Chemistry

Chemistry 1ce by Olmsted, Williams, Burk is a newly adapted general chemistry text designed for the specific needs and requirements of Canadian professors and students for use in one or two semester introductory chemistry courses. This adaptation was based on recommendations from an advisory board of instructors from leading institutions across Canada who worked with our Canadian author throughout the development of this text to reach a consensus on topics that best suit Canadian curriculum. This text also incorporates key Canadian content in the form of SI units, IUPAC standards and significant Canadian research which more accurately reflects the discipline of Canadian chemistry than other textbooks currently on the market. Chemistry instructors will find this text sufficiently rigorous while it engages and retains student interest with accessible language, Canadian research and examples and a clear problem solving program. In order to more directly reflect the varied curriculum of Canadian chemistry courses we have uniquely created flexible options which allow instructors to decide whether they want to include or exclude early chemistry chapters for the purposes of review.

This Canadian edition retains Olmsted & Williams′ innovative approach to teaching chemistry by reinforcing key concepts through molecular–level discussion and graphics. This approach encourages students to move beyond memorization of formulas and equations, to thinking critically about what is really occurring and solving problems based on what they know about the behaviour of molecules and chemical processes.

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–Institut für Biophysikalische Chemie (Göttingen, Germany), and 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 refereed 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 PhD in organic in inorganic chemistry at Princeton University. He had 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.

Robert C. (Bob) Burk, our Canadian author, is an Associate Professor of Chemistry at Carleton University in Ottawa. He received his B.Sc. and M.Sc. degrees from Carleton. Both involved work in the area of radioanalytical chemistry. Bob worked for six years in the nuclear industry, doing research on the production of nuclear fuels, then returned to Carleton University to do a Ph.D. in the area of supercritical fluid extraction. He has been a member of the Carleton Chemistry faculty since 1993. His research involves the use of supercritical fluids for separation purposes, as well as development of analytical methods for organics in water using novel solid phase materials such as carbon nanotubes. Bob is especially interested in the use of technology for teaching chemistry. His lectures are recorded and available for viewing on i–Tunes, and parts of them appear on Youtube. After–hours, Bob uses instant messaging systems, and more recently social networking tools, to communicate with students while they are studying. He was a winner of the 2004 OCUFA teaching award, and a 3M teaching fellowship in 2006. When not at work, Bob loves to sail in the summer, cross–country ski in the winter with his wife Ewa and two children, Ashley and Adam, and renovate houses and build period furniture all year round.

Chapter 1 Fundamental Concepts of Chemistry
1.1 Atoms, Molecules, and Compounds
1.2 Measurements in Chemistry
1.3 Chemical Problem Solving
1.4 Counting Atoms: The Mole
1.5 Amounts of Compounds
1.6 Aqueous Solutions
1.7 Writing Chemical Equations
1.8 The Stoichiometry of Chemical Reactions
1.9 Yields of Chemical Reactions
1.10 The Limiting Reactant

Chapter 2 The Behaviour of Gases
2.1 Pressure
2.2 Describing Gases
2.3 Gas Mixtures
2.4 Gas Stoichiometry
2.5 Molecular View of Gases
2.6 Additional Gas Properties
2.7 Non–Ideal (Real) Gases
2.8 Chemistry of the Earth’s Atmosphere

Chapter 3 Energy and Its Conservation
3.1 Types of Energy
3.2 Thermodynamics
3.3 Energy Changes in Chemical Reactions
3.4 Measuring Energy Changes: Calorimetry
3.5 Enthalpy
3.6 Energy Sources

Chapter 4 Atoms and Light
4.1 Characteristics of Atoms
4.2 Characteristics of Light
4.3 Absorption and Emission Spectra
4.4 Properties of Electrons
4.5 Quantization and Quantum Numbers
4.6 Shapes of Atomic Orbitals
4.7 Sunlight and the Earth

Chapter 5 Atomic Energies and Periodicity
5.1 Orbital Energies
5.2 Structure of the Periodic Table
5.3 Electron Configurations
5.4 Periodicity of Atomic Properties
5.5 Energetics of Ionic Compounds
5.6 Ions and Chemical Periodicity

