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Chemistry: The Central Science 14th edition [Kietas viršelis]

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  • Formatas: Hardback, 1248 pages, aukštis x plotis x storis: 280x220x40 mm, weight: 2754 g
  • Išleidimo metai: 01-Mar-2017
  • Leidėjas: Pearson
  • ISBN-10: 0134414233
  • ISBN-13: 9780134414232
Kitos knygos pagal šią temą:
  • Formatas: Hardback, 1248 pages, aukštis x plotis x storis: 280x220x40 mm, weight: 2754 g
  • Išleidimo metai: 01-Mar-2017
  • Leidėjas: Pearson
  • ISBN-10: 0134414233
  • ISBN-13: 9780134414232
Kitos knygos pagal šią temą:

The trusted, innovative, calibrated leader–now tightly–integrated with MasteringChemistry®.

Unrivaled problems, notable scientific accuracy and currency, and remarkable clarity have madeChemistry: The Central Science the leading general chemistry text for more than a decade. Trusted, innovative, and calibrated, the text increases conceptual understanding and student success in general chemistry by building on the expertise of the dynamic author team of leading researchers and award-winning professors.

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Preface xxiii
1 Introduction: Matter, Energy, and Measurement 2(40)
1.1 The Study of Chemistry
4(3)
The Atomic and Molecular Perspective of Chemistry
4(1)
Why Study Chemistry?
5(2)
1.2 Classifications of Matter
7(5)
States of Matter
7(1)
Pure Substances
7(1)
Elements
8(1)
Compounds
9(1)
Mixtures
10(2)
1.3 Properties of Matter
12(3)
Physical and Chemical Changes
12(1)
Separation of Mixtures
13(2)
1.4 The Nature of Energy
15(2)
Kinetic Energy and Potential Energy
15(2)
1.5 Units of Measurement
17(7)
SI Units
17(2)
Length and Mass
19(1)
Temperature
19(1)
Derived SI Units
20(1)
Volume
20(1)
Density
21(1)
Units of Energy
21(3)
1.6 Uncertainty in Measurement
24(4)
Precision and Accuracy
24(1)
Significant Figures
25(1)
Significant Figures in Calculations
26(2)
1.7 Dimensional Analysis
28(5)
Conversion Factors
28(2)
Using Two or More Conversion Factors
30(1)
Conversions Involving Volume
31(2)
Chapter Summary and Key Terms
33(1)
Learning Outcomes
34(1)
Key Equations
34(1)
Exercises
35(4)
Additional Exercises
39(3)
2 Atoms, Molecules and Ions 42(40)
2.1 The Atomic Theory of Matter
44(1)
2.2 The Discovery of Atomic Structure
45(4)
Cathode Rays and Electrons
45(2)
Radioactivity
47(1)
The Nuclear Model of the Atom
48(1)
2.3 The Modern View of Atomic Structure
49(4)
Atomic Numbers, Mass Numbers, and Isotopes
51(2)
2.4 Atomic Weights
53(2)
The Atomic Mass Scale
53(1)
Atomic Weight
53(2)
2.5 The Periodic Table
55(3)
2.6 Molecules and Molecular Compounds
58(2)
Molecules and Chemical Formulas
58(1)
Molecular and Empirical Formulas
58(1)
Picturing Molecules
59(1)
2.7 Ions and Ionic Compounds
60(5)
Predicting Ionic Charges
61(1)
Ionic Compounds
62(3)
2.8 Naming Inorganic Compounds
65(6)
Names and Formulas of Ionic Compounds
65(4)
Names and Formulas of Acids
69(1)
Names and Formulas of Binary Molecular Compounds
70(1)
2.9 Some Simple Organic Compounds
71(3)
Alkanes
71(1)
Some Derivatives of Alkanes
72(2)
Chapter Summary and Key Terms
74(1)
Learning Outcomes
74(1)
Key Equations
75(1)
Exercises
75(5)
Additional Exercises
80(2)
3 Chemical Reactions and Reaction Stoichiometry 82(38)
3.1 Chemical Equations
84(4)
Balancing Equations
84(1)
A Step-by-Step Example of Balancing a Chemical Equation
85(2)
Indicating the States of Reactants and Products
87(1)
3.2 Simple Patterns of Chemical Reactivity
88(2)
Combination and Decomposition Reactions
88(2)
Combustion Reactions
90(1)
3.3 Formula Weights
90(3)
Formula and Molecular Weights
91(1)
Percentage Composition from Chemical Formulas
92(1)
3.4 Avogadro's Number and the Mole
93(5)
Molar Mass
94(2)
Interconverting Masses and Moles
96(1)
Interconverting Masses and Numbers of Particles
97(1)
3.5 Empirical Formulas from Analyses
98(4)
Molecular Formulas from Empirical Formulas
100(1)
Combustion Analysis
101(1)
3.6 Quantitative Information from Balanced Equations
102(4)
3.7 Limiting Reactants
106(4)
Theoretical and Percent Yields
108(2)
Chapter Summary and Key Terms
110(1)
Learning Outcomes
110(1)
Key Equations
110(1)
Exercises
111(6)
Additional Exercises
117(1)
Integrative Exercises
118(1)
Design an Experiment
119(1)
