Chemistry Sixth Edition by Thomas R. Gilbert, ISBN-13: 978-0393697308

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Chemistry Sixth Edition by Thomas R. Gilbert, ISBN-13: 978-0393697308

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• Publisher: ‎ W. W. Norton & Company; Sixth edition (July 1, 2020)
• Language: ‎ English
• ‎1312 pages
• ISBN-10: ‎ 0393697304
• ISBN-13: ‎ 978-0393697308

A research-based text and assessment package that helps students visualize chemistry as they solve problems.

The exciting new Sixth Edition expands on the visualization pedagogy from coauthor Stacey Lowery Bretz and makes it even easier to implement in the classroom. Based on her chemistry education research on how students construct and interpret multiple representations, art in the book and media has been revised to be more pedagogically effective and to address student misconceptions. New projected visualization questions help instructors assess students’ conceptual understanding in lecture or during exams. A new Interactive Instructor’s Guide provides innovative ways to incorporate research-based active learning pedagogy into the classroom.

Table of Contents:

Cover

Publisher’s Notice

Title Page

Copyright

Brief Contents

Contents

List of Applications

List of Animations

About the Authors

Preface

Half-title Page

Periodic Table of Elements

Atomic Color Palette, Units, and Constants

Chapter 1: Particles of Matter: Measurement and the Tools of Science

1.1 How and Why

1.2 Macroscopic and Particulate Views of Matter

1.3 Mixtures and How to Separate Them

1.4 A Framework for Solving Problems

1.5 Properties of Matter

1.6 States of Matter

1.7 The Scientific Method: Starting Off with a Bang

1.8 SI Units

1.9 Unit Conversions and Dimensional Analysis

1.10 Evaluating and Expressing Experimental Results

1.11 Testing a Theory: The Big Bang Revisited

Summary

Chapter 2: Atoms, Ions, and Molecules: Matter Starts Here

2.1 Atoms in Baby Teeth

2.2 Discovering the Structure of Atoms

2.3 Isotopes

2.4 Average Atomic Mass

2.5 The Periodic Table of the Elements

2.6 Trends in Compound Formation

2.7 Naming Inorganic Compounds and Writing Their Formulas

2.8 Organic Compounds: A First Look

2.9 Nucleosynthesis: The Origin of the Elements

Summary

Chapter 3: Stoichiometry: Mass, Formulas, and Reactions

3.1 Air, Life, and Molecules

3.2 The Mole

3.3 Writing Balanced Chemical Equations

3.4 Combustion Reactions

3.5 Stoichiometric Calculations and the Carbon Cycle

3.6 Limiting Reactants and Percent Yield

3.7 Determining Empirical Formulas from Percent Composition

3.8 Comparing Empirical and Molecular Formulas

3.9 Combustion Analysis

Summary

Chapter 4: Reactions in Solution: Aqueous Chemistry in Nature

4.1 Ions and Molecules in Oceans and Cells

4.2 Expressing Concentrations

4.3 Dilutions

4.4 Electrolytes and Nonelectrolytes

4.5 Acid–Base Reactions: Proton Transfer

4.6 Titrations

4.7 Precipitation Reactions

4.8 Oxidation–Reduction Reactions: Electron Transfer

Summary

Chapter 5: Properties of Gases: The Air We Breathe

5.1 Air: An Invisible Necessity

5.2 Atmospheric Pressure and Collisions

5.3 The Gas Laws

5.4 The Ideal Gas Law

5.5 Gases in Chemical Reactions

5.6 Gas Density

5.7 Dalton’s Law and Mixtures of Gases

5.8 The Kinetic Molecular Theory of Gases

5.9 Real Gases

Summary

Chapter 6: Thermochemistry: Energy Changes in Chemical Reactions

6.1 Sunlight Unwinding

6.2 Forms of Energy

6.3 Systems, Surroundings, and Energy Transfer

6.4 Enthalpy and Enthalpy Changes

6.5 Heating Curves, Molar Heat Capacity, and Specific Heat

6.6 Calorimetry: Measuring Heat Capacity and Enthalpies of Reaction

6.7 Hess’s Law

6.8 Standard Enthalpies of Formation and Reaction

6.9 Fuels, Fuel Values, and Food Values

Summary

Chapter 7: A Quantum Model of Atoms: Waves, Particles, and Periodic Properties

7.1 Rainbows of Light

7.2 Waves of Energy

7.3 Particles of Energy and Quantum Theory

7.4 The Hydrogen Spectrum and the Bohr Model

7.5 Electron Waves

7.6 Quantum Numbers and Electron Spin

7.7 The Sizes and Shapes of Atomic Orbitals

7.8 The Periodic Table and Filling the Orbitals of Multielectron Atoms

7.9 Electron Configurations of Ions

7.10 The Sizes of Atoms and Ions

7.11 Ionization Energies

7.12 Electron Affinities

Summary

Chapter 8: Chemical Bonds: What Makes a Gas a Greenhouse Gas?

8.1 Types of Chemical Bonds and the Greenhouse Effect

8.2 Lewis Structures

8.3 Polar Covalent Bonds

8.4 Resonance

8.5 Formal Charge: Choosing among Lewis Structures

8.6 Exceptions to the Octet Rule

8.7 The Lengths and Strengths of Covalent Bonds

Summary

Chapter 9: Molecular Geometry: Shape Determines Function

9.1 Biological Activity and Molecular Shape

9.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory

9.3 Polar Bonds and Polar Molecules

9.4 Valence Bond Theory

9.5 Shape, Large Molecules, and Molecular Recognition

9.6 Molecular Orbital Theory

Summary

Chapter 10: Intermolecular Forces: The Uniqueness of Water

10.1 Intramolecular Forces versus Intermolecular Forces

10.2 Dispersion Forces

10.3 Interactions Involving Polar Molecules

10.4 Vapor Pressure of Pure Liquids

10.5 Phase Diagrams: Intermolecular Forces at Work

10.6 Some More Remarkable Properties of Water

10.7 Polarity and Solubility

10.8 Solubility of Gases in Water

Summary

Chapter 11: Solutions: Properties and Behavior

11.1 Interactions between Ions

11.2 Energy Changes during Formation and Dissolution of Ionic Compounds

11.3 Vapor Pressure of Solutions

11.4 Mixtures of Volatile Solutes

11.5 Colligative Properties of Solutions

11.6 Ion Exchange

Summary

Chapter 12: Solids: Crystals, Alloys, and Polymers

12.1 The Solid State

12.2 Structures of Metals

12.3 Alloys and Medicine

12.4 Ionic Solids and Salt Crystals

12.5 Allotropes of Carbon

12.6 Polymers

Summary

Chapter 13: Chemical Kinetics: Reactions in the Atmosphere

13.1 Cars, Trucks, and Air Quality

13.2 Reaction Rates

13.3 Effect of Concentration on Reaction Rate

13.4 Reaction Rates, Temperature, and the Arrhenius Equation

13.5 Reaction Mechanisms

13.6 Catalysts

Summary

Chapter 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make?

14.1 The Dynamics of Chemical Equilibrium

14.2 The Equilibrium Constant

14.3 Relationships between Kc and Kp Values

14.4 Manipulating Equilibrium Constant Expressions

14.5 Equilibrium Constants and Reaction Quotients

14.6 Heterogeneous Equilibria

14.7 Le Châtelier’s Principle

14.8 Calculations Based on K

Summary

Chapter 15: Acid–Base Equilibria: Proton Transfer in Biological Systems

15.1 Acids and Bases: A Balancing Act

15.2 The Molecular Structures and Strengths of Acids and Bases

15.3 Conjugate Pairs and Their Complementary Strengths as Acids and Bases

15.4 pH and the Autoionization of Water

15.5 Ka and Kb, and the Ionization of Weak Acids and Bases

15.6 Calculating the pH of Acidic and Basic Solutions

15.7 Polyprotic Acids

15.8 Acidic and Basic Salts

Summary

Chapter 16: Additional Aqueous Equilibria: Chemistry and the Oceans

16.1 Ocean Acidification: Equilibrium under Stress

16.2 The Common-Ion Effect

16.3 pH Buffers

16.4 Indicators and Acid–Base Titrations

16.5 Lewis Acids and Bases

16.6 Formation of Complex Ions

16.7 Hydrated Metal Ions as Acids

16.8 Solubility Equilibria

Summary

Chapter 17: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

17.1 Spontaneous Processes

17.2 Entropy and the Second Law of Thermodynamics

17.3 Absolute Entropy and the Third Law of Thermodynamics

17.4 Calculating Entropy Changes

17.5 Free Energy

17.6 Temperature and Spontaneity

17.7 Free Energy and Chemical Equilibrium

17.8 Influence of Temperature on Equilibrium Constants

17.9 Driving the Human Engine: Coupled Reactions

17.10 Microstates: A Quantized View of Entropy

Summary

Chapter 18: Electrochemistry: The Quest for Clean Energy

18.1 Running on Electrons: Redox Chemistry Revisited

18.2 Voltaic and Electrolytic Cells

18.3 Standard Potentials

18.4 Chemical Energy and Electrical Work

18.5 A Reference Point: The Standard Hydrogen Electrode

18.6 The Effect of Concentration on Ecell

18.7 Relating Battery Capacity to Quantities of Reactants

18.8 Corrosion: Unwanted Electrochemical Reactions

18.9 Electrolytic Cells and Rechargeable Batteries

18.10 Fuel Cells and Flow Batteries

Summary

Chapter 19: Nuclear Chemistry: Applications in Science and Medicine

19.1 Energy and Nuclear Stability

19.2 Unstable Nuclei and Radioactive Decay

19.3 Measuring and Expressing Radioactivity

19.4 Calculations Involving Half-Lives of Radionuclides

19.5 Radiometric Dating

19.6 Biological Effects of Radioactivity

19.7 Medical Applications of Radionuclides

19.8 Nuclear Fission

19.9 Nuclear Fusion and the Quest for Clean Energy

Summary

Chapter 20: Organic and Biological Molecules: The Compounds of Life

20.1 Molecular Structure and Functional Groups

20.2 Organic Molecules, Isomers, and Chirality

20.3 The Composition of Proteins

20.4 Protein Structure and Function

20.5 Carbohydrates

20.6 Lipids

20.7 Nucleotides and Nucleic Acids

20.8 From Biomolecules to Living Cells

Summary

Chapter 21: The Main Group Elements: Life and the Periodic Table

21.1 Main Group Elements and Human Health

21.2 Periodic Properties of Main Group Elements

21.3 Major Essential Elements

21.4 Trace and Ultratrace Essential Elements

21.5 Nonessential Elements

21.6 Elements for Diagnosis and Therapy

Summary

Chapter 22: Transition Metals: Biological and Medical Applications

22.1 Transition Metals in Biology: Complex Ions

22.2 Naming Complex Ions and Coordination Compounds

22.3 Polydentate Ligands and Chelation

22.4 Crystal Field Theory

22.5 Magnetism and Spin States

22.6 Isomerism in Coordination Compounds

22.7 Coordination Compounds in Biochemistry

22.8 Coordination Compounds in Medicine

Summary

Appendix 1: Mathematical Procedures

Appendix 2: SI Units and Conversion Factors

Appendix 3: The Elements and Their Properties

Appendix 4: Chemical Bonds and Thermodynamic Data

Appendix 5: Equilibrium Constants

Appendix 6: Standard Reduction Potentials

Appendix 7: Naming Organic Compounds

Glossary

Answers to Particulate Review, Concept Tests, and Practice Exercises

Answers to Selected End-of-Chapter Questions and Problems

Credits

Index

Thomas R. Gilbert has a BS in chemistry from Clarkson and a PhD in analytical chemistry from MIT. After 10 years with the Research Department of the New England Aquarium in Boston, he joined the faculty of Northeastern University, where he is currently associate professor of chemistry and chemical biology. His research interests are in chemical and science education. He teaches general chemistry and science education courses and conducts professional development workshops for K–12 teachers. He has won Northeastern’s Excellence in Teaching Award and Outstanding Teacher of First-Year Engineering Students Award. He is a fellow of the American Chemical Society and in 2012 was elected to the ACS Board of Directors.

Rein V. Kirss received both a BS in chemistry and a BA in history as well as an MA in chemistry from SUNY Buffalo. He received his PhD in inorganic chemistry from the University of Wisconsin, Madison, where the seeds for this textbook were undoubtedly planted. After two years of postdoctoral study at the University of Rochester, he spent a year at Advanced Technology Materials, Inc., before returning to academics at Northeastern University in 1989. He is an associate professor of chemistry with an active research interest in organometallic chemistry.

Stacey Lowery Bretz is a University Distinguished Professor in the Department of Chemistry and Biochemistry at Miami University in Oxford, Ohio. She earned her BA in chemistry from Cornell University, MS from the Pennsylvania State University, and a PhD in chemistry education research (CER) from Cornell University. Stacey then spent one year at the University of California, Berkeley as a post-doc in the Department of Chemistry. Her research expertise includes the development of assessments to characterize chemistry misconceptions and measure learning in the chemistry laboratory. Of particular interest is method development with regard to the use of multiple representations (particulate, symbolic, and macroscopic) to generate cognitive dissonance, including protocols for establishing the reliability and validity of these measures. She has been honored with both of Miami University’s highest teaching awards: the E. Phillips Knox Award for Undergraduate Teaching in 2009 and the Distinguished Teaching Award for Excellence in Graduate Instruction and Mentoring in 2013. In 2015, she was honored as Chemist of the Year by the ACS Concinnati Local Section.

Natalie Foster is emeritus professor of chemistry at Lehigh University in Bethlehem, Pennsylvania. She received a BS in chemistry from Muhlenberg College and MS, DA, and PhD degrees from Lehigh University. Her research interests included studying poly(vinyl alcohol) gels by NMR as part of a larger interest in porphyrins and phthalocyanines as candidate contrast enhancement agents for MRI. She taught both semesters of the introductory chemistry class to engineering, biology, and other nonchemistry majors and a spectral analysis course at the graduate level. She is the recipient of the Christian R. and Mary F. Lindback Foundation Award for distinguished teaching.

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