Principles of Modern Chemistry 8th Edition by David W. Oxtoby, ISBN-13: 978-1305079113

Description

Principles of Modern Chemistry 8th Edition by David W. Oxtoby, ISBN-13: 978-1305079113

[PDF eBook eTextbook]

• Publisher: ‎ Cengage Learning; 8th edition (March 10, 2015)
• Language: ‎ English
• 1264 pages
• ISBN-10: ‎ 1305079116
• ISBN-13: ‎ 978-1305079113

Long considered the standard for covering chemistry at a high level, PRINCIPLES OF MODERN CHEMISTRY continues to set the standard as the most modern, rigorous, and chemically and mathematically accurate book on the market. This authoritative text features an “atoms first” approach and thoroughly revised chapters on Quantum Mechanics and Molecular Structure (Chapter 6), Electrochemistry (Chapter 17), and Molecular Spectroscopy and Photochemistry (Chapter 20). In addition, the text utilizes mathematically accurate and artistic atomic and molecular orbital art, and is student friendly without compromising its rigor. End-of-chapter learning aids now focus on only the most important key objectives, equations and concepts, making it easier for readers to locate chapter content, while new applications to a wide range of disciplines, such as biology, chemical engineering, biochemistry, and medicine deepen readers’ understanding of the relevance of chemistry in today’s world.

Table of Contents:

Brief Contents

Contents

Applications

Preface

About the Authors

Unit I: Introduction to the Study of Modern Chemistry

Chapter 1: The Atom in Modern Chemistry

1.1 The Nature of Modern Chemistry

1.2 Elements: The Building Blocks of Matter

1.3 Indirect Evidence for the Existence of Atoms: Laws of Chemical Combination

1.4 The Physical Structure of Atoms

1.5 Mass Spectrometry, Isotopes, and the Measurement of Relative Mass

1.6 The Mole: Counting Molecules by Weighing

Chapter 2: Chemical Formulas, Equations, and Reaction Yields

2.1 Empirical and Molecular Formulas

2.2 Chemical Formula and Percentage Composition

2.3 Writing Balanced Chemical Equations

2.4 Mass Relationships in Chemical Reactions

2.5 Limiting Reactant and Percentage Yield

Unit II: Chemical Bonding and Molecular Structure

Chapter 3: Atomic Shells and Classical Models of Chemical Bonding

3.1 Representations of Molecules

3.2 The Periodic Table

3.3 Forces and Potential Energy in Atoms

3.4 Ionization Energies, the Shell Model of the Atom, and Shielding

3.5 Electron Affinity

3.6 Electronegativity: The Tendency of Atoms to Attract Electrons in Molecules

3.7 Forces and Potential Energy in Molecules: Formation of Chemical Bonds

3.8 Ionic Bonding

3.9 Covalent and Polar Covalent Bonding

3.10 Electron Pair Bonds and Lewis Diagrams for Molecules

3.11 The Shapes of Molecules: Valence Shell Electron-Pair Repulsion Theory

3.12 Oxidation Numbers

3.13 Inorganic Nomenclature

Chapter 4: Introduction to Quantum Mechanics

4.1 Preliminaries: Wave Motion and Light

4.2 Evidence for Energy Quantization in Atoms

4.3 The Bohr Model: Predicting Discrete Energy Levels in Atoms

4.4 Evidence for Wave-Particle Duality

4.5 The Schrodinger Equation

4.6 Quantum Mechanics of Particle-in-a-Box Models

4.7 A Deeper Look: Wave Functions for Particles in Two- and Three-Dimensional Boxes

Chapter 5: Quantum Mechanics and Atomic Structure

5.1 The Hydrogen Atom

5.2 Shell Model for Many-Electron Atoms

5.3 Aufbau Principle and Electron Configurations

5.4 Shells and the Periodic Table: Photoelectron Spectroscopy

5.5 Periodic Properties and Electronic Structure

Chapter 6: Quantum Mechanics and Molecular Structure

6.1 Quantum Picture of the Chemical Bond

6.2 Exact Molecular Orbitals for the Simplest Molecule: H+2

6.3 Molecular Orbital Theory and the Linear Combination of Atomic Orbitals Approximation for H+2

6.4 Homonuclear Diatomic Molecules: First-Period Atoms

6.5 Homonuclear Diatomic Molecules: Second-Period Atoms

6.6 Heteronuclear Diatomic Molecules

6.7 Summary Comments for the LCAO Method and Diatomic Molecules

6.8 Valence Bond Theory and the Electron Pair Bond

6.9 Orbital Hybridization for Polyatomic Molecules

6.10 Predicting Molecular Structures and Shapes

6.11 Using the LCAO and Valence Bond Methods Together

6.12 Summary and Comparison of the LCAO and Valence Bond Methods

6.13 A Deeper Look: Properties of the Exact Molecular Orbitals for H+2

Chapter 7: Bonding in Organic Molecules

7.1 Petroleum Refining and the Hydrocarbons

7.2 The Alkanes

7.3 The Alkenes and Alkynes

7.4 Aromatic Hydrocarbons

7.5 Fullerenes

7.6 Functional Groups and Organic Reactions

7.7 Pesticides and Pharmaceuticals

Chapter 8: Bonding in Transition Metal Compounds and Coordination Complexes

8.1 Chemistry of the Transition Metals

8.2 Introduction to Coordination Chemistry

8.3 Structures of Coordination Complexes

8.4 Crystal Field Theory: Optical and Magnetic Properties

8.5 Optical Properties and the Spectrochemical Series

8.6 Bonding in Coordination Complexes

Unit III: Kinetic Molecular Description of the States of Matter

Chapter 9: The Gaseous State

9.1 The Chemistry of Gases

9.2 Pressure and Temperature of Gases

9.3 The Ideal Gas Law

9.4 Mixtures of Gases

9.5 The Kinetic Theory of Gases

9.6 Real Gases: Intermolecular Forces

9.7 A Deeper Look: Molecular Collisions and Rate Processes

Chapter 10: Solids, Liquids, and Phase Transitions

10.1 Bulk Properties of Gases, Liquids, and Solids: Molecular Interpretation

10.2 Intermolecular Forces: Origins in Molecular Structure

10.3 Intermolecular Forces in Liquids

10.4 Phase Equilibrium

10.5 Phase Transitions

10.6 Phase Diagrams

Chapter 11: Solutions

11.1 Composition of Solutions

11.2 Nature of Dissolved Species

11.3 Reaction Stoichiometry in Solutions: Acid-Base Titrations

11.4 Reaction Stoichiometry in Solutions: Oxidation-Reduction Titrations

11.5 Phase Equilibrium in Solutions: Nonvolatile Solutes

11.6 Phase Equilibrium in Solutions: Volatile Solutes

11.7 Colloidal Suspensions

Unit IV: Equilibrium in Chemical Reactions

Chapter 12: Thermodynamic Processes and Thermochemistry

12.1 Systems, States, and Processes

12.2 The First Law of Thermodynamics: Internal Energy, Work, and Heat

12.3 Heat Capacity, Calorimetry, and Enthalpy

12.4 The First Law and Ideal Gas Processes

12.5 Molecular Contributions to Internal Energy and Heat Capacity

12.6 Thermochemistry

12.7 Reversible Processes in Ideal Gases

12.8 A Deeper Look: Distribution of Energy among Molecules

Chapter 13: Spontaneous Processes and Thermodynamic Equilibrium

13.1 The Nature of Spontaneous Processes

13.2 Entropy and Spontaneity: A Molecular Statistical Interpretation

13.3 Entropy and Heat: Macroscopic Basis of the Second Law of Thermodynamics

13.4 Entropy Changes in Reversible Processes

13.5 Entropy Changes and Spontaneity

13.6 The Third Law of Thermodynamics

13.7 The Gibbs Free Energy

13.8 A Deeper Look: Carnot Cycles, Efficiency, and Entropy

Chapter 14: Chemical Equilibrium

14.1 The Nature of Chemical Equilibrium

14.2 The Empirical Law of Mass Action

14.3 Thermodynamic Description of the Equilibrium State

14.4 The Law of Mass Action for Related and Simultaneous Equilibria

14.5 Equilibrium Calculations for Gas-Phase and Heterogeneous Reactions

14.6 The Direction of Change in Chemical Reactions: Empirical Description

14.7 The Direction of Change in Chemical Reactions: Thermodynamic Explanation

14.8 Distribution of a Single Species between Immiscible Phases: Extraction and Separation Processes

Chapter 15: Acid-Base Equilibria

15.1 Classifications of Acids and Bases

15.2 Properties of Acids and Bases in Aqueous Solutions: The Bronsted-Lowry Scheme