4 Reactions in Aqueous Solution 120(42)
4.1 General Properties of Aqueous Solutions
122(4)
Electrolytes and Nonelectrolytes
122(1)
How Compounds Dissolve in Water
123(1)
Strong and Weak Electrolytes
124(2)
4.2 Precipitation Reactions
126(4)
Solubility Guidelines for Ionic Compounds
126(1)
Exchange (Metathesis) Reactions
127(2)
Ionic Equations and Spectator Ions
129(1)
4.3 Acids, Bases, and Neutralization Reactions
130(7)
Acids
130(1)
Bases
131(1)
Strong and Weak Acids and Bases
132(1)
Identifying Strong and Weak Electrolytes
132(2)
Neutralization Reactions and Salts
134(2)
Neutralization Reactions with Gas Formation
136(1)
4.4 Oxidation-Reduction Reactions
137(7)
Oxidation and Reduction
137(1)
Oxidation Numbers
138(2)
Oxidation of Metals by Acids and Salts
140(1)
The Activity Series
141(3)
4.5 Concentrations of Solutions
144(4)
Molarity
144(1)
Expressing the Concentration of an Electrolyte
145(1)
Interconverting Molarity, Moles, and Volume
146(1)
Dilution
147(1)
4.6 Solution Stoichiometry and Chemical Analysis
148(5)
Titrations
150(3)
Chapter Summary and Key Terms
153(1)
Learning Outcomes
154(1)
Key Equations
154(1)
Exercises
154(5)
Additional Exercises
159(1)
Integrative Exercises
160(1)
Design an Experiment
161(1)
5 Thermochemistry 162(50)
5.1 The Nature of Chemical Energy
164(2)
5.2 The First Law of Thermodynamics
166(6)
System and Surroundings
166(1)
Internal Energy
167(1)
Relating DE to Heat and Work
168(2)
Endothermic and Exothermic Processes
170(1)
State Functions
170(2)
5.3 Enthalpy
172(4)
Pressure-Volume Work
172(2)
Enthalpy Change
174(2)
5.4 Enthalpies of Reaction
176(2)
5.5 Calorimetry
178(5)
Heat Capacity and Specific Heat
179(1)
Constant-Pressure Calorimetry
180(2)
Bomb Calorimetry (Constant-Volume Calorimetry)
182(1)
5.6 Hess's Law
183(3)
5.7 Enthalpies of Formation
186(4)
Using Enthalpies of Formation to Calculate Enthalpies of Reaction
188(2)
5.8 Bond Enthalpies
190(4)
Bond Enthalpies and the Enthalpies of Reactions
192(2)
5.9 Foods and Fuels
194(6)
Foods
194(2)
Fuels
196(1)
Other Energy Sources
197(3)
Chapter Summary and Key Terms
200(1)
Learning Outcomes
201(1)
Key Equations
201(1)
Exercises
202(6)
Additional Exercises
208(2)
Integrative Exercises
210(1)
Design an Experiment
211(1)
6 Electronic Structure of Atoms 212(44)
6.1 The Wave Nature of Light
214(2)
6.2 Quantized Energy and Photons
216(3)
Hot Objects and the Quantization of Energy
216(1)
The Photoelectric Effect and Photons
217(2)
6.3 Line Spectra and the Bohr Model
219(5)
Line Spectra
219(1)
Bohr's Model
220(1)
The Energy States of the Hydrogen Atom
221(3)
Limitations of the Bohr Model
224(1)
6.4 The Wave Behavior of Matter
224(3)
The Uncertainty Principle
226(1)
6.5 Quantum Mechanics and Atomic Orbitals
227(4)
Orbitals and Quantum Numbers
228(3)
6.6 Representations of Orbitals
231(3)
The s Orbitals
231(2)
The p Orbitals
233(1)
The d and f Orbitals
234(1)
6.7 Many-Electron Atoms
234(2)
Orbitals and Their Energies
235(1)
Electron Spin and the Pauli Exclusion Principle
236(1)
6.8 Electron Configurations
236(5)
Hund's Rule
238(2)
Condensed Electron Configurations
240(1)
Transition Metals
240(1)
The Lanthanides and Actinides
241(1)
6.9 Electron Configurations and the Periodic Table
241(5)
Anomalous Electron Configurations
244(2)
Chapter Summary and Key Terms
246(1)
Learning Outcomes
247(1)
Key Equations
248(1)
Exercises
248(5)
Additional Exercises
253(2)
Integrative Exercises
255(1)
Design an Experiment
255(1)
7 Periodic Properties of the Elements 256(42)
7.1 Development of the Periodic Table
258(1)
7.2 Effective Nuclear Charge
259(3)
7.3 Sizes of Atoms and Ions
262(6)
Periodic Trends in Atomic Radii
264(1)
Periodic Trends in Ionic Radii
264(4)
7.4 Ionization Energy
268(4)
Variations in Successive Ionization Energies
268(1)
Periodic Trends in First Ionization Energies
269(1)
Electron Configurations of Ions
270(2)
7.5 Electron Affinity
272(1)
Periodic Trends in Electron Affinity
273(1)
7.6 Metals, Nonmetals, and Metalloids
273(5)
Metals
274(2)
Nonmetals
276(2)
Metalloids
278(1)
7.7 Trends for Group 1A and Group 2A Metals
278(5)
Group 1A: The Alkali Metals
278(4)
Group 2A: The Alkaline Earth Metals
282(1)
7.8 Trends for Selected Nonmetals
283(5)
Hydrogen
283(1)
Group 6A: The Oxygen Group
284(1)
Group 7A: The Halogens
285(2)
Group 8A: The Noble Gases
