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The Study Guide reflects the unique problem-solving approach taken by the Chemical Principles text. The new edition of the Study Guide includes many new worked out examples.

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• Note: Chapters 2–21 include Discussion Questions and Exercises
• 1 Chemists and Chemistry
• 1.1 Thinking Like a Chemist
• 1.2 A Real-World Chemistry Problem
• 1.3 The Scientific Method
• 1.4 Industrial Chemistry
• 1.5 Polyvinyl Chloride (PVC): Real-World Chemistry
• 2 Atoms, Molecules, and Ions
• 2.1 The Early History of Chemistry
• 2.2 Fundamental Chemical Laws
• 2.3 Dalton's Atomic Theory
• 2.4 Cannizzaro's Interpretation
• 2.5 Early Experiments to Characterize the Atom
• 2.6 The Modern View of Atomic Structure: An Introduction
• 2.7 Molecules and Ions
• 2.8 An Introduction to the Periodic Table
• 2.9 Naming Simple Compounds
• 3 Stoichiometry
• 3.1 Atomic Masses
• 3.2 The Mole
• 3.3 Molar Mass
• 3.4 Percent Composition of Compounds
• 3.5 Determining the Formula of a Compound
• 3.6 Chemical Equations
• 3.7 Balancing Chemical Equations
• 3.8 Stoichiometric Calculations: Amounts of Reactants and Products
• 3.9 Calculations Involving a Limiting Reactant
• 4 Types of Chemical Reactions and Solution Stoichiometry
• 4.1 Water, the Common Solvent
• 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes
• 4.3 The Composition of Solutions
• 4.4 Types of Chemical Reactions
• 4.5 Precipitation Reactions
• 4.6 Describing Reactions in Solution
• 4.7 Selective Precipitation
• 4.8 Stoichiometry of Precipitation Reactions
• 4.9 Acid-Base Reactions
• 4.10 Oxidation-Reduction Reactions
• 4.11 Balancing Oxidation-Reduction Equations
• 4.12 Simple Oxidation-Reduction Titrations
• 5 Gases
• 5.1 Early Experiments
• 5.2 The Gas Laws of Boyle, Charles, and Avogadro
• 5.3 The Ideal Gas Law
• 5.4 Gas Stoichiometry
• 5.5 Dalton's Law of Partial Pressures
• 5.6 The Kinetic Molecular Theory of Gases
• 5.7 Effusion and Diffusion
• 5.8 Collisions of Gas Particles with the Container Walls
• 5.9 Intermolecular Collisions
• 5.10 Real Gases
• 5.11 Chemistry in the Atmosphere
• 6 Chemical Equilibrium
• 6.1 The Equilibrium Condition
• 6.2 The Equilibrium Constant
• 6.3 Equilibrium Expressions Involving Pressures
• 6.4 The Concept of Activity
• 6.5 Heterogeneous Equilibria
• 6.6 Applications of the Equilibrium Constant
• 6.7 Solving Equilibrium Problems
• 6.8 Le Chacirc;telier's Principle
• 6.9 Equilibria Involving Real Gases
• 7 Acids and Bases
• 7.1 The Nature of Acids and Bases
• 7.2 Acid Strength
• 7.3 The pH Scale
• 7.4 Calculating the pH of Strong Acid Solutions
• 7.5 Calculating the pH of Weak Acid Solutions
• 7.6 Bases
• 7.7 Polyprotic Acids
• 7.8 Acid-Base Properties of Salts
• 7.9 Acid Solutions in Which Water Contributes to the H+ Concentration
• 7.10 Strong Acid Solutions in Which Water Contributes to the H+ Concentration
• 7.11 Strategy for Solving Acid-Base Problems: A Summary
• 8 Applications of Aqueous Equilibria
• 8.1 Solutions of Acids or Bases Containing a Common Ion
• 8.2 Buffered Solutions
• 8.3 Exact Treatment of Buffered Solutions
• 8.4 Buffer Capacity
• 8.5 Titrations and pH Curves
• 8.6 Acid-Base Indicators
• 8.7 Titration of Polyprotic Acids
• 8.8 Solubility Equilibria and the Solubility Product
• 8.9 Precipitation and Qualitative Analysis
• 8.10 Complex Ion Equilibria
• 9 Energy, Enthalpy, and Thermochemistry
• 9.1 The Nature of Energy
• 9.2 Enthalpy
• 9.3 Thermodynamics of Ideal Gases
• 9.4 Calorimetry
• 9.5 Hess's Law
• 9.6 Standard Enthalpies of Formation
• 9.7 Present Sources of Energy
• 9.8 New Energy Sources
• 10 Spontaneity, Entropy, and Free Energy
• 10.1 Spontaneous Processes and Entropy
• 10.2 The Isothermal Expansion and Compression of an Ideal Gas
• 10.3 The Definition of Entropy
