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Chemistry - With Media Guide

Chemistry - With Media Guide - 6th edition

ISBN13: 978-0618544073

Cover of Chemistry - With Media Guide 6TH 03 (ISBN 978-0618544073)
ISBN13: 978-0618544073
ISBN10: 0618544070
Edition: 6TH 03
Copyright: 2003
Publisher: Houghton Mifflin Harcourt
Published: 2003
International: No

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Chemistry - With Media Guide - 6TH 03 edition

ISBN13: 978-0618544073

Steven S. Zumdahl and Susan A. Zumdahl

ISBN13: 978-0618544073
ISBN10: 0618544070
Edition: 6TH 03
Copyright: 2003
Publisher: Houghton Mifflin Harcourt
Published: 2003
International: No

For instructors who want the latest technology--without the frequent textbook revisions--Houghton Mifflin presents Chemistry, 6/e (©2003), with new the Virtual Toolbox for Chemistry. Available for Fall 2005 courses, this suite of teaching and learning technology tools supports new and existing Chemistry users and meets the rapidly changing instructional demands of General Chemistry professors. The Virtual Toolbox offers access to tutoring, assessment, and presentation tools through the comprehensive Eduspace Course Management tool--instructors can also choose selected resources for use separately via CD-ROM or the Web. These resources are certain to make learning more dynamic and course planning, presentation, and management more intuitive.

Chemistry, 6/e, owes its success to its conceptual approach to problem-solving, high-quality end-of-chapter problems, and student friendly writing style. A strong emphasis on models and real-world applications prevails throughout the text.

  • The Virtual Toolbox provides a suite of integrated technology tools for students and instructors. All materials (except restricted testing items) are web accessible, with passwords included in the media guides. In addition, to meet instructor needs, the Media Integration Guide for Instructors includes CD-ROMs containing all teaching resources.
  • To ensure that students devote more time to their study of chemistry, key elements of the Virtual Toolbox are assignable. In the classroom, instructors can gauge student progress though a Classroom Response System. Online homework within Eduspace--using either end-of-chapter questions or interactive ChemWork problems--can be tracked and graded. Even new animations--now with skill-building exercises--can be assigned.
  • To provide instructors with greater assessment capabilities, an expanded set of HM Testing questions and improved test bank functionality now supports the text.
  • For the visual learner, several new resources are provided, including animations on the HM ClassPresent v.2 CD-ROM and/or the student web site/student CD-ROM.
  • To support you and your students as you use our technology, we offer implementation services from our Team UP support staff, as well as carefully revised and expanded media integration guides for both students and instructors, along with significant updates to the textbook web sites--including a 60-day Eduspace trial.
  • The authors emphasize a qualitative approach to chemistry in the text and technology program before quantitative problems are considered, helping build student understanding.
  • Worked-out Examples throughout the text present a thoughtful, step-by-step approach to solving problems.
  • A wealth of end-of-chapter questions reinforce conceptual understanding and sharpen problem solving skills: collaborative In-Class Discussion Questions, Exercises organized by topic, Additional Exercises not keyed by topic, integrative Challenge Problems, comprehensive Marathon Problems, and web-related Media Activities.
  • Eduspace (powered by Blackboard), Houghton Mifflin's complete course management solution, features two sets of online problems: end-of-chapter algorithmic questions and ChemWork interactive online homework with links to corresponding textbook pages for student reference at point of learning. ChemWork assignments help students learn the process of thinking like a chemist: as students work through unique, text-based assignments, a system of interactive, encouraging hints is available to help them think through each problem.

Table of Contents

Note: Each chapter concludes with a Summary, 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 Atomic Masses
3.2 The Mole
3.3 Molar Mass
3.4 Percent Composition of Compounds
3.5 Determining the Formula of a Compound
3.6 Chemical Equations
3.7 Balancing Chemical Equations
3.8 Stoichiometric Calculations: Amounts of Reactants and Products
3.9 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 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 Principles 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 Formation of 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 Châtelier'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 Potential
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
Appendix 2. The Quantitative Kinetic Molecular Model
Appendix 3. Spectral Analysis
Appendix 4. Selected Thermodynamic Data
Appendix 5. Equilibrium Constants and Reduction Potentials
Appendix 6. SI Units and Conversion Factors

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