.1.2.10); for example, PO+, phosphoryl cation; NO+, nitrosyl cation; NOi+, nitryl cation; Oi+ oxygenyl cation

Use of the oxidation number and charge number extends the range for radicals; for example, uoi+ uranyl(VI) or uranyl(2+) cation; UO!, uranyl(V) or uranyl(l+) cation

1.1.3.2 Polytdomit: Cations Polyatomic cations derived by addition of more protons than required to give a neutral unit to polyatomic anions are named by adding the ending -onium to the root of the name of the anion element; for example, PRt phosphonium ion; H2r+, iodonium ion;

H30+, oxonium ion; CH30H! methyl oxonium ion

Exception: The name ammonium is retained for the ~ ion; similarly for substituted ammonium ions; for example, NF.t tetrafluoroammonium ion

Substituted ammonium ions derived from nitrogen bases with names ending in -amine receive names formed by changing -amine into -ammonium When known by a name not ending in -amine, the cation name is formed by adding the ending -ium to the name of the base (eliding the final vowel); e.g., anilinium, hydrazinium, imidazolium, acetonium, dioxanium

Exceptions are the names uranium and thiouronium derived from urea and thiourea, respectively

ionic charges are indicated in their names: N2Hs, hydrazinium(l+) ion; N2~, hydrazinium(2+) ion

See Sees 1.1.2.2 and 1.1.2.8 for naming monatomic and certain polyatomic anions When an organic group occurs in an inorganic compound, organic nomenclature (q.v.) is followed to name the organic part

with the two words written as one following the usual practice for polyatomic anions

1.1.4.2 Other Polyalomic Anion& Names for other polyatomic anions consist of the root name of the central atom with the ending -ate and followed by the valence of the central atom expressed by its oxidation number Atoms and groups attached to the central atom are treated as ligands in a complex

Examples: [Sb(OH)6], hexahydroxoantimonate(V); [Fe(CN6]3-, hexacyanoferrate(III); [Co(N02) 6]3

-, hexanitritocobaltate(III); [TiO(C204) 2(H20h]2-, oxobisoxalatodiaquatitanate (IV); [PCI.J-, hexachlorophosphate(V)

Exceptions to the use of the root name of the central atom are antimonate, bismuthate, carbonate, cobaltate, nickelate (or niccolate), nitrate, phosphate, tungstate (or wolframate), and zincate

number of -oxo groups indicated by a suffix; for example, so;-, trioxosulfate

1.1.5 Acids

The ending -ite, formerly used to denote a lower state of oxidation may be retained in trivial names in these cases (note Sec 1.1.5.3 also):

Asoj arsenite N002 peroxonitrite

Brtr hypobromite POt" phosphite3

NzOt- hyponitrite sear- selenite However, compounds known to be double oxides in the solid state are named as such; for example,

Cr2Cu04 (actually Cr203 • CuO) is chromium(lll) copper(II) oxide (and not copper chromite)

1.1.4.4 lsopolyanions Isopolyanions are named by indicating with numerical prefixes the number of atoms of the characteristic element It is not necessary to give the number of oxygen atoms when the charge of the anion or the number of cations is indicated

heptamo-lybdate; the anion, MOJ<>t", is heptamolybdate(6-); Sz()f-, disulfate(2-); P2~- diphosphate(V)(4-) When the characteristic element is partially or wholly present in a lower oxidation state than cor-responds to its Periodic Group number, oxidation numbers are used; for example, [02HP-Q -PO~]~ dihydrogendiphosphate(lll, V)(2-)

A bridging group should be indicated by adding the Greek letter J.L immediately before its name and separating this from the rest of the complex by a hyphen The atom or atoms of the characteristic element to which the bridging atom is bonded, is indicated by numbers

treated as in Sec 1.1.5.1; for example, H2Ge04, hydrogen germanate; H4[Fe(CN)6], hydrogen hexacyanoferrate(II)

