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Chemistry: A Molecular Approach, Global Edition

Chemistry: A Molecular Approach, Global Edition

Nivaldo J. Tro

(2016)

Additional Information

Book Details

Abstract

For courses in Chemistry.

 

Building 21st Century Data Analysis and Problem-Solving Skills in Modern Chemistry

The Fourth Edition of Niva Tro’s Chemistry: A Molecular Approach reinforces students’ development of 21st century skills including data interpretation and analysis, problem solving and quantitative reasoning, applying conceptual understanding to new situations and peer-to-peer collaboration.

 

Nivaldo Tro presents chemistry visually through multi-level images–macroscopic, molecular, and symbolic representations–helping students see the connections between the world they see around them (macroscopic), the atoms and molecules that compose the world (molecular), and the formulas they write down on paper (symbolic). The benefits of Dr. Tro’s problem-solving approach are reinforced through digital, Interactive Worked Examples that provide students with an office-hour type of environment and expanded coverage on the latest developments in chemistry. New Key Concept Videos explain difficult concepts while new end-of-chapter problems including Group Work questions and Data Interpretation and Analysis questions engage students in applying their understanding of chemistry. The revision has been constructed to easily incorporate material for instructors and students to engage in Before, During, and After class activities.

 

MasteringChemistry™ is not included. Students, if MasteringChemistry is a recommended/mandatory component of the course, please ask your instructor for the correct ISBN and course ID. MasteringChemistry should only be purchased when required by an instructor. Instructors, contact your Pearson representative for more information.


MasteringChemistry from Pearson is the leading online homework, tutorial, and assessment system, designed to improve results by engaging students before, during, and after class with powerful content. Instructors ensure students arrive ready to learn by assigning educationally effective content before class, and encourage critical thinking and retention with in-class resources such as Learning Catalytics™.

 

 


