Chemistry, Global Edition

John E. McMurry; Robert C. Fay; Jill Kirsten Robinson

BOOK

Chemistry, Global Edition

John E. McMurry | Robert C. Fay | Jill Kirsten Robinson

(2016)

Additional Information

Book Details

ISBN: 978-1-292-09276-8
Edition: 7
Language: English
Pages: 1168
Subjects

Abstract

For two-semester general chemistry courses (science majors).
Make critical connections in chemistry clear and visible
McMurry/Fay/Robinson’s Chemistry, Seventh Edition, aims to help students understand the connections between topics in general chemistry and why they matter. The Seventh Edition provides a concise and streamlined narrative that blends the quantitative and visual aspects of chemistry, demonstrates the connections between topics, and illustrates the application of chemistry to their lives and careers. New content offers a better bridge between organic and biochemistry and general chemistry content, and new and improved pedagogical features make the text a true teaching tool rather than just a reference book.
New MasteringChemistry features include conceptual worked examples and integrated Inquiry sections that help make critical connections clear and visible and increase students’ understanding of chemistry. The Seventh Edition fully integrates the text with new MasteringChemistry content and functionality to support the learning process before, during, and after class.

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

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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. Students can further master concepts after class through traditional and adaptive homework assignments that provide hints and answer-specific feedback. The Mastering gradebook records scores for all automatically graded assignments in one place, while diagnostic tools give instructors access to rich data to assess student understanding and misconceptions.

