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包郵 General Chemistry(王欣)(普通化學(xué))
作者：王欣、耿旺昌 等 編
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General Chemistry(王欣)(普通化學(xué)) 版權(quán)信息
- ISBN：9787122413659
- 條形碼：9787122413659 ; 978-7-122-41365-9
- 裝幀：一般膠版紙
- 冊(cè)數(shù)：暫無(wú)
- 重量：暫無(wú)
- 所屬分類：>
General Chemistry(王欣)(普通化學(xué)) 本書(shū)特色
適讀人群 ：本書(shū)可作為高等院校各工科專業(yè)的全英文或雙語(yǔ)化學(xué)基礎(chǔ)課教學(xué)用書(shū)，也可供自學(xué)者、工程技術(shù)人員參考使用。1.本書(shū)是針對(duì)我國(guó)高等院校化學(xué)化工類專業(yè)本科生化學(xué)基礎(chǔ)課EMI（全英語(yǔ)教學(xué)）需求而編寫(xiě)的一本通用型基礎(chǔ)化學(xué)全英文教材。 2.編者在積累了多年的教學(xué)體會(huì)和實(shí)際教學(xué)案例的基礎(chǔ)上，從認(rèn)識(shí)物質(zhì)的基本規(guī)律出發(fā)，緊密聯(lián)系當(dāng)前迅速發(fā)展的材料、信息、能源、環(huán)境、國(guó)防等工程實(shí)例，深入淺出地介紹物質(zhì)的組成及結(jié)構(gòu)、化學(xué)的基本原理及在現(xiàn)代高科技中的應(yīng)用等。 3.教材目的是向?qū)W生傳授工科化學(xué)基礎(chǔ)知識(shí)，健全學(xué)生的知識(shí)結(jié)構(gòu)體系，訓(xùn)練學(xué)生掌握專業(yè)工程實(shí)際應(yīng)中涉及的基礎(chǔ)化學(xué)知識(shí)和實(shí)驗(yàn)操作的技能，學(xué)生能夠應(yīng)用化學(xué)的理論、思維去審視當(dāng)今社會(huì)關(guān)注的如環(huán)境污染、能源及資源危機(jī)、工程材料的選擇等熱點(diǎn)問(wèn)題。 4.本書(shū)突出工程應(yīng)用，弱化理論推導(dǎo)，設(shè)置的例題習(xí)題等盡量與工程實(shí)踐相結(jié)合，強(qiáng)調(diào)工程應(yīng)用中的化學(xué)思維。 5.教材中還融入了化學(xué)史教育。
General Chemistry(王欣)(普通化學(xué)) 內(nèi)容簡(jiǎn)介
General Chemistry（《普通化學(xué)》）根據(jù)我國(guó)高等院校工科專業(yè)學(xué)生對(duì)化學(xué)學(xué)習(xí)的需求及特點(diǎn)編寫(xiě)而成。書(shū)中從物質(zhì)結(jié)構(gòu)出發(fā)，闡明組成物質(zhì)的原子及分子結(jié)構(gòu)及其作用力，結(jié)合熱力學(xué)、動(dòng)力學(xué)、溶液、電化學(xué)、配位化學(xué)等基本化學(xué)原理，探討當(dāng)今迅速發(fā)展的材料、能源、環(huán)境、信息、國(guó)防等工程領(lǐng)域中的一些化學(xué)應(yīng)用問(wèn)題。本書(shū)內(nèi)容精而不簡(jiǎn)，通用性強(qiáng)，注重可靠性、規(guī)范性的同時(shí)體現(xiàn)優(yōu)選性和創(chuàng)新性。 本書(shū)可作為高等院校各工科專業(yè)的全英文或雙語(yǔ)化學(xué)基礎(chǔ)課教學(xué)用書(shū)，也可供自學(xué)者、工程技術(shù)人員參考使用。
General Chemistry(王欣)(普通化學(xué)) 目錄
Chapter 1 Introduction 1
1.1 The Purpose of Chemistry Research and Its Brief History 1
1.1.1 What Is Chemistry? 1
1.1.2 A Brief History of Chemistry 2
1.2 Modern Chemistry and High Technology 4
1.2.1 Aerospace Technology 4
1.2.2 Energy and Environment 6
1.2.3 Flexible Electronic Technology 6
1.3 The Role, Status and Development Prospect of Chemistry 7
1.3.1 The Role and Status of Chemistry 7
1.3.2 The Development Prospect for Chemistry 8
Chapter 2 Chemical Composition and Aggregation of Substances 11
2.1 Chemical Composition of the Substance 11
2.2 Gases 12
2.2.1 Gas Phase 12
2.2.2 Ideal Gases 12
2.2.3 Gas Storage and Transportation 14
2.3 Liquids 15
2.3.1 Basic Properties of Liquids 15
2.3.2 Solution 17
2.4 Solids 18
2.4.1 Introduction of Solids 18
2.4.2 Crystal Characteristics 18
2.4.3 Types of Crystals 19
2.4.4 Solid’s Applications 22
2.5 Other Forms of Matter 22
2.5.1 Liquid Crystals 22
2.5.2 Supercritical State 23
2.5.3 Plasma State 24
2.6 Change of State 25
2.6.1 Three Phase Diagram of Pure Substance 25
2.6.2 Vaporization of Liquids 26
