PART I: GENERAL CHEMISTRY.
1. Basic Concepts About Matter.

1-1Chemistry: The Study of Matter

1-2Physical States of Matter

1-3Properties of Matter

1-4Changes in Matter

1-5Pure Substances and Mixtures

1-6Elements and Compounds

1-7Discovery and Abundance of the Elements

1-8Names and Chemical Symbols of the Elements

1-9Atoms and Molecules

1-10Chemical Formulas

2. Measurements in Chemistry.

2-1Measurement Systems

2-2Metric System Units

Metric Length Units

Metric Mass Units

Metric Volume Units

2-3Exact and Inexact Numbers

2-4Uncertainty in Measurement and Significant Figures

Origin of Measurement Uncertainty

Guidelines for Determining Significant Figures

2-5Significant Figures and Mathematical Operations

Rounding Off Numbers

Operational Rules

2-6Scientific Notation

Converting from Decimal to Scientific Notation

Significant Figures and Scientific Notation

Multiplication and Division in Scientific Notation

Calculators and Scientific Notation

Uncertainty and Scientific Notation

2-7Conversion Factors

Conversion Factors Within a System of Units

Conversion Factors between Systems of Units

2-8Dimensional Analysis

2-9Density

Density as a Conversion Factor

2-10Temperature Scales

Conversions Between Temperature Scales

Temperature Readings and Significant Figures

3. Atomic Structure and the Periodic Table.

  • 3-1Internal Structure of an Atom
  • Arrangement of Subatomic Particles Within an Atom
  • Charge Neutrality of an Atom
  • Size Relationships Within an Atom
  • 3-2Atomic Number and Mass Number
  • Electrons and Chemical Properties
  • 3-3Isotopes and Atomic Masses
  • Isotopes
  • Atomic Masses
  • 3-4The Periodic Law and the Periodic Table
  • Groups and Periods of Elements
  • The Shape of the Periodic Table
  • 3-5Metals and Nonmetals
  • Periodic Table Locations for Metals and Nonmetals
  • 3-6Electron Arrangements Within Atoms
  • Electron Shells
  • Electron Subshells
  • Electron Orbitals
  • Electron Spin
  • 3-7Electron Configurations and Orbital Diagrams
  • Subshell Energy Order
  • Writing Electron Configurations and Orbital Diagrams
  • 3-8The Electronic Basis for the Periodic Law and the Periodic Table
  • Electron Configurations and the Periodic Law
  • Electron Configurations and the Periodic Table
  • 3-9Classification of the Elements

4. Chemical Bonding: The Ionic Bond Model.

  • 4-1Chemical Bonds
  • 4-2Valence Electrons and Lewis Symbols
  • 4-3The Octet Rule
  • 4-4The Ionic Bond Model
  • 4-5The Sign and Magnitude of Ionic Charge
  • Isoelectronic Species
  • 4-6Lewis Structures for Ionic Compounds
  • 4-7Chemical Formulas for Ionic Compounds
  • 4-8The Structure of Ionic Compounds
  • 4-9Recognizing and Naming Binary Ionic Compounds
  • 4-10Polyatomic Ions
  • 4-11Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions

5. Chemical Bonding: The Covalent Bond Model.

  • 5-1The Covalent Bond Model
  • 5-2Lewis Structures for Molecular Compounds
  • 5-3Single, Double, and Triple Covalent Bonds
  • 5-4Valence Electrons and Number of Covalent Bonds Formed
  • 5-5Coordinate Covalent Bonds
  • 5-6Systematic Procedures for Drawing Lewis Structures
  • 5-7Bonding in Compounds with Polyatomic Ions Present
  • 5-8Molecular Geometry
  • Electron Groups
  • Molecules with Two VSEPR Electron Groups
  • Molecules with Three VSEPR Electron Groups
  • Molecules with Four VSEPR Electron Groups
  • Molecules with More Than One Central Atom
  • 5-9Electronegativity
  • 5-10Bond Polarity
  • Bond Polarity and Fractional Charges
  • Bond Classification Based on Electronegativity Difference
  • 5-11Molecular Polarity
  • 5-12Recognizing and Naming Binary Molecular Compounds

6. Chemical Calculations: Formula Masses, Moles, and Chemical Equations.

  • Chapter Introduction
  • 6-1Formula Masses
  • 6-2The Mole: A Counting Unit for Chemists
  • 6-3The Mass of a Mole
  • 6-4Chemical Formulas and the Mole Concept
  • 6-5The Mole and Chemical Calculations
  • 6-6Writing and Balancing Chemical Equations
  • Conventions Used in Writing Chemical Equations
  • Guidelines for Balancing Chemical Equations
  • 6-7Chemical Equations and the Mole Concept
  • 6-8Chemical Calculations Using Chemical Equations
  • 6-9Yields: Theoretical, Actual, and Percent

7. Gases, Liquids, and Solids.

  • 7-1The Kinetic Molecular Theory of Matter
  • 7-2Kinetic Molecular Theory and Physical States
  • 7-3Gas Law Variables
  • Pressure Readings and Significant Figures
  • 7-4Boyle’s Law: A Pressure–Volume Relationship
  • 7-5Charles’s Law: A Temperature–Volume Relationship
  • 7-6The Combined Gas Law
  • 7-7The Ideal Gas Law
  • 7-8Dalton’s Law of Partial Pressures
  • 7-9Changes of State
  • 7-10Evaporation of Liquids
  • Rate of Evaporation and Temperature
  • 7-11Vapor Pressure of Liquids
  • 7-12Boiling and Boiling Point
  • Conditions That Affect Boiling Point
  • 7-13Intermolecular Forces in Liquids
  • Dipole–Dipole Interactions
  • Hydrogen Bonds
  • London Forces