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Section Title	Page	Action	Price
Cover	Cover
Title Page	1
Copyright Page	2
About the Authors	11
Acknowledgments	19
Contents	4
Preface	12
For Instructors	14
1 Chemical Tools: Experimentation and Measurement	29
1.1 The Scientific Method in a Chemical Context: Improved Pharmaceutical Insulin	30
1.2 Experimentation and Measurement	34
1.3 Mass and Its Measurement	36
1.4 Length and Its Measurement	36
1.5 Temperature and Its Measurement	37
1.6 Derived Units: Volume and Its Measurement	39
1.7 Derived Units: Density and Its Measurement	40
1.8 Derived Units: Energy and Its Measurement	42
1.9 Accuracy, Precision, and Significant Figures in Measurement	44
1.10 Rounding Numbers	46
1.11 Calculations: Converting from One Unit to Another	48
INQUIRY What are the unique properties of nanoscale materials?	51
Study Guide	54
Key Terms	55
Key Equations	55
Conceptual Problems	56
Section Problems	56
Chapter Problems	59
2 Atoms, Molecules, and Ions	61
2.1 Chemistry and the Elements	62
2.2 Elements and the Periodic Table	63
2.3 Some Common Groups of Elements and Their Properties	66
2.4 Observations Supporting Atomic Theory: The Conservation of Mass and the Law of Definite Proportions	69
2.5 The Law of Multiple Proportions and Dalton’s Atomic Theory	71
2.6 Atomic Structure: Electrons	73
2.7 Atomic Structure: Protons and Neutrons	75
2.8 Atomic Numbers	77
2.9 Atomic Weights and the Mole	79
2.10 Mixtures and Chemical Compounds; Molecules and Covalent Bonds	82
2.11 Ions and Ionic Bonds	86
2.12 Naming Chemical Compounds	88
INQUIRY How is the principle of atom economy used to minimize waste in a chemical synthesis?	94
Study Guide	96
Key Terms	98
Conceptual Problems	98
Section Problems	100
Chapter Problems	104
3 Mass Relationships in Chemical Reactions	105
3.1 Representing Chemistry on Different Levels	106
3.2 Balancing Chemical Equations	107
3.3 Chemical Arithmetic: Stoichiometry	110
3.4 Yields of Chemical Reactions	114
3.5 Reactions with Limiting Amounts of Reactants	116
3.6 Percent Composition and Empirical Formulas	119
3.7 Determining Empirical Formulas: Elemental Analysis	122
3.8 Determining Molecular Weights: Mass Spectrometry	125
INQUIRY Can alternative fuels decrease CO[Sub2] emissions?	129
Study Guide	132
Key Terms	133
Key Equations	133
Conceptual Problems	133
Section Problems	134
Chapter Problems	137
4 Reactions in Aqueous Solution	139
4.1 Solution Concentration: Molarity	140
4.2 Diluting Concentrated Solutions	142
4.3 Electrolytes in Aqueous Solution	144
4.4 Types of Chemical Reactions in Aqueous Solution	146
4.5 Aqueous Reactions and Net Ionic Equations	147
4.6 Precipitation Reactions and Solubility Guidelines	148
4.7 Acids, Bases, and Neutralization Reactions	151
4.8 Solution Stoichiometry	155
4.9 Measuring the Concentration of a Solution: Titration	156
4.10 Oxidation–Reduction (Redox) Reactions	158
4.11 Identifying Redox Reactions	161
4.12 The Activity Series of the Elements	163
4.13 Redox Titrations	166
4.14 Some Applications of Redox Reactions	169
INQUIRY How do sports drinks replenish the chemicals lost in sweat?	170
Study Guide	172
Key Terms	173
Key Equations	174
Conceptual Problems	174
Section Problems	176
Chapter Problems	179
Multiconcept Problems	180
5 Periodicity and the Electronic Structure of Atoms	182
5.1 The Nature of Radiant Energy and the Electromagnetic Spectrum	183
5.2 Particlelike Properties of Radiant Energy: The Photoelectric Effect and Planck’s Postulate	186
5.3 The Interaction of Radiant Energy with Atoms: Line Spectra	188
5.4 The Bohr Model of the Atom: Quantized Energy	191
5.5 Wavelike Properties of Matter: de Broglie’s Hypothesis	193
