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CHEMISTRY THE CENTRAL SCIENCEpdf电子书版本下载
- THEODORE L.BROWN H.EUGENE LEMAY 著
- 出版社：
- ISBN：013336397X
- 出版时间：未知
- 标注页数：1045页
- 文件大小：240MB
- 文件页数：1108页
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图书目录
1 Introduction: Some Basic Concepts 1
1.1 INTRODUCTION TO MATTER 2
Substances 5
Physical and Chemical Properties 5
Physical and Chemical Changes 5
Mixtures 6
1.2 ELEMENTS AND COMPOUNDS 9
Elements 10
Compounds 10
1.3 UNITS OF MEASUREMENT 11
Length and Mass 13
Temperature 13
Derived SI Units 15
Volume 15
Density 16
Intensive and ExtensiveProperties 19
1.4 UNCERTAINTY IN MEASUREMENT 19
Precision and Accuracy 19
Significant Figures 20
Significant Figures in Calculations 21
1.5 DIMENSIONAL ANALYSIS 23
Summary of Dimensional Analysis 25
Summary 27
Key Terms 28
Exercises 28
2 Atoms, Molecules, and Ions 32
2.1 THE ATOMIC THEORY OF MATTER 33
2.2 THE DISCOVERY OF ATOMIC STRUCTURE 35
Cathode Rays and Electrons 35
Radioactivity 38
The Nuclear Atom 39
2.3 THE MODERN VIEW OF ATOMIC STRUCTURE 41
Isotopes, Atomic Numbers, and Mass Numbers 43
2.4 THE PERIODIC TABLE 44
2.5 MOLECULES AND IONS 48
Molecules and Chemical Formulas 48
Molecular, Empirical, and Structural Formulas 49
Ions 50
Predicting Ionic Charges 52
Ionic Compounds 53
2.6 NAMING INORGANIC COMPOUNDS 55
Ionic Compounds: Cations 55
Ionic Compounds: Anions 56
Acids 59
Molecular Compounds 61
Summary 61
Key Terms 62
Exercises 62
3 Stoichiometry: Calculations with Chemical Formulas and Equations 67
3.1 CHEMICAL EQUATIONS 68
3.2 PATTERNS OF CHEMICAL REACTIVITY 71
Using the Periodic Table 72
Combustion in Air 72
Combination and Decomposition Reactions 73
3.3 ATOMIC AND MOLECULAR WEIGHTS 75
The Atomic Mass Scale 75
Average Atomic Masses 76
Formula and Molecular Weights 77
Percentage Composition from Formulas 79
3.4 THE MOLE 79
Molar Mass 80
Interconverting Masses, Moles, and Numbers of Particles 82
3.5 EMPIRICAL FORMULAS FROM ANALYSES 84
Molecular Formula from Empirical Formula 85
Combustion Analysis 86
3.6 QUANTITATIVE INFORMATION FROM BALANCED EQUATIONS 88
3.7 LIMITING REACTANTS 92
Theoretical Yields 95
Summary 96
Key Terms 97
Exercises 97
4 Aqueous Reactions and Solution Stoichiometry 104
4.1 SOLUTION COMPOSITION 106
Molarity 106
Dilution 108
4.2 ELECTROLYTES 109
Strong and Weak Electrolytes 110
4.3 ACIDS, BASES, AND SALTS 112
Bases 112
Salts 113
Identifying Strong and Weak Electrolytes 114
Neutralization Reactions 115
4.4 IONIC EQUATIONS 115
4.5 METATHESIS REACTIONS 117
Precipitation Reactions 118
Solubility Rules 118
Reactions in Which a Weak Electrolyte or Nonelectrolyte Forms 120
Reactions in Which a Gas Forms 121
4.6 REACTIONS OF METALS 124
Oxidation and Reduction 124
Oxidation of Metals by Acids and Salts 125
The Activity Series 126
4.7 SOLUTION STOICHIOMETRY 128
Titrations 131
Summary 134