2.6.3 Liquefaction of Gases 27
2.6.4 Other State Changes 28
Exercises 28
Chapter 3 Atomic Structure and Periodic Table of Elements 30
3.1 Atomic Structure 30
3.1.1 Electrons in Atom 31
3.1.2 Bohr’s Theory of the Hydrogen 33
3.1.3 Schrodinger Equation for Hydrogen 35
3.1.4 The Shapes of the Orbitals 36
3.1.5 Electron Configurations 40
3.2 Chemical Elements and the Periodic Table 43
3.3 Atomic Chemical Properties 45
3.3.1 Atomic Radius 45
3.3.2 Ionization Energy 47
3.3.3 Electron Affinity 51
Exercises 52
Chapter 4 Chemical Bonding and Molecular Structure 54
4.1 Chemical Bonding 54
4.1.1 Lewis Theory 54
4.1.2 The Covalent Bond: A Quantum Mechanical Concept 56
4.1.3 Introduction to the Valence Bond Method 57
4.1.4 Characteristics of Covalent Bond 57
4.1.5 Types of Covalent Bond 58
4.1.6 Bond Parameters 59
4.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory 62
4.3 Hybrid Orbital Theory and Molecular Structure 64
4.3.1 Hybrid Orbital Theory 64
4.3.2 Hybridization Scheme 64
4.4 Molecular Polarity and Polarization 67
4.4.1 Polar Covalent Bond and Nonpolar Covalent Bond 67
4.4.2 Dipole Moment and Molecular Polarity 68
4.4.3 Molecular Polarization 69
4.5 Intermolecular Forces 70
4.5.1 van der Waals Forces 70
4.5.2 Hydrogen Bonding 74
Exercises 78
Chapter 5 Heat Effect of Chemical Reaction and Energy Utilization 79
5.1 The First Law of Thermodynamics 79
5.1.1 Some Thermodynamic Terminology 79
5.1.2 The First Law of Thermodynamics 87
5.2 Heat Interaction During Chemical Process 88
5.2.1 Heats of Reaction 89
5.2.2 Enthalpy Change of Reaction: ΔrHm 91
5.2.3 Enthalpy Change Accompanying a Change in State of Matter 93
5.2.4 Standard States and Standard Enthalpies of Reaction 94
5.3 Hess’s Law and Its Applications 94
5.3.1 Hess’s Law and Applications 94
5.3.2 Basic Thermodynamics Data: Standard Molar Enthalpies of Formation 96
5.3.3 Standard Molar Combustion Enthalpy 99
5.4 Fuels as Sources of Energy 100
5.4.1 Solar Energy 101
5.4.2 Biomass Energy 104
5.4.3 Hydrogen Energy 105
5.4.4 Natural Gas Hydrate 108
Exercises 109
Chapter 6 Basic Principles of Chemical Reaction 111
6.1 Spontaneous Reaction and Entropy 111
6.1.1 Spontaneous Reaction and Its Thermal Effect 112
6.1.2 Entropy and the Direction of Spontaneous Reaction 113
6.2 Gibbs Function Changes and Judgment of Spontaneous Direction of Reaction 117
6.2.1 Gibbs Function Changes and Gibbs Function Criterion 117
6.2.2 Standard Molar Gibbs Function Variation of Reaction and Its Calculation 118
6.2.3 Application of Gibbs Formula 121
6.2.4 Gibbs Function Changes under Nonstandard Condition 124
6.3 Chemical Equilibrium 126
6.3.1 The Equilibrium Constant 127
6.3.2 The Main Factors Affecting the Chemical Equilibrium 132
6.4 Chemical Reaction Rate 139
6.4.1 Reaction Mechanisms 140
6.4.2 Effect of Concentration on Reaction Rate 144
