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Introduction To Chemical Principles (9TH 08 - Old Edition)

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Introduction To Chemical Principles (9TH 08 - Old Edition) Cover

 

Synopses & Reviews

Please note that used books may not include additional media (study guides, CDs, DVDs, solutions manuals, etc.) as described in the publisher comments.

Publisher Comments:

This solid, yet value-priced paperback gives you the background and confidence you'll need to succeed in chemistry. Stoker focuses on the most important topics—omitting organic and biochemistry chapters—and teaches the problem-solving skills students in this course need. Each topic is developed at “ground level,” and continues step by step until the level of sophistication required for a further chemistry course is attained.

Synopsis:

This text gives readers the background (and confidence) they need in chemistry. Stoker's book focuses on the most important topics (this text omits organic and biochemistrychapters), and teaches the problem-solving skills students need, all at an affordable price.

About the Author

Stephen Stoker of Weber State University in Ogden, UT, has taught the gamut of introductory chemistry courses, specializing in GOB, for the past 30 years. Weber State has a very large Health Professions school, and GOB is geared at students with little or no experience in chemistry (notably Allied Health and Nursing majors).

Table of Contents

1        The Science of Chemistry

1.1      Chemistry–A Scientific Discipline

1.2      Scientific Disciplines and Technology

1.3      The Scope of Chemistry and Chemical Technology

1.4      How Chemists Discover Things–The Scientific Method

1.5      The Limitations of Science

 

2        Numbers from Measurements

2.1      The Importance of Measurement

2.2      Exact and Inexact Numbers

2.3      Accuracy, Precision, and Error

2.4      Uncertainty in Measurements

2.5      Significant Figures

2.6      Significant Figures and Mathematical Operations

2.7      Scientific Notation

2.8      Mathematical Operations in Scientific Notation

 

3        Unit Systems and Dimensional Analysis

3.1      The Metric System of Units

3.2      Metric Units of Length

3.3      Metric Units of Mass

3.4      Metric Units of Volume

3.5      Units in Mathematical Operations

3.6      Conversion Factors

3.7      Dimensional Analysis

3.8      Density

3.9      Equivalence Conversion Factors Other than Density

3.10    Percentage and Percent Error

3.11    Temperature Scales

 

4        Basic Concepts about Matter

4.1      Chemistry–The Study of Matter

4.2      Physical States of Matter

4.3      Properties of Matter

4.4      Changes in Matter

4.5      Pure Substances and Mixtures

4.6      Heterogeneous and Homogeneous Mixtures

4.7      Elements and Compounds

4.8      Discovery and Abundance of the Elements

4.9      Names and Chemical Symbols of the Elements

 

5        Atoms, Molecules, Formulas, and Subatomic Particles

5.1      The Atom

5.2      The Molecule

5.3      Natural and Synthetic Compounds

5.4      Chemical Formulas

5.5      Subatomic Particles: Protons, Neutrons, and Electrons

5.6      Atomic Number and Mass Number

5.7      Isotopes

5.8      Atomic Masses

5.9      Evidence Supporting the Existence and Arrangement of Subatomic Particles

 

6        Electronic Structure and Chemical Periodicity

6.1      The Periodic Law

6.2      The Periodic Table

6.3      The Energy of an Electron 

6.4      Electron Shells 

6.5      Electron Subshells

6.6      Electron Orbitals

6.7      Electron Configurations

6.8      Orbital Diagrams

6.9      Electron Configurations and the Periodic Law

6.10    Electron Configurations and the Periodic Table

6.11    Classification Systems for the Elements

6.12    Chemical Periodicity

 

