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When it was first published, this first-year chemistry text revolutionized the teaching of chemistry by presenting it in terms of unifying principles instead of as a body of unrelated facts. Those principles included modern theories of atomic and molecular structure, quantum mechanics, statistical mechanics, and thermodynamics. In addition, Dr. Pauling attempted to correlate the theories with descriptive chemistry, the observed properties of substances, to introduce the student to the multitude of chemical substances and their properties. In this extensively revised and updated third edition, the Nobel Prize–winning author maintains an excellent balance between theoretical and descriptive material, although the amount of descriptive chemistry has been decreased somewhat, and the presentation of the subject, especially in relation to the nonmetals, has been revised in such a way as to permit greater correlation with the electronic structure of atoms, especially electronegativity. The principles of quantum mechanics are discussed on the basis of the de Broglie wavelength of the electron. The quantized energy levels of a particle in a box are derived by means of a simple assumption about the relation of the de Broglie waves to the walls of the box. No attempt is made to solve the Schrödinger wave equation for other systems, but the wave functions of hydrogen-like electrons are presented and discussed in some detail, and the quantum states for other systems are also covered. Statistical mechanics is introduced before thermodynamics, and the discussion of thermodynamics is based on it. This arrangement reflects the author's belief that beginning students can understand statistical mechanics better than chemical thermodynamics. Aimed at first-year college students who plan to major in chemistry or closely related fields, the book is written in a logical, clear, and understandable style. In addition, many excellent figures are included, along with numerous problems and 75 pages of appendices covering such topics as symmetry of molecules and crystals, hybrid bond orbitals, and magnetic properties of substances. Cover Title Page Copyright Page Contents 1 The Nature and Properties of Matter 1-1 Matter and Chemistry 1-2 Mass and Energy 1-3 The International System of Units 1-4 Temperature 1-5 Kinds of Matter 1-6 The Physical Properties of Substances 1-7 The Chemical Properties of Substances 1-8 The Scientific Method 2 The Atomic and Molecular Structure of Matter 2-1 Hypotheses, Theories, and Laws 2-2 The Atomic Theory 2-3 Modern Methods of Studying Atoms and Molecules 2-4 The Arrangement of Atoms in a Crystal 2-5 The Description of a Crystal Structure 2-6 Crystal Symmetry; the Crystal Systems 2-7 The Molecular Structure of Matter 3 The Electron, the Nuclei of Atoms, and the Photon 3-1 The Nature of Electricity 3-2 The Discovery of the Electron 3-3 The Discovery of X-rays and Radioactivity 3-4 The Nuclei of Atoms 3-5 The Birth of the Quantum Theory 3-6 The Photoelectric Effect and the Photon 3-7 The Diffraction of X-rays by Crystals 3-8 Electron Wave Character and Electron Spin 3-9 What Is Light? What Is an Electron? 3-10 The Uncertainty Principle 4 Elements and Compounds. Atomic and Molecular Masses 4-1 The Chemical Elements 4-2 The Neutron. The Structure of Nuclei 4-3 Chemical Reactions 4-4 Nuclidic Masses and Atomic Weights 4-5 Avogadro's Number. The Mole 4-6 Examples of Weight-relation Calculations 4-7 Determination of Atomic Weights by the Chemical Method 4-8 Determination of Atomic Weights by Use of the Mass Spectrograph 4-9 Determination of Nuclidic Masses by Nuclear Reactions 4-10 The Discovery of the Correct Atomic Weights. Isomorphism 5 Atomic Structure and the Periodic Table of the Elements 5-1 The Bohr Theory of the Hydrogen Atom 5-2 Excitation and Ionization Energies 5-3 The Wave-mechanical Description of Atoms 5-4 The Periodic Table of the Elements 5-5 Electron Energy as the Basis of the Periodic Table 5-6 The History of the Periodic Table 6 The Chemical Bond 6-1 The Nature of Covalence 6-2 The Structure of Covalent Compounds 6-3 The Direction of Valence Bonds in Space 6-4 Tetrahedral Bond Orbitals 6-5 Bond Orbitals with Large p Character 6-6 Molecules and Crystals of the Nonmetallic Elements 6-7 Resonance 6-8 Ionic Valence 6-9 The Partial Ionic Character of Covalent Bonds 6-10 The Electronegativity Scale of the Elements 6-11 Heats of Formation and Relative Electronegativity