Chemistry The Central Science

1246 Pages·2014·85.551 MB·English

by  Theodore E. Brown, H. Eugene LeMay et al.

C he m i s t r y
T h e C e n T r a l S C i e n C e 13Th ediTion

C h e m i s t r y
T h e C e n T r a l S C i e n C e
13Th ediTion
Theodore L. Brown
University of illinois at Urbana-Champaign
H. Eugene LeMay, Jr.
University of Nevada, reno
Bruce E. Bursten
University of tennessee, Knoxville
Catherine J. Murphy
University of illinois at Urbana-Champaign
Patrick M. Woodward
the Ohio state University
Matthew W. Stoltzfus
the Ohio state University
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Library of Congress Cataloging-In Publication Data
Brown, Theodore L. (Theodore Lawrence), 1928- author.
Chemistry the central science.—Thirteenth edition / Theodore L. Brown, University of Illinois at Urbana-Chanmpaign,
H. Euguene LeMay, Jr., University of Nevada, Reno, Bruce E. Bursten, University of Tennessee, Knoxville,
Catherine J. Murphy, University of Illinois at Urbana-Chanmpaign, Patrick M. Woodward, The Ohio State University,
Matthew W. Stoltzfus, The Ohio State University.
pages cm
Includes index.
ISBN-13: 978-0-321-91041-7
ISBN-10: 0-321-91041-9
1. Chemistry--Textbooks. I. Title.
QD31.3.B765 2014
540—dc23 2013036724
1 2 3 4 5 6 7 8 9 10—CRK— 17 16 15 14
Student Edition: 0-321-91041-9 / 978-0-321-91041-7
www.pearsonhighered.com Instructor’s Resource Copy: 0-321-96239-7 / 978-0-321-96239-3
To our students,
whose enthusiasm and curiosity
have often inspired us,
and whose questions and suggestions
have sometimes taught us.
Student Edition: 0-321-91041-9 / 978-0-321-91041-7
Instructor’s Resource Copy: 0-321-96239-7 / 978-0-321-96239-3
BRIEF CONTENTS
Preface  xx
1 Introduction: Matter and Measurement  2
2 Atoms, Molecules, and Ions  40
3 Chemical Reactions and Reaction Stoichiometry  80
4 Reactions in Aqueous Solution  122
5 Thermochemistry  164
6 Electronic Structure of Atoms  212
7 Periodic Properties of the Elements  256
8 Basic Concepts of Chemical Bonding  298
9 Molecular Geometry and Bonding Theories  342
10 Gases  398
11 Liquids and Intermolecular Forces  442
12 Solids and Modern Materials  480
13 Properties of Solutions  530
14 Chemical Kinetics  574
15 Chemical Equilibrium  628
16 Acid–Base Equilibria  670
17 Additional Aspects of Aqueous Equilibria  724
18 Chemistry of the Environment  774
19 Chemical Thermodynamics  812
20 Electrochemistry  856
21 Nuclear Chemistry  908
22 Chemistry of the Nonmetals  952
23 Transition Metals and Coordination Chemistry  996
24 The Chemistry of Life: Organic and Biological Chemistry  1040
APPENdICES  
A Mathematical Operations  1092
B Properties of Water  1099
C Thermodynamic Quantities for Selected Substances at
298.15 K (25 °C)  1100
D Aqueous Equilibrium Constants  1103
E Standard Reduction Potentials at 25 °C  1105
Answers to Selected Exercises  A-1
Answers to Give It Some Thought  A-31
Answers to Go Figure  A-38
Answers to Selected Practice Exercises  A-44
Glossary  G-1
Photo/Art Credits  P-1
Index  I-1
vi
CONTENTS
Preface  xx
2
Atoms, Molecules,
1
Introduction: Matter and Ions  40
and Measurement
  2 2.1 The Atomic Theory of Matter  42
2.2 The discovery of Atomic Structure  43
1.1 The Study of Chemistry  2
Cathode Rays and Electrons  43
The Atomic and Molecular Perspective of
Radioactivity  45 The Nuclear Model of the
Chemistry  4 Why Study Chemistry?  5
Atom  46
1.2 Classifications of Matter  6
2.3 The Modern View of Atomic Structure  47
States of Matter  7 Pure Substances  7
Atomic Numbers, Mass Numbers, and
Elements  7 Compounds  8 Mixtures  10
Isotopes  49
