General Chemistry : Text with Student Technology Package

Name: General Chemistry : Text with Student Technology Package
Availability: OutOfStock
ISBN: 9780618141012

ISBN-10: 0618141014

ISBN-13: 9780618141012

Edition: 7th 2002

Authors: Darrell D. Ebbing, Steven D. Gammon

List price: $142.36

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From the very first edition of this bestselling text, the authors have been committed to writing clear, lucid explanations of general chemistry concepts. A technology learning package offers resources to facilitate learning and teaching.

Book details

List price: $142.36
Edition: 7th
Copyright year: 2002
Publisher: Houghton Mifflin College Division
Binding: CD-ROM
Pages: 1110
Size: 8.25" wide x 10.25" long x 1.75" tall
Weight: 5.588
Language: English

Contents Note: Each chapter concludes with A Checklist for Review, Review Questions, Conceptual Problems, Practice Problems, General Problems, Cumulative-Skills Problems, and Media Activities 1. Chemistry and Measurement An Introduction to Chemistry 1.1 Modern Chemistry: A Brief Glimpse 1.2 Experiment and Explanation A Chemist Looks At: The Birth of the Post-It Note 1.3 Law of Conservation of Mass 1.4 Matter: Physical State and Chemical Constitution Instrumental Methods: Separation of Mixtures by Chromatography Physical Measurements 1.5 Measurement and Significant Figures 1.6 SI Units 1.7 Derived Units 1.8 Units and Dimensional Analysis (Factor-Label Method) 2. Atoms, Molecules, and Ions… Atomic Theory and Atomic Structure 2.1 Atomic Theory of Matter 2.2 The Structure of the Atom 2.3 Nuclear Structure; Isotopes 2.4 Atomic Weights 2.5 Periodic Table of the Elements A Chemist Looks At: Thirty Seconds on the Island of Stability Chemical Substances: Formulas and Names 2.6 Chemical Formulas; Molecular and Ionic Substances 2.7 Organic Compounds 2.8 Naming Simple Compounds Chemical Reactions: Equations 2.9 Writing Chemical Equations 2.10 Balancing Chemical Equations 3. Calculations with Chemical Formulas and Equations Mass and Moles of Substance 3.1 Molecular Weight and Formula Weight 3.2 The Mole Concept Determining Chemical Formulas 3.3 Mass Percentages from the Formula 3.4 Elemental Analysis: Percentages of Carbon, Hydrogen, and Oxygen 3.5 Determining Formulas Instrumental Methods: Mass Spectrometry and Molecular Formula Stoichiometry: Quantitative Relations in Chemical Reactions 3.6 Molar Interpretation of a Chemical Equation 3.7 Amounts of Substances in a Chemical Reaction 3.8 Limiting Reactant: Theoretical and Percentage Yields 4. Chemical Reactions Ions in Aqueous Solution 4.1 Ionic Theory of Solutions and Solubility Rules 4.2 Molecular and Ionic Equations Types of Chemical Reactions 4.3 Precipitation Reactions 4.4 Acid-Base Reactions 4.5 Oxidation-Reduction Reactions 4.6 Balancing Simple Oxidation-Reduction Equations Working with Solutions 4.7 Molar Concentrations 4.8 Diluting Solutions Quantitative Analysis 4.9 Gravimetric Analysis 4.10 Volumetric Analysis 5. Gaseous State Gas Laws 5.1 Gas Pressure and Its Measurement 5.2 Empirical Gas Laws 5.3 The Ideal Gas Law A Chemist Looks At: Nitric Oxide Gas and Biological Signaling 5.4 Stoichiometry Problems Involving Gas Volumes 5.5 Gas Mixtures; Law of Partial Pressure Kinetic-Molecular Theory 5.6 Kinetic Theory of an Ideal Gas 5.7 Molecular Speeds; Diffusion and Effusion 5.8 Real Gases A Chemist Looks At: Carbon Dioxide Gas and the Greenhouse Effect 6. Thermochemistry Understanding Heats of Reaction 6.1 Energy and Its Units 6.2 Heat of Reaction 6.3 Enthalpy and Enthalpy Change 6.4 Thermochemical Equations A Chemist Looks At: Lucifers and Other Matches 6.5 Applying Stoichiometry to Heats of Reaction 6.6 Measuring Heats of Reaction Using Heats of Reaction 6.7 Hess's Law 6.8 Standard Enthalpies of Formation 6.9 FuelsFoods, Commercial Fuels, and