15.3 Acid and Base Strength

15.4 Equilibria Involving Weak Acids and Bases

15.5 Buffer Solutions

15.6 Acid-Base Titration Curves

15.7 Polyprotic Acids

15.8 Organic Acids and Bases: Structure and Reactivity

15.9 A Deeper Look: Exact Treatment of Acid-Base Equilibria

Chapter 16: Solubility and Precipitation Equilibria

16.1 The Nature of Solubility Equilibria

16.2 Ionic Equilibria between Solids and Solutions

16.3 Precipitation and the Solubility Product

16.4 The Effects of pH on Solubility

16.5 Complex Ions and Solubility

16.6 A Deeper Look: Selective Precipitation of Ions

Chapter 17: Electrochemistry

17.1 Electrochemical Cells

17.2 Cell Potentials and the Gibbs Free Energy

17.3 Concentration Effects and the Nernst Equation

17.4 Molecular Electrochemistry

17.5 Batteries and Fuel Cells

17.6 Corrosion and Corrosion Prevention

17.7 Electrometallurgy

17.8 A Deeper Look: Electrolysis of Water and Aqueous Solutions

Unit V: Rates of Chemical and Physical Processes

Chapter 18: Chemical Kinetics

18.1 Rates of Chemical Reactions

18.2 Rate Laws

18.3 Reaction Mechanisms

18.4 Reaction Mechanisms and Rate

18.5 Effect of Temperature on Reaction Rates

18.6 Molecular Theories of Elementary Reactions

18.7 Reactions in Solution

18.8 Catalysis

Chapter 19: Nuclear Chemistry

19.1 Mass-Energy Relationships in Nuclei

19.2 Nuclear Decay Processes

19.3 Kinetics of Radioactive Decay

19.4 Radiation in Biology and Medicine

19.5 Nuclear Fission

19.6 Nuclear Fusion and Nucleosynthesis

Chapter 20: Molecular Spectroscopy and Photochemistry

20.1 Introduction to Molecular Spectroscopy

20.2 Experimental Methods in Molecular Spectroscopy

20.3 Rotational and Vibrational Spectroscopy

20.4 Nuclear Magnetic Resonance Spectroscopy

20.5 Electronic Spectroscopy and Excited State Relaxation Processes

20.6 Introduction to Atmospheric Chemistry

20.7 Photosynthesis

20.8 A Deeper Look: Lasers

Unit VI: Materials

Chapter 21: Structure and Bonding in Solids

21.1 Crystal Symmetry and the Unit Cell

21.2 Crystal Structure

21.3 Cohesion in Solids

21.4 Defects and Amorphous Solids

21.5 A Deeper Look: Lattice Energies of Crystals

Chapter 22: Inorganic Materials

22.1 Minerals: Naturally Occurring Inorganic Materials

22.2 Properties of Ceramics

22.3 Silicate Ceramics

22.4 Nonsilicate Ceramics

22.5 Electrical Conduction in Materials

22.6 Band Theory of Conduction

22.7 Semiconductors

22.8 Pigments and Phosphors: Optical Displays

Chapter 23: Polymeric Materials and Soft Condensed Matter

23.1 Polymerization Reactions for Synthetic Polymers

23.2 Applications for Synthetic Polymers

23.3 Liquid Crystals

23.4 Natural Polymers

Appendices

Appendix A: Scientific Notation and Experimental Error

Appendix B: SI Units, Unit Conversions, and Physics for General Chemistry

Appendix C: Mathematics for General Chemistry

Appendix D: Standard Chemical Thermodynamic Properties

Appendix E: Standard Reduction Potentials at 25 Degrees Celsius

Appendix F: Physical Properties of the Elements

Appendix G: Answers to Odd-Numbered Problems

Index/Glossary

David W. Oxtoby became the ninth president of Pomona College on July 1, 2003. An internationally noted chemist, he previously served as dean of physical sciences at the University of Chicago. At Pomona, he holds a coterminous appointment as president and professor of chemistry. Before coming to Pomona, he was associated with the University of Chicago for nearly three decades, with brief interludes to serve as a visiting professor at such places as the University of Paris; the University of Bristol in Great Britain; and the University of Sydney in Australia. Oxtoby is a fellow of the American Physical Society and a member of the American Chemical Society and the American Association for the Advancement of Science. After earning his bachelor’s degree, summa cum laude, from Harvard University, he went on to earn his Ph.D. at the University of California, Berkeley. As a research chemist, he is author or co-author of more than 165 scientific articles on such subjects as light scattering, chemical reaction dynamics and phase transitions. In addition to co-authoring Principles of Modern Chemistry and Chemistry: Science of Change, he has received fellowships from the Guggenheim, von Humboldt, Dreyfus, Sloan, Danforth and National Science foundations.

H.P. Gillis conducts experimental research in the physical chemistry of electronic materials, emphasizing phenomena at solid surfaces and interfaces. Dr. Gillis received his B.S. (Chemistry and Physics) at Louisiana State University and his Ph.D. (Chemical Physics) at The University of Chicago. After postdoctoral research at the University of California-Los Angeles and 10 years with the technical staff at Hughes Research Laboratories in Malibu, California, Dr. Gillis joined the faculty of Georgia Institute of Technology. Dr. Gillis moved to University of California-Los Angeles, where he currently serves as Adjunct Professor of Materials Science and Engineering. He has taught courses in general chemistry, physical chemistry, quantum mechanics, surface science, and materials science at UCLA and at Georgia Institute of Technology.

Laurie J. Butler received her B.S. at the Massachusetts Institute of Technology, and her Ph.D. at the University of California, Berkeley. After postdoctoral research at the University of Wisconsin, she joined the faculty at The University of Chicago, where she has been a professor since 1987. Professor Butler’s research investigates the fundamental inter- and intramolecular forces that drive the course of chemical reactions. Much of her recent work investigates classes of important chemical reactions where the breakdown of the Born-Oppenheimer approximation (the inability of the electronic wavefunction to readjust rapidly enough during the nuclear dynamics) near the transition state alters the dynamics and markedly reduces the reaction rate. She has been an Alfred P. Sloan Fellow and a Camille and Henry Dreyfus Teacher-Scholar, and was awarded the Llewellyn John and Harriet Manchester Quantrell Award for Excellence in Undergraduate Teaching at The University of Chicago.

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