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Title:
Chemistry
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Edition:
4th ed.
Publication Information:
Hoboken, NJ : John Wiley & Sons, 2006
ISBN:
9780471478119
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30000010077937 QD33.2 O38 2006 Open Access Book Book
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Summary

Summary

100% Pure Chemical Understanding

Every morning many of us are energized by a cup of coffee. Imagine if you were as energized by understanding the chemistry in your morning cup--from the coffee trees, which fill red coffee berries with caffeine and a variety of other chemical substances, to the feathery crystals formed by the caffeine molecules, to the decaffeinating machines, which use liquid solvents to remove this stimulant from some of the beans. Now, that's real chemical understanding!


Olmsted and Williams' Fourth Edition of Chemistry focuses on helping you see and think about the world (and even your coffee) as a chemist. This text helps you understand how chemical phenomena are governed by what happens at the molecular level, apply critical thinking skills to chemical concepts and problems, and master the basic mathematical techniques needed for quantitative reasoning. You'll see the world as chemists do, and learn to appreciate the chemical processes all around us.

A Fourth Edition with a lot of new perks!
* Revisions include a new, early energy chapter; revised coverage of bonding; expanded coverage of intermolecular forces; and increased coverage of multiple equilibria, including polyprotic acids.
* New pedagogy strengthens students' critical thinking and problem-solving skills.
* Visual Summaries at the end of each chapter use molecular and diagrammatic visual elements to summarize essential skills, concepts, equations, and terms.
* eGrade Plus provides an integrated suite of teaching and learning resources, including a complete online version of the text, links between problems and relevant sections in the online text, practice quizzes, the Visual Tutor, Interactive LearningWare problems, and lab demos, as well as homework management and presentation features for instructors.


Author Notes

John Olmsted III is Professor Emeritus of Chemistry at California State University, Fullerton, from which he retired in 2003 after nearly 40 years of teaching and research in general and experimental physical chemistry. John was honored as the CSUF Outstanding Professor in 1997-98 and served as department chair from 1998 to 2001. In addition to 25 years at  CSUF, he taught for 12 years at the American University of Beirut. He had visiting teaching/research appointments at UCLA and the University of North Carolina at Chapel Hill and did research at the Max-Planck-Institute für Biophysikalische Chemie (Göttingen, Germany), the University of California at San Diego, and Sandia National Laboratory in Albuquerque, NM.

John received his BS degree in chemistry from Carnegie Institute of Technology (now Carnegie-Mellon University) and his PhD in physical chemistry from UC Berkeley, where he also did postdoctoral work at the Lawrence Berkeley Laboratory. He has more than 30 referred research publications and has also published regularly on chemical education topics in the Journal of Chemical Education.

In his retirement, besides continuing to write chemistry textbooks, John Keeps busy with his interests in gardening, photography, and the philosophy of chemistry. He and his wife Eileen enjoy traveling, dancing, and  visiting with their three married children and two grandchildren.

Greg Williams is an Adjunct Professor of Chemistry at the University of Oregon. He earned an undergraduate degree in chemistry at UCLA and a Ph.D. in inorganic chemistry at Princeton University. He has taught and conducted research at the University of Oregon, California State University, Fullerton, UCLA, and the University of California, Irvine. Outside the classroom, Greg's professional work is concentrated on developing graphics, digital animation, and interactive multimedia for teaching chemistry.

When he is not teaching or writing about chemistry, Greg can be found somewhere in the western United States, backpacking, climbing, skiing, fly fishing, or kayaking. He also sings low bass with the Eugene Vocal Arts Ensemble. Greg lives in Eugene, Oregon, with his wife Trudy Cameron, a Professor of Economics at the University of Oregon, and their daughters, Casey and Perry. He absolutely insists on enjoying life.