1.1.5.3 Trivial Names Acids given in Table 1.1 retain their trivial names due to long-established usage Anions may be formed from these trivial names by changing -ous acid to -ite, and -ic acid to -ate The prefix hypo- is used to denote a lower oxidation state and the prefix per- designates a higher oxidation state The prefixes ortho- and meta- distinguish acids of differing water content; for exam-ple, l4Si04 is orthosilicic acid and H2Si~ is metasilicic acid The anions would be named silicate (4-) and silicate(2-), respectively

!Named for esters formed from the hypothetical acid P(OH),

1.1.5.4 Peroxo-Group When used in conjunction with the trivial names of acids, the prefix peroxo- indicates substitution of o-by o -o

1.1.5.5 Replacement of Oxygen by Othf!l' Chalcogem Acids derived from oxoacids by ment of oxygen by sulfur are called thioacids, and the number of replacements are given by prefixes di-, tri-, and so on The affixes seleno- and telluro- are used analogously

replace-Examples: HOO c=S, thiocarbonic acid; HSS c=S, trithiocarbonic acid

1.1.5.6 Ligatuh Other than Oxygen and Sulfur See Sec 1.1.7, Coordination Compounds, for acids containing ligands other than oxygen and sulfur (selenium and tellurium)

1.1.5.7 Differences between Organic and Inorganic Nomem:lature Organic nomenclature is largely built upon the scheme of substitution that is, the repla.cement of hydrogen atoms by other atoms

or groups Although rare in inorganic nomenclature: NH2C1 is called chloramine and NHC12 amine Other substitutive names are tluorosulfonic acid and chlorosulfonic acid derived from HS~H

dichloro-These and the names aminosulfonic acid (sulfamic acid), iminodisulfonic acid, and nitrilotrisulfonic acid should be replaced by the following based on the concept that these names are formed by adding hydroxyl, amide, imide, and so on, groups together with oxygen atoms to a sulfur atom:

tluorosulfuric acid chlorosulfuric acid amidosulfuric acid

1.1.6 Salts and Functional Derivatives of Acids

imidobis(sulfuric) acid nitridotris(sulfuric) acid

1.1.6.1 Acid Halogenides For acid halogenides the name is formed from the corresponding acid radical if this has a special name (Sec 1.1.2.10); for example, NOCl, nitrosyl chloride In other cases these compounds are named as halogenide oxides with the ligands listed alphabetically; for example, BiC10, bismuth chloride oxide; VC120, vanadium(lV) dichloride oxide

1.1.6.2 Anhydrides Anhydrides of inorganic acids are named as oxides; for example, N205, trogen pentaoxide

dini-1.1.6.3 Estf!l's Esters of inorganic acids are named as the salts; for example, (CH3hS04, dimethyl sulfate However, if it is desired to specify the constitution of the compound, the nomenclature for coordination compounds should be used

1.1.6.4 Amities Names for amides are derived from the names of the acid radicals (or from the names of acids by replacing acid by amide); for example, S02(NH:zh, sulfonyl diamide (or sulfuric diamide); NH2SO~ sulfamidic acid (or amidosulfuric acid)

1.1.6.5 Salts Salts containing acid hydrogen are named by adding the word hydrogen before the name of the anion (however, see Sec 1.1.4.1), for example, KH2P04, potassium dihydrogen phos-phate; NaHC03, sodium hydrogen carbonate (not bicarbonate); NaHPH03 sodium hydrogen phos-phonate (only one acid hydrogen remaining)

Salts containing 02-and Ho- anions are named oxide and hydroxide, respectively Anions are cited in alphabetical order which may be different in formulas and names

Examples: FeO(OH), iron(lll) hydroxide oxide; VO(S04), vanadium(IV) oxide sulfate

1.1.6.6 Multipliclllive Prefixes The multiplicative prefixes bis, tris, etc., are used with certain anions for indicating stoichiometric proportions when di, tri, etc., have been preempted to designate condensed anions; for example, A1K(S04) 2 • 12H20, aluminum potassium bis(sulfate) 12-water (recall that disulfate refers to the anion S0f')