Chapter 6 Fundamentals of Chemical Bonding
6.1 Overview of Bonding
6.2 Lewis Structures
6.3 Molecular Shapes: Tetrahedral Systems
6.4 Other Molecular Shapes
6.5 Properties of Covalent Bonds

Chapter 7 Theories of Chemical Bonding
7.1 Localized Bonds
7.2 Hybridization of Atomic Orbitals
7.3 Multiple Bonds
7.4 Molecular Orbital Theory: Diatomic Molecules
7.5 Three–Centre ð Orbitals
7.6 Extended ð Systems
7.7 Band Theory of Solids

Chapter 8 Effects of Intermolecular Forces
8.1 Effects of Intermolecular Forces
8.2 Types of Intermolecular Forces
8.3 Liquids
8.4 Forces in Solids
8.5 Order in Solids
8.6 Phase Changes

Chapter 9 Properties of Solutions
9.1 The Nature of Solutions
9.2 Determinants of Solubility
9.3 Characteristics of Aqueous Solutions
9.4 Colligative Properties
9.5 Between Solutions and Mixtures

Chapter 10 Organic Chemistry
10.1 Hydrocarbons
10.2 Aromatic Compounds
10.3 Functional Groups
10.4 Stereochemistry
10.5 Substitution Reactions
10.6 Elimination Reactions
10.7 Addition Reactions

Chapter 11 Spontaneity of Chemical Processes
11.1 Spontaneity
11.2 Entropy: The Measure of Dispersal
11.3 Entropies of Pure Substances
11.4 Spontaneity and Free Energy
11.5 Some Applications of Thermodynamics
11.6 Bioenergetics

Chapter 12 Kinetics: Mechanisms and Rates of Reactions
12.1 What is a Reaction Mechanism
12.2 Rates of Chemical Reactions
12.3 Concentration and Reaction Rates
12.4 Experimental Kinetics
12.5 Linking Mechanisms and Rate Laws
12.6 Reaction Rates and Temperature
12.7 Catalysis

Chapter 13 Principles of Chemical Equilibrium
13.1 Describing Chemical Equilibria
13.2 Properties of Equilibrium Constants
13.3 Thermodynamics and Equilibrium
13.4 Shifts in Equilibrium
13.5 Working with Equilibria
13.6 Equilibria in Aqueous Solutions

Chapter 14 Aqueous Acid Base Equilibria
14.1 Proton Transfers in Water
14.2 The pH Scale
14.3 Weak Acids and Bases
14.4 Recognizing Acids and Bases
14.5 Acidic and Basic Salts
14.6 Factors Affecting Acid Strength
14.7 Multiple Equilibria

Chapter 15 Applications of Aqueous Equilibria
15.1 Buffer Solutions
15.2 Capacity and Preparation of Buffer Solutions
15.3 Acid–Base Titrations
15.4 Solubility Equilibria
15.5 Complexation Equilibria

Chapter 16 Electron Transfer Reactions
16.1 Recognizing Redox Reactions
16.2 Balancing Redox Reactions
16.3 Galvanic Cells
16.4 Cell Potentials
16.5 Free Energy and Electrochemistry
16.6 Redox in Action
16.7 Electrolysis

Chapter 17 Macromolecules
17.1 Starting Materials for Polymers
17.2 Free Radical Polymerization
17.3 Condensation Polymerization
17.4 Types of Polymers
17.5 Carbohydrates
17.6 Nucleic Acids
17.7 Proteins

Chapter 18 The Transition Metals
18.1 Overview of the Transition Metals
18.2 Coordination Complexes
18.3 Bonding in Coordination Complexes
18.4 Transition Metals in Biology
18.5 Metallurgy
18.6 Applications of Transition Metals

Chapter 19 The Main Group Elements
19.1 Lewis Acids and Bases
19.2 Hard and Soft Lewis Acids and Bases
19.3 The Main Group Metals
19.4 The Metalloids
19.5 Phosphorus
19.6 Other Non–Metals

Chapter 20 Nuclear Chemistry and Radiochemistry
20.1 Nuclear Stability
20.2 Nuclear Decay
20.3 Induced Nuclear Reactions
20.4 Nuclear Fission
20.5 Nuclear Fusion
20.6 Effects of Radiation
20.7 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
Index of Equations