of Atoms 6-12 The Electroneutrality Principle 6-13 The Sizes of Atoms and Molecules. Covalent Radii and van der Waals Radii 6-14 Oxidation Numbers of Atoms 7 The Nonmetallic Elements and Some of Their Compounds 7-1 The Elementary Substances 7-2 Hydrides of Nonmetals. Hydrocarbons 7-3 Hydrocarbons Containing Double Bonds and Triple Bonds 7-4 Aromatic Hydrocarbons. Benzene 7-5 Ammonia and Its Compounds 7-6 Other Normal-valence Compounds of the Nonmetals 7-7 Some Transargononic Single-bonded Compounds 7-8 The Argonons 8 Oxygen Compounds of Nonmetallic Elements 8-1 The Oxycompounds of the Halogens 8-2 Oxycompounds of Sulfur, Selenium, and Tellurium 8-3 Oxycompounds of Phosphorus, Arsenic, Antimony, and Bismuth 8-4 Oxycompounds of Nitrogen 8-5 Oxycompounds of Carbon 8-6 Molecules containing Bivalent Carbon. Free Radicals 8-7 Unstable and Highly Reactive Molecules 9 Gases: Quantum Mechanics and Statistical Mechanics 9-1 The Perfect-gas Equation 9-2 Quantum Mechanics of a Monatomic Gas 9-3 The Wave Equation 9-4 The Kinetic Theory of Gases 9-5 The Distribution Law for Molecular Velocities 9-6 The Boltzmann Distribution Law 9-7 Deviations of Real Gases from Ideal Behavior 10 Chemical Thermodynamics 10-1 Heat and Work. Energy and Enthalpy 10-2 The First Law of Thermodynamics 10-3 Heat Capacity. Heats of Fusion, Vaporization, and Transition 10-4 Entropy. The Probable State of an Isolated System 10-5 The Absolute Entropy of a Perfect Gas 10-6 Reversible and Irreversible Changes in State 10-7 The Efficiency of a Heat Engine 10-8 Change in Entropy of Any System with Temperature 10-9 The Third Law of Thermodynamics 10-10 The Heat Capacity of Diatomic Gases 10-11 Quantum States of the Rigid Rotator 10-12 The Rotational Entropy of Diatomic Gases 10-13 Quantum States of the Harmonic Oscillator 10-14 Vibrational States of Diatomic Molecules 10-15 Energy, Heat Capacity, and Entropy of a Harmonic Oscillator 10-16 The Quantum Theory of Low-temperature Heat Capacity of Crystals 11 Chemical Equilibrium 11-1 The Thermodynamic Condition for Chemical Equilibrium 11-2 The Vapor Pressure of a Liquid or Crystal 11-3 Entropy of Transition, Fusion, and Vaporization 11-4 Van der Waals Forces. Melting Points and Boiling Points 11-5 Chemical Equilibrium in Gases 11-6 Change of Equilibrium with Temperature 11-7 Equilibrium in Heterogeneous Systems 11-8 Le Chatelier's Principle 11-9 The Phase Rule—a Method of Classifying All Systems in Equilibrium 11-10 The Conditions under Which a Reaction Proceeds to Completion 12 Water 12-1 The Composition of Water 12-2 The Water Molecule 12-3 The Properties of Water 12-4 The Hydrogen Bond—the Cause of the Unusual Properties of Water 12-5 The Entropy of Ice 12-6 The Importance of Water as an Electrolytic Solvent 12-7 Heavy Water 12-8 Deviation of Water and Some Other Liquids from Hildebrand's Rule 12-9 The Dense Forms of Ice 12-10 The Phase Diagram of Water 13 The Properties of Solutions 13-1 Types of Solutions. Nomenclature 13-2 Solubility 13-3 The Dependence of Solubility on the Nature of Solute and Solvent 13-4 Solubility of Salts and Hydroxides 13-5 The Solubility-Product Principle 13-6 The Solubility of Gases in Liquids: Henry's Law 13-7 The Freezing Point and Boiling Point of Solutions 13-8 The Vapor Pressure of Solutions: Raoult's Law 13-9 The Osmotic Pressure of Solutions 13-10 The Escaping Tendency and the Chemical Potential 13-11 The Properties of Ionic Solutions 13-12 Colloidal Solutions 14 Acids and Bases 14-1 Hydronium-ion (Hydrogen-ion) Concentration 14-2 The Equilibrium between Hydrogen Ion and Hydroxide Ion in Aqueous Solution 14-3 Indicators 14-4 Equivalent Weights of Acids and Bases 14-5 Weak Acids and Bases 14-6 The Titration of Weak Acids and Bases 14-7 Buffered Solutions 14-8 The Strengths of the Oxygen Acids 14-9 The Solution of Carbonates in Acid; Hard Water 14-10 The Precipitation of Sulfides 14-11 Nonaqueous Amphiprotic Solvents 15 Oxidation-Reduction Reactions. Electrolysis 15-1 The Electrolytic Decomposition of Molten Salts 15-2 The Electrolysis of an Aqueous Salt Solution 15-3 Oxidation-Reduction Reactions 15-4 Quantitative Relations in Electrolysis 15-5 The Electromotive-force Series of the Elements 15-6 Equilibrium Constants for Oxidation-Reduction Couples 15-7 The Dependence of the Electromotive Force of Cells on Concentration 15-8 Primary Cells and Storage Cells 15-9 Electrolytic Production of Elements 15-10 The Reduction of Ores. Metallurgy 16 The Rate of Chemical Reactions 16-1 