287(1)
Chapter Summary and Key Terms
288(1)
Learning Outcomes
289(1)
Key Equations
289(1)
Exercises
290(4)
Additional Exercises
294(2)
Integrative Exercises
296(1)
Design an Experiment
297(1)
8 Basic Concepts of Chemical Bonding 298(40)
8.1 Lewis Symbols and the Octet Rule
300(1)
The Octet Rule
300(1)
8.2 Ionic Bonding
301(5)
Energetics of Ionic Bond Formation
302(2)
Electron Configurations of Ions of the s- and p-Block Elements
304(1)
Transition Metal Ions
305(1)
8.3 Covalent Bonding
306(3)
Lewis Structures
307(1)
Multiple Bonds
308(1)
8.4 Bond Polarity and Electronegativity
309(6)
Electronegativity
309(1)
Electronegativity and Bond Polarity
310(1)
Dipole Moments
311(3)
Comparing Ionic and Covalent Bonding
314(1)
8.5 Drawing Lewis Structures
315(4)
Formal Charge and Alternative Lewis Structures
317(2)
8.6 Resonance Structures
319(3)
Resonance in Benzene
321(1)
8.7 Exceptions to the Octet Rule
322(3)
Odd Number of Electrons
323(1)
Less Than an Octet of Valence Electrons
323(1)
More Than an Octet of Valence Electrons
324(1)
8.8 Strengths and Lengths of Covalent Bonds
325(3)
Chapter Summary and Key Terms
328(1)
Learning Outcomes
329(1)
Key Equations
329(1)
Exercises
329(5)
Additional Exercises
334(1)
Integrative Exercises
335(2)
Design an Experiment
337(1)
9 Molecular Geometry and Bonding Theories 338(56)
9.1 Molecular Shapes
340(2)
9.2 The VSEPR Model
342(10)
Applying the VSEPR Model to Determine Molecular Shapes
343(4)
Effect of Nonbonding Electrons and Multiple Bonds on Bond Angles
347(1)
Molecules with Expanded Valence Shells
347(3)
Shapes of Larger Molecules
350(2)
9.3 Molecular Shape and Molecular Polarity
352(2)
9.4 Covalent Bonding and Orbital Overlap
354(1)
9.5 Hybrid Orbitals
355(6)
sp Hybrid Orbitals
355(2)
sp2 and sp3 Hybrid Orbitals
357(2)
Hypervalent Molecules
359(1)
Hybrid Orbital Summary
359(2)
9.6 Multiple Bonds
361(7)
Resonance Structures, Delocalization, and pi Bonding
365(2)
General Conclusions about sigma and pi Bonding
367(1)
9.7 Molecular Orbitals
368(3)
Molecular Orbitals of the Hydrogen Molecule
368(2)
Bond Order
370(1)
9.8 Bonding in Period 2 Diatomic Molecules
371(11)
Molecular Orbitals for Li2 and Be2
372(1)
Molecular Orbitals from 2p Atomic Orbitals
373(3)
Electron Configurations for B2 through Ne2
376(1)
Electron Configurations and Molecular Properties
377(3)
Heteronuclear Diatomic Molecules
380(2)
Chapter Summary and Key Terms
382(1)
Learning Outcomes
383(1)
Key Equations
384(1)
Exercises
384(5)
Additional Exercises
389(3)
Integrative Exercises
392(1)
Design an Experiment
393(1)
10 Gases 394(40)
10.1 Characteristics of Gases
396(1)
10.2 Pressure
397(3)
Atmospheric Pressure and the Barometer
397(3)
10.3 The Gas Laws
400(3)
The Pressure-Volume Relationship: Boyle's Law
400(1)
The Temperature-Volume Relationship: Charles's Law
401(1)
The Quantity-Volume Relationship: Avogadro's Law
402(1)
10.4 The Ideal-Gas Equation
403(4)
Relating the Ideal-Gas Equation and the Gas Laws
406(1)
10.5 Further Applications of the Ideal-Gas Equation
407(3)
Gas Densities and Molar Mass
407(2)
Volumes of Gases in Chemical Reactions
409(1)
10.6 Gas Mixtures and Partial Pressures
410(2)
Partial Pressures and Mole Fractions
411(1)
10.7 The Kinetic-Molecular Theory of Gases
412(3)
Distributions of Molecular Speed
413(1)
Application of Kinetic-Molecular Theory to the Gas Laws
414(1)
10.8 Molecular Effusion and Diffusion
415(4)
Graham's Law of Effusion
416(1)
Diffusion and Mean Free Path
417(2)
10.9 Real Gases: Deviations from Ideal Behavior
419(4)
The van der Waals Equation
421(2)
Chapter Summary and Key Terms
423(1)
Learning Outcomes
424(1)
Key Equations
424(1)
Exercises
424(6)
Additional Exercises
430(2)
Integrative Exercises
432(1)
Design an Experiment
433(1)
11 Liquids and Intermolecular Forces 434(38)
11.1 A Molecular Comparison of Gases, Liquids, and Solids
436(2)
11.2 Intermolecular Forces
438(7)
Dispersion Forces
439(1)
Dipole-Dipole Interactions
440(1)
Hydrogen Bonding
441(3)
lon-Dipole Forces
444(1)
Comparing Intermolecular Forces
444(1)
11.3 Select Properties of Liquids
445(4)
Viscosity
446(1)
Surface Tension
447(1)
Capillary Action
448(1)
11.4 Phase Changes
449(4)
Energy Changes Accompany Phase Changes
449(1)
Heating Curves
450(1)
Critical Temperature and Pressure
451(2)
11.5 Vapor Pressure
453(3)