TABLE 1.1 Trivial Names for Acids

~AS04 11111enic acid HJ'20, diphosphoric acid (or

H3B03 orthoboric acid (or boric acid) HJ'206 peroxodiphosphoric acid HB02 metaboric acid (Flo hoi diphosphoric(IV) acid or

HNCO isocyanic acid H2PH~ phosphonic acid

HONC fulminic acid H 2PzH20s diphosphonic acid

HC104 pen:hloricacid HPH2Dz phosphinic acid (formerly

HClO hypochlorous acid HzRe04 rhenic acid

HzCr20, dichromic acid HzS20, disulfuric acid

Hsl06 orthoperiodic acid H2SOs peroxomonosulfuric acid

HMn04 permanganic acid HzS20:s disulfurous acid

H2Mn04 manganic acid H2S202 thiosulfurousacid

HN04 peroxonitric acid H2S204 dithionous acid

HN03 nitric acid H 2S ,06 polythionic acid

HN02 nitrous acid (l:= 3, 4, ) (tri-, tetra-, )

H2N0z nitroxylic acid H2SOz sulfoxylic acid

H2N20z hyponitrous acid HSb(OH)6 hexahydrooxoantimonic acid HOONO peroxonitrous acid HzSe04 selenic acid

H3P04 orthophosphoric acid H2S~ selenious acid

(or phosphoric acid) ~Si04 orthosilicic acid

~ metaphosphoric acid H2Si~ metasilicic acid

H3POs peroxomonophosphoric acid HTcO pertechnetic acid

H 2Tdi4 technetic acid

~Te06 orthotelluric acid

1.1.6.7 Crystal Structure The structure type of crystals may be added in parentheses and in ics after the name; the latter should be in accordance with the structure When the typename is also the mineral name of the substance itself, italics are not used

ital-Examples: Mg'll03, magnesium titanium trioxide (ilmenite type); FeTi03, iron(II) titanium trioxide (ilmenite)

1.1.7 Coordination Compounds

the ligands are attached directly in front of the name of the central atom The ligands are listed in alphabetical order regardless of the number of each and with the name of a ligand treated as a unit Thus "diammine" is listed under "a" and "dim.ethylamine" under "d." The oxidation number of the central atom is stated last by either the oxidation number or charge number

(eliding the final -e, if present, in the anion name) Enclosing marks are required for inorganic anionic ligands containing numerical prefixes, and for thio, selena, and telluro analogs of oxo anions containing more than one atom

If the coordination entity is negatively charged, the cations paired with the complex anion (with -ate ending) are listed first If the entity is positively charged, the anions paired with the complex cation are listed immediately afterward

The following anions do not follow the nomenclature rules:

l l hydrido (or hydro) CH30- methoxo or methanolato

1.1.7.3 Neutral tmd Cationic Ligmuls Neutral and cationic ligands are used without change in name and are set off with enclosing marks Water and ammonia, as neutral ligands, are called "aqua" and "ammine," respectively The groups NO and CO, when linked directly to a metal atom are called nitrosyl and carbonyl, respectively

1.1 7.4 Attoehment Points of Iigtuuls The different points of attachment of a ligand are denoted

by adding italicized symbol(s) for the atom or atoms through which the attachment occurs at the end of

the name of the ligand; e.g., glycine-Nor glycinato-0, N If the same element is involved in different possible coordination sites, the position in the chain or ring to which the element is attached is indicated

by numerical superscripts: e.g., tartrato(3 )-0\ cfl, or tartrato(4 )-o'-, d or tartrato(2-) 01d 1.1.7.5 AbbreviatWns for Ligtmd Names Except for certain hydrocarbon radicals, for ligand (L)

and metal (M), and a few with H, all abbreviations are in lowercase letters and do not involve hyphens

