CHFJMRAT .PRTNCTPTJFI SThe Quest for Insight

FOURTH EDITIO N

PETER ATKIN S

LORETTA JONES

Fundamentals

F1Introduction and Orientation, Matter and Energy, Elements and Atoms ,

Compounds, The Nomenclature of Compounds, Moles and Molar Masses ,

Determination of Chemical Formulas, Mixtures and Solutions, Chemica l

Equations, Aqueous Solutions and Precipitation, Acids and Bases, Redo x

Reactions, Reaction Stoichiometry, Limiting Reactants

1 ATOMS: THE QUANTUM WORLD

1

2 CHEMICAL BONDS

5 7

MAJOR TECHNIQUE 1 : INFRARED SPECTROSCOPY

92

3 MOLECULAR SHAPE AND STRUCTURE

95

MAJOR TECHNIQUE 2 : ULTRAVIOLET AND VISIBLE SPECTROSCOPY

136

4 THE PROPERTIES OF GASES

13 9

5 LIQUIDS AND SOLIDS

177

MAJOR TECHNIQUE 3 : X-RAY DIFFRACTION

21 2

6 THERMODYNAMICS : THE FIRST LAW

21 57 THERMODYNAMICS : THE SECOND AND THIRD LAWS 26 5

8 PHYSICAL EQUILIBRIA

309

MAJOR TECHNIQUE 4 : CHROMATOGRAPHY

354

9 CHEMICAL EQUILIBRIA

35 7

10 ACIDS AND BASES

395

11 AQUEOUS EQUILIBRIA

445

12 ELECTROCHEMISTRY

48 3

13 CHEMICAL KINETICS

52 9

MAJOR TECHNIQUE 5 : COMPUTATION

580

14 THE ELEMENTS : THE FIRST FOUR MAIN GROUPS

58 1

1S THE ELEMENTS : THE LAST FOUR MAIN GROUPS

623

16 THE ELEMENTS : THE d BLOCK

657

17 NUCLEAR CHEMISTRY

699

18 ORGANIC CHEMISTRY I : THE HYDROCARBONS

729

MAJOR TECHNIQUE 6 : MASS SPECTROMETRY

752

19 ORGANIC CHEMISTRY II : POLYMERS ANDBIOLOGICAL COMPOUNDS

755

MAJOR TECHNIQUE 7 : NUCLEAR MAGNETIC RESONANCE

786

Preface

xv

E2 Determining Empirical Formulas

F47

FUNDAMENTALS

F.3 Determining Molecular Formulas

F49Exercises

F5 0INTRODUCTION AND ORIENTATION

Fl G MIXTURES AND SOLUTIONS

F5 2Chemistry and Society

F1

G.1 Classifying Mixtures

F5 2Chemistry: A Science at Three Levels

F2

G .2 Separation Techniques

F54How Science Is Done

F2

G.3 Molarity

F5 5The Branches of Chemistry

F4

G .4 Dilution

F5 8Mastering Chemistry

F5TOOLBOX G.1 HOW TO CALCULATE THE VOLUME OF

A MATTER AND ENERGY

F5

STOCK SOLUTION REQUIRED FOR A GIVE N

A .1 Physical Properties

F6

DILUTION

F5 8

A .2 Force

F10

Exercises

F5 9A.3 Energy

F11

H CHEMICAL EQUATIONS

F61Exercises

F14

H.1 Symbolizing Chemical Reactions

F61B ELEMENTS AND ATOMS

F15

H.2 Balancing Chemical Equations

F6 2B.1 Atoms

F16

Exercises

F64B.2 The Nuclear Model

F16

I AQUEOUS SOLUTIONS AN DB.3 Isotopes

F18

PRECIPITATION

F66B.4 The Organization of the Elements

F19

I .1 Electrolytes

F6 6Exercises

F22

1 .2 Precipitation Reactions

F67

C COMPOUNDS

F23

L3 Ionic and Net Ionic Equations

F6 8

C.1 What Are Compounds?