Key Terms 134
Exercises 135
5 Energy Relationships in Chemistry:Thermochemistry 139
5.1 THE NATURE OF ENERGY 140
Kinetic and Potential Energy 141
Energy Units 141
Systems and Surroundings 142
Lowering the Energy of the System 142
5.2 THE FIRST LAW OF THERMODYNAMICS 143
Internal Energy 143
Relating △E to Heat and Work 144
State Functions 144
5.3 HEAT AND ENTHALPY CHANGES 146
Enthalpy 147
5.4 ENTHALPIES OF REACTION 147
5.5 CALORIMETRY 152
Heat Capacity and Specific Heat 152
Constant-PressureCalorimetry 153
Bomb Calorimetry （Constant-Volume Calorimetry） 154
5.6 HESS’S LAW 156
5.7 ENTHALPIES OF FORMATION 159
Using Enthalpies of Formation to Calculate Enthalpies of Reaction 160
5.8 FOODS AND FUELS 162
Foods 162
Fuels 164
Other Energy Sources 167
Summary 167
Key Terms 168
Exercises 169
6 Electronic Structure of Atoms 174
6.1 THE WAVE NATURE OF LIGHT 175
6.2 QUANTUM EFFECTS AND PHOTONS 178
The Photoelectric Effect 180
6.3 BOHR’S MODEL OF THE HYDROGEN ATOM 181
Line Spectra 181
Bohr’s Model 184
6.4 THE DUAL NATURE OF THE ELECTRON 186
The Uncertainty Principle 187
6.5 QUANTUM MECHANICS AND ATOMIC ORBITALS 189
Orbitals and Quantum Numbers 190
6.6 REPRESENTATIONS OF ORBITALS 192
The s Orbitals 192
The p Orbitals 193
The d and f Orbitals 194
6.7 ORBITALS IN MANY-ELECTRON ATOMS 195
Effective Nuclear Charge 196
Energies of Orbitals 196
Electron Spin and the Pauli Exclusion Principle 197
6.8 ELECTRON CONFIGURATIONS 199
Writing Electron Configurations 199
6.9 ELECTRON CONFIGURATIONS AND THE PERIODIC TABLE 204
Summary 208
Key Terms 209
Exercises 210
7Periodic Properties of the Elements 215
7.1 DEVELOPMENT OF THE PERIODIC TABLE 216
7.2 ELECTRON SHELLS IN ATOMS 218
7.3 SIZES OF ATOMS 220
7.4 IONIZATION ENERGY 221
Periodic Trends in Ionization Energies 223
7.5 ELECTRON AFFINITIES 224
7.6 METALS, NONMETALS, AND METALLOIDS 226
Metals 227
Nonmetals 229
Metalloids 231
Trends in Metallic and Nonmetallic Character 231
7.7 GROUP TRENDS: THE ACTIVE METALS 232
Group 1A: The Alkali Metals 233
Group 2A: The AlkalineEarth Metals 236
7.8 GROUP TRENDS: SELECTED NONMETALS 238
Hydrogen 238
Group 6A: The Oxygen Family 238
Group 7A: The Halogens 240
Group 8A: The Noble Gases 243
Summary 244
Key Terms 244
Exercises 245
8Basic Concepts of Chemical Bonding 249
8.1 LEWIS SYMBOLS AND THE OCTET RULE 251
8.2 IONIC BONDING 252
Energetics of Ionic Bond Formation 253
Electron Configurations of Ions 254
Polyatomic Ions 256
8.3 SIZES OF IONS 257
8.4 COVALENT BONDING 259
Multiple Bonds 260
8.5 BOND POLARITY AND ELECTRONEGATIVITY 261
Electronegativity 261 Electronegativity and Bond Polarity 262
8.6 DRAWING LEWIS STRUCTURES 263
8.7 RESONANCE STRUCTURES 265
8.8 EXCEPTIONS TO THE OCTET RULE 268
Odd Number of Electrons 268 Less Than an Octet 268
More Than an Octet 269
8.9 STRENGTHS OF COVALENT BONDS 270
Bond Energies and the Enthalpy of Reactions 272
