Chapter 1. Elements and Compounds.
　1.1 Chemistry: A Definition.
　1.2 Elements, Compounds, and Mixtures.
　1.3 Atomic Symbols.
　1.4 Chemical Formulas.
　1.5 Evidence for the Existence of Atoms.
　1.6 The Structure of Atoms.
　1.7 Atomic Number and Mass Number.
　1.8 Isotopes.
　1.9 The Difference between Atoms and Ions.
　1.10 Polyatomic Ions.
　1.11 Predicting the Formulas of Ionic Compounds.
　1.12 The Periodic Table.
　1.13 The Macroscopic, Atomic, and Symbolic Worlds of Chemistry.
　1.14 The Mass of an Atom.
　1.15 The Mole as the Bridge between the Macroscopic and Atomic Scales.
　1.16 The Mole as a Collection of Atoms.
　1.17 Converting Grams into Moles and Number of Atoms.
　1.18 The Mole as a Collection of Molecules.
　1.19 Percent Mass.
　1.20 Determining the Formula of a Compound.
　1.21 Elemental Analysis.
　Problems.
Chapter 2. The Mole: The Link between the Macroscopic and the Atomic World of 　Chemistry.
　2.1 Chemical Reactions and the Law of Conservation of Atoms.
　2.2 Chemical Equations as a Representation of Chemical Reactions.
　2.3 Two Views of Chemical Equations: Molecules Versus Moles.
　2.4 Balancing Chemical Equations.
　2.5 Mole Ratios and Chemical Equations.
　2.6 Stoichiometry.
　Chemistry in the World Around Us: The Stoichiometry of the Breathalyzer.
　2.7 The Nuts and Bolts of Limiting Reagents.
　2.8 Density.
　2.9 Solute, Solvent, and Solution.
　2.10 Concentration.
　2.11 Molarity as a Way of Counting Particles in Solution.
　2.12 Dilution Calculations.
　2.13 Solution Stoichiometry.
　Problems.
Chapter 3. The Structure of the Atom.
　3.1 Rutherford’s Model of the Atom.
　3.2 Particles and Waves.
　3.3 Light and Other Forms of Electromagnetic Radiation.
　3.4 Atomic Spectra.
　3.5 Quantization of Energy.
　3.6 The Bohr Model of the Atom.
　3.7 The Energy States of the Hydrogen Atom.
　Chemistry in the World Around Us: Color.
　3.8 The First Ionization Energy.
　3.9 The Shell Model.
　3.10 The Shell Model and the Periodic Table.
　3.11 Photoelectron Spectroscopy and the Structure of Atoms.
　3.12 Electron Configurations from Photoelectron Spectroscopy.
　3.13 Allowed Combinations of Quantum Numbers.
　3.14 Shells and Subshells of Orbitals.
　3.15 Orbitals and the Pauli Exclusion Principle.
　3.16 Predicting Electron Configurations.
　3.17 Electron Configurations and the Periodic Table.
　3.18 Electron Configurations and Hund’s Rules.
　3.19 The Sizes of Atoms: Metallic Radii.
　3.20 The Sizes of Atoms: Covalent Radii.
　3.21 The Relative Sizes of Atoms and Their Ions.
　3.22 Patterns in Ionic Radii.
　3.23 Second, Third, Fourth, and Higher Ionization Energies.
　3.24 Average Valence Electron Energy (AVEE).
　3.25 AVEE and Metallicity.
　Problems.
Chapter 4. The Covalent Bond.
Chapter 5. Ionic and Metallic Bonds.
Chapter 6. Gases.
Chapter 7. Making and Breaking of Bonds.
Chapter 8. Liquids and Solutions.
Chapter 9. Solids.
Chapter 10. An Introduction to Kinetics and Equilibrium.
Chapter 11. Acids and Bases.
Chapter 12. Oxidation–Reduction Reactions.
Chapter 13. Chemical Thermodynamics.
Chapter 14. Kinetics.
Chapter 15. Nuclear Chemistry.
Chapter 16. Chemical Analysis.
Appendix A.
Appendix B.
Modules (available at www.wiley.com/college/spencer).
　Module 1. Chemistry of the Nonmetals.
　Module 2. Transition Metal Chemistry.
　Module 3. Complex Ion Equilibria.
　Module 4. Organic Chemistry: Structure and Nomenclature of Hydrocarbons.
　Module 5. Organic Chemistry: Functional Groups.
　Module 6. Organic Chemistry: Reaction Mechanisms.
　Module 7. Polymer Chemistry.
　Module 8. Biochemistry.