CHEMICAL PRINCIPLES

William L. Masterton and Emil J. Slowinsky

FOURTH EDITION

1977
W. B. Saunders Company

Kopie als sieben Bände, ehemaliges Bibliotheksexemplar der TU München
(Copy in seven volumes, formerly from the library of the Technical University of Munich)

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Inhaltsverzeichnis
(table of contents)

1
CHEMISTRY: AN EXPERIMENTAL SCIENCE
1.1 Measurements, 2; 1.2 Kinds of Substances, 12; 1.3 Identification of Pure Substances, 13; 1.4 Separation of Matter into Pure Substances, 15; Problems, 20

2
ATOMS, MOLECULES, AND IONS
2.1 Atomic Theory, 23; 2.2 Components of the Atom, 25; 2.3 Molecules and Ions, 29; 2.4 Relative Masses of Atoms: Atomic Weights, 32; 2.5 Masses of Atoms; Avogadro's Number, 35; 2.6 Masses of Molecules. Molecular Weight, 37; Historical Perspective; Atomic Weights in the 19th Century, 37 Problems, 41

3
CHEMICAL FORMULAS AND EQUATIONS
3.1 Chemical Formulas, 45; 3.2 Simplest Formulas from Analysis, 46; 3.3 Molecular Formula from Simplest Formula, 49; 3.4 The Mole, 49; 3.5 Chemical Equations, 51; 3.6 Mass Relations in Reactions, 52; 3.7 Limiting Reagent. Theoretical and Actual Yields, 54; Problems, 56

4
THERMOCHEMISTRY
4.1 The Enthalpy Change: AH, 61; 4.2 Thermochemical Equations, 64; 4.3 Heats of Formation, 66; 4.4 Bond Energies (Enthalpies), 68; 4.5 Measurement of Heat Flow. Calorimetry, 72; 4.6 The First Law of Thermodynamics, 75; 4.7 Sources of Energy, 79; Problems, 85


5
THE PHYSICAL BEHAVIOR OF GASES
5. 1 Some General Properties of Gases, 89; 5.2 Atmospheric Pressure and the Barometer, 90; 5.3 The Ideal Gas Law, 93; 5.4 Using the Ideal Gas Law, 100; 5.5 Mixtures of Gases: Dalton's Law of Partial Pressures, 105; 5.6 Real Gases, 107; The Kinetic Theory of Gases, 110; Problems, 116

6
THE ELECTRONIC STRUCTURE OF ATOMS
6.1 Some Properties of Electrons in Atoms and Molecules, 120; 6.2 Experimental Basis of the Quantum Theory, 122; 6.3 The Bohr Theory of the Hydrogen Atom, 126; 6.4 Waves and Particles, 128; 6.5 Electron Arrangements in Atoms, 135; 6.6 Experimental Support for Electron Configurations, 146; Problems, 148

7
THE PERIODIC TABLE AND THE PROPERTIES OF ELEMENTS
7.1 Structure of the Periodic Table; Vertical Relationships, 151; 7.2 Correlation with Electron Configuration; Horizontal Relationships, 153; 7.3 Trends in Atomic Properties, 155; 7.4 Predictions Based an the Periodic Table, 160; 7.5 Sources of the Elements, 162; Historical Perspective an the Periodic Table, 167 Problems, 170

8
CHEMICAL BONDING
8.1 Ionic Bonding, 173; 8.2 Nature of the Covalent Bond, 179; 8.3 Properties of the Covalent Bond, 182; 8.4 Lewis Structures; The Octet Rule, 186; 8.5 Molecular Geometry, 191; 8.6 Hybrid Atomic Orbitals, 196: 8.7 Molecular Orbitals, 199; Problems, 204

9
PHYSICAL PROPERTIES AS RELATED TO STRUCTURE
9.1 lonic Compounds, 208; 9.2 Molecular Substances, 210; 9.3 Macromolecular Substances, 217; 9.4 Metals, 222; 9.5 Summary, 224; Problems, 225

10
AN INTRODUCTION TO ORGANIC CHEMISTRY
10.1 Nature of Organic Substances, 227; 10.2 Hydrocarbons, 228; 10.3 Sources of Hydrocarbons, 239; 10.4 Oxygen-Containing Compounds, 245; 10.5 Some Halogen-Containing Organic Compounds, 252; Problems, 253


