Chemical Principles. Third Edition

Written by: Richard E Dickerson, Harry B. Gray and Gilbert P. Haight

Since the librarians at Cal Tech have taken the time to scan and include this book in their online library, I suspect it still offers something helpful for students studying general chemistry. It was written in 1979 by Richard E Dickerson, Harry B. Gray and Gilbert P. Haight. They designed their textbook to be used by both science and non-science majors as a general university chemistry course.

Each chapter of Chemical Principles begins with a list of key concepts. They end with a chapter summary and 20-40 self-study questions. In some chapters, the questions have been paired so that the solved odd-numbered problem is similar to the even-numbered problem that instructors might assign students.

It includes a number of “survey chapters” that introduce the sub-specialties within chemistry like inorganic, kinetic chemistry, nuclear, organic, coordination chemistry and biochemistry.

Table of Contents for Chemical Principles, General Chemistry Textbook

Preface
Chapter 1: Atoms, Molecules, and Ions: 1-1 The Structure of Atoms; 1-2 Isotopes; 1-3 Molecules; 1-4 Forces Between Molecules; 1-5 Molecules and Moles; l-6 Ions; 1-7 Ions in Solution; 1-8 Gaseous Ions
Chapter 2: Conservation of Mass and Energy: 2-1 Atomic Weights, Molecular Weights, and Moles; 2-2 Chemical Analyses: Percent Composition and Empirical Formulas; 2-3 Chemical Equations; 2-4 Calculations of Reaction Yields; 2-5 Solutions as Chemical Reagents; 2-6 Heats of Reaction: Conservation of Energy; 2-7 Conservation Principles
Chapter 3: Gas Laws and the Kinetic Theory: 3-l Avogadro’s Law; 3—2 The Pressure of a Gas; 3-3 Boyle’s Law Relating Pressure and Volume; 3-4 Charles’ Law Relating Volume and Temperature; 3-5 The Combined Gas Law; 3—6 The Kinetic Molecular Theory of Gases; 3-7 Predictions of the Kinetic Molecular Theory; 3-8 Real Gases and Deviations from the Ideal Gas Law
Chapter 4: Will it React? An introduction to Chemical Equilibrium: 4-1 Spontaneous Reactions; 4—2 Equilibrium and the Equilibrium Constant; 4-3 General Form of the Equilibrium Constant; 4-4 Natural Atomic Weights; 4-5 Units and Equilibrium Constants; 4—6 Equilibria Involving Gases with Liquids or Solids; 4-7 Factors Affecting Equilibrium: Le Chatelier’s Principle
Chapter 5: Solution Equilibria: Acids and Bases: 5-1 Equilibria in Aqueous Solutions; 5-2 Ionization of Water and the pH Scale; 5-3 Strong and Weak Acids; 5-4 Strong and Weak Bases; 5-5 Solutions of Strong Acids and Bases: Neutralization and Titration; 5-6 Equilibria with Weak Acids and Bases; 5-7 Weak Acids and Their Salts; 5-8 Salts of Weak Acids and Strong Bases: Hydrolysis; 5-9 Polyprotic Acids: Acids that Liberate More than One Hydrogen Ion; 5-10 Equilibria with Slightly Soluble Salts
Chapter 6: Are Atoms Real? From Democritus to Dulong and Petit: 6-1 The Concept of An Element; 6-2 Compounds, Combustion, and the Conservation of Mass; 6-3 Does a Compound Have a Fixed Composition?; 6-4 John Dalton and the Theory of Atoms; 6-5 Equal Numbers in Equal Volumes: Gay-Lussac and Avogadro; 6-6 Cannizzaro and a Rational Method of Calculating Atomic Weights; 6-7 Atomic Weights for the Heavy Elements: Dulong and Petit; 6-8 Combining Capacities, “Valence,” and Oxidation Number
Chapter 7: The Periodic Table: 7-1 Early Classiﬁcation Schemes; 7-2 The Basis for Periodic Classiﬁcation; 7-3 The Modern Periodic Table; 7-4 Periodicity of Chemical Properties as Illustrated by Binary Hydrides and Oxides
Chapter 8: Quantum Theory and Atomic Structure: 8-1 Rutherford and the Nuclear Atom; 8—2 The Quantization of Energy; 8-3 Bohr’s Theory of the Hydrogen Atom; 8-4 Particles of Light and Waves of Matter; 8-5 The Uncertainty Principle; 8-6 Wave Equations; 8-7 The Hydrogen Atom; 8-8 Many-Electron Atoms
Chapter 9: Electronic Structure and Atomic Properties: 9-1 Buildup of Many-Electron Atoms; 9-2 Types of Bonding; 9-3 Electronegativity