Bond Strength and Bond Length 273
8.10 OXIDATION NUMBERS 275
Oxidation Numbers and Nomenclature 277
Summary 279
Key Terms 280
Exercises 280
9Molecular Geometry and Bonding Theories 285
9.1 MOLECULAR GEOMETRIES 286
The Valence-Shell Electron Pair Repulsion Model 287
Predicting Molecular Geometries 288
Four or Fewer Valence-Shell Electron Pairs 290
The Effect of Nonbonding Electrons andMultiple Bonds on Bond Angles 292
Geometries of Moleculeswith Expanded Valence Shells 293
Molecules with No Single Central Atom 296
9.2 POLARITY OF MOLECULES 297
The Polarity of Polyatomic Molecules 298
9.3 COVALENT BONDING AND ORBITAL OVERLAP 301
9.4 HYBRID ORBITALS 302
sp Hybrid Orbitals 302
sp2 and sp3 Hybrid Orbitals 304
Hybridization Involving d Orbitals 306
Summary 306
9.5 MULTIPLE BONDS 309
Delocalized Bonding 313
General Conclusions 314
9.6 MOLECULAR ORBITALS 315
The Hydrogen Molecule 315
Bond Order 317
9.7 SECOND-PERIOD DIATOMIC MOLECULES 318
Molecular Orbitals for Li2 and Be2 318
Molecular Orbitals from 2p Atomic Orbitals 319
Electron Configurations for B 2
Through F2 320
Electron Configurations and Molecular Properties 321
Summary 325
Key Terms 326
Exercises 327
10 Gases 331
10.1 CHARACTERISTICS OF GASES 332
10.2 PRESSURE 333
Atmospheric Pressure and the Barometer 333
Pressures of Enclosed Gases and Manometers 335
10.3 THE GAS LAWS 337
The Pressure-Volume Relationship: Boyle’s Law 337
The Temperature-Volume Relationship: Charles’s Law 339
The Quantity-Volume Relationship: Avogadro’s Law 340
10.4 THE IDEAL-GAS EQUATION 341
Relationship Between the Ideal-Gas Equation and the Gas Laws 344
10.5 MOLAR MASS AND GAS DENSITIES 347
10.6 GAS MIXTURES AND PARTIAL PRESSURES 348
Partial Pressures and Mole Fractions 349
10.7 VOLUMES OF GASES IN CHEMICAL REACTIONS 350
Collecting Gases Over Water 351
10.8 KINETIC-MOLECULAR THEORY 353
Application to the Gas Laws 354
10.9 MOLECULAR EFFUSION AND DIFFUSION 356
Graham’s Law of Effusion 357
Diffusion and Mean Free Path 358
10.10 DEVIATIONS FROM IDEAL BEHAVIOR 360
The van der Waals Equation 361
Summary 363
Key Terms 364
Exercises 364
11 Intermolecular Forces, Liquids, and Solids 371
11.1 THE KINETIC-MOLECULAR DESCRIPTION OF LIQUIDS AND SOLIDS 372
11.2 INTERMOLECULAR FORCES 373
Ion-Dipole Forces 374 Dipole-Dipole Forces 374
London Dispersion Forces 375 Hydrogen Bonding 377
11.3 PROPERTIES OF LIQUIDS: VISCOSITY AND SURFACE TENSION 382
Viscosity 382 Surface Tension 382
11.4 CHANGES OF STATE 383
Energy Changes Accompanying Changes of State 384
Heating Curves 384
Critical Temperature and Pressure 386
11.5 VAPOR PRESSURE 387
Explaining Vapor Pressure on the Molecular Level 388
Volatility, Vapor Pressure, and Temperature 389
Vapor Pressure and Boiling Point 389
11.6 PHASE DIAGRAMS 391
The Phase Diagrams of H2O and CO2 392
11.7 STRUCTURES OF SOLIDS 394
Unit Cells 395