In formulas, the ligand abbreviation is set off with parentheses Some common abbreviations are

H.edta ethylenediaminetetraacetic acid tren 2, 2', 2H-triaminotriethylamine Hedta, edta coordinated ions derived trien triethylenetetraamine

Examples: Li[B(NHi)4 ], lithium tetraamidoborate(l-) or lithium tetraamidoborate(lll); [Co(NH~sCl]

Cl3, pentaamminechlorocobalt(Ill) chloride or pentaamminechlorocobalt(2+) chloride; K3[Fe(CN)sCO], potassium carbonylpentacyanoferrate(II) or potassium carbonylpentacyanoferrate(3-); [Mn{CJI (O) (COO)h(H20)4r, tetraaquabis[salicylato(2-)]manganate(lll) ion; [Ni(C~7N20i):J or [Ni(dmg)] which can be named bis-(2, 3-butanedione dioximate)nickel(ll) or bis[dimethylglyoximato(2-)] nickel (IT)

1.1.8 Addition Compounds

The names of addition compounds are formed by connecting the names of individual compounds

by a dash (-) and indicating the numben; of molecules in the name by Arabic numerals separated by the solidus (diagonal slash) All molecules are cited in order of increasing number; those having the same number are cited in alphabetic order However, boron compounds and water are always cited last and in that order

Examples: 3CdS04 · 8H20, cadmium sulfate-water (3/8); A12(SOJ3 • K2S04 • 24H20, aluminum sulfate potassium sulfate-water (1/tn.4); A1C13 • ~Hs()H, aluminum chloride -ethanol (1/4)

1.1.9 Synonyms and Mineral Names

Acanthite, see Silver sulfide

Alabandite, see Manganese sulfide

Alamosite, see Lead(ll) silicate(2-)

Altaite, see Lead telluride

Alumina, see Aluminum oxide

Alundum, see Aluminum oxide

Alunogenite, see Aluminum sulfate 18-water

Amphibole, see Magnesium silicate(2-)

Andalusite, see Aluminum silicon oxide (111)

Anglesite, see Lead sulfate

Anhydrite, see Calcium sulfate

Anhydrone, see Magnesium perchlorate

Aragonite, see Calcium carbonate

Arcanite, see Potassium sulfate

Argentite, see Silver sulfide

Argo!, see Potassium hydrogen tartrate

Arkanaite, see Titanium(IV) oxide

Arsenolite, see Arsenic(lll) oxide dimer

Arsine, see Arsenic hydride

Auric and aurous, see under Gold

Azoimide, see Hydrogen azide

Azurite, see Copper(II) carbonate dihydroxide

(211) Baddeleyite, see Zin:onium(IV) oxide

Baking soda, see Sodium hydrogen carbonate

Barite (barytes}, see Barium sulfate

Bieberite, see Cobalt sulfate 7-water

Bismuthine, see Bismuth hydride

Bismuthinite, see Bismuth sulfide

Bleaching powder, see Calcium hydrochlorite

Bleaching solution, see Sodium hydrochlorite

Blue copperas, see Copper(II) sulfate 7-water

Boracic acid, see Hydrogen borate

Borax, see Sodium tetmborate 10-water Braunite, see Manganese(lll) oxide Brimstone, see Sulfur

Bromellite, see Beryllium oxide Bromosulfonic acid, see Hydrogen bromosulfate Bromyrite, see Silver bromide

Brookite, see Titanium(IV) oxide Brucite, see Magnesium hydroxide Bunsenite, see Nickel oxide Cacodylate, see Sodium dimethylarsonate 3-water Caesium, see under Cesium

Calamine, see Zinc carbonate Calcia, see Calcium oxide Calcite, see Calcium carbonate Calomel, see Mercury(l) chloride Caro's acid, see Hydrogen peroxosulfate