8. Solutions.

  • 8-1Characteristics of Solutions
  • 8-2Solubility
  • Effect of Temperature on Solubility
  • Effect of Pressure on Solubility
  • Saturated, Supersaturated, and Unsaturated Solutions
  • Aqueous and Nonaqueous Solutions
  • 8-3Solution Formation
  • Factors Affecting the Rate of Solution Formation
  • 8-4Solubility Rules
  • 8-5Percent Concentration Units
  • Percent Concentration
  • Using Percent Concentrations as Conversion Factors
  • Clinical Laboratory Concentration Units
  • 8-6Molarity Concentration Unit
  • Using Molarity as a Conversion Factor
  • 8-7Dilution
  • 8-8Colloidal Dispersions and Suspensions
  • 8-9Colligative Properties of Solutions
  • Vapor-Pressure Lowering
  • Boiling-Point Elevation
  • Freezing-Point Depression
  • 8-10Osmosis and Osmotic Pressure
  • Osmosis
  • Osmotic Pressure
  • Osmolarity
  • Hypotonic, Hypertonic, and Isotonic Solutions
  • Concentration Units for Isotonic Solutions

9. Chemical Reactions.

  • 9-1Types of Chemical Reactions
  • Combination Reactions
  • Decomposition Reactions
  • Displacement Reactions
  • Exchange Reactions
  • Combustion Reactions
  • 9-2Redox and Nonredox Chemical Reactions
  • 9-3Terminology Associated with Redox Processes
  • Oxidizing Agents and Reducing Agents
  • 9-4Collision Theory and Chemical Reactions
  • Molecular Collisions
  • Activation Energy
  • Collision Orientation
  • 9-5Exothermic and Endothermic Chemical Reactions
  • 9-6Factors That Influence Chemical Reaction Rates
  • Physical Nature of Reactants
  • Reactant Concentrations
  • Reaction Temperature
  • Presence of Catalysts
  • 9-7Chemical Equilibrium
  • 9-8Equilibrium Constants
  • Temperature Dependence of Equilibrium Constants
  • Equilibrium Constant Values and Reaction Completeness
  • 9-9Altering Equilibrium Conditions: Le Châtelier’s Principle
  • Concentration Changes
  • Temperature Changes
  • Pressure Changes
  • Addition of Catalysts

10. Acids, Bases, and Salts.

  • 10-1Arrhenius Acid–Base Theory
  • 10-2Brønsted–Lowry Acid–Base Theory
  • Generalizations about Brønsted–Lowry Acids and Bases
  • Conjugate Acid–Base Pairs
  • Amphiprotic Substances
  • 10-3Mono-, Di-, and Triprotic Acids
  • 10-4Strengths of Acids and Bases
  • 10-5Ionization Constants for Acids and Bases
  • 10-6Salts
  • 10-7Acid–Base Neutralization Chemical Reactions
  • Balancing Acid–Base Neutralization Equations
  • 10-8Self-Ionization of Water
  • Ion Product Constant for Water
  • Acidic, Basic, and Neutral Solutions
  • 10-9The pH Concept
  • Integral pH Values
  • Nonintegral pH Values
  • pH Values and Hydronium Ion Concentration
  • Interpreting pH Values
  • pH Values for Human Body Tissues and Acid Rain
  • 10-10The pKaMethod for Expressing Acid Strength
  • 10-11The pH of Aqueous Salt Solutions
  • Types of Salt Hydrolysis
  • Chemical Equations for Salt Hydrolysis Reactions
  • 10-12Buffers
  • 10-13The Henderson–Hasselbalch Equation
  • 10-14Electrolytes
  • 10-15Equivalents and Milliequivalents of Electrolytes
  • Equivalent and Milliequivalent Concentration Units
  • Charge Balance in Electrolytic Solutions
  • 10-16Acid–Base Titrations

11. Nuclear Chemistry.

  • 11-1Stable and Unstable Nuclides
  • 11-2The Nature of Radioactive Emissions
  • 11-3Equations for Radioactive Decay
  • Alpha Particle Decay
  • Beta Particle Decay
  • Gamma Ray Emission
  • 11-4Rate of Radioactive Decay
  • 11-5Transmutation and Bombardment Reactions
  • Synthetic Elements
  • 11-6Radioactive Decay Series
  • 11-7Detection of Radiation
  • 11-8Chemical Effects of Radiation
  • 11-9Biochemical Effects of Radiation
  • Alpha Particle Effects
  • Beta Particle Effects
  • Gamma Radiation Effects
  • Comparisons of Effects of Various Types of Radiations
  • Short-Term Radiation Exposure
  • 11-10Sources of Radiation Exposure
  • 11-11Nuclear Medicine
  • Diagnostic Uses for Radionuclides
  • Therapeutic Uses for Radionuclides
  • 11-12Nuclear Fission and Nuclear Fusion
  • Fission Reactions
  • Fusion Reactions
  • 11-13Nuclear and Chemical Reactions Compared

PART II: ORGANIC CHEMISTRY.
12. Saturated Hydrocarbons.
13. Unsaturated Hydrocarbons.
14. Alcohols, Phenols, and Ethers.
15. Aldehydes and Ketones.
16. Carboxylic Acids, Esters, and Other Acid Derivatives.
17. Amines and Amides.
PART III: BIOLOGICAL CHEMISTRY.
18. Carbohydrates.
19. Lipids.
20. Proteins.
21. Enzymes and Vitamins.
22. Nucleic Acids.
23. Biochemical Energy Production.
24. Carbohydrate Metabolism.
25. Lipid Metabolism.
26. Protein Metabolism.