The Crystal Structure of Sodium Chloride 396
Close Packing of Spheres 398
11.8 BONDING IN SOLIDS 400
Molecular Solids 400
Covalent-Network Solids 402
Ionic Solids 404
Metallic Solids 405
Summary 406
Key Terms 407
Exercises 408
12 Modern Materials 413
12.1 LIQUID CRYSTALS 415
Types of Liquid-Crystalline Phases 416
12.2 POLYMERS 421
Types of Polymers 424
Structures and Physical Properties of Polymers 425
Crosslinking of Polymers 428
12.3 CERAMICS 430
Processing of Ceramics 432
Ceramic Composites 433
Applications of Ceramics 434
Superconducting Ceramics 434
12.4 THIN FILMS 437
Uses of Thin Films 438
Formation of Thin Films 439
Summary 442
Key Terms 443
Exercises 443
13 Properties of Solutions 447
13.1 THE SOLUTION PROCESS 448
Energy Changes and Solution Formation 449
SolutionFormation, Spontaneity, and Disorder 451
Solution Formationand Chemical Reactions 453
13.2 WAYS OF EXPRESSING CONCENTRATION 453
13.3 SATURATED SOLUTIONS AND SOLUBILITY 458
13.4 FACTORS AFFECTING SOLUBILITY 459
Solute-Solvent Interactions 460
Pressure Effects 462
Temperature Effects 464
13.5 COLLIGATIVE PROPERTIES 465
Lowering the Vapor Pressure 466
Raoult’s Law 467
Boiling-Point Elevation 469
Freezing-Point Depression 470
Osmosis 472
Determination of Molar Mass 475
13.6 COLLOIDS 476
Hydrophilic and Hydrophobic Colloids 477
Removal of Colloidal Particles 480
Summary 480
Key Terms 481
Exercises 481
14 Chemical Kinetics 487
14.1 REACTION RATES 488
Reaction Rates and Stoichiometry 491
14.2 THE DEPENDENCE OF RATE ON CONCENTRATION 492
Reaction Order 494
Units of Rate Constants 494
Using Initial Rates to Determine Rate Laws 495
14.3 CHANGE OF CONCENTRATION WITH TIME 496
First-Order Reactions 497
Half-Life 499
Second-Order Reactions 500
14.4 TEMPERATURE AND RATE 501
The Collision Model 502
Activation Energy 503
The Arrhenius Equation 505
14.5 REACTION MECHANISMS 509
Elementary Steps 509
Rate Laws of Elementary Processes 511
Rate Laws of Multistep Mechanisms 512
Mechanisms with an Initial Fast Step 514
14.6 CATALYSIS 517
Homogeneous Catalysis 517
Heterogeneous Catalysis 518
Enzymes 522
Summary 524
Key Terms 525
Exercises 525
15 Chemical Equilibrium 533
15.1 THE CONCEPT OF EQUILIBRIUM 535
15.2 THE EQUILIBRIUM CONSTANT 537
Expressing Equilibrium Constants in Terms of Pressure, Kp 540
The Magnitude of Equilibrium Constants 541
The Direction of the Chemical Equation and K 542
15.3 HETEROGENEOUS EQUILIBRIA 543
15.4 CALCULATING EQUILIBRIUM CONSTANTS 545
Relating Kc and Kp 547
15.5 APPLICATIONS OF EQUILIBRIUM CONSTANTS 548
Predicting the Direction of Reaction 548 Calculation of Equilibrium Concentrations 549
15.6 FACTORS AFFECTING EQUILIBRIUM:LE CHATELIER’S PRINCIPLE 552
Change in Reactant or Product Concentrations 553
Effects of Volume and Pressure Changes 555
Effect of Temperature Changes 556
The Effect of Catalysts 559
Summary 561
Key Terms 561
Exercises 562
