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Overview

General Chemistry, 8/e, Media Enhanced Edition provides instructors the latest technology for their courses. Created to meet the rapidly changing instructional needs of General Chemistry professors, this edition includes an enhanced technology program that reinforces the approach of the text and updated information within the text to help students and instructors use these resources effectively. The Media Enhanced Edition provides access to assessment, tutoring, and presentation materials, including online homework, video lessons from Thinkwell, and a multimedia eBook, through Eduspace, Houghton Mifflin's Online Learning Tool. These resources make learning more dynamic and course planning, presentation, and management more intuitive. Known for its carefully developed, thoroughly integrated approach to problem solving, this market-leading text emphasizes the conceptual understanding and visualization skills essential for first-year chemistry and science majors. General Chemistry, 8/e, Media Enhanced Edition retains the hallmark pedagogical features of General Chemistry, 8/e, and expands upon the conceptual focus and art program through new interactive tutorials and animations.

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Product Details

  • ISBN-13: 9780395433027
  • Publisher: Houghton Mifflin Company College Division
  • Publication date: 12/1/1989
  • Edition description: 3rd ed
  • Edition number: 3

Meet the Author

Darrell Ebbing has taught general chemistry for more than thirty years and is now retired from Wayne State University. He received his Ph.D. in physical chemistry from Indiana University.

Steven D. Gammon is a professor of chemistry at Western Washington University and a leader in the development of multimedia-based software for chemical education. He has contributed greatly to the increased emphasis on conceptual understanding in the text.