7        Chemical Bonds

7.1      Types of Chemical Bonds

7.2      Valence Electrons and Lewis Symbols

7.3      The Octet Rule

7.4      The Ionic Bond Model

7.5      The Sign and Magnitude of Ionic Charge

7.6      Ionic Compound Formation

7.7      Chemical Formulas for Ionic Compounds

7.8      Structure of Ionic Compounds

7.9      Polyatomic Ions

7.10    The Covalent Bond Model

7.11    Lewis Structures for Molecular Compounds

7.12    Single, Double, and Triple Covalent Bonds

7.13    Valence Electron Count and Number of Covalent Bonds Formed

7.14    Coordinate Covalent Bonds

7.15    Resonance Structures

7.16    Systematic Procedures for Drawing Lewis Structures

7.17    Molecular Geometry

7.18    Electronegativity

7.19    Bond Polarity

7.20    Molecular Polarity

 

8        Chemical Nomenclature

8.1      Classification of Compounds for Nomenclature Purposes

8.2      Types of Binary Ionic Compounds

8.3      Nomenclature for Binary Ionic Compounds

8.4      Nomenclature for Ionic Compounds Containing Polyatomic Ions

8.5      Nomenclature for Binary Molecular Compounds

8.6      Nomenclature for Acids

8.7      Nomenclature Rules–A Summary

 

9        Chemical Calculations: The Mole Concept and Chemical Formulas

9.1      The Law of Definite Proportions

9.2      Calculation of Formula Masses

9.3      Significant Figures and Atomic Mass

9.4      Percent Composition

9.5      The Mole: The Chemist’s Counting Unit

9.6      The Mass of a Mole

9.7      Significant Figures and Avogadro’s Number

9.8      Relationship Between Atomic Mass Units and Gram Units

9.9      The Mole and Chemical Formulas

9.10    The Mole and Chemical Calculations

9.11    Purity of Samples

9.12    Empirical and Molecular Formulas

9.13    Determination of Empirical Formulas

9.14    Determination of Molecular Formulas

 

10      Chemical Calculations Involving Chemical Equations

10.1    The Law of Conservation of Mass

10.2    Writing Chemical Equations

10.3    Balancing Chemical Equations

10.4    Special Symbols Used in Chemical Equations

10.5    Classes of Chemical Reactions

10.6    Chemical Equations and the Mole Concept

10.7    Balanced Chemical Equations and the Law of Conservation of Mass

10.8    Calculations Based on Chemical Equations–Stoichiometry

10.9    The Limiting Reactant Concept

10.10  Yields: Theoretical, Actual, and Percent

10.11  Simultaneous and Sequential Chemical Reactions

 

11      States of Matter

11.1    Factors That Determine Physical State

11.2    Property Differences Among Physical States

11.3    The Kinetic Molecular Theory of Matter

11.4    The Solid State

11.5    The Liquid State

11.6    The Gaseous State

11.7    A Comparison of Solids, Liquids, and Gases

11.8    Endothermic and Exothermic Changes of State

11.9    Heat Energy and Specific Heat

11.10  Temperature Changes as a Substance Is Heated

11.11  Energy and Changes of State

11.12  Heat Energy Calculations

11.13  Evaporation of Liquids

11.14  Vapor Pressure of Liquids

11.15  Boiling and Boiling Points

11.16  Intermolecular Forces in Liquids

11.17  Types of Solids

 

12      Gas Laws

12.1    Properties of Some Common Gases

12.2    Gas Law Variables

12.3    Boyle’s Law: A Pressure—Volume Relationship

12.4    Charles’s Law: A Temperature—Volume Relationship

12.5    Gay-Lussac’s Law: A Temperature—Pressure Relationship

12.6    The Combined Gas Law

12.7    Standard Conditions for Temperature and Pressure

12.8    Avogadro’s Law

12.9    Standard Molar Volume of a Gas

12.10  The Ideal Gas Law

12.11  Modified Forms of the Ideal Gas Law

12.12  Volumes of Gases in Chemical Reactions

12.13  Volumes of Gases and the Limiting Reactant Concept

12.14  Chemical Calculations using Standard Molar Volume

12.15  Chemical Calculations at non-STP Conditions

12.16  Mixture of Gases

12.17  Dalton’s Law of Partial Pressures 

 