16 Acid-Base Equilibria 567
16.1 THE DISSOCIATION OF WATER 568
The Proton in Water 570
16.2 BR？NSTED-LOWRY ACIDS AND BASES 570
Proton-Transfer Reactions 571
Conjugate Acid-Base Pairs 572
Conjugate Acid-Base Strengths 573
16.3 THE pH SCALE 575
Measuring pH 577
16.4 STRONG ACIDS AND BASES 578
Strong Acids 578
Strong Bases 579
16.5 WEAK ACIDS 580
Calculating pH for Solutions of Weak Acids 582
Polyprotic Acids 587
16.6 WEAK BASES 590
Types of Weak Bases 592
16.7 RELATION BETWEEN Ka AND Kb 594
16.8 ACID-BASE PROPERTIES OF SALT SOLUTIONS 596
16.9 ACID-BASE BEHAVIOR AND CHEMICAL STRUCTURE 599
Effect of Bond Polarity and Bond Strength 599
Oxyacids 600
Carboxylic Acids 602
16.10 LEWIS ACIDS AND BASES 603
Hydrolysis of Metal Ions 606
Summary 607
Key Terms 608
Exercises 608
17 Additional Aspects of Aqueous Equilibria 614
17.1 THE COMMON-ION EFFECT 615
17.2 ACID-BASE TITRATIONS 618
Strong Acid-Strong Base Titrations 619
The Addition of a Strong Base to a Weak Acid 622
Titration Curves for Weak Acids or Weak Bases 624
Titrations of Polyprotic Acids 626
17.3 BUFFERED SOLUTIONS 628
Composition and Action of Buffered Solutions 628
Buffer Capacity and pH 629
Addition of Strong Acids or Bases toBuffers 632
17.4 SOLUBILITY EQUILIBRIA 637
The Solubility-Product Constant, Ksp 637
Solubility and Ksp 638
The Common-Ion Effect 640
17.5 CRITERIA FOR PRECIPITATION OR DISSOLUTION 640
Solubility and pH 643 Selective Precipitation of Ions 645
Effect of Complex Formation on Solubility 647
Amphoterism 649
17.6 QUALITATIVE ANALYSES FOR METALLIC ELEMENTS 651
Summary 654
Key Terms 654
Exercises 655
18 Chemistry of the Environment 661
18.1 EARTH’S ATMOSPHERE 662
Composition of the Atmosphere 663
18.2 THE OUTER REGIONS OF THE ATMOSPHERE 664
Photodissociation 665
Photoionization 666
18.3 OZONE IN THE UPPER ATMOSPHERE 667
Depletion of the Ozone Layer 669
18.4 CHEMISTRY OF THE TROPOSPHERE 670
Sulfur Compounds and Acid Rain 672
Carbon Monoxide 675
Nitrogen Oxides and Photochemical Smog 676
Water Vapor,Carbon Dioxide, and Climate 677
18.5 THE WORLD OCEAN 679
Seawater 679
Desalination 680
Ocean Pollution 682
18.6 FRESH WATER 682
Dissolved Oxygen and Water Quality 683
Treatment of Municipal Water Supplies 684
Summary 686
Key Terms 687
Exercises 687
19 Chemical Thermodynamics 691
19.1 SPONTANEOUS PROCESSES 692
19.2 SPONTANEITY, ENTHALPY, AND ENTROPY 694
Spontaneity and Entropy Change 694
The Second Law of Thermodynamics 697
19.3 A MOLECULAR INTERPRETATION OF ENTROPY 699
19.4 CALCULATION OF ENTROPY CHANGES 704
19.5 GIBBS FREE ENERGY 705
Standard Free-Energy Changes 706
19.6 FREE ENERGY AND TEMPERATURE 708
19.7 FREE ENERGY AND THE EQUILIBRIUM CONSTANT 710
Summary 713
Key Terms 714
Exercises 714
20 Electrochemistry 719
20.1 OXIDATION-REDUCTION REACTIONS 721
20.2 BALANCING OXIDATION-REDUCTION EQUATIONS 722
Half-Reactions 722
