Enhanced descriptions from Syndetics:

Authors Steven and Susan Zumdahl offer all the elements instructors need for their general chemistry course. They bring a conceptual approach to chemistry and integrate problem-solving skills throughout, helping students transition from theory to practice. A strong emphasis on models, real-world applications, and visual learning prevails throughout the text. The Seventh Edition seamlessly integrates the strengths of the Zumdahl approach through a comprehensive and interwoven print and technology program. Enhanced Sample Exercises, online homework problems, and Classroom Response System content help instructors assess conceptual understanding and problem-solving skills, while new animations and images support visual learning. In addition, Houghton Mifflin offers implementation services through our TeamUP program to help instructors and students get the most out of the text and its supplements.

Table of contents provided by Syndetics

• 1 Chemical Foundations
• 1.1 Chemistry: An Overview
• 1.2 The Scientific Method
• 1.3 Units of Measurement
• 1.4 Uncertainty in Measurement
• 1.5 Significant Figures and Calculations
• 1.6 Dimensional Analysis
• 1.7 Temperature
• 1.8 Density
• 1.9 Classification of Matter
• 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 Early Experiments to Characterize the Atom
• 2.5 The Modern View of Atomic Structure: An Introduction
• 2.6 Molecules and Ions
• 2.7 An Introduction to the Periodic Table
• 2.8 Naming Simple Compounds
• 3 Stoichiometry
• 3.1 Counting by Weighing
• 3.2 Atomic Masses
• 3.3 The Mole
• 3.4 Molar Mass
• 3.5 Percent Composition of Compounds
• 3.6 Determining the Formula of a Compound
• 3.7 Chemical Equations
• 3.8 Balancing Chemical Equations
• 3.9 Stoichiometric Calculations: Amounts of Reactants and Products
• 3.10 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 Stoichiometry of Precipitation Reactions
• 4.8 Acid-Base Reactions
• 4.9 Oxidation-Reduction Reactions
• 4.10 Balancing Oxidation-Reduction Equations
• 5 Gases
• 5.1 Pressure
• 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 Real Gases
• 5.9 Characteristics of Several Real Gases
• 5.10 Chemistry in the Atmosphere
• 6 Thermochemistry
• 6.1 The Nature of Energy
• 6.2 Enthalpy and Calorimetry
• 6.3 Hess's Law
• 6.4 Standard Enthalpies of Formation
• 6.5 Present Sources of Energy
• 6.6 New Energy Sources
• 7 Atomic Structure and Periodicity
• 7.1 Electromagnetic Radiation
• 7.2 The Nature of Matter
• 7.3 The Atomic Spectrum of Hydrogen
• 7.4 The Bohr Model
• 7.5 The Quantum Mechanical Model of the Atom
• 7.6 Quantum Numbers
• 7.7 Orbital Shapes and Energies
• 7.8 Electron Spin and the Pauli Principle
• 7.9 Polyelectronic Atoms
• 7.10 The History of the Periodic Table
• 7.11 The Aufbau Principle and the Periodic Table
• 7.12 Periodic Trends in Atomic Properties
• 7.13 The Properties of a Group: The Alkali Metals
• 8 Bonding: General Concepts
• 8.1 Types of Chemical Bonds
• 8.2 Electronegativity
• 8.3 Bond Polarity and Dipole Moments
• 8.4 Ions: Electron Configurations and Sizes
• 8.5 Energy Effects in Binary Ionic Compounds
• 8.6 Partial Ionic Character of Covalent Bonds
• 8.7 The Covalent Chemical Bond: A Model
• 8.8 Covalent Bond Energies and Chemical Reactions
• 8.9 The Localized Electron Bonding Model
• 8.10 Lewis Structures
• 8.11 Exceptions to the Octet Rule
• 8.12 Resonance
• 8.13 Molecular Structure: The VSEPR Model
• 9 Covalent Bonding: Orbitals
• 9.1 Hybridization and the Localized Electron Model
• 9.2 The Molecular Orbital Model
• 9.3 Bonding in Homonuclear Diatomic Molecules
• 9.4 Bonding in Heteronuclear Diatomic Molecules
• 9.5 Combining the Localized Electron and Molecular Orbital Models
• 10 Liquids and Solids
• 10.1 Intermolecular Forces
• 10.2 The Liquid State
• 10.3 An Introduction to Structures and Types of Solids
• 10.4 Structure and Bonding in Metals
• 10.5 Carbon and Silicon: Network Atomic Solids
• 10.6 Molecular Solids
• 10.7 Ionic Solids
• 10.8 Vapor Pressure and Changes of State
• 10.9 Phase Diagrams
• 11 Properties of Solutions
• 11.1 Solution Composition
• 11.2 The Energies of Solution Formation
• 11.3 Factors Affecting Solubility
• 11.4 The Vapor Pressures of Solutions
• 11.5 Boiling-Point Elevation and Freezing-Point Depression
• 11.6 Osmotic Pressure