C&~~siopeium, see Lutetium Cassiterite, see Tin(IV) oxide Caustic potash, see Potassium hydroxide Caustic soda, see Sodium hydroxide Celestite, see Strontium sulfate Cementite, see tri-Iron carbide Cerargyrite, see Silver chloride Cerussite, see Lead carbonate Chalcanthite, see Copper(II) sulfate 5-water Chalcocite, see Copper(l) sulfide

Cbalk, see Calcium carbonate Chile nitre, see Sodium nitrate

Chile saltpeter, see Sodium nitrate Chloromagnesite, see Magnesium chloride Chlorosulfonic acid, see Hydrogen chlorosulfate Cinnabar, see Men:ury(ll) sulfide

Claudetite, see Arsenic(lll) oxide dimer

(Continued)

TABLE 1.2 SynonymB and Mineral Names (Continued)

Clausthalite, see Lead selenide

Clinoenstatite, see Magnesium silicate(2-)

Columbium, see under Niobium

Corrosive sublimate, see Men:ury(II) chloride

Comndum, see Aluminum oxide

Cotunite, see Lead chloride

Covellite, see Copper(H) sulfide

Cream of tartar, see Potassium hydrogen tartrate

Crocoite, see Lead chromate(VI)(2-)

Cryolite, see Sodium hexafluoroaluminate

Cryptohalite, see Ammonium hexafluorosilicate

Cupric and cuprous, see under Copper

Cuprite, see Copper(l) oxide

Dakin's solution, see Sodium hypochlorite

Dehydrite, see Magnesium perchlorate

Dental gas, see Nitrogen(!) oxide

Diamond, see Carbon

Dichlorodisulfane, see di-Sulfur dichloride

Diuretic salt, see Potassium acetate

Dolomite, see Calcium magnesium carbonate (1/1)

Dry ice, see Carbon dioxide (solid)

Enstatite, see Magnesium silicate(2-)

Epsom salts, see Magnesium sulfate 7-water

Epsomite, see Magnesium sulfate 7-water

Briochalcite, see Copper(II) chloride

Fayalite, see Iron(II) silicate(4-)

Ferric and ferrous, see under Iron

Fluorine oxide, see Oxygen difluoride

Fluoristan, see Tin(II) fluoride

Fluorite, see Calcium fluoride

Fluorosulfonic acid, see Hydrogen tluorosulfate

Fluorspar, see Calcium fluoride

Forsterite, see Magnesium silicate( 4-)

Freezing salt, see Sodium chloride

Fulminating mercury, see Mercury fulminate

Galena, see Lead sulfite

Glauber's salt, see Sodium sulfate 10-water

Goethite, see lron(II) hydroxide oxide

Goslarite, see Zinc sulfate 7-water

Graham's salt, see Sodium phosphate(!-)

Graphite, see Carbon

Greenockite, see Cadmium sulfide

Gruenerite, see Iron(II) silicate(2-)

Guanajuatite, see Bismuth selenide

Gypsum, see Calcium sulfate 2-water

Halite, see Sodium chloride

Hausmannite, see Manganese(ll,IV) oxide

Heavy hydrogen, see HydrogenfH] or name followed

by-d Heavy water, see Hydrogen fH] oxide

Heazlewoodite, see tri-Nickel disulfide

Hematite, see lron(III) oxide

Hermannite, see Manganese silicate

Hessite, see Silver telluride

Hieratite, see Potassium hexafluorosilicate Hydroazoic acid, see Hydrogen azide Hydrophilite, see Calcium chloride Hydrosulfite, see Sodium dithionate(III) Hypo (photographic), see Sodium thiosulfate 5-water

Hypophosphite, see under Phosphinate Ice, see Hydrogen oxide (solid) Iceland spar, see Calcium carbonate Iodyrite, see Silver iodide Jeweler's borax, see Sodium te1raborate 10-water Jeweler's rouge, au lron(III) oxide

Kalinite, see Aluminum potassium bis(sulfate) Kemite, see Sodium tetraborate

Kyanite, see Aluminum silicon oxide (1/1) Laughing gas, see Nitrogen(!) oxide Lautarite, see Calcium iodate Lawrencite, see lron(II) chloride Lechatelierite, see Silicon dioxide

