Chemistry

The Practical Science

Inbunden, Engelska, 2007

Av Paul Kelter, Michael Mosher, Andrew Scott

1 009 kr

Slutsåld

From core concepts to current applications, "Chemistry: The Practical Science" promotes an interrogative approach that develops effective problem solvers and critical thinkers for today's world. Using the text and its pedagogical features as a model, students learn to appreciate the role of questioning in the process of chemistry and begin to think like chemists. In addition applications woven throughout the narrative, examples, and exercises present core chemical concepts in the context of everyday life. This integrated approach encourages curiosity and demonstrates the relevance of chemistry and its uses in students' lives, their future careers, and their world. "Chemistry" introduces new topics as an instructor would in the classroom. The authors' approach to problem solving prompts students to begin by asking questions about the topic, think critically to arrive at a solution, evaluate their answers, and uncover related information about the concepts being explored. A dynamic art program, comprehensive end-of-chapter materials, and powerful technology resources complete this innovative textbook program.

Produktinformation

Utgivningsdatum2007-01-02
Mått226 x 284 x 40 mm
Vikt2 460 g
FormatInbunden
SpråkEngelska
FörlagCengage Learning, Inc
ISBN9780618000722

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Note: Each chapter concludes with "The Bottom Line," Key Words, and "Focus Your Learning." 1. The World of Chemistry 1.1 What Do Chemists do? 1.2 The Chemist's Shorthand 1.3 The Scientific Method 1.4 Units and Measurement 1.5 Conversions and Dimensional Analysis 1.6 Uncertainty, Precision, Accuracy, and Significant Figures 1.7 The Chemical Challenges of the Future 2. Atoms: A Quest for Understanding 2.1 Early Attempts to Explain Matter 2.2 Dalton's Atomic Theory and Beyond 2.3 The Structure of the Atom 2.4 Atoms and Isotopes 2.5 Atomic Mass 2.6 The Periodic Table 2.7 Ionic Compounds 2.8 Molecules 2.9 Naming Compounds 2.10 Naming Acids 3. Introducing Quantitative Chemistry 3.1 Formula Masses 3.2 Counting by Weighing 3.3 Working with Moles 3.4 Percentages by Mass 3.5 Finding the Formula 3.6 Chemical Equations 3.7 Working with Equations 4. Solution Stoichiometry and Types of Reactions 4.1 Water--A Most Versatile Solvent 4.2 The Concentration of Solutions 4.3 Stoichiometric Analysis of Solutions 4.4 Types of Chemical Reactions 4.5 Precipitation Reactions 4.6 Acid-Base Reactions 4.7 Oxidation-Reduction Reactions 4.8 Fresh Water--Issues of Quantitative Chemistry 5. Energy 5.1 The Concept of Energy 5.2 Keeping Track of Energy 5.3 Specific Heat Capacity and Heat Capacity 5.4 Enthalpy 5.5 Hess's Law 5.6 Energy Choices 6. Quantum Chemistry: The Strange World of Atoms 6.1 Introducing Quantum Chemistry 6.2 Electromagnetic Radiation 6.3 Atomic Emission and Absorption Spectroscopy, Chemical Analysis and the Quantum Number 6.4 The Bohr Model of Atomic Structure 6.5 Wave-Particle Duality 6.6 Why Treating Things as "Waves" Allows Us to Quantize Their Behavior 6.7 The Heisenberg Uncertainty Principle 6.8 More About the Photon--The de Broglie and Heisenberg Discussions 6.9 The Mathematical Language of Quantum Chemistry 6.10 Atomic Orbitals 6.11 Electron Spin and the Pauli Exclusion Principle 6.12 Orbitals and Energy Levels in Multielectron Atoms 6.13 Electron Configurations and the Aufbau Principle 7. Periodic Properties of the Elements 7.1 The Big Picture--Building the Periodic Table 7.2 The First Level of Structure--Metals, Non-Metals and Metalloids 7.3 The Next Level of Structure--Groups in the Periodic Table 7.4 The Concept of Periodicity 7.5 Atomic Size 7.6 Ionization Energies 7.7 Electron Affinity 7.8 Electronegativity 7.9 Reactivity 7.10 The Elements and the Environment 8. Bonding Basics 8.1 Modeling Bonds 8.2 Ionic Bonding 8.3 Covalent Bonding 8.4 VSEPR Theory--A Better Model 8.5 Properties of Ionic and Molecular Compounds 9. Advanced Models of Bonding 9.1 Valence Bond Theory 9.2 Hybridization 9.3 Molecular Orbital Theory 9.4 Putting It All Together 9.5 Molecular Models in the Chemist's Toolbox 10. The Behavior and Applications of Gases 10.1 The Nature of Gases 10.2 Production of Hydrogen and the Meaning of Pressure 10.3 Mixtures of Gases--Dalton's Law and Food Packaging 10.4 The Gas Laws--Relating the Behavior of Gases to Key Properties 10.5 