1.3 Properties of Matter  11
2.4 Atomic Weights  50
Physical and Chemical Changes  12
The Atomic Mass Scale  50 Atomic Weight  51
Separation of Mixtures  13
2.5 The Periodic Table  52
1.4 Units of Measurement  14
2.6 Molecules and Molecular
SI Units  15 Length and Mass  17
Compounds  56
Temperature  17 derived SI Units  19
Molecules and Chemical Formulas  56
Volume  19 density  19
Molecular and Empirical Formulas  56
1.5 Uncertainty in Measurement  22
Picturing Molecules  57
Precision and Accuracy  22 Significant
2.7 Ions and Ionic Compounds  58
Figures  22 Significant Figures in
Predicting Ionic Charges  59 Ionic
Calculations  22
Compounds  60
1.6 dimensional Analysis  27
2.8 Naming Inorganic Compounds  62
Using Two or More Conversion Factors  28
Names and Formulas of Ionic Compounds  62
Conversions Involving Volume  29
Names and Formulas of Acids  67 Names and
Chapter Summary and Key Terms  32
Formulas of Binary Molecular Compounds  68
Learning Outcomes  32
Key Equations  32 Exercises  32 Additional 2.9 Some Simple Organic Compounds  69
Exercises  37 Alkanes  69 Some derivatives of Alkanes  70
Chemistry Put to Work Chemistry and the Chapter Summary and Key Terms  72
Chemical Industry  6 Learning Outcomes  72 Key
Equations  73 Exercises  73
A Closer Look The Scientific Method  14
Additional Exercises  78
Chemistry Put to Work Chemistry in
the News  20 A Closer Look Basic Forces  49
Strategies in Chemistry Estimating Answers  28 A Closer Look The Mass Spectrometer  52
Strategies in Chemistry The Importance of A Closer Look What Are Coins Made Of?  54
Practice  31 Chemistry and Life Elements Required by Living
Strategies in Chemistry The Features of This Organisms  61
Book  32 Strategies in Chemistry How to Take a Test  71
vii
viii Contents
Electrolytes and Nonelectrolytes  124 How
Compounds dissolve in Water  125 Strong
and Weak Electrolytes  126
4.2 Precipitation Reactions  128
3 Solubility Guidelines for Ionic
Chemical Reactions Compounds  129 Exchange (Metathesis)
Reactions  130 Ionic Equations and Spectator
and Reaction
Ions  131
Stoichiometry 4.3 Acids, Bases, and Neutralization
  80
Reactions  132
3.1 Chemical Equations  82 Acids  132 Bases  133 Strong and Weak
Acids and Bases  133 Identifying Strong
Balancing Equations  82 Indicating the States
and Weak Electrolytes  135 Neutralization
of Reactants and Products  85
Reactions and Salts  135 Neutralization
3.2 Simple Patterns of Chemical Reactivity  86
Reactions with Gas Formation  138
Combination and decomposition
4.4 Oxidation–Reduction Reactions  138
Reactions  86 Combustion Reactions  89
Oxidation and Reduction  138 Oxidation
3.3 Formula Weights  89
Numbers  140 Oxidation of Metals by Acids
Formula and Molecular Weights  90 and Salts  142 The Activity Series  143
Percentage Composition from Chemical
4.5 Concentrations of Solutions  146
Formulas  91
Molarity  146 Expressing the Concentration
3.4 Avogadro’s Number and the Mole  91
of an Electrolyte  147 Interconverting Molarity,
Molar Mass  93 Interconverting Masses Moles, and Volume  148 dilution  149
and Moles  95 Interconverting Masses and
4.6 Solution Stoichiometry and Chemical
Numbers of Particles  96
Analysis  151
3.5 Empirical Formulas from Analyses  98
Titrations  152
Molecular Formulas from Empirical
Chapter Summary and Key Terms  155
Formulas  100 Combustion Analysis  101
Learning Outcomes  156 Key
3.6 Quantitative Information from Balanced Equations  156 Exercises  156
Equations  103 Additional Exercises  161 Integrative
Exercises  161 design an
3.7 Limiting Reactants  106
Experiment  163
Theoretical and Percent Yields  109