Lime, see Calcium oxide Litharge, see Lead(II) oxide Lithium aluminum hydride, see Lithium tetrahydri-doaluminate

LodestDne, see lron(II,Ill) oxide Lunar caustic, see Silver nitrate Lye, see Sodium hydroxide Magnesia, see Magnesium oxide Magnesite, su Magnesium carbonate Magnetite, see Iron(II,III) oxide Malachite, see Copper carbonate dihydroxide Manganosite, see Manganese(II) oxide Marcasite, see lron disulfide Marshite, see Copper(I) iodide Mascagnite, see Ammonium sulfate Massicotite, see Lead oxide Mercuric and mercurous, see under Mercury Metacinnabar, see Mercury(II) su11ide Millerite, see Nickel sulfide Mirabilite, see Sodium sulfate Mohr's salt, see Ammonium iron(II) sulfate 6-water Moissanite, see Silicon carbide

Molybdenite, see Molybdenum disu11ide Molybdite, see Molybdenum(VI) oxide Molysite, see Iron(III) chloride Montroydite, see Mercury(II) oxide Morenosite, see Nickel sulfate 7-water Mosaic gold, see Tin disu11ide Muriatic acid, see Hydrogen chloride, aqueous solutions

Nantok:ite, see Copper(!) chloride Natron, see Sodium carbonate Naumannite, see Silver selenide Neutral verdigris, see Copper(li) acetate Nitre (niter), see Potassium nitrate

TABLE 1.2 Synonyms and Mineral Names (Continued)

Nitric oxide, see Nitrogen(ll) oxide

Nitrobarite, see Barium nitrate

Nitromagnesite, see Magnesium nitrate 6-water

Nitroprusside, see Sodium

pentacyanonitrosylfer-rate(ll) 2-water

Oldhamite, see Calcium sulfide

Opal, see Silicon dioxide

Orpiment, see Arsenic trisulfide

Oxygen powder, see Sodium peroxide

Paris green, see Copper acetate arsenate(III) (113)

Pawellite, see Calcium molybdate(VI)(2-)

Pearl ash, see Potassium carbonate

Perborax, see Sodium peroxoborate

Periclase, see Magnesium oxide

Persulfate, see Peroxodisulfate

Phosgene, see Carbonyl chloride

Phosphine, see Hydrogen phosphide

Pickling acid, see Hydrogen sulfate

Pitchblende, see Uranium(IV) oxide

Plaster of Paris, see Calcium sulfate hemihydrate

Plattnerite, see Lead(IV) oxide

Polianite, see Manganese(IV) oxide

Polishing powder, see Silicon dioxide

Potash, see Potassium carbonate

Potassium acid phthalate, see Potassium hydrogen

phthalate

Prussic acid, see Hydrogen cyanide

Pyrite, see Iron disulfide

Pyrochroite, see Manganese(H) hydroxide

Pyrohytpophosphite, see diphosphate(IV)

Pyrolusite, see Manganese(IV) oxide

Pyrophanite, see Manganese titanate(IV)(2-)

Pyrophosphate, see Diphosphate(V)

Pyrosulfuric acid, see Hydrogen disulfate

Quartz, see Silicon dioxide

Quicksilver, see Mercury

Realgar, see di-Arsenic disulfide

Red lead, see Lead(II,IV) oxide

Rhodochrosite, see Manganese carbonate

Rhodonite, see Manganese silicate(l-)

Rochelle salt, see Potassium sodium tarttate 4-water

Rock crystal, see Silicon dioxide

Rutile, see Titanium(IV) oxide

Sal soda, see Sodium carbonate 10-water

Saltpeter, see Potassium nitrate

Seacehite, see Manganese chloride

Scbeelite, see Calcium tungstate(VI)(2-)