Chapter 10: Oxidation-Reduction and Chemical Properties: 10-1 Oxidation Numbers; 10-2 Oxidation-Reduction Reactions; 10-3 Balancing Oxidation-Reduction Equations; 10-4 Redox Titrations; 10-5 Oxidation and Reduction Potentials; 10-6 Chemical Properties: The s-Orbital Metals; 10-7 The Filling of the d Orbitals: Transition Metals; 10-8 The Filling of f Orbitals: Lanthanides and Actinides; 10-9 The p-Orbital or Representative Elements
Chapter 11: Lewis Structures and the VSEPR Method: 11-1 Lewis Structures; 11-2 Acidity of Oxyacids; 11-3 The VSEPR Method and Molecular Geometry
Chapter 12: Diatomic Molecules: 12-1 Molecular Orbitals; 12-2 Diatomic Molecules with One Type of Atom; 12-3 Diatomic Molecules with Different Atoms
Chapter 13: Polyatomic Molecules: 13-1 Localized Molecular Orbitals for BeH2, BH3, and CH4; 13-2 Hydrogen in Bridge Bonds; 13-3 Localized-Molecular-Orbital Theory for Molecules with Lone Electron Pairs; 13-4 Single and Multiple Bonds in Carbon Compounds; 13-5 Benzene and Delocalized Orbitals; 13-6 Polar and Nonpolar Polyatomic Molecules; 13-7 Molecular Spectroscopy
Chapter 14: Bonding in Solids and Liquids: 14-1 Elemental Molecular Solids; 14-2 Ionic Solids; 14-3 Molecular Solids and Liquids; 14-4 Metals; 14-5 Nonmetallic Network Solids; 14-6 The Framework of the Planet: Silicate Minerals
Chapter 15: Energy and Enthalpy in Chemical Systems: 15-1 Work, Heat, and Caloric; 15-2 The First Law of Thermodynamics; 15-3 Energy, Enthalpy, and Heat Capacity; 15-4 The First Law and Chemical Reactions; 15-5 Bond Energies
Chapter 16: Entropy, Free Energy, and Chemical Reactions: 16-1 Spontaneity, Reversibility, and Equilibrium; 16-2 Heat, Energy, and Molecular Motion; 16-3 Entropy and Disorder; 16-4 Third-Law Entropies and Chemical Intuition; 16-5 Free Energy and Spontaneity in Chemical Reactions; 16-6 Free Energy and Concentration
Chapter 17: Free Energy and Equilibrium: 17-1 The Properties of Equilibrium; 17-2 Reactions Involving Cases; 17-3 Le Chatelier’s Principle; 17-4 The Anatomy of a Reaction
Chapter 18: Equilibria Involving Liquids and Solids: 18-1 Melting, Evaporation, and Sublimation; 18-2 Free Energy of Vaporization and Vapor Pressure; 18-3 The Critical Point; 18-4 Phase Diagrams; 18-5 Solutions and Raoult’s Law; 18-6 Colligative Properties
Chapter 19: Oxidation-Reduction Equilibria and Electrochemistry: 19-1 Harnessing Spontaneous Reactions; 19-2 Electrochemical Cells; 19-3 Cell EMF and Free Energy; 19-4 Half-Reactions and Reduction Potentials; 19-5 The Effect of Concentration on Cell Voltage: The Nernst Equation; 19-6 Solubility Equilibria and Potentials; 19-7 Redox Chemistry Gone Astray: Corrosion
Chapter 20: Coordination Chemistry: 20-1 Properties of Transition-Metal Complexes; 20-2 Nomenclature for Coordination Compounds; 20-3 Theories of Bonding in Coordination Complexes; 20-4 Tetrahedral and Square Planar Coordination; 20-5 Equilibria Involving Complex Ions
Chapter 21: The Special Role of Carbon: 21-1 The Special Talents of Carbon; 21-2 The Chemistry of the Neighbors of Carbon; 21-3 Saturated Hydrocarbons or Alkanes; 21-4 Unsaturated Hydrocarbons; 21-5 Derivatives of Hydrocarbons: Functional Groups; 21-6 Aromatic Compounds; 21-7 Aromatic Compounds and the Absorption of Light; 21-8 Carbohydrates; 21-9 Proteins and Enzymes; 21-10 The Mechanism of Action of an Enzyme; 21-11 Energy and Metabolism in Living Systems
Chapter 22: Rates and Mechanisms of Chemical Reactions: 22-1 What Happens When Molecules React?; 22-2 Measurement of Reaction Rates; 22-3 Calculating Rate Constants from Molecular Information; 22-4 Complex Reactions; 22—5 Catalysis
Chapter 23: Nuclear Chemistry: 23-1 The Nucleus; 23-2 Nuclear Decay; 23-3 Stability Series; 23-4 Nuclear Reactions; 23-5 Applications of Nuclear Chemistry and Isotopes
Appendix 1: The Systeme Internationale (SI) of Units
Appendix 2: Physical Constants and Conversion Factors
Appendix 3: Standard Enthalpies and Free Energies of Formation,and Standard Third-Law Entropies, at 298 K
Appendix 4: Significant Figures and Exponential (Scientific) Notation
Appendix 5: A More Exact Treatment of Acid- Base Equilibria
Appendix 6: Answers to Odd-Numbered Problems
Index

Chemical Principles. Third Edition

Table of Contents for Chemical Principles, General Chemistry Textbook

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