Balancing Equations by the Method of Half-Reactions 723
Balancing Equations for Reactions Occurring in Basic Solution 726
20.3 VOLTAIC CELLS 727
20.4 CELL EMF 731
Standard Electrode Potentials 732
Oxidizing and Reducing Agents 735
20.5 SPONTANEITY OF REDOX REACTIONS 736
Emf and Free-Energy Change 737
20.6 EFFECT OF CONCENTRATION ON CELL EMF 739
The Nernst Equation 739
Equilibrium Constants for Redox Equations 741
20.7 COMMERCIAL VOLTAIC CELLS 743
Lead Storage Battery 744
Dry Cell 745
Nickel-Cadmium Batteries 746
Fuel Cells 746
20.8 ELECTROLYSIS 747
Electrolysis of Aqueous Solutions 748
Electrolysis with Active Electrodes 750
20.9 QUANTITATIVE ASPECTS OF ELECTROLYSIS 751
Electrical Work 753
20.10 CORROSION 755
Corrosion of Iron 756
Prevention of Corrosion 757
Summary 759
Key Terms 760
Exercises 761
21 Nuclear Chemistry 768
21.1 RADIOACTIVITY 769
Nuclear Equations 770
Types of Radioactive Decay 771
21.2 PATTERNS OF NUCLEAR STABILITY 773
Neutron-to-Proton Ratio 773 Radioactive Series 775
Further Observations 776
21.3 NUCLEAR TRANSMUTATIONS 777
Using Charged Particles 778
Using Neutrons 779
Transuranium Elements 779
21.4 RATES OF RADIOACTIVE DECAY 780
Dating 781
Calculations Based on Half-Life 782
21.5 DETECTION OF RADIOACTIVITY 784
Radiotracers 785
21.6 ENERGY CHANGES IN NUCLEAR REACTIONS 786
Nuclear Binding Energies 789
21.7 NUCLEAR FISSION 790
Nuclear Reactors 794
21.8 NUCLEAR FUSION 795
21.9 BIOLOGICAL EFFECTS OF RADIATION 797
Radiation Doses 798
Radon 798
Summary 801
Key Terms 802
Exercises 803
22 Chemistry of Hydrogen, Oxygen, Nitrogen,and Carbon 807
22.1 PERIODIC TRENDS 808
22.2 CHEMICAL REACTIONS 810
22.3 HYDROGEN 812
Isotopes of Hydrogen 812
Properties of Hydrogen 813
Preparation of Hydrogen 815
Uses of Hydrogen 816
Binary Hydrogen Compounds 816
22.4 OXYGEN 818
Properties of Oxygen 819
Preparation of Oxygen 820
Uses of Oxygen 820
Ozone 821
Oxides 822
Peroxides and Superoxides 823
The Oxygen Cycle 824
22.5 NITROGEN 824
Properties of Nitrogen 825
Preparation and Uses of Nitrogen 826
Hydrogen Compounds of Nitrogen 826
Oxides and Oxyacids of Nitrogen 828
The Nitrogen Cycle in Nature 832
22.6 CARBON 833
Elemental Forms of Carbon 833
Oxides of Carbon 835
Carbonic Acid and Carbonates 837
Carbides 839
Other Inorganic Compounds of Carbon 839
Summary 840
Key Terms 840
Exercises 841
23 Chemistry of Other Nonmetallic Elements 845
23.1 THE NOBLE-GAS ELEMENTS 846
Noble-Gas Compounds 846
23.2 THE HALOGENS 848
Occurrences of the Halogens 848
Properties and Preparation ofthe Halogens 849
Uses of the Halogens 851
The HydrogenHalides 852
Interhalogen Compounds 855
Oxyacids and Oxyanions 857
23.3 THE GROUP 6A ELEMENTS 858
General Characteristics of the Group 6A Elements 859
Occurrences and Preparation of Sulfur, Selenium, and Tellurium 860
Properties and Uses of Sulfur, Selenium, and Tellurium 861
Oxides, Oxyacids, and Oxyanions of Sulfur 862