Table of Contents

Chapter 1 The Science of Chemistry.
1.1 What Is Chemistry?
1.2 Atoms, Molecules, and Compounds
1.3 The Periodic Table of the Elements
1.4 Characteristics of Matter
1.5 Measurements in Chemistry
1.6 Calculations in Chemistry
1.7 Chemical Problem Solving
Chapter 2 The Atomic Nature of Matter.
2.1 Atomic Theory
2.2 Atomic Architecture: Electrons and Nuclei
2.3 Atomic Diversity: The Elements
2.4 Counting Atoms: The Mole
2.5 Charged Atoms: Ions
Chapter 3 The Composition of Molecules.
3.1 Representing Molecules
3.2 Naming Chemical Compounds
3.3 Formulas and Names of Ionic Compounds
3.4 Amounts of Compounds
3.5 Determining Chemical Formulas
3.6 Aqueous Solutions
Chapter 4 Chemical Reactions and Stoichiometry.
4.1 Writing Chemical Equations
4.2 The Stoichiometry of Chemical Reactions
4.3 Yields of Chemical Reactions
4.4 The Limiting Reactant
4.5 Precipitation Reactions
4.6 Acid-Base Reactions
4.7 Oxidation-Reduction Reactions
Chapter 5. The Behavior of Gases.
5.1 Pressure
5.2 Describing Gases
5.3 Molecular View of Gases
5.4 Additional Gas Properties
5.5 Gas Mixtures
5.6 Gas Stoichiometry
5.7 Chemistry of the Atmosphere
Chapter 6 Energy and Its Conservation.
6.1 Types of Energy
6.2 Thermodynamics
6.3 Energy Changes in Chemical Reactions
6.4 Measuring Energy Changes
6.5 Enthalpy
6.6 Energy Sources
Chapter 7 Atoms and Light.
7.1 Characteristics of Atoms
7.2 Characteristics of Light
7.3 Absorption and Emission Spectra
7.4 Properties of Electrons
7.5 Quantization and Quantum Numbers
7.6 Shapes of Atomic Orbitals
7.7 Sunlight and the Earth
Chapter 8 Atomic Energies and Periodicity.
8.1 Orbital Energies
8.2 Structure of the Periodic Table
8.3 Electron Configurations
8.4 Periodicity of Atomic Properties
8.5 Energetics of Ionic Compounds
8.6 Ions and Chemical Periodicity
Chapter 9 Fundamentals of Chemical Bonding.
9.1 Overview of Bonding
9.2 Lewis Structures
9.3 Molecular Shapes: Tetrahedral Systems
9.4 Other Molecular Shapes
9.5 Properties of Covalent Bonds
Chapter 10 Theories of Chemical Bonding.
10.1 Localized Bonds
10.2 Hybridization of Atomic Orbitals
10.3 Multiple Bonds
10.4 Molecular Orbital Theory: Diatomic Molecules
10.5 Three-Center _ Orbitals
10.6 Extended _ Systems
10.7 Band Theory of Solids
Chapter 11 Effects of Intermolecular Forces.
11.1 Real Gases and Intermolecular Forces
11.2 Types of Intermolecular Forces
11.3 Liquids
11.4 Forces in Solids
11.5 Order in Solids
11.6 Phase Changes
Chapter 12 Properties of Solutions.
12.1 The Nature of Solutions
12.2 Determinants of Solubility
12.3 Characteristics of Aqueous Solutions
12.4 Colligative Properties
12.5 Between Solutions and Mixtures
Chapter 13 Macromolecules.
13.1 Starting Materials for Polymers
13.2 Free Radical Polymerization
13.3 Condensation Polymerization
13.4 Types of Polymers
13.5 Carbohydrates
13.6 Nucleic Acids
13.7 Proteins
Chapter 14 Spontaneity of Chemical Processes.
14.1 Spontaneity
14.2 Entropy: The Measure of Dispersal
14.3 Entropies of Pure Substances
14.4 Spontaneity and Free Energy
14.5 Some Applications of Thermodynamics
14.6 Bioenergetics
Chapter 15 Kinetics: Mechanisms and Rates of Reactions.
15.1 What Is a Reaction Mechanism?
15.2 Rates of Chemical Reactions
15.3 Concentration and Reaction Rates
15.4 Experimental Kinetics
15.5 Linking Mechanisms and Rate Laws
15.6 Reaction Rates and Temperature
15.7 Catalysis
Chapter 16 Principles of Chemical Equilibrium.
16.1 Describing Chemical Equilibria
16.2 Properties of Equilibrium Constants
16.3 Thermodynamics and Equilibrium
16.4 Shifts in Equilibrium
16.5 Working with Equilibria
16.6 Equilibria in Aqueous Solutions
Chapter 17 Aqueous Acid-Base Equilibria.
17.1 Proton Transfers in Water
17.2 The pH Scale
17.3 Weak Acids and Bases
17.4 Recognizing Acids and Bases
17.5 Acidic and Basic Salts
17.6 Factors Affecting Acid Strength
17.7 Multiple Equilibria
Chapter 18 Applications of Aqueous Equilibria.
18.1 Buffer Solutions
18.2 Capacity and Preparation of Buffer Solutions
18.3 Acid-Base Titrations
18.4 Solubility Equilibria
18.5 Complexation Equilibria
Chapter 19 Electron Transfer Reactions.
19.1 Recognizing Redox Reactions
19.2 Balancing Redox Reactions
19.3 Galvanic Cells
19.4 Cell Potentials
19.5 Free Energy and Electrochemistry
19.6 Redox in Action
19.7 Electrolysis
Chapter 20 The Transition Metals.
20.1 Overview of the Transition Metals
20.2 Coordination Complexes
20.3 Bonding in Coordination Complexes
20.4 Metallurgy
20.5 Applications of Transition Metals
20.6 Transition Metals in Biology
Chapter 21 The Main Group Elements.
21.1 Lewis Acids and Bases
21.2 Hard and Soft Lewis Acids and Bases
21.3 The Main Group Metals
21.4 The Metalloids
21.5 Phosphorus
21.6 Other Nonmetals
Chapter 22 Nuclear Chemistry and Radiochemistry.
22.1 Nuclear Stability
22.2 Nuclear Decay
22.3 Induced Nuclear Reactions
22.4 Nuclear Fission
22.5 Nuclear Fusion
22.6 Effects of Radiation
22.7 Applications of Radioactivity
Appendix A Scientific Notation.
Appendix B Quantitative Observations.
Appendix C Ionization Energies and Electron Affinities.
Appendix D Standard Thermodynamic Functions.
Appendix E Equilibrium Constants.
Appendix F Standard Reduction Potentials.
Solutions to Odd-Numbered Problems.
Photo Credits.
Glossary.
Index of Equations.
Index.
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