11
LIOUIDS AND SOLIDS; PHASE CHANGES
11.1 Nature of the Liquid State, 256; 11.2 Liquid-Vapor Equilibrium, 257; 11.3 Nature of the Solid State, 266; 11.4 Phase Equilibria, 273; 11.5 Nonequilibrium Phase Changes, 278; Problems, 279

12
SOLUTIONS
12.1 Introduction, 283; 12.2 Concentration Units, 285; 12.3 Principles of Solubility, 288; 12.4 Effect of Temperature and Pressure an Solubility, 291; 12.5 Colligative Properties of Nonelectrolyte Solutions, 294; Problems, 301

13
WATER, PURE AND OTHERWISE
13.1 Water As a Solvent; Electrolyte Solutions, 306; 13.2 Natural Sources of Water, 312; Water Pollution, 314; 13.4 Water Purification, 321; Problems, 330

14
SPONTANEITY OF REACTION; AG AND .A S
14.1 Criteria of Spontaneity. Useful work, 333; 14.2 Free Energy Change, AG, 337; 14.3 Entropy Change, AS, 340; 14.4 The GibbsHelmholtz Equation, 344; Historical Perspective: J. Willard Gibbs, 349 Problems, 350

15
CHEMICAL EQUILIBRIUM IN GASEOUS SYSTEMS
15.1 The N204-NO2 Equilibrium System. Concept of K, 356; 15.2 General Form and Properties of K„ 358; 15.3 Applications of K, 361; 15.4 Effect of Changes in Conditions upon the Position of an Equilibrium, 365; 15.5 Relation Between the Free Energy Change and the Equilibrium Constant, 371; Problems, 373

16
RATES OF REACTION
16.1 Meaning of Reaction Rate, 377; 16.2 Dependence of Reaction Rate upon Concentration, 379; 16.3 Dependence of Reaction Rate upon Temperature, 387; 16.4 Catalysis, 390; 16.5 Collision Theory of Reaction Rates. 393: 16.6 Reaction Mechanisms. 395: Problems, 400

17
- THE ATMOSPHERE 404
17.1 The Composition of the Atmosphere, 404; 17.2 Nitrogen, 406; 17.3 Oxygen, 409; 17.4 The Noble Gases, 413; 17.5 Carbon Dioxide, 414; 17.6 Water Vapor, 415; 17.7 The Upper Atmosphere, 417; 17.8 Air Pollution, 419; Problems, 427

18
PRECIPITATION REACTIONS 431
18.1 Net Tonic Equations, 431; 18.2 Solubilities of lonic Compounds, 433; 18.3 Solubility Equilibria. 435; 18.4 Precipitation Reactions in Analytical Chemistry, 439; 18.5 Precipitation Reactions in Inorganic Preparations, 442; Problems, 443

19
ACIDS AND BASES 447
19.1 The Dissociation of Water; Nature of Acids and Bases, 447; 19.2 pH, 488; 19.3 Strong Acids and Bases, 450; 19.4 Weak Acids, 452; 19.5 Weak Bases, 457; 19.6 Acid-Base Properties of Salt Solutions, 461; 19.7 General Theories of Acids and Bases, 463; Historical Perspective: G. N. Lewis, 466 Problems, 467

20
ACID-BASE REACTIONS 470
20.1 Types of Acid-Base Reactions, 470; 20.2 Acid-Base Titrations, 476; 20.3 Buffers, 483; 20.4 Application of Acid-Base Reactions in Inorganic Syntheses, 486; 20.5 Applications of Acid-Base Reactions in Qualitative Analysis, 488; 20.6 An Industrial Application of AcidBase Reactions: The Solvay Process, 491; Problems, 494

21
COMPLEX IONS; COORDINATION COMPOUNDS 498
21.1 Structures of Coordination Compounds. Charges of Complex Ions, 499; 21.2 Composition of Complex Ions, 501; 21.3 Geometry of Complex Ions, 505; 21.4 Electronic Structure of Complex Ions, 509; 21.5 Rate of Complex Ion Formation, 515; 21.6 Complex Ion Equilibria, 516; 21.7 Complex Ions in Analytical Chemistry, 517; Problems, 521