Table of Contents

Section Title Page Action Price
Cover Cover
Title Page 1
Copyright Page 2
ABOUT THE AUTHOR 3
Acknowledgments 22
Contents 7
PREFACE 20
1 Matter, Measurement, and Problem Solving 38
1.1 Atoms and Molecules 39
1.2 The Scientific Approach to Knowledge 41
The Nature of Science: Thomas S. Kuhn and Scientific 43
1.3 The Classification of Matter 43
The States of Matter: Solid, Liquid, and Gas 44
Classifying Matter according to Its Composition: Elements, Compounds, and Mixtures 45
Separating Mixtures 46
1.4 Physical and Chemical Changes and Physical and Chemical Properties 47
1.5 Energy: A Fundamental Part of Physical and Chemical Change 50
1.6 The Units of Measurement 51
Standard Units 51
The Meter: A Measure of Length 52
The Kilogram: A Measure of Mass 52
The Second: A Measure of Time 52
The Kelvin: A Measure of Temperature 53
Prefix Multipliers 55
Derived Units: Volume and Density 55
Calculating Density 57
Chemistry and Medicine: Bone Density 58
1.7 The Reliability of a Measurement 58
Counting Significant Figures 60
Exact Numbers 60
Significant Figures in Calculations 61
Precision and Accuracy 63
Chemistry in Your Day: Integrity in Data Gathering 64
1.8 Solving Chemical Problems 64
Converting from One Unit to Another 64
General Problem-Solving Strategy 66
Units Raised to a Power 68
Order-of-Magnitude Estimations 69
Problems Involving an Equation 70
CHAPTER IN REVIEW: Self-Assessment Quiz 71
Key Terms 72
Key Concepts 73
Key Equations and Relationships 73
Key Learning Outcomes 74
EXERCISES: Review Questions 74
Problems by Topic 74
Cumulative Problems 78
Challenge Problems 79
Conceptual Problems 80
Questions for Group Work 80
Data Interpretation and Analysis 81
Answers to Conceptual Connections 81
2 Atoms and Elements 82
2.1 Brownian Motion: Atoms Comfirmed 83
2.2 Early Ideas about the Building Blocks of Matter 85
2.3 Modern Atomic Theory and the Laws That Led to It 85
The Law of Conservation of Mass 85
The Law of Definite Proportions 86
The Law of Multiple Proportions 87
John Dalton and the Atomic Theory 88
Chemistry in Your Day: Atoms and Humans 88
2.4 The Discovery of the Electron 89
Cathode Rays 89
Millikan’s Oil Drop Experiment: The Charge of the Electron 90
2.5 The Structure of the Atom 91
2.6 Subatomic Particles: Protons, Neutrons, and Electrons in Atoms 93
Elements: Defined by Their Numbers of Protons 94
Isotopes: When the Number of Neutrons Varies 95
Ions: Losing and Gaining Electrons 97
Chemistry in Your Day: Where Did Elements Come From? 98
2.7 Finding Patterns: The Periodic Law and the Periodic Table 98
Modern Periodic Table Organization 100
Ions and the Periodic Table 102
Chemistry and Medicine: The Elements of Life 103
2.8 Atomic Mass: The Average Mass of an Element’s Atoms 103
Mass Spectrometry: Measuring the Mass of Atoms and Molecules 104
Chemistry in Your Day: Evolving Atomic Masses 106
2.9 Molar Mass: Counting Atoms by Weighing Them 107
The Mole: A Chemist’s “Dozen” 107
Converting between Number of Moles and Number of Atoms 108
Converting between Mass and Amount (Number of Moles) 109
CHAPTER IN REVIEW: Self-Assessment Quiz 112
Key Terms 113
Key Concepts 114
Key Equations and Relationships 114
Key Learning Outcomes 115
EXERCISES: Review Questions 115
Problems by Topic 116
Cumulative Problems 119
Challenge Problems 120
Conceptual Problems 121
Questions for Group Work 121
Data Interpretation and Analysis 122
Answers to Conceptual Connections 123
3 Molecules, Compounds, and Chemical Equations 124
3.1 Hydrogen, Oxygen, and Water 125
3.2 Chemical Bonds 127
Ionic Bonds 127
Covalent Bonds 128
3.3 Representing Compounds: Chemical Formulas and Molecular Models 128
Types of Chemical Formulas 128
Molecular Models 130
3.4 An Atomic-Level View of Elements and Compounds 130
3.5 Ionic Compounds: Formulas and Names 134
Writing Formulas for Ionic Compounds 134
Naming Ionic Compounds 135
Naming Binary Ionic Compounds Containing a Metal That Forms Only One Type of Cation 136
Naming Binary Ionic Compounds Containing a Metal That Forms More Than One Kind of Cation 137
Naming Ionic Compounds Containing Polyatomic Ions 138
Hydrated Ionic Compounds 139
3.6 Molecular Compounds: Formulas and Names 139
Naming Molecular Compounds 140
Naming Acids 141
Naming Binary Acids 141
Naming Oxyacids 142
Chemistry in the Environment: Acid Rain 142
3.7 Summary of Inorganic Nomenclature 143
3.8 Formula Mass and the Mole Concept for Compounds 145
Molar Mass of a Compound 145
Using Molar Mass to Count Molecules by Weighing 145
3.9 Composition of Compounds 147
Mass Percent Composition as a Conversion Factor 148
Conversion Factors from Chemical Formulas 150
Chemistry and Medicine: Methylmercury in Fish 152
3.10 Determining a Chemical Formula from Experimental Data 152
Determining Molecular Formulas for Compounds 154
Combustion Analysis 155
3.11 Writing and Balancing Chemical Equations 157
3.12 Organic Compounds 161
Hydrocarbons 162
Functionalized Hydrocarbons 163
CHAPTER IN REVIEW: Self-assessment Quiz 165
Key Terms 165
Key Concepts 166
Key Equations and Relationships 166
Key Learning Outcomes 167
EXERCISES: Review Questions 167
Problems by Topic 168
Cumulative Problems 172
Challenge Problems 173
Conceptual Problems 173
Questions for Group Work 173
Data Interpretation and Analysis 174
Answers to Conceptual Connections 174
4 Chemical Quantities and Aqueous Reactions 176
4.1 Climate Change and the Combustion of Fossil Fuels 177
4.2 Reaction Stoichiometry: How Much Carbon Dioxide? 179
Making Pizza: The Relationships among Ingredients 179
Making Molecules: Mole-to-Mole Conversions 179
Making Molecules: Mass-to-Mass Conversions 180
4.3 Limiting Reactant, Theoretical Yield, and Percent Yield 183
Calculating Limiting Reactant, Theoretical Yield, and Percent Yield 184