Sellaite, see Magnesium fluoride

Senarmontite, see Antimony(lll) oxide

Siderite, see Iron(ll) carbonate

Siderotil, see Iron(ll) sulfate 5-water

Silica, see Silicon dioxide

Silicotungstic acid, see Silicon oxide-tungsten

oxide-water (1112126)

Sillimanite, see Aluminum silicon oxide (111)

Smithsonite, see Zinc carbonate Soda ash, see Sodium carbonate

Spelter, see Zinc metal Sphalerite, see Zinc sulfide Spherocobaltite, see Cobalt(II) carbonate

Spinel, see Magnesium alwninate(2-) Stannic and stannous, see under Tin

Stibine, see Antimony hydride Stibnite, see Antimony(lll) sulfide

Stolzite, see Lead tungstate(VI)(2-) Strengite, see Jron(lll) phosphate Strontianite, see Strontium carbonate

Sugar of lead, see Lead acetate Sulfamate, see Amidosulfate

Sulphate, see Sulfate Sulfurated lime, see Calcium sulfide

Sulfuretted hydrogen, see Hydrogen sulfide

Sulphur, see Sulfur

Sulfuryl, see Sulfonyl Sycoporite, see Cobalt sulfide Sylvite, see Potassium chloride Szmik.ite, see Manganese(ll) sulfate hydrate

Thrapacaite, see Potassium chromate(VI)

Tellurite, see Tellurium dioxide Tenorite, see Copper(II) oxide Tephroite, see Manganese silicate(!-)

Thenardite, see Sodium sulfate Thionyl, see Sul.finyl

Thorianite, see Thorium dioxide Topaz, see Aluminum hexafluorosilicate 1iidymite, see Silicon dioxide

Troilite, see Jron(II) sulfide

Trona, see Sodium carbonate hydrogen carbonate

dihydrate Tschennigite, see Aluminum ammonium bis(sulfate)

Tungstenite, see Tungsten disulfide

Tungstite, see Hydrogen tungstate Uraninite, see Uranium(IV) oxide

Valentinite, see Antimony (Ill) oxide Verdigris, see Copper acetate hydrate

Vermillion, see Mercury(ll) sulfide Villiaumite, see Sodium fluoride

Vitamin B3, see Calcium (+)pantothenate

Washing soda, see Sodium carbonate 10-water Whitlockite, see Calcium phosphate Wlllemite, see Zinc silicate( 4-)

Wolfram, see Tungsten

Wuestite, see Iron(II) oxide

Wulfenite, see Lead molybdate(VI)(2-) Wurtzite, see Zinc sulfide

Zincite, see Zinc oxide Zincosite, see Zinc sulfate Zincspar, see Zinc carbonate

Zirconia, see Zirconium oxide

1.1.10 Classification of Inorganic Substances

Simple substances Molecules consist of one-type atoms (atoms of one element) In chemical reactions, molecules cannot be decomposed with formation of other substances

Complex substances (or chemical compounds) Molecules consist of different types of atoms (atoms

of different chemical elements) In chemical reactions, molecules are decomposed with the formation

of several other substances

Simple Complex

MetalB Nonmetals Oxides Bases Acids Salts

A sharp transition border between metals and nonmetals does not exist, since they are simple substances showing dual properties

Bases Complex substances in which atoms of metals bond with one or several hydroxyl groups [according to electrolytic dissociation theory, bases are complex substances which under the dissoci-ating in water solution form metal cations (NH.t) and hydroxide anions (011)]

Classification Soluble in water (alkalis) and insoluble Amphoteric bases also show properties

Oxides Complex substances consisting of two elements, one of which is oxygen

CkJssification

Nonsalts forming (CO, N20, and NO)

A metal oxide in which metals display low oxidation number+ 1, +2 N~O; MgO; and CuO

Amphoteric:

(for metals with oxidation number+ 3, +4)

As hydrates it corn:Bponds with amphoteric hydroxide ZoO; Al203 ; Cr203; and Sn02

Acid:

An oxide of nonmetals and metals with oxidation number fmm+S to+7

S02; S~; P20~; Mn20,; and Cr03 Basic, amphotcric-<:OtTesponding bases; amphoteric, acid-corresponding acids

to 2Pb(N~)z +® 2PbO + 4N02 + 02

HzS04 (cone.)

