عنوان

Chemistry :

(Number (ISBN

0547053932

(Number (ISBN

9780547053936

Number

b604265

Title Proper

Chemistry :

General Material Designation

[Book]

Other Title Information

the practical science

First Statement of Responsibility

Paul Kelter, Michael Mosher, Andrew Scott; contributing writer, Charles Wiliam McLaughlin.

Edition Statement

Media enhanced ed

Place of Publication, Distribution, etc.

Boston

Name of Publisher, Distributor, etc.

Houghton Mifflin

Date of Publication, Distribution, etc.

©2009.

Specific Material Designation and Extent of Item

xxxii, 969, 86 pages : color illustrations ; 29 cm

Text of Note

Includes index.

Text of Note

Note: Each chapter begins with "Contents and Applications." 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 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 Energy Flows Between a System and Its Surroundings 5.3 Keeping Track of Energy 5.4 Specific Heat Capacity and Heat Capacity 5.5 Enthalpy 5.6 Hess's Law 5.7 Energy Choices 6. Quantum Chemistry--The Strange World of Atoms 6.1 Introducing Quantum Chemistry 6.2 Electromagnetic Radiation 6.3 Atomic Emission Spectroscopy 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 deBroglie and Heisenberg Discussions 6.9 The Mathematical Language of Quantum Chemistry 6.10 Atomic Orbitals 6.11 Electron Spin and Pauli's Exclusion Principle 6.12 Orbitals and Energy Levels in Multi-electron Atoms 6.13 Electron Configurations and the Aufbau Principle 7. Periodic Properties of the Elements 7.1 Building the Periodic Table 7.2 Metals, Non-Metals and Metalloids 7.3 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 Compounds and Molecules 9. Advanced Models of Bonding 9.1 Valence Bond Theory 9.2 Hybridization 9.3 Molecular Orbital Theory 9.4 Putting it all together 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 11.4 Phase Diagrams 11.5 Water: The Universal Solvent 11.6 Measures of Solution Concentration 11.7 The Effect of Temperature and Pressure on Solubility 11.8 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 and the C=C bond 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 The Carbon Cycle 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 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 Review of 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 Credits Index/Glossary

Chemistry -- Textbooks.

Chemistry.

Class number

Book number

Paul Kelter, Michael Mosher, Andrew Scott; contributing writer, Charles Wiliam McLaughlin.

Andrew Scott

Michael D Mosher

Paul B Kelter

Electronic name

[Book]

Y