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