6.4.3 Effect of Temperature on Reaction Rate 149
6.4.4 Effect of Catalyst on Reaction Rate 153
Exercises 158
Chapter 7 Solution and Ion Equilibrium 165
7.1 Colligative Properties 166
7.1.1 Vapor Pressure Lowering 166
7.1.2 Freezing Point Depression and Boiling Point Elevation 169
7.1.3 Osmotic Pressure of Solution 173
7.2 Weak Electrolyte Dissociation Equilibrium and Buffer Solution 175
7.2.1 The Development of Acid-Base Theory 175
7.2.2 The Self-ionization of Water and the pH Scale 177
7.2.3 Single-phase Dissociation Equilibrium: The Dissociation of Weak Acid and Weak Base 178
7.2.4 Buffer Solution 183
7.3 Precipitation Dissolution Equilibrium of Insoluble Strong Electrolytes 187
7.3.1 Solubility Product 187
7.3.2 Solubility Product Rules 189
Exercises 195
Chapter 8 Applied Electrochemistry 197
8.1 Voltaic Cell and Cell Diagram 197
8.1.1 Voltaic Cell 197
8.1.2 Electrode, Cell Reaction and Cell Diagram 199
8.2 Generation, Determination, Influencing Factors and Application of Electrode Potential 201
8.2.1 Generation of Electrode Potential: Electric Double Layer Theory 202
8.2.2 Measurement of Standard Electrode Potential 203
8.2.3 Nernst Equation: Effect of Concentration on Electrode Potential 208
8.2.4 Application of Electrode Potential and EMF 211
8.3 Electrolytic Cell 216
8.3.1 Composition and Electrode Reaction of Electrolytic Cells 216
8.3.2 Main Factors Affecting Electrode Reaction 217
8.3.3 Decomposition Voltage and over Voltage 221
8.3.4 General Law of Electrolytic Products 224
8.3.5 Application of Electrolysis 225
8.4 Chemical Power Supply 228
8.4.1 Classification of Chemical Power Sources 228
8.4.2 Electromotive Force, Open Circuit Voltage and Working Voltage of Chemical Power Supply 228
8.4.3 Voltaic Cells 229
8.4.4 Secondary Battery 231
8.4.5 Fuel Cells 232
8.4.6 Environmental Pollution Caused by Chemical Power Supply and
Its Treatment Measures 236
Exercises 238
Chapter 9 Corrosion and Material Protection 242
9.1 Principle and Rate of Metal Corrosion 242
9.1.1 Principle of Electrochemical Corrosion 243
9.1.2 Polarization of Corrosion Battery and Factors Affecting Corrosion Rate 244
9.2 Main Methods to Prevent Metal Corrosion 248
9.2.1 Improve the Anticorrosion Performance of Metal 248
9.2.2 The Use of Various Protective Layers 249
9.2.3 Corrosion Inhibitor Method 249
9.2.4 Electrochemical Protection 250
9.3 Protection of Polymer Materials 251
9.3.1 Influence Mechanism of Environmental Factors 252
9.3.2 Anti-aging Measures 255
9.4 Electronic Packaging Materials 257
9.4.1 Main Performance Requirements for Electronic Packaging Materials 257
9.4.2 Commonly Used Electronic Packaging Materials 258
9.4.3 Preparation Method of Metal-based Composite Electronic Packaging Materials 261
Exercises 262
Chapter 10 Metal Coordination Compound 263
10.1 Basic Concepts and Nomenclature 264