Calculating Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Reactant Masses 185
4.4 Solution Concentration and Solution Stoichiometry 189
Solution Concentration 189
Using Molarity in Calculations 191
Solution Dilution 192
Solution Stoichiometry 194
4.5 Types of Aqueous Solutions and Solubility 196
Electrolyte and Nonelectrolyte Solutions 196
The Solubility of Ionic Compounds 198
4.6 Precipitation Reactions 200
4.7 Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations 204
4.8 Acid–Base and Gas-Evolution Reactions 205
Acid–Base Reactions 206
Gas-Evolution Reactions 211
4.9 Oxidation–Reduction Reactions 213
Oxidation States 214
Identifying Redox Reactions 216
Chemistry in Your Day: Bleached Blonde 219
Combustion Reactions 219
CHAPTER IN REVIEW: Self-assessment Quiz 220
Key Terms 221
Key Concepts 222
Key Equations and Relationships 223
Key Learning Outcomes 223
EXERCISES: Review Questions 224
Problems by Topic 224
Cumulative Problems 228
Challenge Problems 230
Conceptual Problems 230
Questions for Group Work 231
Data Interpretation and Analysis 232
Answers to Conceptual Connections 233
5 Gases 234
5.1 Supersonic Skydiving and the Risk of Decompression 235
5.2 Pressure: The Result of Molecular Collisions 236
Pressure Units 237
The Manometer: A Way to Measure Pressure in the Laboratory 238
Chemistry and Medicine: Blood Pressure 239
5.3 The Simple Gas Laws: Boyle’s Law, Charles’s Law, and Avogadro’s Law 239
Boyle’s Law: Volume and Pressure 240
Charles’s Law: Volume and Temperature 242
Chemistry in Your Day: Extra-Long Snorkels 243
Avogadro’s Law: Volume and Amount (in Moles) 245
5.4 The Ideal Gas Law 246
5.5 Applications of the Ideal Gas Law: Molar Volume, Density, and Molar Mass of a Gas 249
Molar Volume at Standard Temperature and Pressure 249
Density of a Gas 250
Molar Mass of a Gas 251
5.6 Mixtures of Gases and Partial Pressures 252
Deep-Sea Diving and Partial Pressures 255
Collecting Gases over Water 257
5.7 Gases in Chemical Reactions: Stoichiometry Revisited 259
Molar Volume and Stoichiometry 260
5.8 Kinetic Molecular Theory: A Model for Gases 262
How Kinetic Molecular Theory Explains Pressure and the Simple Gas Laws 263
Kinetic Molecular Theory and the Ideal Gas Law 264
Temperature and Molecular Velocities 265
5.9 Mean Free Path, Diffusion, and Effusion of Gases 268
5.10 real Gases: The Effects of Size and Intermolecular Forces 270
The Effect of the Finite Volume of Gas Particles 271
The Effect of Intermolecular Forces 272
Van der Waals Equation 273
Real Gases 273
CHAPTER IN REVIEW: Self-Assessment Quiz 274
Key Terms 275
Key Concepts 275
Key Equations and Relationships 276
Key Learning Outcomes 276
EXERCISES: Review Questions 277
Problems by Topic 278
Cumulative Problems 281
Challenge Problems 283
Conceptual Problems 283
Questions for Group Work 284
Data Interpretation and Analysis 284
Answers to Conceptual Connections 285
6 Thermochemistry 286
6.1 Chemical Hand Warmers 287
6.2 The Nature of Energy: Key Definitions 288
Types of Energy 288
Energy Conservation and Energy Transfer 289
Units of Energy 289
6.3 The First Law of Thermodynamics: There Is No Free Lunch 291
Internal Energy 291
Chemistry in Your Day: Redheffer’s Perpetual Motion Machine 291
Heat and Work 294
6.4 Quantifying Heat and Work 296
Heat 296
Work: Pressure–Volume Work 300
6.5 Measuring & 302
6.6 Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure 305
Exothermic and Endothermic Processes: A Molecular View 307
Stoichiometry Involving & 307
6.7 Constant-Pressure Calorimetry: Measuring & 308
6.8 Relationships Involving & 310
6.9 Determining Enthalpies of Reaction from Standard Enthalpies of Formation 313
Standard States and Standard Enthalpy Changes 313
Calculating the Standard Enthalpy Change for a Reaction 315
6.10 Energy Use and the Environment 318
Energy Consumption 318
Environmental Problems Associated with Fossil Fuel Use 319
Air Pollution 319
Global Climate Change 320
Chemistry in the Environment: Renewable Energy 322
CHAPTER IN REVIEW: Self-Assessment Quiz 323
Key Terms 324
Key Concepts 324
Key Equations and Relationships 325
Key Learning Outcomes 325
EXERCISES: Review Questions 326
Problems by Topic 327
Cumulative Problems 330
Challenge Problems 331
Conceptual Problems 331
Questions for Group Work 332
Data Interpretation and Analysis 332
Answers to Conceptual Connections 333
7 The Quantum-Mechanical Model of the Atom 334
7.1 Schrödinger’s Cat 335
7.2 The Nature of Light 336
The Wave Nature of Light 337
The Electromagnetic Spectrum 339
Chemistry and Medicine: Radiation Treatment for Cancer 341
Interference and Diffraction 341
The Particle Nature of Light 343
7.3 Atomic Spectroscopy and the Bohr Model 346
Chemistry in Your Day: Atomic Spectroscopy, a Bar Code for Atoms 348
7.4 The Wave Nature of Matter: The de Broglie Wavelength, the Uncertainty Principle, and Indeterminacy 349
The de Broglie Wavelength 351
The Uncertainty Principle 352
Indeterminacy and Probability Distribution Maps 353
7.5 Quantum Mechanics and the Atom 355
Solutions to the Schrödinger Equation for the Hydrogen Atom 355
Atomic Spectroscopy Explained 358
7.6 The Shapes of Atomic Orbitals 361
s Orbitals (l=0) 361
p Orbitals (l=1) 364
d Orbitals (l=2) 364
f Orbitals (l=3) 364
The Phase of Orbitals 365
The Shape of Atoms 366
CHAPTER IN REVIEW: Self-Assessment Quiz 366
Key Terms 367
Key Concepts 367
Key Equations and Relationships 368
Key Learning Outcomes 368
EXERCISES: Review Questions 368
Problems by Topic 369
Cumulative Problems 370
Challenge Problems 371
Conceptual Problems 372
Questions for Group Work 372
Data Interpretation and Analysis 372
Answers to Conceptual Connections 373
8 Periodic Properties of the Elements 374
8.1 Nerve Signal Transmission 375