Volatility, Vapor Pressure, and Temperature
454(1)
Vapor Pressure and Boiling Point
455(1)
11.6 Phase Diagrams
456(3)
The Phase Diagrams of H2O and CO2
457(2)
11.7 Liquid Crystals
459(3)
Types of Liquid Crystals
459(3)
Chapter Summary and Key Terms
462(1)
Learning Outcomes
463(1)
Exercises
463(5)
Additional Exercises
468(2)
Integrative Exercises
470(1)
Design an Experiment
471(1)
12 Solids and Modern Materials 472(52)
12.1 Classification of Solids
474(1)
12.2 Structures of Solids
475(3)
Crystalline and Amorphous Solids
475(1)
Unit Cells and Crystal Lattices
475(2)
Filling the Unit Cell
477(1)
12.3 Metallic Solids
478(8)
The Structures of Metallic Solids
479(1)
Close Packing
480(3)
Alloys
483(3)
12.4 Metallic Bonding
486(3)
Electron-Sea Model
486(1)
Molecular Orbital Model
487(2)
12.5 Ionic Solids
489(5)
Structures of Ionic Solids
490(4)
12.6 Molecular Solids
494(1)
12.7 Covalent-Network Solids
494(6)
Semiconductors
495(2)
Semiconductor Doping
497(3)
12.8 Polymers
500(6)
Making Polymers
501(3)
Structure and Physical Properties of Polymers
504(2)
12.9 Nanomaterials
506(6)
Semiconductors on the Nanoscale
506(1)
Metals on the Nanoscale
507(2)
Carbon on the Nanoscale
509(3)
Chapter Summary and Key Terms
512(1)
Learning Outcomes
513(1)
Key Equations
513(1)
Exercises
514(7)
Additional Exercises
521(1)
Integrative Exercises
522(1)
Design an Experiment
523(1)
13 Properties of Solutions 524(44)
13.1 The Solution Process
526(4)
The Natural Tendency toward Mixing
526(1)
The Effect of Intermolecular Forces on Solution Formation
527(1)
Energetics of Solution Formation
528(2)
Solution Formation and Chemical Reactions
530(1)
13.2 Saturated Solutions and Solubility
530(2)
13.3 Factors Affecting Solubility
532(6)
Solute-Solvent Interactions
532(2)
Pressure Effects
534(3)
Temperature Effects
537(1)
13.4 Expressing Solution Concentration
538(4)
Mass Percentage, ppm, and ppb
538(1)
Mole Fraction, Molarity, and Molality
539(1)
Converting Concentration Units
540(2)
13.5 Colligative Properties
542(10)
Vapor-Pressure Lowering
542(2)
Boiling-Point Elevation
544(1)
Freezing-Point Depression
545(2)
Osmosis
547(3)
Determination of Molar Mass from Colligative Properties
550(2)
13.6 Colloids
552(4)
Hydrophilic and Hydrophobic Colloids
553(2)
Colloidal Motion in Liquids
555(1)
Chapter Summary and Key Terms
556(1)
Learning Outcomes
557(1)
Key Equations
558(1)
Exercises
558(6)
Additional Exercises
564(1)
Integrative Exercises
565(2)
Design an Experiment
567(1)
14 Chemical Kinetics 568(54)
14.1 Factors That Affect Reaction Rates
570(1)
14.2 Reaction Rates
571(4)
Change of Rate with Time
572(1)
Instantaneous Rate
573(1)
Reaction Rates and Stoichiometry
574(1)
14.3 Concentration and Rate Laws
575(6)
Reaction Orders: The Exponents in the Rate Law
577(2)
Magnitudes and Units of Rate Constants
579(1)
Using Initial Rates to Determine Rate Laws
580(1)
14.4 The Change of Concentration with Time
581(6)
First-Order Reactions
581(2)
Second-Order Reactions
583(2)
Zero-Order Reactions
585(1)
Half-Life
585(2)
14.5 Temperature and Rate
587(6)
The Collision Model
587(1)
The Orientation Factor
588(1)
Activation Energy
588(2)
The Arrhenius Equation
590(1)
Determining the Activation Energy
591(2)
14.6 Reaction Mechanisms
593(7)
Elementary Reactions
593(1)
Multistep Mechanisms
593(2)
Rate Laws for Elementary Reactions
595(1)
The Rate-Determining Step for a Multistep Mechanism
596(1)
Mechanisms with a Slow Initial Step
597(1)
Mechanisms with a Fast Initial Step
598(2)
14.7 Catalysis
600(8)
Homogeneous Catalysis
600(2)
Heterogeneous Catalysis
602(1)
Enzymes
603(5)
Chapter Summary and Key Terms
608(1)
Learning Outcomes
608(1)
Key Equations
609(1)
Exercises
609(8)
Additional Exercises
617(3)
Integrative Exercises
620(1)
Design an Experiment
621(1)
15 Chemical Equilibrium 622(42)
15.1 The Concept of Equilibrium
625(2)
15.2 The Equilibrium Constant
627(5)
Evaluating KC
629(1)
Equilibrium Constants in Terms of Pressure, Kp
630(1)
Equilibrium Constants and Units
631(1)
15.3 Understanding and Working with Equilibrium Constants
632(4)
The Magnitude of Equilibrium Constants
632(1)
The Direction of the Chemical Equation and K
633(1)
Relating Chemical Equation Stoichiometry and Equilibrium Constants
634(2)
15.4 Heterogeneous Equilibria
636(2)
15.5 Calculating Equilibrium Constants