F23

1 .4 Putting Precipitation to Work

F6 9

C.2 Molecules and Molecular Compounds

F24

Exercises

F70

C.3 Ions and Ionic Compounds

F25

J ACIDS AND BASES

F72

Exercises

F29

J .1 Acids and Bases in Aqueous Solution

F72

D THE NOMENCLATURE OF

J .2 Strong and Weak Acids and Bases

F74

COMPOUNDS

F30

J.3 Neutralization

F75

D.1 Names of Cations

F30

Exercises

F76

D.2 Names of Anions

F30

K REDOX REACTIONS

F77

D.3 Names of Ionic Compounds

F32

K.1 Oxidation and Reduction

F77

TOOLBOX D.1 HOW TO NAME IONIC COMPOUNDS

F32

K.2 Oxidation Numbers : Keeping Track

D.4 Names of Inorganic Molecular Compounds F33

of Electrons

F79

TOOLBOX D.2 HOW TO NAME SIMPLE INORGANIC

TOOLBOX K .1 HOW TO ASSIGN OXIDATION NUMBERS F80

MOLECULAR COMPOUNDS

F34

K.3 Oxidizing and Reducing Agents

F8 1

D.5 Names of Some Common Organic

K .4 Balancing Simple Redox Equations

F82

Compounds

F35

Exercises

F83

Exercises

F37

L REACTION STOICHIOMETRY

F8 5

E MOLES AND MOLAR MASSES

F38

L .1 Mole-to-Mole Predictions

F85

E.1 The Mole

F38

L .2 Mass-to-Mass Predictions

F86

E.2 Molar Mass

F40

TOOLBOX L.1 HOW TO CARRY OUT MASS-TO-MASS

Exercises

F44

CALCULATIONS

F86

F DETERMINATION OF CHEMICAL

L.3 Volumetric Analysis

F8 8

FORMULAS

F46

TOOLBOX L.2 HOW TO INTERPRET A TITRATION

F89

El Mass Percentage Composition

F46

Exercises

F91

M LIMITING REACTANTS

F93

Chapter 2 CHEMICAL BONDSM.1 Reaction Yield

F93M.2 The Limits of Reaction

F94

IONIC BONDS

5 7TOOLBOX M .1 HOW TO IDENTIFY THE LIMITING

2 .1 The Ions That Elements Form

5 8REACTANT

F95

2 .2 Lewis Symbols

60M.3 Combustion Analysis

F97

2 .3 The Energetics of Ionic Bond Formation

6 0Exercises

F100

2 .4 Interactions Between Ions

6 1COVALENT BONDS

64

Chapter 1 ATOMS: THE

2 .5 Lewis Structures

6 5

QUANTUM WORLD

2 .6 Lewis Structures for Polyatomic Species

66ig„

TOOLBOX 2 .1 HOW TO WRITE THE LEWIS STRUCTUR E

INVESTIGATING ATOMS

1

OF A POLYATOMIC SPECIES

6 7

1 .1 The Nuclear Atom

2

2 .7 Resonance

6 9

1 .2 The Characteristics of Electromagnetic

2 .8 Formal Charge

71

Radiation

4

TOOLBOX 2 .2 HOW TO USE FORMAL CHARGE TO

1 .3 Atomic Spectra

6

DETERMINE THE MOST LIKELY LEWI S

QUANTUM THEORY

8

STRUCTURE

72

1 .4 Radiation, Quanta, and Photons

8

EXCEPTIONS TO THE OCTET RULE

73

1 .5 The Wave-Particle Duality of Matter

13

2 .9 Radicals and Biradicals

73

1 .6 The Uncertainty Principle

15

What Has This to Do with (Box 2 .1) . . .

1 .7 Wavefunctions and Energy Levels

16

Staying Alive? Chemical Self-Preservation

74

THE HYDROGEN ATOM

21

2 .10 Expanded Valence Shells

74

1 .8 The Principal Quantum Number

21

2 .11 The Unusual Structures of Some

1 .9 Atomic Orbitals

22

Group 13/III Compounds

77

1 .10 Electron Spin

29

IONIC VERSUS COVALENT BONDS

77

1 .11 The Electronic Structure of Hydrogen

30

2 .12 Correcting the Covalent Model :

How Do We Know (Box 1 .1) . . .

Electronegativity

77

That an Electron Has Spin?

