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ISBN-10: 0547125321

ISBN-13: 9780547125329

Edition: 8th 2010

Authors: Steven S. Zumdahl, Susan A. Zumdahl

List price: $359.95
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CHEMISTRY outlines chemistry basics using a thoughtful approach built on problem solving. The book speaks directly to the reader about how to approach and solve chemical problems—to learn to think like a chemist—so that they can apply the process of problem-solving to all aspects of their lives.
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Book details

List price: $359.95
Edition: 8th
Copyright year: 2010
Publisher: Brooks/Cole
Publication date: 12/3/2008
Binding: Hardcover
Pages: 1184
Size: 8.75" wide x 10.75" long x 1.50" tall
Weight: 5.434

Steve Zumdahl is the author of market-leading textbooks in introductory chemistry, general chemistry, honors-level chemistry, and high school chemistry. Recently retired from his long-time position as Director of Undergraduate Programs at the University of Illinois, he has received numerous awards for his contributions to chemical education. These include the National Catalyst Award in recognition of his contribution to chemical education, the University of Illinois Teaching Award, the UIUC Liberal Arts and Sciences Advising Award, and the School of Chemical Sciences Teaching Award (five times). He earned his B.S. in Chemistry from Wheaton College (IL), and his Ph.D. from the University of…    

Susan A. Zumdahl earned a B.S. and M.A. in Chemistry at California State University--Fullerton. She has taught science and mathematics at all levels, including middle school, high school, community college, and university. She is past director of the Merit Program for Emerging Scholars in Chemistry at the University of Illinois. In addition, she spearheaded the development of a sophisticated web-based electronic homework system for chemistry and is co-author on several chemistry textbooks.