638(2)
15.6 Applications of Equilibrium Constants
640(4)
Predicting the Direction of Reaction
641(1)
Calculating Equilibrium Concentrations
642(2)
15.7 Le Chatelier's Principle
644(10)
Change in Reactant or Product Concentration
646(1)
Effects of Volume and Pressure Changes
647(2)
Effect of Temperature Changes
649(2)
The Effect of Catalysts
651(3)
Chapter Summary and Key Terms
654(1)
Learning Outcomes
655(1)
Key Equations
655(1)
Exercises
656(5)
Additional Exercises
661(1)
Integrative Exercises
662(1)
Design an Experiment
663(1)
16 Acid-Base Equilibria 664(52)
16.1 Arrhenius Acids and Bases
666(1)
16.2 Bronsted-Lowry Acids and Bases
667(5)
The H+ Ion in Water
667(1)
Proton-Transfer Reactions
667(1)
Conjugate Acid-Base Pairs
668(2)
Relative Strengths of Acids and Bases
670(2)
16.3 The Autoionization of Water
672(2)
The Ion Product of Water
672(2)
16.4 The pH Scale
674(4)
pOH and Other "p" Scales
676(1)
Measuring pH
677(1)
16.5 Strong Acids and Bases
678(2)
Strong Acids
678(1)
Strong Bases
679(1)
16.6 Weak Acids
680(10)
Calculating Ka from pH
681(1)
Percent Ionization
682(1)
Using Ka to Calculate pH
683(4)
Polyprotic Acids
687(3)
16.7 Weak Bases
690(3)
Types of Weak Bases
690(3)
16.8 Relationship between Ka and Kb
693(3)
16.9 Acid-Base Properties of Salt Solutions
696(3)
An Anion's Ability to React with Water
696(1)
A Cation's Ability to React with Water
696(1)
Combined Effect of Cation and Anion in Solution
697(2)
16.10 Acid-Base Behavior and Chemical Structure
699(5)
Factors That Affect Acid Strength
699(1)
Binary Acids
700(1)
Oxyacids
701(2)
Carboxylic Acids
703(1)
16.11 Lewis Acids and Bases
704(3)
Chapter Summary and Key Terms
707(1)
Learning Outcomes
707(1)
Key Equations
708(1)
Exercises
708(5)
Additional Exercises
713(2)
Integrative Exercises
715(1)
Design an Experiment
715(1)
17 Additional Aspects of Aqueous Equilibria 716(50)
17.1 The Common-Ion Effect
718(3)
17.2 Buffers
721(8)
Composition and Action of Buffers
721(2)
Calculating the pH of a Buffer
723(3)
Buffer Capacity and pH Range
726(1)
Addition of Strong Acids or Bases to Buffers
726(3)
17.3 Acid-Base Titrations
729(10)
Strong Acid-Strong Base Titrations
730(2)
Weak Acid-Strong Base Titrations
732(4)
Titrating with an Acid-Base Indicator
736(2)
Titrations of Polyprotic Acids
738(1)
17.4 Solubility Equilibria
739(4)
The Solubility-Product Constant, Ksp
740(1)
Solubility and Ksp
741(2)
17.5 Factors That Affect Solubility
743(8)
The Common-lon Effect
743(1)
Solubility and pH
744(2)
Formation of Complex Ions
746(3)
Amphoterism
749(2)
17.6 Precipitation and Separation of Ions
751(2)
Selective Precipitation of Ions
752(1)
17.7 Qualitative Analysis for Metallic Elements
753(3)
Chapter Summary and Key Terms
756(1)
Learning Outcomes
757(1)
Key Equations
757(1)
Exercises
758(5)
Additional Exercises
763(1)
Integrative Exercises
764(1)
Design an Experiment
765(1)
18 Chemistry of the Environment 766(42)
18.1 Earth's Atmosphere
768(6)
Composition of the Atmosphere
769(1)
Photochemical Reactions in the Atmosphere
770(3)
Ozone in the Stratosphere
773(1)
18.2 Human Activities and Earth's Atmosphere
774(10)
The Ozone Layer and Its Depletion
774(2)
Sulfur Compounds and Acid Rain
776(3)
Nitrogen Oxides and Photochemical Smog
779(1)
Greenhouse Gases: Water Vapor, Carbon Dioxide, and Climate
780(4)
18.3 Earth's Water
784(3)
The Global Water Cycle
784(1)
Salt Water: Earth's Oceans and Seas
785(1)
Freshwater and Groundwater
786(1)
18.4 Human Activities and Water Quality
787(5)
Dissolved Oxygen and Water Quality
788(1)
Water Purification: Desalination
788(1)
Water Purification: Municipal Treatment
789(3)
18.5 Green Chemistry
792(5)
Supercritical Solvents
794(1)
Greener Reagents and Processes
794(3)
Chapter Summary and Key Terms
797(1)
Learning Outcomes
797(1)
Exercises
798(5)
Additional Exercises
803(1)
Integrative Exercises
804(1)
Design an Experiment
805(3)
19 Chemical Thermodynamics 808(40)
19.1 Spontaneous Processes
808(4)
Seeking a Criterion for Spontaneity
809(1)
Reversible and Irreversible Processes
810(2)
19.2 Entropy and the Second Law of Thermodynamics
812(3)
The Relationship between Entropy and Heat
812(1)
AS for Phase Changes
813(1)
The Second Law of Thermodynamics
814(1)
19.3 The Molecular Interpretation of Entropy and the Third Law of Thermodynamics