8.2 The Development of the Periodic Table 376
8.3 Electron Configurations: How Electrons Occupy Orbitals 377
Electron Spin and the Pauli Exclusion Principle 378
Sublevel Energy Splitting in Multielectron Atoms 379
Electron Configurations for Multielectron Atoms 382
8.4 Electron Configurations, Valence Electrons, and the Periodic Table 385
Orbital Blocks in the Periodic Table 386
Writing an Electron Configuration for an Element from Its Position in the Periodic Table 387
The Transition and Inner Transition Elements 388
8.5 The Explanatory Power of the Quantum-Mechanical Model 389
8.6 Periodic Trends in the Size of Atoms and Effective Nuclear Charge 390
Effective Nuclear Charge 391
Atomic Radii and the Transition Elements 393
8.7 Ions: Electron Configurations, Magnetic Properties, Ionic Radii, and Ionization Energy 395
Electron Configurations and Magnetic Properties of Ions 395
Ionic Radii 397
Ionization Energy 399
Trends in First Ionization Energy 399
Exceptions to Trends in First Ionization Energy 401
Trends in Second and Successive Ionization Energies 402
8.8 Electron Affinities and Metallic Character 403
Electron Affinity 403
Metallic Character 404
8.9 Some Examples of Periodic Chemical Behavior: The Alkali Metals, the Halogens, and the Noble Gases 407
The Alkali Metals (Group 1A) 407
The Halogens (Group 7A) 408
The Noble Gases (Group 8A) 409
CHAPTER IN REVIEW: Self-Assessment Quiz 410
Key Terms 411
Key Concepts 412
Key Equations and Relationships 412
Key Learning Outcomes 413
EXERCISES: Review Questions 413
Problems by Topic 414
Cumulative Problems 416
Challenge Problems 417
Conceptual Problems 417
Questions for Group Work 418
Data Interpretation and Analysis 418
Answers to Conceptual Connections 419
9 Chemical Bonding I: The Lewis Model 420
9.1 Bonding Models and AIDS Drugs 421
9.2 Types of Chemical Bonds 422
9.3 Representing Valence Electrons with Dots 424
9.4 Ionic Bonding: Lewis Symbols and Lattice Energies 425
Ionic Bonding and Electron Transfer 425
Lattice Energy: The Rest of the Story 426
The Born–Haber Cycle 426
Trends in Lattice Energies: Ion Size 429
Trends in Lattice Energies: Ion Charge 429
Ionic Bonding: Models and Reality 430
Chemistry and Medicine: Ionic Compounds in Medicine 431
9.5 Covalent Bonding: Lewis Structures 432
Single Covalent Bonds 432
Double and Triple Covalent Bonds 432
Covalent Bonding: Models and Reality 433
9.6 Electronegativity and Bond Polarity 434
Electronegativity 435
Bond Polarity, Dipole Moment, and Percent Ionic Character 436
9.7 Lewis Structures of Molecular Compounds and Polyatomic Ions 438
Writing Lewis Structures for Molecular Compounds 438
Writing Lewis Structures for Polyatomic Ions 440
9.8 Resonance and Formal Charge 440
Resonance 440
Formal Charge 442
9.9 Exceptions to the Octet Rule: Odd-Electron Species, Incomplete Octets, and Expanded Octets 445
Odd-Electron Species 446
Incomplete Octets 446
Chemistry in the Environment: Free Radicals and the Atmospheric Vacuum Cleaner 447
Expanded Octets 448
9.10 Bond Energies and Bond Lengths 449
Bond Energy 450
Using Average Bond Energies to Estimate Enthalpy Changes for Reactions 451
Bond Lengths 452
9.11 Bonding in Metals: The Electron Sea Model 453
Chemistry in the Environment: The Lewis Structure of Ozone 454
CHAPTER IN REVIEW: Self-Assessment Quiz 455
Key Terms 456
Key Concepts 456
Key Equations and Relationships 457
Key Learning Outcomes 457
EXERCISES: Review Questions 458
Problems by Topic 459
Cumulative Problems 460
Challenge Problems 462
Conceptual Problems 462
Questions for Group Work 462
Data Interpretation and Analysis 463
Answers to Conceptual Connections 463
10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 464
10.1 Artificial Sweeteners: Fooled by Molecular Shape 465
10.2 VSEPR Theory: The Five Basic Shapes 466
Two Electron Groups: Linear Geometry 467
Three Electron Groups: Trigonal Planar Geometry 467
Four Electron Groups: Tetrahedral Geometry 467
Five Electron Groups: Trigonal Bipyramidal Geometry 469
Six Electron Groups: Octahedral Geometry 469
10.3 VSEPR Theory: The Effect of Lone Pairs 470
Four Electron Groups with Lone Pairs 470
Five Electron Groups with Lone Pairs 472
Six Electron Groups with Lone Pairs 473
10.4 VSEPR Theory: Predicting Molecular Geometries 475
Representing Molecular Geometries on Paper 477
Predicting the Shapes of Larger Molecules 477
10.5 Molecular Shape and Polarity 478
Vector Addition 480
Chemistry in Your Day: How Soap Works 482
10.6 Valence Bond Theory: Orbital Overlap as a Chemical Bond 483
10.7 Valence Bond Theory: Hybridization of Atomic Orbitals 485
sp[Sup(3)] Hybridization 486
sp[Sup(2)] Hybridization and Double Bonds 488
Chemistry in Your Day: The Chemistry of Vision 492
sp Hybridization and Triple Bonds 492
sp[Sup(3)] d and sp[Sup(3)] d[Sup(2)] Hybridization 494
Writing Hybridization and Bonding Schemes 495
10.8 Molecular Orbital Theory: Electron Delocalization 498
Linear Combination of Atomic Orbitals (LCAOs) 499
Period Two Homonuclear Diatomic Molecules 503
Second-Period Heteronuclear Diatomic Molecules 508
Polyatomic Molecules 510
CHAPTER IN REVIEW: Self-Assessment Quiz 511
Key Terms 512
Key Concepts 512
Key Equations and Relationships 512
Key Learning Outcomes 513
EXERCISES: Review Questions 513
Problems by Topic 514
Cumulative Problems 516
Challenge Problems 518
Conceptual Problems 519
Questions for Group Work 519
Data Interpretation and Analysis 520
Answers to Conceptual Connections 520
11 Liquids, Solids, and Intermolecular Forces 522
11.1 Water, No Gravity 523
11.2 Solids, Liquids, and Gases: A Molecular Comparison 524
Differences between States of Matter 524
Changes between States 526
11.3 Intermolecular Forces: The Forces That Hold Condensed States Together 527
Dispersion Force 528