5.6 The Quantum Mechanical Model of the Atom: Heisenberg’s Uncertainty Principle	195
5.7 The Quantum Mechanical Model of the Atom: Orbitals and Quantum Numbers	196
5.8 The Shapes of Orbitals	198
5.9 Electron Spin and the Pauli Exclusion Principle	202
5.10 Orbital Energy Levels in Multielectron Atoms	203
5.11 Electron Configurations of Multielectron Atoms	204
5.12 Anomalous Electron Configurations	206
5.13 Electron Configurations and the Periodic Table	206
5.14 Electron Configurations and Periodic Properties: Atomic Radii	209
INQUIRY How does knowledge of atomic emission spectra help us build more efficient light bulbs?	212
Study Guide	213
Key Terms	215
Key Equations	216
Conceptual Problems	216
Section Problems	217
Chapter Problems	220
Multiconcept Problems	222
6 Ionic Compounds: Periodic Trends and Bonding Theory	223
6.1 Electron Configurations of Ions	224
6.2 Ionic Radii	226
6.3 Ionization Energy	228
6.4 Higher Ionization Energies	230
6.5 Electron Affinity	232
6.6 The Octet Rule	234
6.7 Ionic Bonds and the Formation of Ionic Solids	236
6.8 Lattice Energies in Ionic Solids	239
INQUIRY How has an understanding of ionic compounds led to the production of safer solvents?	242
Study Guide	244
Key Terms	245
Key Equations	245
Conceptual Problems	245
Section Problems	247
Chapter Problems	248
Multiconcept Problems	249
7 Covalent Bonding and Electron-Dot Structures	250
7.1 Covalent Bonding in Molecules	251
7.2 Strengths of Covalent Bonds	253
7.3 Polar Covalent Bonds: Electronegativity	254
7.4 A Comparison of Ionic and Covalent Compounds	257
7.5 Electron-Dot Structures: The Octet Rule	259
7.6 Procedure for Drawing Electron-Dot Structures	262
7.7 Drawing Electron-Dot Structures for Radicals	266
7.8 Electron-Dot Structures of Compounds Containing Only Hydrogen and Second-Row Elements	268
7.9 Electron-Dot Structures and Resonance	270
7.10 Formal Charges	274
INQUIRY How do we make organophosphate insecticides less toxic to humans?	278
Study Guide	280
Key Terms	282
Key Equations	282
Conceptual Problems	282
Section Problems	283
Chapter Problems	287
Multiconcept Problems	288
8 Covalent Compounds: Bonding Theories and Molecular Structure	289
8.1 Molecular Shapes: The VSEPR Model	290
8.2 Valence Bond Theory	298
8.3 Hybridization and sp[Sup(3)] Hybrid Orbitals	299
8.4 Other Kinds of Hybrid Orbitals	301
8.5 Polar Covalent Bonds and Dipole Moments	306
8.6 Intermolecular Forces	310
8.7 Molecular Orbital Theory: The Hydrogen Molecule	319
8.8 Molecular Orbital Theory: Other Diatomic Molecules	322
8.9 Combining Valence Bond Theory and Molecular Orbital Theory	325
INQUIRY Why do different drugs have different physiological responses?	327
Study Guide	330
Key Terms	331
Conceptual Problems	331
Section Problems	333
Chapter Problems	336
Multiconcept Problems	337
9 Thermochemistry: Chemical Energy	339
9.1 Energy and Its Conservation	340
9.2 Internal Energy and State Functions	342
9.3 Expansion Work	344
9.4 Energy and Enthalpy	346
9.5 Thermochemical Equations and the Thermodynamic Standard State	349
9.6 Enthalpies of Chemical and Physical Changes	351
9.7 Calorimetry and Heat Capacity	353
9.8 Hess’s Law	357
9.9 Standard Heats of Formation	359
9.10 Bond Dissociation Energies	362
9.11 Fossil Fuels, Fuel Efficiency, and Heats of Combustion	363
9.12 An Introduction to Entropy	365
9.13 An Introduction to Free Energy	368
INQUIRY How is the energy content of new fuels determined?	372
Study Guide	374
Key Terms	376
Key Equations	376
Conceptual Problems	377
Section Problems	378
Chapter Problems	383
Multiconcept Problems	384
10 Gases: Their Properties and Behavior	386
10.1 Gases and Gas Pressure	387
10.2 The Gas Laws	392
10.3 The Ideal Gas Law	397
10.4 Stoichiometric Relationships with Gases	400