22
OXIDATION AND REDUCTION: ELECTROCHEMICAL CELLS 524
22.1 Oxidation Number, 525; 22.2 Balancing Oxidation-Reduction Equations, 529; 22.3 Electrolytic Cells, 533; 22.4 Voltaic Cells, 541; Historical Perspective: Michael Faraday, 547 Problems, 549

17
THE ATMOSPHERE 404
17.1 The Composition of the Atmosphere, 404; 17.2 Nitrogen, 406; 17.3 Oxygen, 409; 17.4 The Noble Gases, 413; 17.5 Carbon Dioxide, 414; 17.6 Water Vapor, 415; 17.7 The Upper Atmosphere, 417; 17.8 Air Pollution, 419; Problems, 427

18
PRECIPITATION REACTIONS 431
18.1 Net Tonic Equations, 431; 18.2 Solubilities of lonic Compounds, 433; 18.3 Solubility Equilibria. 435; 18.4 Precipitation Reactions in Analytical Chemistry, 439; 18.5 Precipitation Reactions in Inorganic Preparations, 442; Problems, 443

19
ACIDS AND BASES 447
19.1 The Dissociation of Water; Nature of Acids and Bases, 447; 19.2 pH, 488; 19.3 Strong Acids and Bases, 450; 19.4 Weak Acids, 452; 19.5 Weak Bases, 457; 19.6 Acid-Base Properties of Salt Solutions, 461; 19.7 General Theories of Acids and Bases, 463; Historical Perspective: G. N. Lewis, 466 Problems, 467

20
ACID-BASE REACTIONS 470
20.1 Types of Acid-Base Reactions, 470; 20.2 Acid-Base Titrations, 476; 20.3 Buffers, 483; 20.4 Application of Acid-Base Reactions in Inorganic Syntheses, 486; 20.5 Applications of Acid-Base Reactions in Qualitative Analysis, 488; 20.6 An Industrial Application of AcidBase Reactions: The Solvay Process, 491; Problems, 494

21
COMPLEX IONS; COORDINATION COMPOUNDS 498
21.1 Structures of Coordination Compounds. Charges of Complex Ions, 499; 21.2 Composition of Complex Ions, 501; 21.3 Geometry of Complex Ions, 505; 21.4 Electronic Structure of Complex Ions, 509; 21.5 Rate of Complex Ion Formation, 515; 21.6 Complex Ion Equilibria, 516; 21.7 Complex Ions in Analytical Chemistry, 517; Problems, 521

22
OXIDATION AND REDUCTION: ELECTROCHEMICAL CELLS 524
22.1 Oxidation Number, 525; 22.2 Balancing Oxidation-Reduction Equations, 529; 22.3 Electrolytic Cells, 533; 22.4 Voltaic Cells, 541; Historical Perspective: Michael Faraday, 547 Problems, 549

23
OXIDATION-REDUCTION REACTIONS: SPONTANEITY AND
EXTENT 553
23.1 Standard Potentials, 553; 23.2 Spontaneity and Extent of Redox Reactions, 558; 23.3 Effect of Concentration an Voltage, 562; 23.4 Strong Oxidizing Agents, 566; 23.5 Oxygen; The Corrosion of Iron, 571; 23.6 Redox Reactions in Analytical Chemistry, 574; Problems, 576

24
NUCLEAR REACTIONS 580
24.1 Radioactivity, 580; 24.2 Rate of Radioactive Decay, 589; 24.3 Mass-Energy Relations, 592; 24.4 Nuclear Fission, 596; 24.5 Nuclear Fusion, 600; Problems, 603

25
POLYMERS: NATURAL AND SYNTHETIC 607
25.1 Synthetic Polymers: Addition Type, 608; 25.2 Synthetic Poly
mers: Condensation Type, 614; 25.3 Natural Polymers: Carbohy
drates, 618; 25.4 Natural Polymers: Proteins, 623; Problems, 633

Appendix 1
CONSTANTS, PROPERTIES OF WATER, AND UNIT
CONVERSIONS A.1

Appendix 2
ATOMIC AND IONIC RADII A.8

Appendix 3
NOMENCLATURE OF INORGANIC COMPOUNDS A.10

Appendix 4
EXPONENTS AND LOGARITHMS A.14

Appendix 5
ANSWERS TO PROBLEMS A.24

GLOSSARY A.41

INDEX

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