Factors Influencing the Rate of Reactions 16-2 The Rate of a First-order Reaction at Constant Temperature 16-3 Reactions of Higher Order 16-4 Mechanism of Reactions. Dependence of Reaction Rate on Temperature 16-5 Catalysis 16-6 Kinetics of Enzyme Reactions 16-7 Chain Reactions 17 The Nature of Metals and Alloys 17-1 The Metallic Elements 17-2 The Structure of Metals 17-3 The Nature of the Transition Metals 17-4 The Metallic State 17-5 Metallic Valence 17-6 The Free-electron Theory of Metals 17-7 The Nature of Alloys 17-8 Experimental Methods of Studying Alloys 17-9 Interstitial Solid Solutions and Substitutional Solid Solutions 17-10 Physical Metallurgy 18 Lithium, Beryllium, Boron, and Silicon and Their Congeners 18-1 The Electronic Structures of Lithium, Beryllium, Boron, and Silicon and Their Congeners 18-2 Radius Ratio, Ligancy, and the Properties of Substances 18-3 The Alkali Metals and Their Compounds 18-4 The Alkaline-earth Metals and Their Compounds 18-5 Boron 18-6 The Boranes. Electron-deficient Substances 18-7 Aluminum and Its Congeners 18-8 Silicon and Its Simpler Compounds 18-9 Silicon Dioxide 18-10 Sodium Silicate and Other Silicates 18-11 The Silicate Minerals 18-12 Glass 18-13 Cement 18-14 The Silicones 18-15 Germanium 18-16 Tin 18-17 Lead 19 Inorganic Complexes and the Chemistry of the Transition Metals 19-1 The Nature of Inorganic Complexes 19-2 Tetrahedral, Octahedral, and Square Bond Orbitals 19-3 Ammonia Complexes 19-4 Cyanide Complexes 19-5 Complex Halides and Other Complex Ions 19-6 Hydroxide Complexes 19-7 Sulfide Complexes 19-8 The Quantitative Treatment of Complex Formation 19-9 Polydentate Complexing Agents 19-10 The Structure and Stability of Carbonyls and Other Covalent Complexes of the Transition Metals 19-11 Polynuclear Complexes 20 Iron, Cobalt, Nickel, and the Platinum Metals 20-1 The Electronic Structures and Oxidation States of Iron, Cobalt, Nickel, and the Platinum Metals 20-2 Iron 20-3 Steel 20-4 Compounds of Iron 20-5 Cobalt 20-6 Nickel 20-7 The Platinum Metals 21 Copper, Zinc, and Gallium and Their Congeners 21-1 The Electronic Structures and Oxidation States of Copper, Silver, and Gold 21-2 The Properties of Copper, Silver, and Gold 21-3 The Compounds of Copper 21-4 The Compounds of Silver 21-5 Photochemistry and Photography 21-6 The Compounds of Gold 21-7 Color and Mixed Oxidation States 21-8 The Properties and Uses of Zinc, Cadmium, and Mercury 21-9 Compounds of Zinc and Cadmium 21-10 Compounds of Mercury 21-11 Gallium, Indium, and Thallium 22 Titanium, Vanadium, Chromium, and Manganese and Their Congeners 22-1 The Electronic Structures of Titanium, Vanadium, Chromium, and Manganese and Their Congeners 22-2 Titanium, Zirconium, Hafnium, and Thorium 22-3 Vanadium, Niobium, Tantalum, and Protactinium 22-4 Superconductivity 22-5 Chromium 22-6 The Congeners of Chromium 22-7 Manganese 22-8 Acid-forming and Base-forming Oxides and Hydroxides 22-9 The Congeners of Manganese 23 Organic Chemistry 23-1 The Nature and Extent of Organic Chemistry 23-2 Petroleum and the Hydrocarbons 23-3 Alcohols and Phenols 23-4 Aldehydes and Ketones 23-5 The Organic Acids and Their Esters 23-6 Amines and Other Organic Compounds of Nitrogen 23-7 Carbohydrates, Sugars, Polysaccharides 23-8 Fibers and Plastics 24 Biochemistry 24-1 The Nature of Life 24-2 The Structure of Living Organisms 24-3 Amino Acids and Proteins 24-4 Nucleic Acids. The Chemistry of Heredity 24-5 Metabolic Processes. Enzymes and Their Action 24-6 Vitamins 24-7 Hormones 24-8 Chemistry and Medicine 25 The Chemistry of the Fundamental Particles 25-1 The Classification of the Fundamental Particles 25-2 The Discovery of the Fundamental Particles 25-3 The Forces between Nucleons. Strong Interactions 25-4 The Structure of Nucleons 25-5 Leptons and Antileptons 25-6 Mesons and Antimesons 25-7 Baryons and Antibaryons 25-8 The Decay Reactions of the Fundamental Particles 25-9 Strangeness (Xenicity) 25-10 Resonance Particles and Complexes 25-11 The Structure of the Fundamental Particles. Quarks 25-12 Positronium, Muonium, Mesonic Atoms 26 Nuclear Chemistry 26-1 Natural Radioactivity 26-2 The Age of the Earth 26-3 Artificial Radioactivity 26-4 The Kinds of Nuclear Reactions 26-5 The Use of Radioactive Elements as Tracers 26-6 Dating Objects by Use of Carbon 26-7 The Properties of Nucleides 26-8 The Shell Model of Nuclear Structure 26-9 The Helion-Triton Model 26-10 Nuclear Fission and Nuclear Fusion Appendixes I. Units of Measurement II. Values of Some