815(7)
Expansion of a Gas at the Molecular Level
815(1)
Boltzmann's Equation and Microstates
816(2)
Molecular Motions and Energy
818(1)
Making Qualitative Predictions about AS
819(2)
The Third Law of Thermodynamics
821(1)
19.4 Entropy Changes in Chemical Reactions
822(3)
Temperature Variation of Entropy
822(1)
Standard Molar Entropies
823(1)
Calculating the Standard Entropy Change for a Reaction
824(1)
Entropy Changes in the Surroundings
824(1)
19.5 Gibbs Free Energy
825(5)
Standard Free Energy of Formation
828(2)
19.6 Free Energy and Temperature
830(2)
19.7 Free Energy and the Equilibrium Constant
832(4)
Free Energy under Nonstandard Conditions
832(2)
Relationship between DeltaG° and K
834(2)
Chapter Summary and Key Terms
836(1)
Learning Outcomes
837(1)
Key Equations
837(1)
Exercises
838(6)
Additional Exercises
844(2)
Integrative Exercises
846(1)
Design an Experiment
847(1)
20 Electrochemistry 848(52)
20.1 Oxidation States and Oxidation-Reduction Reactions
850(2)
20.2 Balancing Redox Equations
852(5)
Half-Reactions
852(1)
Balancing Equations by the Method of Half-Reactions
852(3)
Balancing Equations for Reactions Occurring in Basic Solution
855(2)
20.3 Voltaic Cells
857(3)
20.4 Cell Potentials under Standard Conditions
860(8)
Standard Reduction Potentials
861(5)
Strengths of Oxidizing and Reducing Agents
866(2)
20.5 Free Energy and Redox Reactions
868(3)
Emf, Free Energy, and the Equilibrium Constant
869(2)
20.6 Cell Potentials under Nonstandard Conditions
871(6)
The Nernst Equation
872(2)
Concentration Cells
874(3)
20.7 Batteries and Fuel Cells
877(5)
Lead-Acid Battery
878(1)
Alkaline Battery
878(1)
Nickel-Cadmium and Nickel-Metal Hydride Batteries
878(1)
Lithium-lon Batteries
879(1)
Hydrogen Fuel Cells
879(3)
20.8 Corrosion
882(2)
Corrosion of Iron (Rusting)
882(1)
Preventing Corrosion of Iron
883(1)
20.9 Electrolysis
884(5)
Quantitative Aspects of Electrolysis
886(3)
Chapter Summary and Key Terms
889(1)
Learning Outcomes
890(1)
Key Equations
890(1)
Exercises
890(7)
Additional Exercises
897(1)
Integrative Exercises
898(1)
Design an Experiment
899(1)
21 Nuclear Chemistry 900(42)
21.1 Radioactivity and Nuclear Equations
902(3)
Nuclear Equations
902(1)
Types of Radioactive Decay
903(2)
21.2 Patterns of Nuclear Stability
905(4)
Neutron-to-Proton Ratio
905(2)
Radioactive Decay Chains
907(1)
Further Observations
908(1)
21.3 Nuclear Transmutations
909(3)
Accelerating Charged Particles
910(1)
Reactions Involving Neutrons
911(1)
Transuranium Elements
911(1)
21.4 Rates of Radioactive Decay
912(5)
Radiometric Dating
913(2)
Calculations Based on Half-Life
915(2)
21.5 Detection of Radioactivity
917(2)
Radiotracers
917(2)
21.6 Energy Changes in Nuclear Reactions
919(3)
Nuclear Binding Energies
921(1)
21.7 Nuclear Power: Fission
922(6)
Nuclear Reactors
925(2)
Nuclear Waste
927(1)
21.8 Nuclear Power: Fusion
928(2)
21.9 Radiation in the Environment and Living Systems
930(3)
Radiation Doses
931(2)
Chapter Summary and Key Terms
933(1)
Learning Outcomes
934(1)
Key Equations
935(1)
Exercises
935(4)
Additional Exercises
939(1)
Integrative Exercises
940(1)
Design an Experiment
941(1)
22 Chemistry of the Nonmetals 942(44)
22.1 Periodic Trends and Chemical Reactions
944(2)
Chemical Reactions
945(1)
22.2 Hydrogen
946(4)
Isotopes of Hydrogen
946(1)
Properties of Hydrogen
947(1)
Production of Hydrogen
948(1)
Uses of Hydrogen
949(1)
Binary Hydrogen Compounds
949(1)
22.3 Group 8A: The Noble Gases
950(2)
Noble-Gas Compounds
951(1)
22.4 Group 7A: The Halogens
952(3)
Properties and Production of the Halogens
952(2)
Uses of the Halogens
954(1)
The Hydrogen Halides
954(1)
Interhalogen Compounds
954(1)
Oxyacids and Oxyanions
954(1)
22.5 Oxygen
955(3)
Properties of Oxygen
955(1)
Production of Oxygen
956(1)
Uses of Oxygen
956(1)
Ozone
956(1)
Oxides
956(2)
Peroxides and Superoxides
958(1)
22.6 The Other Group 6A Elements: S, Se, Te, and Po
958(4)
Occurrence and Production of S, Se, and Te
959(1)
Properties and Uses of Sulfur, Selenium, and Tellurium
959(1)
Sulfides
959(1)
Oxides, Oxyacids, and Oxyanions of Sulfur
960(2)
22.7 Nitrogen
962(3)
Properties of Nitrogen
962(1)
Production and Uses of Nitrogen
962(1)
Hydrogen Compounds of Nitrogen
962(1)
Oxides and Oxyacids of Nitrogen
963(2)
22.8 The Other Group 5A Elements: P, As, Sb, and Bi
965(4)