10.5 Mixtures of Gases: Partial Pressure and Dalton’s Law	403
10.6 The Kinetic–Molecular Theory of Gases	406
10.7 Gas Diffusion and Effusion: Graham’s Law	408
10.8 The Behavior of Real Gases	411
10.9 The Earth’s Atmosphere and Air Pollution	412
10.10 The Greenhouse Effect	417
10.11 Climate Change	422
INQUIRY Which gases are greenhouse gases?	420
Study Guide	425
Key Terms	426
Key Equations	427
Conceptual Problems	428
Section Problems	430
Chapter Problems	434
Multiconcept Problems	436
11 Liquids, Solids, and Phase Changes	438
11.1 Properties of Liquids	439
11.2 Phase Changes between Solids, Liquids, and Gases	440
11.3 Evaporation, Vapor Pressure, and Boiling Point	445
11.4 Kinds of Solids	448
11.5 Probing the Structure of Solids: X-Ray Crystallography	450
11.6 The Packing of Spheres in Crystalline Solids: Unit Cells	453
11.7 Structures of Some Ionic Solids	458
11.8 Structures of Some Covalent Network Solids	460
11.9 Phase Diagrams	463
INQUIRY How is caffeine removed from coffee?	465
Study Guide	467
Key Terms	468
Key Equations	468
Conceptual Problems	469
Section Problems	470
Chapter Problems	472
Multiconcept Problems	474
12 Solutions and Their Properties	475
12.1 Solutions	476
12.2 Energy Changes and the Solution Process	477
12.3 Concentration Units for Solutions	482
12.4 Some Factors That Affect Solubility	486
12.5 Physical Behavior of Solutions: Colligative Properties	490
12.6 Vapor-Pressure Lowering of Solutions: Raoult’s Law	490
12.7 Boiling-Point Elevation and Freezing-Point Depression of Solutions	497
12.8 Osmosis and Osmotic Pressure	501
12.9 Fractional Distillation of Liquid Mixtures	505
INQUIRY How does hemodialysis cleanse the blood of patients with kidney failure?	507
Study Guide	509
Key Terms	510
Key Equations	510
Conceptual Problems	511
Section Problems	513
Chapter Problems	516
Multiconcept Problems	518
13 Chemical Kinetics	519
13.1 Reaction Rates	520
13.2 Rate Laws and Reaction Order	525
13.3 Method of Initial Rates: Experimental Determination of a Rate Law	528
13.4 Integrated rate Law: Zeroth-Order Reactions	531
13.5 Integrated Rate law: First-Order Reactions	533
13.6 Integrated Rate Law: Second-Order Reactions	538
13.7 Reaction Rates and Temperature: The Arrhenius Equation	542
13.8 Using the Arrhenius Equation	546
13.9 Reaction Mechanisms	548
13.10 Rate Laws for Elementary Reactions	552
13.11 Rate Laws for Overall Reactions	554
13.12 Catalysis	558
13.13 Homogeneous and Heterogeneous Catalysts	561
13.14 Enzyme Catalysis	564
INQUIRY What causes the ozone hole?	565
Study Guide	568
Key Terms	569
Key Equations	569
Conceptual Problems	570
Section Problems	572
Chapter Problems	576
Multiconcept Problems	579
14 Chemical Equilibrium	581
14.1 The Equilibrium State	582
14.2 The Equilibrium Constant K[Sub(c)]	584
14.3 The Equilibrium Constant K[Sub(p)]	589
14.4 Heterogeneous Equilibria	592
14.5 Using the Equilibrium Constant	593
14.6 Factors that Alter the Composition of an Equilibrium Mixture: Le Châtelier’s Principle	602
14.7 Altering an Equilibrium Mixture: Changes in Concentration	603
14.8 Altering an Equilibrium Mixture: Changes in Pressure and Volume	607
14.9 Altering an Equilibrium Mixture: Changes in Temperature	609
14.10 The Link between Chemical Equilibrium and Chemical Kinetics	612
INQUIRY How does equilibrium affect oxygen transport in the bloodstream?	616
Study Guide	618
Key Terms	619
Key Equations	619
Conceptual Problems	620
Section Problems	622
Chapter Problems	626
Multiconcept Problems	629
15 Aqueous Equilibria: Acids and Bases	631
15.1 Acid–Base Concepts: The Brønsted–Lowry Theory	632
15.2 Acid Strength and Base Strength	636
15.3 Factors That Affect Acid Strength	638
15.4 Dissociation of Water	641