13      Solutions

13.1    Characteristics of Solutions 

13.2    Solubility

13.3    Solution Formation

13.4    Solubility Rules

13.5    Solution Concentrations

13.6    Concentration: Percentage of Solute

13.7    Concentration: Parts per Million and Parts per Billion

13.8    Concentration: Molarity

13.9    Concentration: Molality

13.10  Dilution

13.11  Molarity and Chemical Equations

13.12  Calculations Involving Volume: A Summary

 

14      Acids, Bases, and Salts

14.1    Arrhenius Acid—Base Theory

14.2    Brønsted—Lowry Acid—Base Theory

14.3    Conjugate Acids and Bases

14.4    Mono-, Di-, and Triprotic Acids

14.5    Strengths of Acids and Bases

14.6    Salts

14.7    Ionic and Net Ionic Equations

14.8    Reactions of Acids

14.9    Reactions of Bases

14.10  Reactions of Salts 

14.11  Self-Ionization of Water

14.12  The pH Scale

14.13  Hydrolysis of Salts

14.14  Buffers

14.15  Acid—Base Titrations

14.16  Acid and Base Stock Solutions

 

15      Oxidation and Reduction

15.1    Oxidation—Reduction Terminology

15.2    Oxidation Numbers

15.3    Types of Chemical Reactions

15.4    Balancing Oxidation—Reduction Equations

15.5    Oxidation-Number Method for Balancing Redox Equations

15.6    Half-Reaction Method for Balancing Redox Equations

15.7    Disproportionation Reactions

15.8    Some Important Oxidation—Reduction Reactions

 

16      Reaction Rates and Chemical Equilibrium

16.1    Collision Theory

16.2    Endothermic and Exothermic Reactions

16.3    Factors That Influence Reaction Rates

16.4    Chemical Equilibrium

16.5    Equilibrium Mixture Stoichiometry

16.6    Equilibrium Constants

16.7    Equilibrium Position

16.8    Temperature Dependency of Equilibrium Constants

16.9    Le Châtelier’s Principle

16.10  Forcing Reactions to Completion

 

17      Nuclear Chemistry

17.1    Unstable Nuclides and Radioactivity

17.2    Discovery of Radioactivity

17.3    Nature of Natural Radioactive Emissions

17.4    Radioactive Decay

17.5    Rate of Radioactive Decay

17.6    Transmutation and Bombardment Reactions

17.7    Positron Emission and Electron Capture

17.8    Nuclear Stability

17.9    Radioactive Decay Series

17.10  Chemical Effects of Radiation

17.11  Biochemical Effects of Radiation

17.12  Detection of Radiation

17.13  Sources of Radiation Exposure

17.14  Nuclear Medicine

17.15  Nuclear Fission and Nuclear Fusion

17.16  A Comparison of Nuclear and Chemical Reactions

 

Appendix A Mathematical Review

Glossary

Answers to Odd-Numbered Problems

Index

Product Details

ISBN:
9780132379946
Author:
Stoker, H. Stephen
Publisher:
Academic Internet Publishers
Author:
Gardner, Nancy J.
Author:
Cram101 Textbook Reviews
Subject:
Chemistry - General
Subject:
Chemistry
Subject:
Education-General
Copyright:
Edition Number:
9
Edition Description:
Trade paper
Publication Date:
20070524
Binding:
TRADE PAPER
Grade Level:
College/higher education:
Language:
English
Illustrations:
Y
Pages:
736
Dimensions:
10.7 x 8.3 x 0.43 in 454 gr

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Introduction To Chemical Principles (9TH 08 - Old Edition) Used Trade Paper
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Product details 736 pages Prentice Hall - English 9780132379946 Reviews:
"Synopsis" by , This text gives readers the background (and confidence) they need in chemistry. Stoker's book focuses on the most important topics (this text omits organic and biochemistrychapters), and teaches the problem-solving skills students need, all at an affordable price.
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