31

2 .13 Correcting the Ionic Model : Polarizability 7 9

MANY ELECTRON ATOMS

3 1 THE STRENGTHS AND LENGTHS O F

1 .12 Orbital Energies

32

COVALENT BONDS

80

1 .13 The Building-Up Principle

33

2 .14 Bond Strengths

80

TOOLBOX 1 .1 HOW TO PREDICT THE GROUND-STATE

2.15 Variation in Bond Strength

8 1ELECTRON CONFIGURATION OF AN ATOM

37

2 .16 Bond Lengths

83

1 .14 Electronic Structure and the

How Do We Know (Box 2 .2) . . . the Length

Periodic Table

38

of a Chemical Bond?

84

The Development of the Periodic Table

Exercises

85

(Box 1 .2)

38

MAJOR TECHNIQUE 1 : INFRARED SPECTROSCOPY

92THE PERIODICITY OF ATOMI C

PROPERTIES

391 .15 Atomic Radius

401 .16 Ionic Radius

41

Chapter 3 MOLECULAR1 .17 Ionization Energy

43

SHAPE AND STRUCTURE1 .18 Electron Affinity

451 .19 The Inert-Pair Effect

46

THE VSEPR MODEL

951 .20 Diagonal Relationships

47

Frontiers of Chemistry (Box 3 .1) :THE IMPACT ON MATERIALS

47

Drugs by Design and Discovery

961 .21 The Main-Group Elements

47

3 .1 The Basic VSEPR Model

961 .22 The Transition Metals

48

3 .2 Molecules with Lone Pairs on th eExercises

50

Central Atom

99

TOOLBOX 3 .1 HOW TO USE THE VSEPR MODEL

102

4.11 The Maxwell Distribution of Speeds

1643.3 Polar Molecules

103

How Do We Know (Box 4 .1) . . . theVALENCE-BOND THEORY

106

Distribution of Molecular Speeds?

1653 .4 Sigma and Pi Bonds

107

THE IMPACT ON MATERIALS :3.5 Electron Promotion and the Hybridization

REAL GASES

165of Orbitals

108

4 .12 Deviations from Ideality

1653 .6 Other Common Types of Hybridization

110

4 .13 The Liquefaction of Gases

1663 .7 Characteristics of Multiple Bonds

112

4 .14 Equations of State of Real Gases

16 7MOLECULAR ORBITAL THEORY

115

Exercises

1703 .8 The Limitations of Lewis's Theory

11 5How Do We Know (Box 3 .2) . . .

That Electrons Are Not Paired?

116

Chapter S LIQUIDS AND SOLID S3 .9 Molecular Orbitals

11 73 .10 The Electron Configurations of

INTERMOLECULAR FORCES

177

Diatomic Molecules

118

5 .1 The Formation of Condensed Phases

17 8

How Do W e Know (Box 3 .3) . . . the

5 .2 Ion-Dipole Forces

178

Energies of Molecular Orbitals?

120

5 .3 Dipole-Dipole Forces

179

TOOLBOX 3.2 HOW TO DETERMINE THE ELECTRON

5 .4 London Forces

18 1

CONFIGURATION AND BOND ORDER OF A

5 .5 Hydrogen Bonding

184HOMONUCLEAR DIATOMIC SPECIES

121

LIQUID STRUCTURE

185

3 .11 Bonding in Heteronuclear

5 .6 Order in Liquids

18 6

Diatomic Molecules

122

5 .7 Viscosity and Surface Tension

18 6

3.12 Orbitals in Polyatomic Molecules

124

SOLID STRUCTURES

188

IMPACT ON MATERIALS : ELECTRONIC

5 .8 Classification of Solids

18 8

CONDUCTION IN SOLIDS

126

How Do We Know (Box 5 .1) . . . What a

3.13 Bonding in the Solid State

126

Surface Looks Like?