15.5 The pH Scale	644
15.6 Measuring pH	646
15.7 The pH in Solutions of Strong Acids and Strong Bases	647
15.8 Equilibria in Solutions of Weak Acids	649
15.9 Calculating Equilibrium Concentrations in Solutions of Weak Acids	651
15.10 Percent Dissociation in Solutions of Weak Acids	655
15.11 Polyprotic Acids	656
15.12 Equilibria in Solutions of Weak Bases	660
15.13 Relation between K[Sub(a)] and K[Sub(b)]	662
15.14 Acid–Base Properties of Salts	664
15.15 Lewis Acids and Bases	668
INQUIRY What is acid rain and what are its effects?	671
Study Guide	673
Key Terms	674
Key Equations	675
Conceptual Problems	675
Section Problems	677
Chapter Problems	681
Multiconcept Problems	682
16 Applications of Aqueous Equilibria	684
16.1 Neutralization Reactions	685
16.2 The Common-Ion Effect	688
16.3 Buffer Solutions	692
16.4 The Henderson–Hasselbalch Equation	697
16.5 pH Titration Curves	700
16.6 Strong Acid–Strong Base Titrations	701
16.7 Weak Acid–Strong Base Titrations	704
16.8 Weak Base–Strong Acid Titrations	709
16.9 Polyprotic Acid–Strong Base Titrations	710
16.10 Solubility Equilibria for Ionic Compounds	714
16.11 Measuring K[Sub(sp)] and Calculating Solubility from K[Sub(sp)]	716
16.12 Factors That Affect Solubility	718
16.13 Precipitation of Ionic Compounds	726
16.14 Separation of Ions by Selective Precipitation	728
16.15 Qualitative Analysis	728
INQUIRY What is causing a decrease in the pH of the oceans?	731
Study Guide	733
Key Terms	734
Key Equations	734
Conceptual Problems	735
Section Problems	737
Chapter Problems	740
Multiconcept Problems	742
17 Thermodynamics: Entropy, Free Energy, and Equilibrium	743
17.1 Spontaneous Processes	744
17.2 Enthalpy, Entropy, and Spontaneous Processes: A Brief Review	745
17.3 Entropy and Probability	748
17.4 Entropy and Temperature	752
17.5 Standard Molar Entropies and Standard Entropies of Reaction	754
17.6 Entropy and the Second Law of Thermodynamics	756
17.7 Free Energy and the Spontaneity of Chemical Reactions	758
17.8 Standard Free-Energy Changes for Reactions	761
17.9 Standard Free Energies of Formation	764
17.10 Free-Energy Changes for Reactions under Nonstandard-State Conditions	766
17.11 Free Energy and Chemical Equilibrium	768
INQUIRY Does entropy prevent the evolution of biological complexity?	772
Study Guide	774
Key Terms	775
Key Equations	775
Conceptual Problems	776
Section Problems	777
Chapter Problems	781
Multiconcept Problems	783
18 Electrochemistry	784
18.1 Balancing Redox Reactions by the Half-Reaction Method	785
18.2 Galvanic Cells	789
18.3 Shorthand Notation for Galvanic Cells	794
18.4 Cell Potentials and Free-Energy Changes for Cell Reactions	795
18.5 Standard Reduction Potentials	797
18.6 Using Standard Reduction Potentials	801
18.7 Cell Potentials under Nonstandard-State Conditions: The Nernst Equation	803
18.8 Electrochemical Determination of pH	805
18.9 Standard Cell Potentials and Equilibrium Constants	807
18.10 Batteries	810
18.11 Corrosion	813
18.12 Electrolysis and Electrolytic Cells	815
18.13 Commercial Applications of Electrolysis	818
18.14 Quantitative Aspects of Electrolysis	821
INQUIRY How do hydrogen fuel cells work?	823
Study Guide	825
Key Terms	826
Key Equations	826
Conceptual Problems	827
Section Problems	828
Chapter Problems	832
Multiconcept Problems	834
19 Nuclear Chemistry	836
19.1 Nuclear Reactions and Their Characteristics	837
19.2 Radioactivity	838
19.3 Nuclear Stability	841
19.4 Radioactive Decay Rates	844
19.5 Energy Changes during Nuclear Reactions	847
19.6 Nuclear Fission and Fusion	850
19.7 Nuclear Transmutation	855
19.8 Detecting and Measuring Radioactivity	856
19.9 Some Applications of Nuclear Chemistry	858
INQUIRY Are there any naturally occurring nuclear reactors?	861