Chemistry Put to Work Antacids  139
Chapter Summary and Key Terms  111
Strategies in Chemistry Analyzing Chemical
Learning Outcomes  111 Key Equations  112
Exercises  112 Additional Exercises  118 Reactions  146
Integrative Exercises  120 design an
Experiment  120
Strategies in Chemistry Problem Solving  92
Chemistry and Life Glucose Monitoring  95
Strategies in Chemistry Design an
5
Experiment  110
Thermochemistry
  164
5.1 Energy  166
Kinetic Energy and Potential Energy  166
Units of Energy  168 System and
4 Surroundings  169 Transferring Energy: Work
and Heat  169
Reactions in Aqueous
5.2 The First Law of Thermodynamics  170
Solution
  122
Internal Energy  171 Relating ∆E to Heat and
Work  172 Endothermic and Exothermic
4.1 General Properties of Aqueous
Processes  173 State Functions  174
Solutions  124
Contents ix
5.3 Enthalpy  175 Orbitals and Quantum Numbers  228
Pressure–Volume Work  175 Enthalpy 6.6 Representations of Orbitals  230
Change  177 The s Orbitals  230 The p Orbitals  233
5.4 Enthalpies of Reaction  179 The d and f Orbitals  233
6.7 Many-Electron Atoms  234
5.5 Calorimetry  181
Orbitals and Their Energies  234 Electron Spin
Heat Capacity and Specific Heat  181
and the Pauli Exclusion Principle  235
Constant-Pressure Calorimetry  183
Bomb Calorimetry (Constant-Volume 6.8 Electron Configurations  237
Calorimetry)  185 Hund’s Rule  237 Condensed Electron
5.6 Hess’s Law  187 Configurations  239 Transition
Metals  240 The Lanthanides and
5.7 Enthalpies of Formation  189
Actinides  240
Using Enthalpies of Formation to Calculate
6.9 Electron Configurations and the
Enthalpies of Reaction  192
Periodic Table  241
5.8 Foods and Fuels  194
Anomalous Electron Configurations  245
Foods  194 Fuels  197 Other Energy
Chapter Summary and Key Terms  246
Sources  198 Learning Outcomes  247 Key Equations  247
Exercises  248 Additional Exercises  252
Chapter Summary and Key Terms  200
Integrative Exercises  255 design an
Learning Outcomes  201 Key Equations  202
Experiment  255
Exercises  202 Additional Exercises  209
Integrative Exercises  210 design an A Closer Look Measurement and the Uncertainty
Experiment  211 Principle  225
A Closer Look Energy, Enthalpy, and P–V A Closer Look Thought Experiments and
Work  178 Schrödinger’s Cat  227
Strategies in Chemistry Using Enthalpy as a A Closer Look Probability Density and Radial
Guide  181 Probability Functions  232
Chemistry and Life Nuclear Spin and Magnetic
Chemistry and Life The Regulation of Body
Resonance Imaging  236
Temperature  186
Chemistry Put to Work The Scientific and
Political Challenges of Biofuels  198
7
Periodic Properties of
6 the Elements
  256
Electronic Structure of
7.1 development of the Periodic
Atoms
  212
Table  258
7.2 Effective Nuclear Charge  259
6.1 The Wave Nature of Light  214
7.3 Sizes of Atoms and Ions  262
6.2 Quantized Energy and Photons  216
Periodic Trends in Atomic Radii  264 Periodic
Hot Objects and the Quantization of Energy  216
Trends in Ionic Radii  265
The Photoelectric Effect and Photons  217
7.4 Ionization Energy  268
6.3 Line Spectra and the Bohr Model  219
Variations in Successive Ionization
Line Spectra  219 Bohr’s Model  220
Energies  268 Periodic Trends in First
The Energy States of the Hydrogen Atom  221
Ionization Energies  268 Electron
Limitations of the Bohr Model  223
Configurations of Ions  271
6.4 The Wave Behavior of Matter  223
7.5 Electron Affinity  272
The Uncertainty Principle  225
7.6 Metals, Nonmetals, and
6.5 Quantum Mechanics and Atomic
Metalloids  273
Orbitals  226
Metals  274 Nonmetals  276 Metalloids  277