Dipole–Dipole Force 530
Hydrogen Bonding 533
Ion–Dipole Force 535
Chemistry and Medicine: Hydrogen Bonding in DNA 536
11.4 Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action 537
Surface Tension 537
Viscosity 539
Chemistry in Your Day: Viscosity and Motor Oil 539
Capillary Action 539
11.5 Vaporization and Vapor Pressure 540
The Process of Vaporization 540
The Energetics of Vaporization 541
Vapor Pressure and Dynamic Equilibrium 543
The Critical Point: The Transition to an Unusual State of Matter 549
11.6 Sublimation and Fusion 550
Sublimation 550
Fusion 551
Energetics of Melting and Freezing 551
11.7 Heating Curve for Water 552
11.8 Phase Diagrams 555
The Major Features of a Phase Diagram 555
Navigation within a Phase Diagram 556
The Phase Diagrams of Other Substances 557
11.9 Water: An Extraordinary Substance 558
Chemistry in the Environment: Water Pollution 559
CHAPTER IN REVIEW: Self-Assessment Quiz 560
Key Terms 561
Key Concepts 561
Key Equations and Relationships 562
Key Learning Outcomes 562
EXERCISES: Review Questions 562
Problems by Topic 563
Cumulative Problems 566
Challenge Problems 566
Conceptual Problems 567
Questions for Group Work 567
Data Interpretation and Analysis 568
Answers to Conceptual Connections 569
12 Solids and Modern Materials 570
12.1 Friday Night Experiments: The Discovery of Graphene 571
12.2 X-Ray Crystallography 572
12.3 Unit Cells and Basic Structures 575
Cubic Unit Cells 575
Closest-Packed Structures 581
12.4 The Fundamental Types of Crystalline Solids 582
Molecular Solids 583
Chemistry in Your Day: Chocolate, An Edible Material 584
Ionic Solids 585
Atomic Solids 585
12.5 The Structures of Ionic Solids 586
12.6 Network Covalent Atomic Solids: Carbon and Silicates 588
Carbon 588
Silicates 591
12.7 Ceramics, Cement, and Glass 591
Ceramics 591
Cement 592
Glass 593
12.8 Semiconductors and Band Theory 593
Molecular Orbitals and Energy Bands 593
Doping: Controlling the Conductivity of Semiconductors 595
12.9 Polymers and Plastics 595
Chemistry in Your Day: Kevlar 598
CHAPTER IN REVIEW: Self-Assessment Quiz 598
Key Terms 599
Key Concepts 600
Key Equations and Relationships 600
Key Learning Outcomes 600
EXERCISES: Review Questions 601
Problems by Topic 601
Cumulative Problems 604
Challenge Problems 605
Conceptual Problems 605
Questions for Group Work 606
Data Interpretation and Analysis 606
Answers to Conceptual Connections 607
13 Solutions 608
13.1 Thirsty Solutions: Why You Shouldn’t Drink Seawater 609
13.2 Types of Solutions and Solubility 611
Nature’s Tendency toward Mixing: Entropy 612
The Effect of Intermolecular Forces 612
13.3 Energetics of Solution Formation 615
Energy Changes in Solution Formation 616
Aqueous Solutions and Heats of Hydration 617
13.4 Solution Equilibrium and Factors Affecting Solubility 619
The Temperature Dependence of the Solubility of Solids 620
Factors Affecting the Solubility of Gases in Water 621
13.5 Expressing Solution Concentration 623
Chemistry in the Environment: Lake Nyos 624
Molarity 624
Molality 626
Parts by Mass and Parts by Volume 626
Using Parts by Mass (or Parts by Volume) in Calculations 626
Mole Fraction and Mole Percent 627
Chemistry in the Environment: The Dirty Dozen 628
13.6 Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure 631
Vapor Pressure Lowering 631
Vapor Pressures of Solutions Containing a Volatile (Nonelectrolyte) Solute 635
Freezing Point Depression and Boiling Point Elevation 638
Chemistry in Your Day: Antifreeze in Frogs 641
Osmotic Pressure 641
13.7 Colligative Properties of Strong Electrolyte Solutions 643
Strong Electrolytes and Vapor Pressure 644
Colligative Properties and Medical Solutions 645
13.8 Colloids 646
CHAPTER IN REVIEW: Self-Assessment Quiz 649
Key Terms 650
Key Concepts 650
Key Equations and Relationships 651
Key Learning Outcomes 651
EXERCISES: Review Questions 652
Problems by Topic 652
Cumulative Problems 656
Challenge Problems 657
Conceptual Problems 657
Questions for Group Work 658
Data Interpretation and Analysis 658
Answers to Conceptual Connections 659
14 Chemical Kinetics 660
14.1 Catching Lizards 661
14.2 The Rate of a Chemical Reaction 662
Definition of Reaction Rate 662
Measuring Reaction Rates 665
14.3 The Rate Law: The Effect of Concentration on Reaction Rate 667
The Three Common Reaction Orders (n= 0, 1, and 2) 667
Determining the Order of a Reaction 668
Reaction Order for Multiple Reactants 670
14.4 The Integrated Rate Law: The Dependence of Concentration on Time 672
The Integrated Rate Law 672
The Half-Life of a Reaction 676
14.5 The Effect of Temperature on Reaction Rate 680
The Arrhenius Equation 680
The Activation Energy, Frequency Factor, and Exponential Factor 681
Arrhenius Plots: Experimental Measurements of the Frequency Factor and the Activation Energy 682
The Collision Model: A Closer Look at the Frequency Factor 685
14.6 Reaction Mechanisms 686
Rate Laws for Elementary Steps 687
Rate-Determining Steps and Overall Reaction Rate Laws 688
Mechanisms with a Fast Initial Step 689
14.7 Catalysis 691
Homogeneous and Heterogeneous Catalysis 693
Enzymes: Biological Catalysts 694
Chemistry and Medicine: Enzyme Catalysis and the Role of Chymotrypsin in Digestion 696
CHAPTER IN REVIEW: Self-Assessment Quiz 697
Key Terms 699
Key Concepts 699
Key Equations and Relationships 700
Key Learning Outcomes 700
EXERCISES: Review Questions 701
Problems by Topic 701
Cumulative Problems 706
Challenge Problems 708
Conceptual Problems 709
Questions for Group Work 710
Data Interpretation and Analysis 710
Answers to Conceptual Connections 711
15 Chemical Equilibrium 712
15.1 fetal Hemoglobin and Equilibrium 713
15.2 The Concept of Dynamic Equilibrium 715
15.3 The Equilibrium Constant (K) 718
Expressing Equilibrium Constants for Chemical Reactions 718