189

3 .14 Semiconductors

128

5 .9 Molecular Solids

190

Exercises

129

5 .10 Network Solids

19 1

MAJOR TECHNIQUE 2 : ULTRAVIOLET AND VISIBLE

Frontiers of Chemistry (Box 5.2): High

SPECTROSCOPY

136

Temperature Superconductors

1925 .11 Metallic Solids

194

5 .12 Unit Cells

196

L

Chapter 4 THE PROPERTIES

5 .13 Ionic Structures

199

OF GASES

THE IMPACT ON MATERIALS

201

5 .14 The Properties of Solids

201

THE NATURE OF GASES

140

5 .15 Alloys

202

4 .1 Observing Gases

140

5 .16 Liquid Crystals

203

4.2 Pressure

140

5 .17 Ionic Liquids

20 5

4.3 Alternative Units of Pressure

143

Exercises

205

THE GAS LAWS

144

MAJOR TECHNIQUE 3 : X-RAY DIFFRACTION

212

4.4 The Experimental Observations

145

4.5 Applications of the Ideal Gas Law

148

TOOLBOX 4 .1 HOW TO USE THE IDEAL GAS LAW

148

hapter 6 THERMODYNAMICS:

4.6 Gas Density

151

;_ ''THE FIRST LAW4 .7 The Stoichiometry of Reacting Gases

153

4 .8 Mixtures of Gases

155

SYSTEMS, STATES, AND ENERGY

21 5

MOLECULAR MOTION

158

6 .1 Systems

21 6

4 .9 Diffusion and Effusion

158

6 .2 Work and Energy

21 6

4 .10 The Kinetic Model of Gases

160

6 .3 Expansion Work

217

6.4 Heat

222

7 .10 The Overall Change in Entropy

2866.5 The Measurement of Heat

222

7 .11 Equilibrium

2906 .6 The First Law

225

GIBBS FREE ENERGY

29 16.7 A Molecular Interlude : The Origin of

7 .12 Focusing on the System

29 1Internal Energy

229

7 .13 Gibbs Free Energy of Reaction

294ENTHALPY

230

7 .14 The Gibbs Free Energy an d6 .8 Heat Transfers at Constant Pressure

231

Nonexpansion Work

2976 .9 Heat Capacities at Constant Volume and

7 .15 The Effect of Temperature

299Constant Pressure

232

7.16 Impact on Biology : Gibbs Free Energy6 .10 A Molecular Interlude : The Origin of

Changes in Biological Systems

30 1the Heat Capacities of Gases

233

Exercises

3026 .11 The Enthalpy of Physical Change

2356 .12 Heating Curves

23 8How Do W e Know (Box 6 .1) . . . the

Chapter 8 PHYSICAL EQUILIBRIAShape of a Heating Curve?

23 9

THE ENTHALPY OF CHEMICAL CHANGE 240

PHASES AND PHASE TRANSITIONS

3096 .13 Reaction Enthalpies

240

8 .1 Vapor Pressure

3106 .14 The Relation Between AH and AU

241

8 .2 Volatility and Intermolecular Forces

31 16.15 Standard Reaction Enthalpies

242

8 .3 The Variation of Vapor Pressur e6 .16 Combining Reaction Enthalpies :

with Temperature

31 1Hess's Law

243

8 .4 Boiling

31 3TOOLBOX 6.1 HOW TO USE HESS'S LAW

244

8 .5 Freezing and Melting

31 56.17 The Heat Output of Reactions

245

8 .6 Phase Diagrams

31 5What Has This to Do with (Box 6 .2) . . .

8 .7 Critical Properties

31 8the Environment? Alternative Fuels

246

SOLUBILITY

31 96.18 Standard Enthalpies of Formation

248

8 .8 The Limits of Solubility

31 96.19 The Born-Haber Cycle

252

8 .9 The Like-Dissolves-Like Rule

3206.20 Bond Enthalpies

253

8 .10 Pressure and Gas Solubility :6 .21 The Variation of Reaction Enthalpy

Henry's Law

322with Temperature

255

8 .11 Temperature and Solubility

323Exercises

257

8 .12 The Enthalpy of Solution

3238.13 The Gibbs Free Energy of Solution

326COLLIGATIVE PROPERTIES

327Chapter 7 THERMODYNAMICS :