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Table of Contents

Note: Each

Chapter concludes with A Checklist for Review, Review Questions, Conceptual Problems, Practice Problems, General Problems, Cumulative-Skills Problems, Online Study Center, and Media Summary.
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 Chemical Substances: Formulas and Names
2.6 Chemical Formulas; Molecular and Ionic Substances A Chemist Looks At: Thirty Seconds on the Island of Stability
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: QuantitativeRelations 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 Concentration
4.8 Diluting Solutions Quantitative Analysis
4.9 Gravimetric Analysis
4.10 Volumetric Analysis
5.The 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 Pressures 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 Fuels—Foods, 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 A Chemist Looks At: Levitating Frogs and People Periodicity of the Elements
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
9.2 Electron Configurations of Ions A Chemist Looks At: Ionic Liquids and Green Chemistry
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 A Chemist Looks At: Left-Handed and Right-Handed Molecules
10.2 Dipole Moment and Molecular Geometry
10.3 Valence Bond Theory
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
11.8 Structures of Some Crystalline Solids A Chemist Looks At: Liquid-Crystal Displays
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 A Chemist Looks At: Superconductivity Nonmetallic Materials
13.4 Diamond, Graphite, the Fullerenes, and Nanotechnology A Chemist Looks At: Buckminsterfullerene—A Third Form of Carbon
13.5 Semiconductors
13.6 Silicon, Silica, and Silicates A Chemist Looks At: Silica Aerogels, the Lightest "Solids"
13.7 Ceramics
13.8 Composites
14.Rates of Reaction Reaction Rates
14.1 Definition of Reaction Rate
14.2 Experimental Determination of Rate
14.3 Dependence of Rate on Concentration
14.4 Change of Concentration with Time
14.5 Temperature and Rate; Collision and Transition-State Theories
14.6 Arrhenius Equation Reaction Mechanisms
14.7 Elementary Reactions
14.8 The Rate Law and the Mechanism
14.9 Catalysis A Chemist Looks At: Seeing Molecules React
15.Chemical Equilibrium Describing Chemical Equilibrium
15.1 Chemical Equilibrium—A Dynamic Equilibrium
15.2 The Equilibrium Constant
15.3 Heterogeneous Equilibria; Solvents in Homogeneous Equilibria A Chemist Looks At: Slime Molds and Leopards' Spots Using the Equilibrium Constant
15.4 Qualitatively Interpreting the Equilibrium Constant
15.5 Predicting the Direction of Reaction
15.6 Calculating Equilibrium Concentrations Changing the Reaction Conditions; Le Chatelier's Principle
15.7 Removing Products or Adding Reactants
15.8 Changing the Pressure and Temperature
15.9 Effect of a Catalyst
16.Acids and Bases Acid-Base Concepts
16.1 Arrhenius Concept of Acids and Bases
16.2 Bronsted-Lowry Concept of Acids and Bases
16.3 Lewis Concept of Acids and Bases Acid and Base Strengths A Chemist Looks At: Taking Your Medicine
16.4 Relative Strengths of Acids and Bases
16.5 Molecular Structure and Acid Strength Self-Ionization of Water and pH
16.6 Self-Ionization of Water
16.7 Solutions of a Strong Acid or Base
16.8 The pH of a Solution A Chemist Looks At: Unclogging the Sink and Other Chores
17.Acid-Base Equilibria Solutions of a Weak Acid or Base
17.1 Acid-Ionization Equilibria
17.2 Polyprotic Acids A Chemist Looks At: Acid Rain
17.3 Base-Ionization Equilibria
17.4 Acid-Base Properties of Salt Solutions Solutions of a Weak Acid or Base with Another Solute
17.5 Common-Ion Effect
17.6 Buffers
17.7 Acid-Base Titration Curves
18.Solubility and Complex-Ion Equilibria Solubility Equilibria
18.1 The Solubility Product Constant
18.2 Solubility and the Common-Ion Effect
18.3 Precipitation Calculations
18.4 Effect of pH on Solubility A Chemist Looks At: Limestone Caves Complex-Ion Equilibria
18.5 Complex-Ion Formation
18.6 Complex Ions and Solubility An Application of Solubility Equilibria
18.7 Qualitative Analysis of Metal Ions
19.Thermodynamics and Equilibrium
19.1 First Law of Thermodynamics; Enthalpy Spontaneous Processes and Entropy
19.2 Entropy and the Second Law of Thermodynamics
19.3 Standard Entropies and the Third Law of Thermodynamics Free-Energy Concept
19.4 Free Energy and Spontaneity A Chemist Looks At: Coupling of Reactions
19.5 Interpretation of Free Energy Free Energy and Equilibrium Constants
19.6 Relating G to the Equilibrium Constant
19.7 Change of Free Energy with Temperature
20.Electrochemistry Half-Reactions
20.1 Balancing Oxidation-Reduction Reactions in Acidic and Basic Solutions Voltaic Cells
20.2 Construction of Voltaic Cells
20.3 Notation for Voltaic Cells
20.4 Electromotive Force
20.5 Standard Cell emfs and Standard Electrode Potentials
20.6 Equilibrium Constants from emfs
20.7 Dependence of emf on Concentration
20.8 Some Commercial Voltaic Cells Electrolytic Cells
20.9 Electrolysis of Molten Salts
20.10 Aqueous Electrolysis
20.11 Stoichiometry of Electrolysis
21.Nuclear Chemistry Radioactivity and Nuclear Bombardment Reactions
21.1 Radioactivity
21.2 Nuclear Bombardment Reactions
21.3 Radiations and Matter: Detection and Biological Effects
21.4 Rate of Radioactive Decay
21.5 Applications of Radioactive Isotopes Energy of Nuclear Reactions A Chemist Looks At: Positron Emission Tomography (PET)
21.6 Mass-Energy Calculations
21.7 Nuclear Fission and Nuclear Fusion A Chemist Looks At: The Chernobyl Nuclear Accident
22.Chemistry of the Main-Group Elements
22.1 General Observations About the Main-Group Elements Chemistry of the Main-Group Metals
22.2 Group IA: The Alkali Metals
22.3 Group IIA: The Alkaline Earth Metals
22.4 Group IIIA and Group IVA Metals Chemistry of the Nonmetals
22.5 Hydrogen
22.6 Group IVA: The Carbon Family
22.7 Group VA: Nitrogen and the Phosphorus Family
22.8 Group VIA: Oxygen and the Sulfur Family
22.9 Group VIIA: The Halogens
22.10 Group VIIIA: The Noble Gases
23.The Transition Elements and Coordination Compounds Properties of the Transition Elements
23.1 Periodic Trends in the Transition Elements
23.2 The Chemistry of Two Transition Elements Complex Ions and Coordination Compounds
23.3 Formation and Structure of Complexes
23.4 Naming Coordination Compounds A Chemist Looks At: Salad Dressing and Chelate Stability
23.5 Structure and Isomerism in Coordination Compounds
23.6 Valence Bond Theory of Complexes
23.7 Crystal Field Theory A Chemist Looks At: The Cooperative Release of Oxygen from Oxyhemoglobin
24.Organic Chemistry
24.1 The Bonding of Carbon Hydrocarbons
24.2 Alkanes and Cycloalkanes
24.3 Alkenes and Alkynes
24.4 Aromatic Hydrocarbons
24.5 Naming Hydrocarbons Derivatives of Hydrocarbons
24.6 Organic Compounds Containing Oxygen
24.7 Organic Compounds Containing Nitrogen
25.Polymer Materials: Synthetic and Biological Synthetic Polymers
25.1 Synthesis of Organic Polymers A Chemist Looks At: The Discovery of Nylon
25.2 Electrically Conducting Polymers Biological Polymers
25.3 Proteins
25.4 Nucleic Acids A Chemist Looks At: Tobacco Mosaic Virus and Atomic Force Microscopy Appendices A. Mathematical Skills B. Vapor Pressure of Water at Various Temperatures C. Thermodynamic Quantities for Substances and Ions at 25 C D. Electron Configurations of Atoms in the Ground State E. Acid-Ionization Constants at 25 C F. Base-Ionization Constants at 25 C G. Solubility Product Constants at 25 C H. Formation Constants of Complex Ions at 25 C I. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25 C Answers to Exercises Answers to Concept Checks Answers to Odd-Numbered Problems Glossary Photo Credits
Index

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