The Significance of the Equilibrium Constant 719
Chemistry and Medicine: Life and Equilibrium 720
Relationships between the Equilibrium Constant and the Chemical Equation 721
15.4 Expressing the Equilibrium Constant in Terms of Pressure 722
15.5 Heterogeneous Equilibria: Reactions Involving Solids and Liquids 725
15.6 Calculating the Equilibrium Constant from Measured Equilibrium Concentrations 726
15.7 The Reaction Quotient: Predicting the Direction of Change 729
15.8 finding Equilibrium Concentrations 731
Relationship Between K[Sub(p)] and K[Sub(c)] 723
Units of K 724
Finding Equilibrium Concentrations from the Equilibrium Constant and All but One of the Equilibrium Concentrations of the Reactants and Products 732
Finding Equilibrium Concentrations from the Equilibrium Constant and Initial Concentrations or Pressures 733
Simplifying Approximations in Working Equilibrium Problems 737
15.9 Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances 741
The Effect of a Concentration Change on Equilibrium 742
The Effect of a Volume (or Pressure) Change on Equilibrium 744
The Effect of a Temperature Change on Equilibrium 746
CHAPTER IN REVIEW: Self-Assessment Quiz 748
Key Terms 749
Key Concepts 749
Key Equations and Relationships 750
Key Learning Outcomes 750
EXERCISES: Review Questions 751
Problems by Topic 752
Cumulative Problems 755
Challenge Problems 756
Conceptual Problems 757
Questions for Group Work 757
Data Interpretation and Analysis 758
Answers to Conceptual Connections 759
16 Acids and Bases 760
16.1 Heartburn 761
16.2 The Nature of Acids and Bases 762
16.3 Definitions of Acids and Bases 764
The Arrhenius Definition 764
The Brønsted–Lowry Definition 765
16.4 Acid Strength and the Acid Ionization Constant (K[Sub(a)] 767
Strong Acids 767
Weak Acids 768
The Acid Ionization Constant (K[Sub(a)]) 769
16.5 Autoionization of Water and pH 770
The pH Scale: A Way to Quantify Acidity and Basicity 772
pOH and Other p Scales 773
Chemistry and Medicine: Ulcers 774
16.6 Finding the [H[Sub(3)]O[Sup(+)]] and pH of Strong and Weak Acid Solutions 775
Strong Acids 775
Weak Acids 775
Percent Ionization of a Weak Acid 780
Mixtures of Acids 781
16.7 Base Solutions 784
Strong Bases 784
Weak Bases 784
Finding the [OH[Sup(-)]] and pH of Basic Solutions 786
Chemistry and Medicine: What’s in My Antacid? 788
16.8 The Acid–Base Properties of Ions and Salts 788
Anions as Weak Bases 789
Cations as Weak Acids 792
Classifying Salt Solutions as Acidic, Basic, or Neutral 793
16.9 Polyprotic Acids 795
Finding the pH of Polyprotic Acid Solutions 796
Finding the Concentration of the Anions for a Weak Diprotic Acid Solution 798
16.10 Acid Strength and Molecular Structure 800
Binary Acids 800
Oxyacids 801
16.11 Lewis Acids and Bases 802
Molecules That Act as Lewis Acids 802
Cations That Act as Lewis Acids 803
16.12 Acid Rain 803
Effects of Acid Rain 804
Acid Rain Legislation 805
CHAPTER IN REVIEW: Self-Assessment Quiz 805
Key Terms 806
Key Concepts 806
Key Equations and Relationships 807
Key Learning Outcomes 808
EXERCISES: Review Questions 808
Problems by Topic 809
Cumulative Problems 812
Challenge Problems 813
Conceptual Problems 814
Questions for Group Work 814
Data Interpretation and Analysis 814
Answers to Conceptual Connections 815
17 Aqueous Ionic Equilibrium 816
17.1 The Danger of Antifreeze 817
17.2 Buffers: Solutions That Resist pH Change 818
Calculating the pH of a Buffer Solution 820
The Henderson–Hasselbalch Equation 821
Calculating pH Changes in a Buffer Solution 824
Buffers Containing a Base and Its Conjugate Acid 828
17.3 Buffer Effectiveness: Buffer Range and Buffer Capacity 829
Relative Amounts of Acid and Base 829
Absolute Concentrations of the Acid and Conjugate Base 830
Buffer Range 831
Chemistry and Medicine: Buffer Effectiveness in Human Blood 832
Buffer Capacity 832
17.4 Titrations and pH Curves 833
The Titration of a Strong Acid with a Strong Base 834
The Titration of a Weak Acid with a Strong Base 838
The Titration of a Weak Base with a Strong Acid 843
The Titration of a Polyprotic Acid 843
Indicators: pH-Dependent Colors 844
17.5 Solubility Equilibria and the Solubility Product Constant 847
K[Sub(sp)] and Molar Solubility 847
Chemistry in Your Day: Hard Water 849
K[Sub(sp)] and Relative Solubility 850
The Effect of a Common Ion on Solubility 850
The Effect of pH on Solubility 852
17.6 Precipitation 853
Selective Precipitation 854
17.7 Qualitative Chemical Analysis 856
Group 1: Insoluble Chlorides 857
Group 2: Acid-Insoluble Sulfides 857
Group 3: Base-Insoluble Sulfides and Hydroxides 858
Group 4: Insoluble Phosphates 858
Group 5: Alkali Metals and NH[Sub(4)][Sup(+)] 858
17.8 Complex Ion Equilibria 859
The Effect of Complex Ion Equilibria on Solubility 861
The Solubility of Amphoteric Metal Hydroxides 862
CHAPTER IN REVIEW: Self-Assessment Quiz 863
Key Terms 864
Key Concepts 864
Key Equations and Relationships 865
Key Learning Outcomes 865
EXERCISES: Review Questions 866
Problems by Topic 867
Cumulative Problems 872
Challenge Problems 873
Conceptual Problems 873
Questions for Group Work 874
Data Interpretation and Analysis 874
Answers to Conceptual Connections 875
18 Free Energy and Thermodynamics 876
18.1 Nature’s Heat Tax: You Can’t Win and You Can’t Break Even 877
18.2 Spontaneous and Nonspontaneous Processes 879
18.3 Entropy and the Second Law of Thermodynamics 881
Entropy 882
The Entropy Change upon the Expansion of an Ideal Gas 884
18.4 Entropy Changes Associated with State Changes 886
Entropy and State Change: The Concept 887
Entropy and State Changes: The Calculation 888
18.5 Heat Transfer and Changes in the Entropy of the Surroundings 890
The Temperature Dependence of & 891
Quantifying Entropy Changes in the Surroundings 892
