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

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

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