8 .14 Molality

327

THE SECOND AND THIRD LAWS

TOOLBOX 8 .1 HOW TO USE THE MOLALITY

3288.15 Vapor-Pressure Lowering

330ENTROPY

265

8 .16 Boiling-Point Elevation an d7.1 Spontaneous Change

265

Freezing-Point Depression

3327.2 Entropy and Disorder

266

8 .17 Osmosis

3347.3 Changes in Entropy

268

TOOLBOX 8 .2 HOW TO USE COLLIGATIVE PROPERTIES

7.4 Entropy Changes Accompanying Changes

TO DETERMINE MOLAR MASS

336in Physical State

273

BINARY LIQUID MIXTURES

3387.5 A Molecular Interpretation of Entropy

275

8 .18 The Vapor Pressure of a Binary7.6 The Equivalence of Statistical and

Liquid Mixture

338Thermodynamic Entropies

279

8 .19 Distillation

3407.7 Standard Molar Entropies

280

8 .20 Azeotropes

34 17.8 Standard Reaction Entropies

283

IMPACT ON BIOLOGY AND MATERIALS 34 2GLOBAL CHANGES IN ENTROPY

284

8 .21 Colloids

3427.9 The Surroundings

284

8 .22 Bio-based and Biomimetic Materials

343

Frontiers of Chemistry (Box 8 .1) : Drug Delivery 344

THE pH OF SOLUTIONS OF WEAK ACID SExercises

346

AND BASES

41 4

MAJOR TECHNIQUE 4 : CHROMATOGRAPHY

354

10 .11 Solutions of Weak Acids

41 4TOOLBOX 10.1 HOW TO CALCULATE THE pH OF A

SOLUTION OF A WEAK ACID

41 6

Chapter 9 CHEMICAL EQUILIBRIA

10.12 Solutions of Weak Bases

41 8TOOLBOX 10 .2 HOW TO CALCULATE THE pH OF A

REACTIONS AT EQUILIBRIUM

358

SOLUTION OF A WEAK BASE

41 8

9 .1 The Reversibility of Reactions

359

10.13 The pH of Salt Solutions

42 0

9.2 Equilibrium and the Law of

POLYPROTIC ACIDS AND BASES

424

Mass Action

359

10.14 The pH of a Polyprotic Acid Solution 42 4

9.3 The Thermodynamic Origin of

10.15 Solutions of Salts of Polyprotic Acids

425

Equilibrium Constants

363

10.16 The Concentrations of Solute Species

427

9 .4 The Extent of Reaction

368

TOOLBOX 10.3 HOW TO CALCULATE TH ECONCENTRATIONS OF ALL SPECIES IN A9.5 The Direction of Reaction

369

POLYPROTIC ACID SOLUTION

427EQUILIBRIUM CALCULATIONS

370

What Has This to Do with (Box 10 .1) . . .9.6 The Equilibrium Constant in Terms of