Study Guide	862
Key Terms	863
Key Equations	863
Conceptual Problems	864
Section Problems	864
Chapter Problems	866
Multiconcept Problems	867
20 Transition Elements and Coordination Chemistry	868
20.1 Electron Configurations	870
20.2 Properties of Transition Elements	872
20.3 Oxidation States of Transition Elements	875
20.4 Chemistry of Selected Transition Elements	877
20.5 Coordination Compounds	882
20.6 Ligands	884
20.7 Naming Coordination Compounds	886
20.8 Isomers	890
20.9 Enantiomers and Molecular Handedness	895
20.10 Color of Transition Metal Complexes	897
20.11 Bonding in Complexes: Valence Bond Theory	898
20.12 Crystal Field Theory	902
INQUIRY How does cisplatin kill cancer cells?	908
Study Guide	910
Key Terms	912
Key Equations	912
Conceptual Problems	912
Section Problems	913
Chapter Problems	917
Multiconcept Problems	918
21 Metals and Solid-State Materials	920
21.1 Sources of the Metallic Elements	921
21.2 Metallurgy	922
21.3 Iron and Steel	925
21.4 Bonding in Metals	927
21.5 Semiconductors	930
21.6 Semiconductor Applications	933
21.7 Superconductors	937
21.8 Ceramics	940
21.9 Composites	943
INQUIRY What are quantum dots and what controls their color?	944
Study Guide	946
Key Terms	947
Conceptual Problems	947
Section Problems	948
Chapter Problems	952
Multiconcept Problems	953
22 The Main-Group Elements	955
22.1 A Review of General Properties and Periodic Trends	956
22.2 Distinctive Properties of the Second-Row Elements	958
22.3 Group 1A: Hydrogen	960
22.4 Group 1A: Alkali Metals	965
22.5 Group 2A: Alkaline-Earth Metals	967
22.6 Group 3A: Elements	968
22.7 Group 4A: Carbon	970
22.8 Group 4A: Silicon	974
22.9 Group 5A: Nitrogen	978
22.10 Group 5A: Phosphorus	982
22.11 Group 6A: Oxygen	985
22.12 Group 6A: Sulfur	989
22.13 Group 7A: The Halogens	992
22.14 Group 8A: Noble Gases	994
INQUIRY What are the barriers to a hydrogen economy?	995
Study Guide	997
Key Terms	998
Conceptual Problems	998
Section Problems	1001
Chapter Problems	1004
Multiconcept Problems	1005
23 Organic and Biological Chemistry	1006
23.1 Organic Molecules and Their Structures: Alkanes	1007
23.2 Families of Organic Compounds: Functional Groups	1011
23.3 Naming Organic Compounds	1013
23.4 Carbohydrates: A Biological Example of Isomers	1018
23.5 Valence Bond Theory and Orbital Overlap Pictures	1021
23.6 Lipids: A Biological Example of Cis–Trans Isomerism	1025
23.7 Formal Charge and Resonance in Organic Compounds	1029
23.8 Conjugated Systems	1034
23.9 Proteins: A Biological Example of Conjugation	1037
23.10 Aromatic Compounds and Molecular Orbital Theory	1042
23.11 Nucleic Acids: A Biological Example of Aromaticity	1045
INQUIRY Which is better, natural or synthetic?	1049
Study Guide	1050
Key Terms	1051
Conceptual Problems	1051
Section Problems	1052
Chapter Problems	1059
Multiconcept Problems	1060
Appendix A: Mathematical Operations	A-1
A.1 Scientific Notation	A-1
A.2 Logarithms	A-4
A.3 Straight-Line Graphs and Linear Equations	A-6
A.4 Quadratic Equations	A-7
Appendix B: Thermodynamic Properties at 25 °C	A-8
Appendix C: Equilibrium Constants at 25 °C	A-13
Appendix D: Standard Reduction Potentials at 25 °C	A-17
Appendix E: Properties of Water	A-19
Answers to Selected Problems	A-21
Glossary	G-1
A	G-1
B	G-2
C	G-2
D	G-4
E	G-4
F	G-5
G	G-5
H	G-5
H	G-6
J	G-6
K	G-6
L	G-7
M	G-7
N	G-8
O	G-8
P	G-9
Q	G-9
R	G-9
S	G-10
T	G-11
U	G-11
V	G-12
W	G-12
Y	G-12
Z	G-12
Index	I-1
A	I-1
B	I-2
C	I-3
D	I-6
E	I-7
F	I-8
G	I-9
H	I-10
I	I-11
J	I-11
K	I-11
L	I-11
M	I-12
N	I-13
O	I-14
P	I-15
Q	I-16
R	I-16
S	I-16
T	I-18
U	I-19
V	I-19
W	I-19
X	I-20
Y	I-20
Z	I-20
Photo/Text Credits	C-1

Chemistry, Global Edition

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