Occurrence, Isolation, and Properties of Phosphorus
966(1)
Phosphorus Halides
966(1)
Oxy Compounds of Phosphorus
967(2)
22.9 Carbon
969(3)
Elemental Forms of Carbon
969(1)
Oxides of Carbon
970(1)
Carbonic Acid and Carbonates
971(1)
Carbides
972(1)
22.10 The Other Group 4A Elements: Si, Ge, Sn, and Pb
972(4)
General Characteristics of the Group 4A Elements
972(1)
Occurrence and Preparation of Silicon
973(1)
Silicates
973(2)
Glass
975(1)
Silicones
976(1)
22.11 Boron
976(2)
Chapter Summary and Key Terms
978(1)
Learning Outcomes
979(1)
Exercises
979(4)
Additional Exercises
983(1)
Integrative Exercises
984(1)
Design an Experiment
985(1)
23 Transition Metals and Coordination Chemistry 986(44)
23.1 The Transition Metals
988(4)
Physical Properties
989(1)
Electron Configurations and Oxidation States
990(1)
Magnetism
991(1)
23.2 Transition-Metal Complexes
992(5)
The Development of Coordination Chemistry: Werner's Theory
993(2)
The Metal-Ligand Bond
995(1)
Charges, Coordination Numbers, and Geometries
996(1)
23.3 Common Ligands in Coordination Chemistry
997(6)
Metals and Chelates in Living Systems
999(4)
23.4 Nomenclature and Isomerism in Coordination Chemistry
1003(6)
Isomerism
1005(1)
Structural Isomerism
1005(1)
Stereoisomerism
1006(3)
23.5 Color and Magnetism in Coordination Chemistry
1009(2)
Color
1009(2)
Magnetism of Coordination Compounds
1011(1)
23.6 Crystal-Field Theory
1011(10)
Electron Configurations in Octahedral Complexes
1015(2)
Tetrahedral and Square-Planar Complexes
1017(4)
Chapter Summary and Key Terms
1021(1)
Learning Outcomes
1021(1)
Exercises
1022(4)
Additional Exercises
1026(2)
Integrative Exercises
1028(1)
Design an Experiment
1029(1)
24 The Chemistry of Life: Organic and Biological Chemistry 1030(50)
24.1 General Characteristics of Organic Molecules
1032(2)
The Structures of Organic Molecules
1032(1)
The Stability of Organic Compounds
1033(1)
Solubility and Acid-Base Properties of Organic Compounds
1033(1)
24.2 Introduction to Hydrocarbons
1034(7)
Structures of Alkanes
1035(1)
Structural Isomers
1035(1)
Nomenclature of Alkanes
1036(3)
Cycloalkanes
1039(1)
Reactions of Alkanes
1039(2)
24.3 Alkenes, Alkynes, and Aromatic Hydrocarbons
1041(7)
Alkenes
1041(2)
Alkynes
1043(1)
Addition Reactions of Alkenes and Alkynes
1044(1)
Aromatic Hydrocarbons
1045(1)
Stabilization of 7T Electrons by Delocalization
1046(1)
Substitution Reactions of Aromatic Hydrocarbons
1046(2)
24.4 Organic Functional Groups
1048(7)
Alcohols
1048(2)
Ethers
1050(1)
Aldehydes and Ketones
1050(1)
Carboxylic Acids and Esters
1051(3)
Amines and Amides
1054(1)
24.5 Chirality in Organic Chemistry
1055(2)
24.6 Introduction to Biochemistry
1057(1)
24.7 Proteins
1057(5)
Amino Acids
1057(2)
Polypeptides and Proteins
1059(1)
Protein Structure
1060(2)
24.8 Carbohydrates
1062(3)
Disaccharides
1063(1)
Polysaccharides
1064(1)
24.9 Lipids
1065(2)
Fats
1065(1)
Phospholipids
1066(1)
24.10 Nucleic Acids
1067(4)
Chapter Summary and Key Terms
1071(1)
Learning Outcomes
1072(1)
Exercises
1072(5)
Additional Exercises
1077(1)
Integrative Exercises
1078(1)
Design an Experiment
1079(1)
Appendices
A Mathematical Operations
1080(7)
B Properties of Water
1087(1)
C Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C)
1088(4)
D Aqueous Equilibrium Constants
1092(2)
E Standard Reduction Potentials at 25 °C
1094
About our authors

THEODORE L. BROWN received his Ph.D. from Michigan State University in 1956. Since then, he has been a member of the faculty of the University of Illinois, Urbana-Champaign, where he is now Professor of Chemistry, Emeritus. He served as Vice Chancellor for Research, and Dean of The Graduate College, from 1980 to 1986, and as Founding Director of the Arnold and Mabel Beckman Institute for Advanced Science and Technology from 1987 to 1993. Professor Brown has been an Alfred P. Sloan Foundation Research Fellow and has been awarded a Guggenheim Fellowship. In 1972 he was awarded the American Chemical Society Award for Research in Inorganic Chemistry and received the American Chemical Society Award for Distinguished Service in the Advancement of Inorganic Chemistry in 1993. He has been elected a Fellow of the American Association for the Advancement of Science, the American Academy of Arts and Sciences, and the American Chemical Society.