the Environment? Acid Rain and th eMolar Concentrations of Gases

371

Gene Pool

43 09 .7 Alternative Forms of the

10.17 Composition and pH

43 1Equilibrium Constant

372

AUTOPYROLYSIS AND pH

4339.8 Using Equilibrium Constants

374

10.18 Very Dilute Solutions of Stron gTOOLBOX 9 .1 HOW TO SET UP AND USE AN

Acids and Bases

433EQUILIBRIUM TABLE

374

10.19 Very Dilute Solutions of Weak Acids

435THE RESPONSE OF EQUILIBRIA TO

Exercises

437CHANGES IN CONDITIONS

3779.9 Adding and Removing Reagents

3789.10 Compressing a Reaction Mixture

381

Chapter 11 AQUEOUS EQUILIBRIA9 .11 Temperature and Equilibrium

382

9 .12 Catalysts and Haber's Achievement

385

MIXED SOLUTIONS AND BUFFERS

4459 .13 The Impact on Biology : Homeostasis

386

11 .1 Buffer Action

446Exercises

387

11 .2 Designing a Buffer

44611 .3 Buffer Capacity

45 1TITRATIONS

45 2

_Chapter 10 ACIDS AND BASES

11 .4 Strong Acid-Strong Base Titrations

45 2

What Has This to Do with (Box 11 .2) . . .THE NATURE OF ACIDS AND BASES

395

Staying Alive? Physiological Buffers

45310 .1 Bronsted-Lowry Acids and Bases

395

TOOLBOX 11 .1 HOW TO CALCULATE THE pH DURING A

10.2 Lewis Acids and Bases

398

STRONG AC1D-STRONG BASE TITRATION

454

10 .3 Acidic, Basic, and Amphoteric Oxides

399

11 .5 Strong Acid-Weak Base and Wea k

10.4 Proton Exchange Between Water

Acid-Strong Base Titrations

455

Molecules

400

TOOLBOX 11 .2 HOW TO CALCULATE THE pH DURING A

10 .5 The pH Scale

402

TITRATION OF A WEAK ACID OR A WEAK BASE

45 9

10 .6 The pOH of Solutions

405

11 .6 Acid-Base Indicators

46 1WEAK ACIDS AND BASES

406

11 .7 Stoichiometry of Polyproti c

10 .7 Acidity and Basicity Constants

406

Acid Titrations

464

10 .8 The Conjugate Seesaw

409

SOLUBILITY EQUILIBRIA

466

10 .9 Molecular Structure and Acid Strength

411

11 .8 The Solubility Product

46 6

10 .10 The Strengths of Oxoacids and

11 .9 The Common-Ion Effect

46 8Carboxylic Acids

412

11 .10 Predicting Precipitation

470

11 .11 Selective Precipitation

471

CONCENTRATION AND TIME

54011 .12 Dissolving Precipitates

473

13 .4 First-Order Integrated Rate Laws

54011 .13 Complex Ion Formation

473

13 .5 Half-Lives for First-Order Reactions

54311 .14 Qualitative Analysis

475

13 .6 Second-Order Integrated Rate Laws

545Exercises

477

REACTION MECHANISMS

54713 .7 Elementary Reactions

54713.8 The Rate Laws of Elementar y

chapter 12 ELECTROCHEMISTRY

Reactions

54913 .9 Chain Reactions

45 3REPRESENTING REDOX REACTIONS

483

13 .10 Rates and Equilibrium

55412.1 Half-Reactions

484

MODELS OF REACTIONS

55 512.2 Balancing Redox Equations

484

13 .11 The Effect of Temperature

55 6TOOLBOX 12.1 HOW TO BALANCE COMPLICATED

13 .12 Collision Theory

55 9REDOX EQUATIONS

485

How Do We Know (Box 13 .2) . . . WhatGALVANIC CELLS

490

Happens During a Molecular Collision?