Oxides, Oxyacids, and Oxyanions of Se and Te 865
Sulfides, Selenides, and Tellurides 865
23.4 THE GROUP 5A ELEMENTS 866
General Characteristics of the Group 5A Elements 866
Occurrence, Isolation, and Properties of Phosphorus 867
Phosphorus Halides 867
Oxy Compounds of Phosphorus 869
Arsenic, Antimony, and Bismuth 871
23.5 THE GROUP 4A ELEMENTS 872
General Characteristics of the Group 4A Elements 872
Occurrence and Preparation of Silicon 873
Silicates 874
Aluminosilicates 876
Glass 877
Silicones 878
23.6 BORON 879
Summary 880
Key Terms 880
Exercises 881
24 Metals and Metallurgy 885
24.1 OCCURRENCE AND DISTRIBUTION OF METALS 886
Minerals 887
Metallurgy 888
24.2 PYROMETALLURGY 890
The Pyrometallurgy of Iron 891
Formation of Steel 893
24.3 HYDROMETALLURGY 894
The Hydrometallurgy of Aluminum 895
24.4 ELECTROMETALLURGY 895
Electrometallurgy of Sodium 896
Electrometallurgy of Aluminum 896
Electrorefining of Copper 897
24.5 METALLIC BONDING 899
Physical Properties of Metals 900
Electron-Sea Model forMetallic Bonding 901
Molecular-Orbital Model for Metals 901
24.6 ALLOYS 905
Intermetallic Compounds 906
24.7 TRANSITION METALS 907
Physical Properties 907
Electron Configurations and OxidationStates 909
Magnetism 911
24.8 CHEMISTRY OF SELECTED TRANSITION METALS 912
Chromium 912
Iron 913
Copper 914
Summary 916
Key Terms 917
Exercises 917
25 Chemistry of Coordination Compounds 921
25.1 STRUCTURE OF COMPLEXES 922
Charges, Coordination Numbers, and Geometries 923
25.2 CHELATES 925
Metals and Chelates in Living Systems 928
25.3 NOMENCLATURE 932
25.4 ISOMERISM 934
Structural Isomerism 935 Stereoisomerism 936
25.5 LIGAND-EXCHANGE RATES 939
25.6 COLOR AND MAGNETISM 940
Color 941 Magnetism 942
25.7 CRYSTAL-FIELD THEORY 943
Electron Configurations in Octahedral Complexes 948
Tetrahedral and Square-Planar Complexes 949
Summary 951
Key Terms 952
Exercises 952
26 The Chemistry of Life: Organic and BiologicalChemistry 956
26.1 ALKANES 958
Structures of Alkanes 959
Structural Isomers 960
Nomenclature of Alkanes 960
Cycloalkanes 963
Reactions of Alkanes 964
26.2 UNSATURATED HYDROCARBONS 966
Alkenes 966
Alkynes 967
Addition Reactions of Alkenes andAlkynes 968
Aromatic Hydrocarbons 970
26.3 HYDROCARBON DERIVATIVES 972
Alcohols 973
Ethers 975
Aldehydes and Ketones 975
Carboxylic Acids 976
Esters 978
Amines and Amides 979
26.4 INTRODUCTION TO BIOCHEMISTRY 980
26.5 PROTEINS 981
Amino Acids 981
Polypeptides and Proteins 983
Protein Structure 985
26.6 CARBOHYDRATES 986
Disaccharides 988
Polysaccharides 989
26.7 NUCLEIC ACIDS 991
Summary 994
Key Terms 995
Exercises 996
A Mathematical Operations 1003
B Properties of Water 1011
C Thermodynamic Quantities for Selected Substances at 298.15 K （25℃） 1012
D Aqueous-Equilibrium Constants 1016
E Standard Electrode Potentials at 25℃ 1018
Answers to Selected Exercises 1020