Rocket Fuels 7. Quantum Theory of the Atom Light Waves, Photons, and the Bohr Theory 7.1 The Wave Nature of Light 7.2 Quantum Effects and Photons A Chemist Looks At: Zapping Hamburger with Gamma Rays 7.3 The Bohr Theory of the Hydrogen Atom A Chemist Looks At: Lasers and Compact Disc Players Quantum Mechanics and Quantum Numbers 7.4 Quantum Mechanics Instrumental Methods: Scanning Tunneling Microscopy 7.5 Quantum Numbers and Atomic Orbitals 8. Electron Configurations and Periodicity Electronic Structure of Atoms 8.1 Electron Spin and the Pauli Exclusion Principle Instrumental Methods: Nuclear Magnetic Resonance (NMR) 8.2 Building-Up Principle and the Periodic Table Instrumental Methods: X Rays, Atomic Numbers, and Orbital Structure (Photoelectron Spectroscopy) 8.3 Writing Electron Configurations Using the Periodic Table 8.4 Orbital Diagrams of Atoms; Hund's Rule Periodicity of the Elements A Chemist Looks At: Levitating Frogs and People 8.5 Mendeleev's Predictions from the Periodic Table 8.6 Some Periodic Properties 8.7 Periodicity in the Main-Group Elements 9. Ionic and Covalent Bonding Ionic Bonds 9.1 Describing Ionic Bonds A Chemist Looks At: Ionic Liquids and Green Chemistry 9.2 Electron Configurations of Ions 9.3 Ionic Radii Covalent Bonds 9.4 Describing Covalent Bonds A Chemist Looks At: Chemical Bonds in Nitroglycerin 9.5 Polar Covalent Bonds; Electronegativity 9.6 Writing Lewis Electron-Dot Formulas 9.7 Delocalized Bonding: Resonance 9.8 Exceptions to the Octet Rule 9.9 Formal Charge and Lewis Formulas 9.10 Bond Length and Bond Order 9.11 Bond Energy Instrumental Methods: Infrared Spectroscopy and Vibrations of Chemical Bonds 10. Molecular Geometry and Chemical Bonding Theory Molecular Geometry and Directional Bonding 10.1 The Valence-Shell Electron-Pair Repulsion (VSEPR) Model 10.2 Dipole Moment and Molecular Geometry A Chemist Looks At: Left-Handed and Right-Handed Molecules 10.3 Valence Bond Theory A Chemist Looks At: OrbitalsThe Glue of Chemical Bonding 10.4 Description of Multiple Bonding Molecular Orbital Theory 10.5 Principles of Molecular Orbital Theory 10.6 Electron Configurations of Diatomic Molecules of the Second-Period Elements 10.7 Molecular Orbitals and Delocalized Bonding A Chemist Looks At: Human Vision A Chemist Looks At: Stratospheric Ozone (An Absorber of Ultraviolet Rays) 11. States of Matter; Liquids and Solids 11.1 Comparison of Gases, Liquids, and Solids Changes of State 11.2 Phase Transitions 11.3 Phase Diagrams A Chemist Looks At: Removing Caffeine from Coffee Liquid State 11.4 Properties of Liquids: Surface Tension and Viscosity 11.5 Intermolecular Forces; Explaining Liquid Properties Solid State 11.6 Classification of Solids by Type of Attraction of Units 11.7 Crystalline Solids; Crystal Lattices and Unit Cells A Chemist Looks At: Liquid-Crystal Displays 11.8 Structures of Some Crystalline Solids 11.9 Calculations Involving Unit-Cell Dimensions 11.10 Determining Crystal Structure by X-Ray Diffraction Instrumental Methods: Automated X-Ray Diffractometry A Chemist Looks At: Water (A Special Substance for Planet Earth) 12. Solutions Solution Formation 12.1 Types of Solutions 12.2 Solubility and the Solution Process A Chemist Looks At: Hemoglobin Solubility and Sickle-Cell Anemia 12.3 Effects of Temperature and Pressure on Solubility Colligative Properties 12.4 Ways of Expressing Concentration 12.5 Vapor Pressure of a Solution 12.6 Boiling-Point Elevation and Freezing-Point Depression 12.7 Osmosis 12.8 Colligative Properties of Ionic Solutions Colloid Formation 12.9 Colloids A Chemist Looks At: The World's Smallest Test Tubes 13. Materials of Technology Metals and Metallurgy 13.1 Natural Sources of the Metallic Elements 13.2 Metallurgy 13.3 Bonding in Metals Nonmetallic Materials A Chemist Looks At: Superconductivity 13.4 Diamond, Graphite, t