56212.3 The Structure of Galvanic Cells

490

13 .13 Transition State Theory

56 312.4 Cell Potential and Reaction Gibbs

IMPACT ON MATERIALS AND BIOLOGY :Free Energy

492

ACCELERATING REACTIONS

56512.5 The Notation for Cells

494

13 .14 Catalysis

565TOOLBOX 12 .2 HOW TO WRITE A CELL REACTION

What Has This to Do with (Box 13.3) . . .FOR A CELL DIAGRAM

497

the Environment? Protecting the12.6 Standard Potentials

498

Ozone Layer

56 812.7 The Electrochemical Series

502

13 .15 Living Catalysts : Enzymes

56 912 .8 Standard Potentials and Equilibrium

Exercises

571Constants

504

MAJOR TECHNIQUE 5 : COMPUTATION

580TOOLBOX 12 .3 HOW TO CALCULATE EQUILIBRIU M

CONSTANTS FROM ELECTROCHEMICAL DATA

50512 .9 The Nernst Equation

50612 .10 Ion-Selective Electrodes

508

Chapter 14 THE ELEMENTS :ELECTROLYTIC CELLS

509

THE FIRST FOUR MAIN GROUPS12 .11 Electrolysis

51 012 .12 The Products of Electrolysis

51 l

PERIODIC TRENDS

582TOOLBOX 12 .4 HOW TO PREDICT THE RESULT

OF ELECTROLYSIS

513

14 .1 Atomic Properties

582

THE IMPACT ON MATERIALS

514

14 .2 Bonding Trends

583

12 .13 Applications of Electrolysis

514

HYDROGEN

58514.3 The Element

58512 .14 Corrosion

515

14 .4 Compounds of Hydrogen

58612 .15 Practical Cells

517

GROUP 1 : THE ALKALI METALS

58 7

Frontiers of Chemistry (Box 12 .1) : Fuel Cells 519

14.5 The Group 1 Elements

580Exercises

521 14.6 Chemical Properties of theAlkali Metals

589

IMki

13 CHEMICAL KINETICS

14.7 Compounds of Lithium, Sodium ,and Potassium

590REACTION RATES

529 GROUP 2: THE ALKALINE EART H13.1 Concentration and Reaction Rate

529

METALS

592How Do W e Know (Box 13 .1) . . . What

14.8 The Group 2 Elements

592Happens to Atoms During a Reaction?

532

14.9 Compounds of Beryllium and13.2 The Instantaneous Rate of Reaction

532

Magnesium

59413.3 Rate Laws and Reaction Order

534

14 .10 Compounds of Calcium

595

GROUP 13/III : THE BORON FAMILY

597

Chapter 16 THE ELEMENTS :14.11 The Group 13/III Elements

598

THE d BLOCK14.12 Group 13/III Oxides

60 014 .13 Nitrides and Halides

601

THE d-BLOCK ELEMENTS AND THEIR14 .14 Boranes, Borohydrides, and Borides

602

COMPOUNDS

65 7GROUP 14/IV: THE CARBON FAMILY

603

16 .1 Trends in Physical Properties

65 814.15 The Group 14/IV Elements

605

16 .2 Trends in Chemical Properties

66014.16 The Different Forms of Carbon

605

SELECTED ELEMENTS : A SURVEY

66214.17 Silicon, Germanium, Tin, and Lead

607

16 .3 Scandium Through Nickel

662Frontiers of Chemistry (Box 14 .1):

16.4 Groups 11 and 12

665Nanotubes, Nature's Smallest Pipes

608

COORDINATION COMPOUNDS

66914 .18 Oxides of Carbon

609

What Has This to Do with (Box 16 .1) . . .What Has This to Do with (Box 14 .2) . . .

Staying Alive? Why We Need t othe Environment? The Greenhouse Effect 610

Eat d -Metals

67014.19 Oxides of Silicon : The Silicates

612

16 .5 Coordination Complexes

67 114.20 Other Important Group 14/IV

TOOLBOX 16.1 HOW TO NAME d-METAL COMPLEXE SCompounds

614

AND COORDINATION COMPOUNDS

673THE IMPACT ON MATERIALS

615

16 .6 The Shapes of Complexes

67414 .21 Glasses

615

16 .7 Isomers

67514 .22 Ceramics

616

How Do We Know (Box 16 .2) . . . That aExercises

618

Complex Is Optically Active?

678THE ELECTRONIC STRUCTURE S

OF COMPLEXES

680Chapter 15 THE ELEMENTS :

16.8 Crystal Field Theory

68 1THE LAST FOUR MAIN GROUPS

16.9 The Spectrochemical Series

683

16.10 The Colors of Complexes

686GROUP 15/V: THE NITROGEN FAMILY

623

16.11 Magnetic Properties of Complexes

68615 .1 The Group 15/V Elements

624

16 .12 Ligand Field Theory

68815.2 Compounds with Hydrogen

THE IMPACT ON MATERIALS

690and the Halogens

625

16 .13 Steel

69015 .3 Nitrogen Oxides and Oxoacids

628

16 .14 Nonferrous Alloys

69215 .4 Phosphorus Oxides and Oxoacids

630

16 .15 Magnetic Materials

692GROUP 16/VI: THE OXYGEN FAMILY

632

Exercises

694

15 .5 The Group 16/VI Elements

632

15 .6 Compounds with Hydrogen

635

15.7 Sulfur Oxides and Oxoacids

637

Chapter 17 NUCLEAR CHEMISTRY15.8 Sulfur Halides

638",

GROUP 17/VII : THE HALOGENS

639

NUCLEAR DECAY

699

15 .9 The Group 17/VII Elements

639

17.1 The Evidence for Spontaneous

15 .10 Compounds of the Halogens

641

Nuclear Decay

700

GROUP 18/VIII : THE NOBLE GASES

644

17.2 Nuclear Reactions

70 1

15 .11 The Group 18/VIII Elements

644

17.3 The Pattern of Nuclear Stability

704

15 .12 Compounds of the Noble Gases

645

17.4 Predicting the Type of Nuclear Decay

705

THE IMPACT ON MATERIALS

647

17.5 Nucleosynthesis

707

15 .13 Luminescent Materials

647

What Has This to Do with (Box 17.1) . . .