• 10.4 Entropy and Physical Changes
• 10.5 Entropy and the Second Law of Thermodynamics
• 10.6 The Effect of Temperature on Spontaneity
• 10.7 Free Energy
• 10.8 Entropy Changes in Chemical Reactions
• 10.9 Free Energy and Chemical Reactions
• 10.10 The Dependence of Free Energy on Pressure
• 10.11 Free Energy and Equilibrium
• 10.12 Free Energy and Work
• 10.13 Reversible and Irreversible Processes: A Summary
• 11 Electrochemistry
• 11.1 Galvanic Cells
• 11.2 Standard Reduction Potentials
• 11.3 Cell Potential, Electrical Work, and Free Energy
• 11.4 Dependence of the Cell Potential on Concentration
• 11.5 Batteries
• 11.6 Corrosion
• 11.7 Electrolysis
• 11.8 Commercial Electrolytic Processes
• 12 Quantum Mechanics and Atomic Theory
• 12.1 Electromagnetic Radiation
• 12.2 The Nature of Matter
• 12.3 The Atomic Spectrum of Hydrogen
• 12.4 The Bohr Model
• 12.5 The Quantum Mechanical Description of the Atom
• 12.6 The Particle in a Box
• 12.7 The Wave Equation for the Hydrogen Atom
• 12.8 The Physical Meaning of a Wave Function
• 12.9 The Characteristics of Hydrogen Orbitals
• 12.10 Electron Spin and the Pauli Principle
• 12.11 Polyelectronic Atoms
• 12.12 The History of the Periodic Table
• 12.13 The Aufbau Principle and the Periodic Table
• 12.14 Further Development of the Polyelectronic Model
• 12.15 Periodic Trends in Atomic Properties
• 12.16 The Properties of a Group: The Alkali Metals
• 13 Bonding: General Concepts
• 13.1 Types of Chemical Bonds
• 13.2 Electronegativity
• 13.3 Bond Polarity and Dipole Moments
• 13.4 Ions: Electron Configurations and Sizes
• 13.5 Formation of Binary Ionic Compounds
• 13.6 Partial Ionic Character of Covalent Bonds
• 13.7 The Covalent Chemical Bond: A Model
• 13.8 Covalent Bond Energies and Chemical Reactions
• 13.9 The Localized Electron Bonding Model
• 13.10 Lewis Structure
• 13.11 Resonance
• 13.12 Exceptions to the Octet Rule
• 13.13 Molecular Structure: The VSEPR Model
• 14 Covalent Bonding: Orbitals
• 14.1 Hybridization and the Localized Electron Model
• 14.2 The Molecular Orbital Model
• 14.3 Bonding in Homonuclear Diatomic Molecules
• 14.4 Bonding in Heteronuclear Diatomic Molecules
• 14.5 Combining the Localized Electron and Molecular Orbital Models
• 14.6 Orbitals: Human Invention
• 14.7 Molecular Spectroscopy
• 15 Chemical Kinetics
• 15.1 Reaction Rates
• 15.2 Rate Laws: An Introduction
• 15.3 Determining the Form of the Rate Law
• 15.4 The Integrated Rate Law
• 15.5 Rate Laws: A Summary
• 15.6 Reaction Mechanisms
• 15.7 The Steady-State Approximation
• 15.8 A Model for Chemical Kinetics
• 15.9 Catalysis
• 16 Liquids and Solids
• 16.1 Intermolecular Forces
• 16.2 The Liquid State
• 16.3 An Introduction to Structures and Types of Solids
• 16.4 Structure and Bonding in Metals
• 16.5 Carbon and Silicon: Network Atomic Solids
• 16.6 Molecular Solids
• 16.7 Ionic Solids
• 16.8 Structures of Actual Ionic Solids
• 16.9 Lattice Defects
• 16.10 Vapor Pressure and Changes of State
• 16.11 Phase Diagrams
• 17 Properties of Solutions
• 17.1 Solution Composition
• 17.2 The Thermodynamics of Solution Formation
• 17.3 Factors Affecting Solubility
• 17.4 The Vapor Pressures of Solutions
• 17.5 Boiling-Point Elevation and Freezing-Point Depression
• 17.6 Osmotic Pressure
• 17.7 Colligative Properties of Electrolyte Solutions
• 17.8 Colloids
• 18 The Representative Elements: Groups 1A Through 4A
• 18.1 A Survey of the Representative Elements
• 18.2 The Group 1A Elements
• 18.3 The Chemistry of Hydrogen
• 18.4 The Group 2A Elements
• 18.5 The Group 3A Elements
• 18.6 The Group 4A Elements
• 19 The Representative Elements: Groups 5A Through 8A
• 19.1 The Group 5A Elements
• 19.2 The Chemistry of Nitrogen
• 19.3 The Chemistry of Phosphorus
• 19.4 The Group 6A Elements
• 19.5 The Chemistry of Oxygen
• 19.6 The Chemistry of Sulfu