The Ideal Gas Equation 10.6 Applications of the Ideal Gas Equation 10.7 Kinetic Molecular Theory 10.8 Effusion and Diffusion 10.9 Industrialization: A Wonderful, Yet Cautionary, Tale 11. Chemistry of Water and the Nature of Liquids 11.1 The Structure of Water: An Introduction to Intermolecular Forces 11.2 A Closer Look at Intermolecular Forces 11.3 Impact of Intermolecular Forces on the Physical Properties of Water I 11.4 Phase Diagrams 11.5 Impact of Intermolecular Forces on the Physical Properties of Water II 11.6 Water: The Universal Solvent 11.7 Measures of Solution Concentration 11.8 The Effect of Temperature and Pressure on Solubility 11.9 Colligative Properties 12. Carbon 12.1 Elemental Carbon 12.2 Crude Oil--The Basic Resource 12.3 Hydrocarbons 12.4 Separating the Hydrocarbons by Fractional Distillation 12.5 Processing Hydrocarbons 12.6 Typical Reactions of the Alkanes 12.7 The Functional Group Concept 12.8 Ethene, the C=C Bond, and Polymers 12.9 Alcohols 12.10 From Alcohols to Aldehydes, Ketones, and Carboxylic Acids 12.11 From Alcohols and Carboxylic Acids to Esters 12.12 Condensation Polymers 12.13 Polyethers 12.14 Handedness in Molecules 12.15 Organic Chemistry and Modern Drug Discovery 13. Modern Materials 13.1 The Structure of Crystals 13.2 Metals 13.3 Ceramics 13.4 Plastics 13.5 Thin Films and Surface Analysis 13.6 On the Horizon--What Does the Future Hold? 14. Thermodynamics: A Look at Why Reactions Happen 14.1 Probability as a Predictor of Chemical Behavior 14.2 Why Do Chemical Reactions Happen? Entropy and the Second Law of Thermodynamics 14.3 Temperature and Spontaneous Processes 14.4 Calculating Entropy Changes in Chemical Reactions 14.5 Free Energy 14.6 When ?G = 0; A Taste of Equilibrium 15. Chemical Kinetics 15.1 Reaction Rates 15.2 An Introduction to Rate Laws 15.3 Changes in Time--The Integrated Rate Law 15.4 Methods of Determining Rate Laws 15.5 Looking Back at Rate Laws 15.6 Reaction Mechanisms 15.7 Applications of Catalysts 16. Chemical Equilibrium 16.1 The Concept of Chemical Equilibrium 16.2 Why Is Chemical Equilibrium a Useful Concept? 16.3 The Meaning of the Equilibrium Constant 16.4 Working With Equilibrium Constants 16.5 Solving Equilibrium Problems--A Different Way of Thinking 16.6 Le Chatelier's Principle 16.7 Free Energy and the Equilibrium Constant 17. Acids and Bases 17.1 What Are Acids and Bases? 17.2 Acid Strength 17.3 The pH Scale 17.4 Determining the pH of Acid Solutions 17.5 Determining the pH of Basic Solutions 17.6 Polyprotic Acids 17.7 Assessing the Acid-Base Behavior of Salts in Aqueous Solution 17.8 Anhydrides in Aqueous Solution 18. Applications of Aqueous Equilibria 18.1 Buffers and the Common-Ion Effect 18.2 Acid-Base Titrations 18.3 Solubility Equilibria 18.4 Complex-Ion Equilibria 19. Electrochemistry 19.1 What Is Electrochemistry? 19.2 Oxidation States--Electronic Bookkeeping 19.3 Redox Equations 19.4 Electrochemical Cells 19.5 Chemical Reactivity Series 19.6 Not-So-Standard Conditions: The Nernst Equation 19.7 Electrolytic Reactions 20. Coordination Complexes 20.1 Bonding in Coordination Complexes 20.2 Ligands 20.3 Coordination Number 20.4 Structure 20.5 Isomers 20.6 Formulas and Names 20.7 Color and Coordination Compounds 20.8 Chemical Reactions 21. Nuclear Chemistry 21.1 Isotopes and More Isotopes 21.2 Types of Radioactive Decay 21.3 Interaction of Radiation with Matter 21.4 The Kinetics of Radioactive Decay 21.5 Mass and Binding Energy 21.6 Nuclear Stability and Human-made Radioactive Nuclides 21.7 Splitting the Atom: Nuclear Fission 21.8 Medical Uses of Radioisotopes 22. The Chemistry of Life 22.1 DNA--The Basic Structure 22.2 Proteins 22.3 How Genes Code for Proteins 22.4 Enzymes 22.5 The Diversity of Protein Functions 22.6 Carbohydrates 22.7 Lipids 22.8 The Maelstrom of Metabolism 22.9 Biochemistry and Chirality 22.10 A Look to the Future Appendix 1. Mathematical Operations. A1.1 Working with Exponents. A1.2 Working with Logarithms. A1.3 Solving the Quadratic Equation. A1.4 Graphing Appendix 2. Calculating Uncertainties in Measurements Appendix 3. Thermodynamic Data for Selected Compounds at 298 K Appendix 4. Colligative Property Constants for Selected Compounds Appendix 5. Selected Equilibrium Constants at 298 K Appendix 6. Water Vapor Pressure Table Appendix 7. Standard Reduction Potentials at 298 K Appendix 8. Common Radioactive Nuclei Answers to Practice Exercises and Selected Exercises Index/Glossary