10.1.1 Coordinate Bonds and Coordination Compounds 264
10.1.2 Composition and Type of Complexes 264
10.1.3 Ligands 266
10.1.4 Naming Coordination Compounds 268
10.2 Complex Ion Equilibria 270
10.2.1 Dissociation Balance and Equilibrium Constant of Complex Ion 270
10.2.2 The Coordination Equilibria 272
10.3 The Chemical Bond Theory in Coordination Compounds 275
10.3.1 Valence Bond Theory 275
10.3.2 Crystal Field Theory (CFT) 278
10.4 Applications of Coordination Chemistry 283
10.4.1 Nitrogenase (Nitrogen Fixation) 283
10.4.2 Cisplatin: A Cancer-fighting Drug 284
10.4.3 Sequestering Metal Ions 285
10.4.4 Photosynthesis 286
10.4.5 Metalloprotein and Metalloenzyme 287
Exercises 290
Appendix 291
Ⅰ Some Basic Constants of Physics and Chemistry 291
Ⅱ Thermodynamic Properties of Substances at 298.15K 291
Ⅲ Dissociation Equilibrium Constants of Weak Electrolytes in Water at 298.15K 295
Ⅳ Solubility Product of Common Insoluble Electrolytes 297
Ⅴ Standard Electrode (Reduction) Potentials at 298.15K 298
Ⅵ Saturated Vapor Pressure of Water at Different Temperatures 302
Ⅶ Ground-state Electron Configurations 305
References 307
riodic Table of the Elements 308
1.1 The Purpose of Chemistry Research and Its Brief History 1
1.1.1 What Is Chemistry? 1
1.1.2 A Brief History of Chemistry 2
1.2 Modern Chemistry and High Technology 4
1.2.1 Aerospace Technology 4
1.2.2 Energy and Environment 6
1.2.3 Flexible Electronic Technology 6
1.3 The Role, Status and Development Prospect of Chemistry 7
1.3.1 The Role and Status of Chemistry 7
1.3.2 The Development Prospect for Chemistry 8
Chapter 2 Chemical Composition and Aggregation of Substances 11
2.1 Chemical Composition of the Substance 11
2.2 Gases 12
2.2.1 Gas Phase 12
2.2.2 Ideal Gases 12
2.2.3 Gas Storage and Transportation 14
2.3 Liquids 15
2.3.1 Basic Properties of Liquids 15
2.3.2 Solution 17
2.4 Solids 18
2.4.1 Introduction of Solids 18
2.4.2 Crystal Characteristics 18
2.4.3 Types of Crystals 19
2.4.4 Solid’s Applications 22
2.5 Other Forms of Matter 22
2.5.1 Liquid Crystals 22
2.5.2 Supercritical State 23
2.5.3 Plasma State 24
2.6 Change of State 25
2.6.1 Three Phase Diagram of Pure Substance 25
2.6.2 Vaporization of Liquids 26
2.6.3 Liquefaction of Gases 27
2.6.4 Other State Changes 28
Exercises 28
Chapter 3 Atomic Structure and Periodic Table of Elements 30
3.1 Atomic Structure 30
3.1.1 Electrons in Atom 31
3.1.2 Bohr’s Theory of the Hydrogen 33
3.1.3 Schrodinger Equation for Hydrogen 35
3.1.4 The Shapes of the Orbitals 36
3.1.5 Electron Configurations 40
3.2 Chemical Elements and the Periodic Table 43
3.3 Atomic Chemical Properties 45
3.3.1 Atomic Radius 45
3.3.2 Ionization Energy 47
3.3.3 Electron Affinity 51
Exercises 52
Chapter 4 Chemical Bonding and Molecular Structure 54
4.1 Chemical Bonding 54
4.1.1 Lewis Theory 54
4.1.2 The Covalent Bond: A Quantum Mechanical Concept 56