EUGENE LEMAY, JR., received his B.S. degree in Chemistry from Pacific Lutheran University (Washington) and his Ph.D. in Chemistry in 1966 from the University of Illinois, Urbana-Champaign. He then joined the faculty of the University of Nevada, Reno, where he is currently Professor of Chemistry, Emeritus. He has enjoyed Visiting Professorships at the University of North Carolina at Chapel Hill, at the University College of Wales in Great Britain, and at the University of California, Los Angeles. Professor LeMay is a popular and effective teacher, who has taught thousands of students during more than 40 years of university teaching. Known for the clarity of his lectures and his sense of humor, he has received several teaching awards, including the University Distinguished Teacher of the Year Award (1991) and the first Regents' Teaching Award given by the State of Nevada Board of Regents (1997).

BRUCE E. BURSTEN received his Ph.D. in Chemistry from the University of Wisconsin in 1978. After two years as a National Science Foundation Postdoctoral Fellow at Texas A&M University, he joined the faculty of The Ohio State University, where he rose to the rank of Distinguished University Professor. In 2005, he moved to the University of Tennessee, Knoxville, as Distinguished Professor of Chemistry and Dean of the College of Arts and Sciences. Professor Bursten has been a Camille and Henry Dreyfus Foundation Teacher-Scholar and an Alfred P. Sloan Foundation Research Fellow, and he is a Fellow of both the American Association for the Advancement of Science and the American Chemical Society. At Ohio State he has received the University Distinguished Teaching Award in 1982 and 1996, the Arts and Sciences Student Council Outstanding Teaching Award in 1984, and the University Distinguished Scholar Award in 1990. He received the Spiers Memorial Prize and Medal of the Royal Society of Chemistry in 2003, and the Morley Medal of the Cleveland Section of the American Chemical Society in 2005. He was President of the American Chemical Society for 2008. In addition to his teaching and service activities, Professor Bursten's research program focuses on compounds of the transition-metal and actinide elements.

CATHERINE J. MURPHY received two B.S. degrees, one in Chemistry and one in Biochemistry, from the University of Illinois, Urbana-Champaign, in 1986. She received her Ph.D. in Chemistry from the University of Wisconsin in 1990. She was a National Science Foundation and National Institutes of Health Postdoctoral Fellow at the California Institute of Technology from 1990 to 1993. In 1993, she joined the faculty of the University of South Carolina, Columbia, becoming the Guy F. Lipscomb Professor of Chemistry in 2003. In 2009 she moved to the University of Illinois, Urbana-Champaign, as the Peter C. and Gretchen Miller Markunas Professor of Chemistry. Professor Murphy has been honored for both research and teaching as a Camille Dreyfus Teacher-Scholar, an Alfred P. Sloan Foundation Research Fellow, a Cottrell Scholar of the Research Corporation, a National Science Foundation CAREER Award winner, and a subsequent NSF Award for Special Creativity. She has also received a USC Mortar Board Excellence in Teaching Award, the USC Golden Key Faculty Award for Creative Integration of Research and Undergraduate Teaching, the USC Michael J. Mungo Undergraduate Teaching Award, and the USC Outstanding Undergraduate Research Mentor Award. Since 2006, Professor Murphy has served as a Senior Editor for the Journal of Physical Chemistry. In 2008 she was elected a Fellow of the American Association for the Advancement of Science. Professor Murphy's research program focuses on the synthesis and optical properties of inorganic nanomaterials, and on the local structure and dynamics of the DNA double helix.

PATRICK M. WOODWARD received B.S. degrees in both Chemistry and Engineering from Idaho State University in 1991. He received a M.S. degree in Materials Science and a Ph.D. in Chemistry from Oregon State University in 1996. He spent two years as a postdoctoral researcher in the Department of Physics at Brookhaven National Laboratory. In 1998, he joined the faculty of the Chemistry Department at The Ohio State University where he currently holds the rank of Professor. He has enjoyed visiting professorships at the University of Bordeaux in France and the University of Sydney in Australia. Professor Woodward has been an Alfred P. Sloan Foundation Research Fellow and a National Science Foundation CAREER Award winner. He currently serves as an Associate Editor to the Journal of Solid State Chemistry and as the director of the Ohio REEL program, an NSF-funded center that works to bring authentic research experiments into the laboratories of first- and second-year chemistry classes in 15 colleges and universities across the state of Ohio. Professor Woodward's research program focuses on understanding the links between bonding, structure, and properties of solid-state inorganic functional materials.

MATTHEW W. STOLTZFUS received his B.S. degree in Chemistry from Millersville University in 2002 and his Ph. D. in Chemistry in 2007 from The Ohio State University. He spent two years as a teaching postdoctoral assistant for the Ohio REEL program, an NSF-funded center that works to bring authentic research experiments into the general chemistry lab curriculum in 15 colleges and universities across the state of Ohio. In 2009, he joined the faculty of Ohio State where he currently holds the position of Chemistry Lecturer. In addition to lecturing general chemistry, Stoltzfus accepted the Faculty Fellow position for the Digital First Initiative, inspiring instructors to offer engaging digital learning content to students through emerging technology. Through this initiative, he developed an iTunes U general chemistry course, which has attracted over 120,000 students from all over the world. Stoltzfus has received several teaching awards, including the inaugural Ohio State University 2013 Provost's Award for Distinguished Teaching by a Lecturer and he is recognized as an Apple Distinguished Educator.