Introduction to Chemical Principles
9th Edition
Published on 28. June 2007
Book
Paperback/Softback
800 pages
978-0-13-237994-6 (ISBN)
Description
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 biochemistry chapters), and teaches the problem-solving skills students need.
More details
Edition
9th edition
Language
English
Place of publication
United States
Publishing group
Pearson Education (US)
Target group
Professional and scholarly
Dimensions
Height: 256 mm
Width: 204 mm
Thickness: 28 mm
Weight
1406 gr
ISBN-13
978-0-13-237994-6 (9780132379946)
Copyright in bibliographic data and cover images is held by Nielsen Book Services Limited or by the publishers or by their respective licensors: all rights reserved.
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Introduction to Chemical Principles
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Introduction to Chemical Principles
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Content
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 Bronsted-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 Chatelier'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
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 Bronsted-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 Chatelier'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