18.6 Gibbs Free Energy 893
The Effect of & 894
18.7 Entropy Changes in Chemical Reactions: Calculating & 897
Defining Standard States and Standard Entropy Changes 897
Standard Molar Entropies (S°) and the Third Law of Thermodynamics 897
Calculating the Standard Entropy Change (& 901
18.8 Free Energy Changes in Chemical Reactions: Calculating & 901
Calculating Standard Free Energy Changes with & 902
Calculating & 903
Chemistry in Your Day: Making a Nonspontaneous Process Spontaneous 905
Calculating & 905
Why Free Energy Is “Free” 906
18.9 Free Energy Changes for Nonstandard States: The Relationship between & 908
Standard versus Nonstandard States 908
The Free Energy Change of a Reaction under Nonstandard Conditions 908
18.10 Free Energy and Equilibrium: Relating & 911
The Relationship between & 911
The Temperature Dependence of the Equilibrium Constant 913
CHAPTER IN REVIEW: Self-Assessment Quiz 914
Key Terms 915
Key Concepts 915
Key Equations and Relationships 916
Key Learning Outcomes 916
EXERCISES: Review Questions 917
Problems by Topic 918
Cumulative Problems 921
Challenge Problems 922
Conceptual Problems 923
Questions for Group Work 923
Data Interpretation and Analysis 924
Answers to Conceptual Connections 925
19 Electrochemistry 926
19.1 Pulling the Plug on the Power Grid 927
19.2 Balancing Oxidation–Reduction Equations 928
19.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions 931
The Voltaic Cell 932
Current and Potential Difference 933
Anode, Cathode, and Salt Bridge 934
Electrochemical Cell Notation 935
19.4 Standard Electrode Potentials 936
Predicting the Spontaneous Direction of an Oxidation–Reduction Reaction 940
Predicting Whether a Metal Will Dissolve in Acid 943
19.5 Cell Potential, Free Energy, and the Equilibrium Constant 943
The Relationship Between & 944
The Relationship between E°[Sub(cell)] and K 946
19.6 Cell Potential and Concentration 947
Cell Potential under Nonstandard Conditions: The Nernst Equation 947
Concentration Cells 950
Chemistry and Medicine: Concentration Cells in Human Nerve Cells 952
19.7 Batteries: Using Chemistry to Generate Electricity 952
Dry-Cell Batteries 952
Lead–Acid Storage Batteries 953
Other Rechargeable Batteries 954
Fuel Cells 955
Chemistry in Your Day: The Fuel-Cell Breathalyzer 956
19.8 Electrolysis: Driving Nonspontaneous Chemical Reactions with Electricity 956
Predicting the Products of Electrolysis 559
Stoichiometry of Electrolysis 962
19.9 Corrosion: Undesirable Redox Reactions 963
Corrosion of Iron 964
Preventing the Corrosion of Iron 965
CHAPTER IN REVIEW: Self-Assessment Quiz 965
Key Terms 966
Key Concepts 967
Key Equations and Relationships 967
Key Learning Outcomes 968
EXERCISES: Review Questions 968
Problems by Topic 969
Cumulative Problems 972
Challenge Problems 974
Conceptual Problems 974
Questions for Group Work 974
Data Interpretation and Analysis 975
Answers to Conceptual Connections 975
20 Radioactivity and Nuclear Chemistry 976
20.1 Diagnosing Appendicitis 977
20.2 The Discovery of Radioactivity 978
20.3 Types of Radioactivity 979
Alpha (& 980
Beta (& 981
Gamma (& 981
Positron Emission 982
Electron Capture 982
20.4 The Valley of Stability: Predicting the Type of Radioactivity 984
Magic Numbers 985
Radioactive Decay Series 986
20.5 Detecting Radioactivity 986
20.6 The Kinetics of Radioactive Decay and Radiometric Dating 987
The Integrated Rate Law 989
Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Artifacts 990
Chemistry in Your Day: Radiocarbon Dating and the Shroud of Turin 992
Uranium/Lead Dating 992
20.7 The Discovery of Fission: The Atomic Bomb and Nuclear Power 994
The Manhattan Project 994
Nuclear Power: Using Fission to Generate Electricity 996
Problems with Nuclear Power 997
20.8 Converting Mass to Energy: Mass Defect and Nuclear Binding Energy 998
Mass Defect and Nuclear Binding Energy 998
The Nuclear Binding Energy Curve 1000
20.9 Nuclear Fusion: The Power of the Sun 1000
20.10 Nuclear Transmutation and Transuranium Elements 1001
20.11 The Effects of Radiation on Life 1002
Acute Radiation Damage 1003
Increased Cancer Risk 1003
Genetic Defects 1003
Measuring Radiation Exposure and Dose 1003
20.12 Radioactivity in Medicine and Other Applications 1005
Diagnosis in Medicine 1005
Radiotherapy in Medicine 1006
Other Applications 1007
CHAPTER IN REVIEW: Self-Assessment Quiz 1007
Key Terms 1008
Key Concepts 1008
Key Equations and Relationships 1009
Key Learning Outcomes 1010
EXERCISES: Review Questions 1010
Problems by Topic 1011
Cumulative Problems 1012
Challenge Problems 1013
Conceptual Problems 1014
Questions for Group Work 1014
Data Interpretation and Analysis 1015
Answers to Conceptual Connections 1015
21 Organic Chemistry 1016
21.1 Fragrances and Odors 1017
21.2 Carbon: Why It Is Unique 1018
Chemistry in Your Day: Vitalism and the Perceived Differences between Organic and Inorganic Compounds 1019
21.3 Hydrocarbons: Compounds Containing Only Carbon and Hydrogen 1020
Drawing Hydrocarbon Structures 1021
Stereoisomerism and Optical Isomerism 1023
21.4 Alkanes: Saturated Hydrocarbons 1026
Naming Alkanes 1027
21.5 Alkenes and Alkynes 1030
Naming Alkenes and Alkynes 1031
Geometric (Cis–Trans) Isomerism in Alkenes 1034
21.6 Hydrocarbon Reactions 1035
Reactions of Alkanes 1035
Reactions of Alkenes and Alkynes 1036
21.7 Aromatic Hydrocarbons 1038
Naming Aromatic Hydrocarbons 1038
Reactions of Aromatic Compounds 1040
21.8 Functional Groups 1041
21.9 Alcohols 1042
Naming Alcohols 1042
About Alcohols 1042
Alcohol Reactions 1042
21.10 Aldehydes and Ketones 1044
Naming Aldehydes and Ketones 1045
About Aldehydes and Ketones 1045
Aldehyde and Ketone Reactions 1046
21.11 Carboxylic Acids and Esters 1047
Naming Carboxylic Acids and Esters 1047