2HMn04 + Mnz07 + H20

to

Interaction with acid or base

On reactions with acid, salt, and water are formed

t°C

MgO + H2S04 ~ MgS04 + H20

t°C CuO + 2HCl ~ CuCl2 + H20

Amphoteric oxides interact

with acids as basic:

On reactions with base, salt, and water are formed

C02 + Ba(OHh ~ BaC03 + llzO

S02 + 2Na0H ~ N~S03 + H20

with bases as acid:

ZnO + 2NaOH ~ N~02 + H20 (ZnO + 2NaOH + H20 ~ N~[Zn(OH)4])

Interaction of basic and acid oxide with each other leads to salt formation

N~O + C02 ~ N~C03

Reduction up to simple substances

3Cu0 + 2NH3 ~ 3Cu + N2 + 3H20

P20s + 5C + 2P + 5CO

Acids Complex substances consisting of hydrogen atoms and acid radicals (according to

electro-lytic dissociation theory, acids-electrolytes, which under the dissociating form only W in the capacity of cations)

Classification

1 On composition: oxygenless and oxoacids

2 On hydrogen atoms number, which are capable of being substituted on metal: mono-, di-, tribasic

HCl-hydrogen chloride (hydrochloric) Monobasic Chloride HBr-hydrogen bromide Monobasic Bromide Hl -hydrogeniodide Monobasic Iodide HF hydrogen fluorine (hydrofluoric) Monobasic Fluoride

H2S -hydrogensulphide Bibasic Sulphide Containing oxygen

H2S04 11ulphuric Bibasic Sulphate

NazSi03 + 2HC1 ~ H2Si03 + 2NaCl

3 Interaction with basic oxides

4 Interaction with metals

t°C CuO + 2HN~ ~ Cu(N~2 + H20

Zn + 2HC1 ~ ZnClz +Hz 2Al + 6HC1 ~ 2A1Cl3 + 3Hz (metals standing in the electrochemical series before hydrogen, acid-oxidizers)

5 Interaction with salts (reactions of exchange) at which stands out gas or formed residual

H2S04 + BaC12 ~ BaS04 +2HC1 2HC1 + KzC03 ~ 2KC1 + H20 + C02

Salls Complex substances which consist of atoms of metal and acid residuals This is the most numerous class of inorganic compounds

2Cl-Acid salts In the time of dissociation, acid salts give only metal cations (or~~ hydrogen anions, and anions of acid radical Products of full substitution hydrogen atoms of multi basic acid

to atoms of metal:

NaRC~~ Na+ + HCO:J ~ Na+ + W +

co:r-Basic salts In the time of dissociation, basic salts give only metal cations, hydroxyl anions, and

anions of acid radical Products of incomplete substitution OH groups, corresponding bases to acid radicals:

Zn(OH)Cl ~ [Zn(OH)]+ + cr ~ Znu + 011 + cr

Double salts In the time of dissociation, double salts give two cations and one anion:

KAl(SO•h ~ K+ + Al3+ +

2SO]-Mixed salts Formed by means of one cation and two anions:

Ca0Cl2 ~ Cau + cr +ocr

Complex salts Contain complex cations and anions:

[Ag(NH3)z]Br ~ [Ag(NH3)i]+ + Na[Ag(CN)z] ~ Na+ + [Ag(CN)z]-

2 Metal with acid:

3 Metal with solution of salt of less active metal:

4 Basic oxide with the acid oxide:

5 Basic oxide with acid:

to CuO + H2S04 -+ CuS04 + H20

6 Bases with acid oxide:

7 Bases with acid: