Active Learning Guide for Zumdahl/Zumdahl's Chemistry, 7th / Edition 7

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Presents React questions and activities that can be used as teaching tools in lectures or recitation, requiring the student to complete the activities in the guide. The approach stresses active learning, thereby underscoring one of the traditional strengths of the text--the book's conceptual approach to problem solving. For the instructor, PowerPoint slides are available on the HM ClassPrep CD and on the Online Teaching Center containing the questions from the Active Learning Guide as well as relevant figures from the text and animations. Answers to the React questions are in the Instructor's Resource Guide.
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Product Details

  • ISBN-13: 9780618528479
  • Publisher: Cengage Learning
  • Publication date: 12/5/2005
  • Format: Spiral Bound
  • Edition description: New Edition
  • Edition number: 7
  • Pages: 96
  • Product dimensions: 8.30 (w) x 10.60 (h) x 0.20 (d)

Meet the Author

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 Illinois.

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.

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Table of Contents

Note: Each chapter concludes with For Review, Key Terms, and Questions and Exercises. 1. Chemical Foundations 1.1 Chemistry: An Overview 1.2 The Scientific Method 1.3 Units of Measurement 1.4 Uncertainty in Measurement 1.5 Significant Figures and Calculations 1.6 Dimensional Analysis 1.7 Temperature 1.8 Density 1.9 Classification of Matter 2. Atoms, Molecules, and Ions 2.1 The Early History of Chemistry 2.2 Fundamental Chemical Laws 2.3 Dalton's Atomic Theory 2.4 Early Experiments to Characterize the Atom 2.5 The Modern View of Atomic Structure: An Introduction 2.6 Molecules and Ions 2.7 An Introduction to the Periodic Table 2.8 Naming Simple Compounds 3. Stoichiometry 3.1 Counting by Weighing 3.2 Atomic Masses 3.3 The Mole 3.4 Molar Mass 3.5 Percent Composition of Compounds 3.6 Determining the Formula of a Compound 3.7 Chemical Equations 3.8 Balancing Chemical Equations 3.9 Stoichiometric Calculations: Amounts of Reactants and Products 3.10 Calculations Involving a Limiting Reactant 4. Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions 4.4 Types of Chemical Reactions 4.5 Precipitation Reactions 4.6 Describing Reactions in Solution 4.7 Stoichiometry of Precipitation Reactions 4.8 Acid-Base Reactions 4.9 Oxidation-Reduction Reactions 4.10 Balancing Oxidation-Reduction Equations 5. Gases 5.1 Pressure 5.2 The Gas Laws of Boyle, Charles, and Avogadro 5.3 The Ideal Gas Law 5.4 Gas Stoichiometry 5.5 Dalton's Law of Partial Pressures 5.6 The Kinetic Molecular Theory of Gases 5.7 Effusion and Diffusion 5.8 Real Gases 5.9 Characteristics of Several Real Gases 5.10 Chemistry in the Atmosphere 6. Thermochemistry 6.1 The Nature of Energy 6.2 Enthalpy and Calorimetry 6.3 Hess's Law 6.4 Standard Enthalpies of Formation 6.5 Present Sources of Energy 6.6 New Energy Sources 7. Atomic Structure and Periodicity 7.1 Electromagnetic Radiation 7.2 The Nature of Matter 7.3 The Atomic Spectrum of Hydrogen 7.4 The Bohr Model 7.5 The Quantum Mechanical Model of the Atom 7.6 Quantum Numbers 7.7 Orbital Shapes and Energies 7.8 Electron Spin and the Pauli Principle 7.9 Polyelectronic Atoms 7.10 The History of the Periodic Table 7.11 The Aufbau Principle and the Periodic Table 7.12 Periodic Trends in Atomic Properties 7.13 The Properties of a Group: The Alkali Metals 8. Bonding: General Concepts 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character of Covalent Bonds 8.7 The Covalent Chemical Bond: A Model 8.8 Covalent Bond Energies and Chemical Reactions 8.9 The Localized Electron Bonding Model 8.10 Lewis Structures 8.11 Exceptions to the Octet Rule 8.12 Resonance 8.13 Molecular Structure: The VSEPR Model 9. Covalent Bonding: Orbitals 9.1 Hybridization and the Localized Electron Model 9.2 The Molecular Orbital Model 9.3 Bonding in Homonuclear Diatomic Molecules 9.4 Bonding in Heteronuclear Diatomic Molecules 9.5 Combining the Localized Electron and Molecular Orbital Models 10. Liquids and Solids 10.1 Intermolecular Forces 10.2 The Liquid State 10.3 An Introduction to Structures and Types of Solids 10.4 Structure and Bonding in Metals 10.5 Carbon and Silicon: Network Atomic Solids 10.6 Molecular Solids 10.7 Ionic Solids 10.8 Vapor Pressure and Changes of State 10.9 Phase Diagrams 11. Properties of Solutions 11.1 Solution Composition 11.2 The Energies of Solution Formation 11.3 Factors Affecting Solubility 11.4 The Vapor Pressures of Solutions 11.5 Boiling-Point Elevation and Freezing-Point Depression 11.6 Osmotic Pressure 11.7 Colligative Properties of Electrolyte Solutions 11.8 Colloids 12. Chemical Kinetics 12.1 Reaction Rates 12.2 Rate Laws: An Introduction 12.3 Determining the Form of the Rate Law 12.4 The Integrated Rate Law 12.5 Rate Laws: A Summary 12.6 Reaction Mechanisms 12.7 A Model for Chemical Kinetics 12.8 Catalysis 13. Chemical Equilibrium 13.1 The Equilibrium Condition 13.2 The Equilibrium Constant 13.3 Equilibrium Expressions Involving Pressures 13.4 Heterogeneous Equilibria 13.5 Applications of the Equilibrium Constant 13.6 Solving Equilibrium Problems 13.7 Le Ch√Ętelier's Principle 14. Acids and Bases 14.1 The Nature of Acids and Bases 14.2 Acid Strength 14.3 The pH Scale 14.4 Calculating the pH of Strong Acid Solutions 14.5 Calculating the pH of Weak Acid Solutions 14.6 Bases 14.7 Polyprotic Acids 14.8 Acid-Base Properties of Salts 14.9 The Effect of Structure on Acid-Base Properties 14.10 Acid-Base Properties of Oxides 14.11 The Lewis Acid-Base Model 14.12 Strategy for Solving Acid-Base Problems: A Summary 15. Applications of Aqueous Equilibria Acid-Base Equilibria 15.1 Solutions of Acids or Bases Containing a Common Ion 15.2 Buffered Solutions 15.3 Buffer Capacity 15.4 Titrations and pH Curves 15.5 Acid-Base Indicators Solubility Equilibria 15.6 Solubility Equilibria and the Solubility Product 15.7 Precipitation and Qualitative Analysis Complex Ion Equilibria 15.8 Equilibria Involving Complex Ions 16. Spontaneity, Entropy, and Free Energy 16.1 Spontaneous Processes and Entropy 16.2 Entropy and the Second Law of Thermodynamics 16.3 The Effect of Temperature on Spontaneity 16.4 Free Energy 16.5 Entropy Changes in Chemical Reactions 16.6 Free Energy and Chemical Reactions 16.7 The Dependence of Free Energy on Pressure 16.8 Free Energy and Equilibrium 16.9 Free Energy and Work 17. Electrochemistry 17.1 Galvanic Cells 17.2 Standard Reduction Potentials 17.3 Cell Potential, Electrical Work, and Free Energy 17.4 Dependence of Cell Potential on Concentration 17.5 Batteries 17.6 Corrosion 17.7 Electrolysis 17.8 Commercial Electrolytic Processes 18. The Nucleus: A Chemist's View 18.1 Nuclear Stability and Radioactive Decay 18.2 The Kinetics of Radioactive Decay 18.3 Nuclear Transformations 18.4 Detection and Uses of Radioactivity 18.5 Thermodynamic Stability of the Nucleus 18.6 Nuclear Fission and Nuclear Fusion 18.7 Effects of Radiation 19. The Representative Elements: Groups 1A Through 4A 19.1 A Survey of the Representative Elements 19.2 The Group 1A Elements 19.3 Hydrogen 19.4 The Group 2A Elements 19.5 The Group 3A Elements 19.6 The Group 4A Elements 20. The Representative Elements: Groups 5A Through 8A 20.1 The Group 5A Elements 20.2 The Chemistry of Nitrogen 20.3 The Chemistry of Phosphorus 20.4 The Group 6A Elements 20.5 The Chemistry of Oxygen 20.6 The Chemistry of Sulfur 20.7 The Group 7A Elements 20.8 The Group 8A Elements 21. Transition Metals and Coordination Chemistry 21.1 The Transition Metals: A Survey 21.2 The First-Row Transition Metals 21.3 Coordination Compounds 21.4 Isomerism 21.5 Bonding in Complex Ions: The Localized Electron Model 21.6 The Crystal Field Model 21.7 The Biologic Importance of Coordination Complexes 21.8 Metallurgy and Iron and Steel Production 22. Organic and Biological Molecules 22.1 Alkanes: Saturated Hydrocarbons 22.2 Alkenes and Alkynes 22.3 Aromatic Hydrocarbons 22.4 Hydrocarbon Derivatives 22.5 Polymers 22.6 Natural Polymers Appendix 1: Mathematical Procedures A1.1. Exponential Notation A1.2 Logarithms A1.3 Graphing Functions A1.4 Solving Quadratic Equations A1.5 Uncertainties in Measurements Appendix 2: The Quantitative Kinetic Molecular Model Appendix 3: Spectral Analysis Appendix 4: Selected Thermodynamic Data Appendix 5: Equilibrium Constants and Reduction Potentials A5.1 Values of Ka for Some Common Monoprotic Acids A5.2 Stepwise Dissociation Constants for Several Common Polyprotic Acids A5.3 Values of Kb for Some Common Weak Bases A5.4 Ksp Values at 25 degrees Celsius for Common Ionic Solids A5.5 Standard Reduction Potentials at 25 degrees Celsius (298K) for Many Common Half-Reactions Appendix 6: SI Units and Conversion Factors
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