About Carboxylic Acids and Esters 1047
Carboxylic Acid and Ester Reactions 1048
21.12 Ethers 1049
Naming Ethers 1049
About Ethers 1050
21.13 Amines 1050
Amine Reactions 1050
CHAPTER IN REVIEW: Self-Assessment Quiz 1051
Key Terms 1052
Key Concepts 1052
Key Equations and Relationships 1053
Key Learning Outcomes 1054
EXERCISES: Review Questions 1055
Problems by Topic 1055
Cumulative Problems 1061
Challenge Problems 1063
Conceptual Problems 1064
Questions for Group Work 1064
Data Interpretation and Analysis 1064
Answers to Conceptual Connections 1065
22 Biochemistry 1066
22.1 Diabetes and the Synthesis of Human Insulin 1067
22.2 Lipids 1068
Fatty Acids 1068
Fats and Oils 1070
Other Lipids 1071
22.3 Carbohydrates 1073
Simple Carbohydrates: Monosaccharides and Disaccharides 1073
Complex Carbohydrates 1075
22.4 Proteins and Amino Acids 1076
Amino Acids: The Building Blocks of Proteins 1077
Peptide Bonding between Amino Acids 1079
22.5 Protein Structure 1080
Primary Structure 1082
Secondary Structure 1082
Tertiary Structure 1083
Quaternary Structure 1084
22.6 Nucleic Acids: Blueprints for Proteins 1084
The Basic Structure of Nucleic Acids 1084
The Genetic Code 1086
22.7 DNA Replication, the Double Helix, and Protein Synthesis 1088
DNA Replication and the Double Helix 1088
Protein Synthesis 1089
Chemistry and Medicine: The Human Genome Project 1090
CHAPTER IN REVIEW: Self-Assessment Quiz 1091
Key Terms 1092
Key Concepts 1092
Key Learning Outcomes 1093
EXERCISES: Review Questions 1094
Problems by Topic 1094
Cumulative Problems 1097
Challenge Problems 1098
Conceptual Problems 1098
Questions for Group Work 1099
Data Interpretation and Analysis 1099
Answers to Conceptual Connections 1099
23 Chemistry of the Nonmetals 1100
23.1 Insulated Nanowires 1101
23.2 The Main-Group Elements: Bonding and Properties 1102
23.3 Silicates: The Most Abundant Matter in Earth’s Crust 1104
Quartz 1104
Aluminosilicates 1104
Individual Silicate Units, Silicate Chains, and Silicate Sheets 1105
23.4 Boron and Its Remarkable Structures 1108
Elemental Boron 1108
Boron–Halogen Compounds: Trihalides 1108
Boron–Oxygen Compounds 1109
Boron–Hydrogen Compounds: Boranes 1109
23.5 Carbon, Carbides, and Carbonates 1110
Amorphous Carbon 1110
Carbides 1111
Carbon Oxides 1113
Carbonates 1113
23.6 Nitrogen and Phosphorus: Essential Elements for Life 1114
Elemental Nitrogen and Phosphorus 1114
Nitrogen Compounds 1116
Phosphorus Compounds 1119
23.7 Oxygen 1121
Elemental Oxygen 1121
Uses for Oxygen 1122
Oxides 1122
Ozone 1122
23.8 Sulfur: A Dangerous but Useful Element 1123
Elemental Sulfur 1123
Hydrogen Sulfide and Metal Sulfides 1125
Sulfur Dioxide 1126
Sulfuric Acid 1126
23.9 Halogens: Reactive Elements with High Electronegativity 1127
Elemental Fluorine and Hydrofluoric Acid 1128
Elemental Chlorine 1129
Halogen Compounds 1129
CHAPTER IN REVIEW: Self-Assessment Quiz 1131
Key Terms 1132
Key Concepts 1132
Key Learning Outcomes 1133
EXERCISES: Review Questions 1133
Problems by Topic 1133
Cumulative Problems 1135
Challenge Problems 1136
Conceptual Problems 1136
Questions for Group Work 1136
Data Interpretation and Analysis 1137
Answers to Conceptual Connections 1137
24 Metals and Metallurgy 1138
24.1 Vanadium: A Problem and an Opportunity 1139
24.2 The General Properties and Natural Distribution of Metals 1140
24.3 Metallurgical Processes 1142
Separation 1142
Pyrometallurgy 1142
Hydrometallurgy 1143
Electrometallurgy 1144
Powder Metallurgy 1145
24.4 Metal Structures and Alloys 1146
Alloys 1146
Substitutional Alloys 1146
Alloys with Limited Solubility 1148
Interstitial Alloys 1149
24.5 Sources, Properties, and Products of Some of the 3d Transition Metals 1151
Titanium 1151
Chromium 1152
Manganese 1153
Cobalt 1154
Copper 1155
Nickel 1155
Zinc 1156
CHAPTER IN REVIEW: Self-Assessment Quiz 1156
Key Terms 1158
Key Concepts 1158
Key Equations and Relationships 1158
Key Learning Outcomes 1159
EXERCISES: Review Questions 1159
Problems by Topic 1159
Cumulative Problems 1161
Challenge Problems 1161
Conceptual Problems 1161
Questions for Group Work 1162
Data Interpretation and Analysis 1162
Answers to Conceptual Connections 1163
25 Transition Metals and Coordination Compounds 1164
25.1 The Colors of rubies and Emeralds 1165
25.2 Properties of Transition Metals 1166
Electron Configurations 1166
Atomic Size 1168
Ionization Energy 1168
Electronegativity 1169
Oxidation States 1169
25.3 Coordination Compounds 1170
Naming Coordination Compounds 1173
25.4 Structure and Isomerization 1175
Structural Isomerism 1175
Stereoisomerism 1177
25.5 Bonding in Coordination Compounds 1180
Valence Bond Theory 1180
Crystal Field Theory 1181
25.6 Applications of Coordination Compounds 1185
Chelating Agents 1186
Chemical Analysis 1186
Coloring Agents 1186
Biomolecules 1186
CHAPTER IN REVIEW: Self-Assessment Quiz 1189
Key Terms 1189
Key Concepts 1190
Key Equations and Relationships 1190
Key Learning Outcomes 1190
EXERCISES: Review Questions 1191
Problems by Topic 1191
Cumulative Problems 1193
Challenge Problems 1193
Conceptual Problems 1194
Questions for Group Work 1194
Data Interpretation and Analysis 1194
Answers to Conceptual Connections 1195
Appendix I: Common Mathematical Operations in Chemistry A-1
Appendix II: Useful Data A-5
Appendix III: Answers to Selected Exercises A-15
Appendix IV: Answers to In-Chapter Practice Problems A-54
Glossary G-1
A G-1
B G-2
C G-3
D G-5
E G-6
F G-7
G G-8
H G-8
I G-9
J G-10
K G-10
L G-10
M G-11
N G-12
O G-13
P G-13
Q G-15
R G-15
S G-16
T G-18
U G-18
V G-19
W G-19
X G-19
Photo and Text Credits C-1
Index I-1
A I-1
B I-3
C I-4
D I-7
E I-8
F I-10
G I-10
H I-11
I I-13
J I-14
K I-14
L I-14
M I-15
N I-17
O I-18
P I-19
Q I-21
R I-21
S I-22
T I-25
U I-26
V I-26
W I-27
X I-27
Y I-27
Z I-27