• 11.7 Colligative Properties of Electrolyte Solutions
• 11.8 Colloids
• 12 Chemical Kinetics
• 12.1 Reaction Rates
• 12.2 Rate Laws: An Introduction
• 12.3 Determining the Form of the Rate Law
• 12.4 The Integrated Rate Law
• 12.5 Rate Laws: A Summary
• 12.6 Reaction Mechanisms
• 12.7 A Model for Chemical Kinetics
• 12.8 Catalysis
• 13 Chemical Equilibrium
• 13.1 The Equilibrium Condition
• 13.2 The Equilibrium Constant
• 13.3 Equilibrium Expressions Involving Pressures
• 13.4 Heterogeneous Equilibria
• 13.5 Applications of the Equilibrium Constant
• 13.6 Solving Equilibrium Problems
• 13.7 Le Ch?telier's Principle
• 14 Acids and Bases
• 14.1 The Nature of Acids and Bases
• 14.2 Acid Strength
• 14.3 The pH Scale
• 14.4 Calculating the pH of Strong Acid Solutions
• 14.5 Calculating the pH of Weak Acid Solutions
• 14.6 Bases
• 14.7 Polyprotic Acids
• 14.8 Acid-Base Properties of Salts
• 14.9 The Effect of Structure on Acid-Base Properties
• 14.10 Acid-Base Properties of Oxides
• 14.11 The Lewis Acid-Base Model
• 14.12 Strategy for Solving Acid-Base Problems: A Summary
• 15 Applications of Aqueous Equilibria Acid-Base Equilibria
• 15.1 Solutions of Acids or Bases Containing a Common Ion
• 15.2 Buffered Solutions
• 15.3 Buffer Capacity
• 15.4 Titrations and pH Curves
• 15.5 Acid-Base Indicators Solubility Equilibria
• 15.6 Solubility Equilibria and the Solubility Product
• 15.7 Precipitation and Qualitative Analysis Complex Ion Equilibria
• 15.8 Equilibria Involving Complex Ions
• 16 Spontaneity, Entropy, and Free Energy
• 16.1 Spontaneous Processes and Entropy
• 16.2 Entropy and the Second Law of Thermodynamics
• 16.3 The Effect of Temperature on Spontaneity
• 16.4 Free Energy
• 16.5 Entropy Changes in Chemical Reactions
• 16.6 Free Energy and Chemical Reactions
• 16.7 The Dependence of Free Energy on Pressure
• 16.8 Free Energy and Equilibrium
• 16.9 Free Energy and Work
• 17 Electrochemistry
• 17.1 Galvanic Cells
• 17.2 Standard Reduction Potentials
• 17.3 Cell Potential, Electrical Work, and Free Energy
• 17.4 Dependence of Cell Potential on Concentration
• 17.5 Batteries
• 17.6 Corrosion
• 17.7 Electrolysis
• 17.8 Commercial Electrolytic Processes
• 18 The Nucleus: A Chemist's View
• 18.1 Nuclear Stability and Radioactive Decay
• 18.2 The Kinetics of Radioactive Decay
• 18.3 Nuclear Transformations
• 18.4 Detection and Uses of Radioactivity
• 18.5 Thermodynamic Stability of the Nucleus
• 18.6 Nuclear Fission and Nuclear Fusion
• 18.7 Effects of Radiation
• 19 The Representative Elements: Groups 1A Through 4A
• 19.1 A Survey of the Representative Elements
• 19.2 The Group 1A Elements
• 19.3 Hydrogen
• 19.4 The Group 2A Elements
• 19.5 The Group 3A Elements
• 19.6 The Group 4A Elements
• 20 The Representative Elements: Groups 5A Through 8A
• 20.1 The Group 5A Elements
• 20.2 The Chemistry of Nitrogen
• 20.3 The Chemistry of Phosphorus
• 20.4 The Group 6A Elements
• 20.5 The Chemistry of Oxygen
• 20.6 The Chemistry of Sulfur
• 20.7 The Group 7A Elements
• 20.8 The Group 8A Elements
• 21 Transition Metals and Coordination Chemistry
• 21.1 The Transition Metals: A Survey
• 21.2 The First-Row Transition Metals
• 21.3 Coordination Compounds
• 21.4 Isomerism
• 21.5 Bonding in Complex Ions: The Localized Electron Model
• 21.6 The Crystal Field Model
• 21.7 The Biologic Importance of Coordination Complexes
• 21.8 Metallurgy and Iron and Steel Production
• 22 Organic and Biological Molecules
• 22.1 Alkanes: Saturated Hydrocarbons
• 22.2 Alkenes and Alkynes
• 22.3 Aromatic Hydrocarbons
• 22.4 Hydrocarbon Derivatives
• 22.5 Polymers
• 22.6 Natural Polymers
• Appendix 1 Mathematical Procedures
• A1.1 Exponential Notation
• A1.2 Logarithms
• A1.3 Graphing Functions
• A1.4 Solving Quadratic Equations
• A1.5 Uncertainties in Measurements
• Appendix 2 The Quantitative Kinetic Molecular Model
• Appendix 3 Spectral Analysis
• Appendix 4 Selected Thermodynamic Data
• Appendix 5 Equilibrium Constants and Reduction Potentials
• A5.1 Values of Ka for Some Common Monoprotic Acids
• A5.2 Stepwise Dissociation Constants for Several Common Polyprotic Acids
• A5.3 Values of Kb for Some Common Weak Bases
• A5.4 Ksp Values at 25 degrees Celsius for Common Ionic Solids
• A5.5 Standard Reduction Potentials at 25 degrees Celsius (298K) for Many Common Half-Reactions
• Appendix 6 SI Units and Conversion Factors