Physical and Chemical Constants III. Symmetry of Molecules and Crystals IV. X-rays and Crystal Structure V. Hydrogenlike Orbitals VI. Russell-Saunders States of Atoms Allowed by the Pauli Exclusion Principle VII. Hybrid Bond Orbitals VIII. Bond Energy and Bond-dissociation Energy IX. The Vapor Pressure of Water at Different Temperatures X. An Alternative Derivation of the Boltzmann Distribution Law XI. The Boltzmann Distribution Law in Classical Mechanics XII. The Entropy of a Perfect Gas XIII. Electric Polarizabilities and Electric Dipole Moments XIV. The Magnetic Properties of Substances XV. Values of Thermodynamic Properties of Some Substances at °C and atm XVI. Selected Readings Index "An excellent text, highly recommended." — Choice When it was first published, this first-year chemistry text revolutionized the teaching of chemistry by presenting it in terms of unifying principles instead of as a body of unrelated facts. Those principles included modern theories of atomic and molecular structure, quantum mechanics, statistical mechanics and thermodynamics. In addition, Dr. Pauling attempted to correlate the theories with descriptive chemistry, the observed properties of substances, to introduce the student to the multitude of chemical substances and their properties. In this extensively revised and updated third edition, the Nobel Prize–winning author maintains an excellent balance between theoretical and descriptive material, although the amount of descriptive chemistry has been decreased somewhat, and the presentation of the subject, especially in relation to the nonmetals, has been revised in such a way as to permit greater correlation with the electronic structure of atoms, especially electronegativity. The principles of quantum mechanics are discussed on the basis of the de Broglie wavelength of the electron. The quantized energy levels of a particle in a box are derived by means of a simple assumption about the relation of the de Broglie waves to the walls of the box. No attempt is made to solve the Schrodinger wave equation for other systems, but the wave functions of hydrogen-like electrons are presented and discussed in some detail, and the quantum states for other systems are also covered. Statistical mechanics is introduced before thermodynamics, and the discussion of thermodynamics is based on it. This arrangement reflects the author's belief that beginning students can understand statistical mechanics better than chemical thermodynamics. Aimed at first-year college students who plan to major in chemistry or closely related fields, the book is written in a logical, clear and understandable style. In addition, many excellent figures are included, along with numerous problems and 75 pages of appendixes covering such topics as symmetry of molecules and crystals, hybrid bond orbitals, and magnetic properties of substances. General Chemistry Linus Pauling 0 / 0 0 comments When it was first published, this first-year chemistry text revolutionized the teaching of chemistry by presenting it in terms of unifying principles instead of as a body of unrelated facts. Those principles included modern theories of atomic and molecular structure, quantum mechanics, statistical mechanics and thermodynamics. In addition, Dr. Pauling attempted to correlate the theories with descriptive chemistry, the observed properties of substances, to introduce the student to the multitude of chemical substances and their properties. In this extensively revised and updated third edition, the Nobel Prize–winning author maintains an excellent balance between theoretical and descriptive material, although the amount of descriptive chemistry has been decreased somewhat, and the presentation of the subject, especially in relation to the nonmetals, has been revised in such a way as to permit greater correlation with the electronic structure of atoms, especially electronegativity. Aimed at first-year college students who plan to major in chemistry or closely related fields, the book is written in a logical, clear and understandable style. In addition, many excellent figures are included, along with numerous problems and 75 pages of appendixes covering such topics as symmetry of molecules and crystals, hybrid bond orbitals, and magnetic properties of substances.Year:1988Edition:3rd EditionPublisher:Dover PublicationsLanguage:EnglishPages: 959 ISBN 10:0486656225ISBN 13:9780486656229File:EPUB, 45.94 MB Download (epub, 45.94 MB) Send-to-Kindle or Email