Chemistry: An Overview
The Scientific Method
Units of Measurement
Uncertainty in Measurement
Significant Figures and Calculations
Dimensional Analysis
Classification of Matter
Atoms, Molecules, and Ions
The Early History of Chemistry
Fundamental Chemical Laws
Dalton's Atomic Theory
Early Experiments to Characterize the Atom
The Modern View of Atomic Structure: An Introduction
Molecules and Ions
An Introduction to the Periodic Table
Naming Simple Compounds
Counting by Weighing
Atomic Masses
The Mole
Molar Mass
Learning to Solve Problems
Percent Composition of Compounds
Determining the Formula of a Compound
Chemical Equations
Balancing Chemical Equations
Stoichiometric Calculations: Amounts of Reactants and Products
The Concept of Limiting Reagent
Types of Chemical Reactions and Solution Stoichiometry
Water, the Common Solvent
The Nature of Aqueous Solutions: Strong and Weak Electrolytes
The Composition of Solutions
Types of Chemical Reactions
Precipitation Reactions
Describing Reactions in Solution
Stoichiometry of Precipitation Reactions
Acid-Base Reactions
Oxidation-Reduction Reactions
Balancing Oxidation-Reduction Equations
The Gas Laws of Boyle, Charles, and Avogadro
The Ideal Gas Law
Gas Stoichiometry
Dalton's Law of Partial Pressures
The Kinetic Molecular Theory of Gases
Effusion and Diffusion
Real Gases
Characteristics of Several Real Gases
Chemistry in the Atmosphere
The Nature of Energy
Enthalpy and Calorimetry
Hess's Law
Standard Enthalpies of Formation
Present Sources of Energy
New Energy Sources
Atomic Structure and Periodicity
Electromagnetic Radiation
The Nature of Matter
The Atomic Spectrum of Hydrogen
The Quantum Mechanical Model of the Atom
Quantum Numbers
Orbital Shapes and Energies
Electron Spin and the Pauli Principle
Polyelectronic Atoms
The History of the Periodic Table
The Aufbau Principle and the Periodic Table
Periodic Trends in Atomic Properties
The Properties of a Group: The Alkali Metals
Bonding: General Concepts
Types of Chemical Bonds
Bond Polarity and Dipole Moments
Ions: Electron Configurations and Sizes
Energy Effects in Binary Ionic Compounds
Partial Ionic Character of Covalent Bonds
The Covalent Chemical Bond: A Model
Covalent Bond Energies and Chemical Reactions
The Localized Electron Bonding Model
Lewis Structures
Exceptions to the Octet Rule
Molecular Structure: The VSEPR Model
Covalent Bonding: Orbitals
Hybridization and the Localized Electron Model
The Molecular Orbital Model
Bonding in Homonuclear Diatomic Molecules
Bonding in Heteronuclear Diatomic Molecules
Combining the Localized Electron and Molecular Orbital Models 4?
Liquids and Solids
Intermolecular Forces
The Liquid State
An Introduction to Structures and Types of Solids
Structure and Bonding in Metals
Carbon and Silicon: Network Atomic Solids Circuits
Molecular Solids
Ionic Solids
Properties of Solutions
Solution Composition
The Energies of Solution Formation
Factors Affecting Solubility
The Vapor Pressures of Solutions
Boiling-Point Elevation and Freezing-Point Depression
Osmotic Pressure
Colligative Properties of Electrolyte Solutions
Chemical Kinetics
Reaction Rates
Rate Laws: An Introduction
Determining the Form of the Rate Law
The Integrated Rate Law
Reaction Mechanisms
A Model for Chemical Kinetics
Chemical Equilibrium
The Equilibrium Condition
The Equilibrium Constant
Equilibrium Expressions Involving Pressures
Heterogeneous Equilibria
Applications of the Equilibrium Constant
Solving Equilibrium Problems
Le Ch?telier's Principle
Acids and Bases
The Nature of Acids and Bases
Acid Strength
The pH Scale
Calculating the pH of Strong Acid Solutions
Calculating the pH of Weak Acid Solutions
Polyprotic Acids
Acid-Base Properties of Salts
The Effect of Structure on Acid-Base Properties
Acid-Base Properties of Oxides
The Lewis Acid-Base Model
Strategy for Solving Acid-Base Problems: A Summary
Acid-Base Equilibria
Solutions of Acids or Bases Containing a Common Ion
Buffered Solutions
Buffering Capacity
Titrations and pH Curves
Acid-Base Indicators
Solubility and Complex Ion Equilibria
Solubility Equilibria and the Solubility Product
Precipitation and Qualitative Analysis
Equilibria Involving Complex Ions
Spontaneity, Entropy, and Free Energy
Spontaneous Processes and Entropy
Entropy and the Second Law of Thermodynamics
The Effect of Temperature on Spontaneity
Free Energy
Entropy Changes in Chemical Reactions
Free Energy and Chemical Reactions
The Dependence of Free Energy on Pressure
Free Energy and Equilibrium
Free Energy and Work
Balancing Oxidation-Reduction Equations
Galvanic Cells
Standard Reduction Potentials
Cell Potential, Electrical Work, and Free Energy
Dependence of Cell Potential on Concentration
Commercial Electrolytic Processes
The Nucleus: A Chemist's View
Nuclear Stability and Radioactive Decay
The Kinetics of Radioactive Decay
Nuclear Transformations
Detection and Uses of Radioactivity
Thermodynamic Stability of the Nucleus
Nuclear Fission and Nuclear Fusion
Effects of Radiation
The Representative Elements
A Survey of the Representative Elements
The Chemistry of Hydrogen
The Chemistry of Nitrogen
The Chemistry of Phosphorus
The Chemistry of Oxygen
The Chemistry of Sulfur
Transition Metals and Coordination Chemistry
The Transition Metals: A Survey
The First-Row Transition Metals
Coordination Compounds
Bonding in Complex Ions: The Localized Electron Model
The Crystal Field Model
The Biologic Importance of Coordination Complexes l982
Metallurgy and Iron and Steel Production
Organic and Biological Molecules
Alkanes: Saturated Hydrocarbons
Alkenes and Alkynes
Aromatic Hydrocarbons
Hydrocarbon Derivatives
Natural Polymers
Mathematical Procedures
Exponential Notation
Graphing Functions
Solving Quadratic Equations
Uncertainties in Measurements
The Quantitative Kinetic Molecular Model
Spectral Analysis
Selected Thermodynamic Data
Equilibrium Constants and Reduction Potentials
Values of Ka for Some Common Monoprotic Acids
Stepwise Dissociation Constants for Several Common Polyprotic Acids
Values of Kb for Some Common Weak Bases
Ksp Values at 25_C for Common Ionic Solids
Standard Reduction Potentials at 25_C (298K) for Many Common Half-Reactions
Units and conversion
Photo Credits
Answers to Selected Exercises