15 .14 Nanomaterials

648

Staying Alive? Nuclear Medicine

708

Frontiers of Chemistry (Box 15.1) :

NUCLEAR RADIATION

709

Self-Assembling Materials

649

17.6 The Biological Effects of Radiation

709

Exercises

651

17.7 Measuring the Rate of Nuclear Decay

710

How Do We Know (Box 17.2) . . . How

19 .8 Amines, Amino Acids, and Amides

76 1Radioactive a Material Is?

711

TOOLBOX 19 .1 HOW TO NAME SIMPLE COMPOUND S

17.8 Uses of Radioisotopes

715

WITH FUNCTIONAL GROUPS

763NUCLEAR ENERGY

715 THE IMPACT ON MATERIALS

76417 .9 Mass-Energy Conversion

715

19 .9 Addition Polymerization

76417.10 Nuclear Fission

717

19 .10 Condensation Polymerization

76717 .11 Nuclear Fusion

721

19 .11 Copolymers and Composites

76917 .12 The Chemistry of Nuclear Power

722

19 .12 Physical Properties of Polymers

77 1Exercises

724

THE IMPACT ON BIOLOGY

771Frontiers of Chemistry (Box 19.1) :

Conducting Polymers

772

Chapter 18 ORGANIC CHEMISTRY

19 .13 Proteins

77 1

I THE HYDROCARBONS

19 .14 Carbohydrates

77519 .15 Nucleic Acids

777

ALIPHATIC HYDROCARBONS

729

Exercises

779

18.1 Types of Aliphatic Hydrocarbons

730

MAJOR TECHNIQUE 7 : NUCLEA R

TOOLBOX 18 .1 HOW TO NAME ALIPHATIC

MAGNETIC RESONANCE

786

HYDROCARBONS

73 2

18.2 Isomers

734

Appendix 1 Symbols, Units, an d

18.3 Properties of Alkanes

737

Mathematical Techniques

A l

18.4 Alkane Substitution Reactions

738

1A Symbols

A l

18.5 Properties of Alkenes

739

1B Units and Unit Conversions

A3

18 .6 Electrophilic Addition

740

IC Scientific Notation

AS

AROMATIC COMPOUNDS

742

1D Exponents and Logarithms

A6

18 .7 Nomenclature of Arenes

742

1E Equations and Graphs

A7

18 .8 Electrophilic Substitution

743

IF Calculus

A8

IMPACT ON MATERIALS : FUELS

745

Appendix 2 Experimental Data

A1 1

18 .9 Gasoline

74 .5

2A Thermodynamic Data at 25°C

Al l

18 .10 Coal

746

2B Standard Potentials at 25°C

A1 8

Exercises

748

2C Ground-State Electron

MAJOR TECHNIQUE 6 : MASS SPECTROMETRY

752

Configurations

A22D The Elements

A2222E The Top 23 Chemicals by Industria l

Production in the United States in 2005

A3 2Chapter 19 ORGANIC

Appendix 3 Nomenclature

A33

CHEMISTRY II : POLYMERS AND

3A The Nomenclature o f

BIOLOGICAL COMPOUNDS

Polyatomic Ions

A333B Common Names of Chemicals

A34COMMON FUNCTIONAL GROUPS

755

3C Names of Some Common Cations with19 .1 Haloalkanes

756

Variable Charge Numbers

A3419 .2 Alcohols

756

Glossary

B 119 .3 Ethers

757

Answers

C l19 .4 Phenols

758

Self-Tests B

C l19 .5 Aldehydes and Ketones

758

Odd-Numbered Exercises

C1 019 .6 Carboxylic Acids

759

Illustration Credits

D 119 .7 Esters

760

Index

E1