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
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Chemical Principles. Third Edition