4.1.3 Introduction to the Valence Bond Method 57
4.1.4 Characteristics of Covalent Bond 57
4.1.5 Types of Covalent Bond 58
4.1.6 Bond Parameters 59
4.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory 62
4.3 Hybrid Orbital Theory and Molecular Structure 64
4.3.1 Hybrid Orbital Theory 64
4.3.2 Hybridization Scheme 64
4.4 Molecular Polarity and Polarization 67
4.4.1 Polar Covalent Bond and Nonpolar Covalent Bond 67
4.4.2 Dipole Moment and Molecular Polarity 68
4.4.3 Molecular Polarization 69
4.5 Intermolecular Forces 70
4.5.1 van der Waals Forces 70
4.5.2 Hydrogen Bonding 74
Exercises 78
Chapter 5 Heat Effect of Chemical Reaction and Energy Utilization 79
5.1 The First Law of Thermodynamics 79
5.1.1 Some Thermodynamic Terminology 79
5.1.2 The First Law of Thermodynamics 87
5.2 Heat Interaction During Chemical Process 88
5.2.1 Heats of Reaction 89
5.2.2 Enthalpy Change of Reaction: ΔrHm 91
5.2.3 Enthalpy Change Accompanying a Change in State of Matter 93
5.2.4 Standard States and Standard Enthalpies of Reaction 94
5.3 Hess’s Law and Its Applications 94
5.3.1 Hess’s Law and Applications 94
5.3.2 Basic Thermodynamics Data: Standard Molar Enthalpies of Formation 96
5.3.3 Standard Molar Combustion Enthalpy 99
5.4 Fuels as Sources of Energy 100
5.4.1 Solar Energy 101
5.4.2 Biomass Energy 104
5.4.3 Hydrogen Energy 105
5.4.4 Natural Gas Hydrate 108
Exercises 109
Chapter 6 Basic Principles of Chemical Reaction 111
6.1 Spontaneous Reaction and Entropy 111
6.1.1 Spontaneous Reaction and Its Thermal Effect 112
6.1.2 Entropy and the Direction of Spontaneous Reaction 113
6.2 Gibbs Function Changes and Judgment of Spontaneous Direction of Reaction 117
6.2.1 Gibbs Function Changes and Gibbs Function Criterion 117
6.2.2 Standard Molar Gibbs Function Variation of Reaction and Its Calculation 118
6.2.3 Application of Gibbs Formula 121
6.2.4 Gibbs Function Changes under Nonstandard Condition 124
6.3 Chemical Equilibrium 126
6.3.1 The Equilibrium Constant 127
6.3.2 The Main Factors Affecting the Chemical Equilibrium 132
6.4 Chemical Reaction Rate 139
6.4.1 Reaction Mechanisms 140
6.4.2 Effect of Concentration on Reaction Rate 144
6.4.3 Effect of Temperature on Reaction Rate 149
6.4.4 Effect of Catalyst on Reaction Rate 153
Exercises 158
Chapter 7 Solution and Ion Equilibrium 165
7.1 Colligative Properties 166
7.1.1 Vapor Pressure Lowering 166
7.1.2 Freezing Point Depression and Boiling Point Elevation 169
7.1.3 Osmotic Pressure of Solution 173
7.2 Weak Electrolyte Dissociation Equilibrium and Buffer Solution 175
7.2.1 The Development of Acid-Base Theory 175
7.2.2 The Self-ionization of Water and the pH Scale 177
7.2.3 Single-phase Dissociation Equilibrium: The Dissociation of Weak Acid and Weak Base 178
7.2.4 Buffer Solution 183
7.3 Precipitation Dissolution Equilibrium of Insoluble Strong Electrolytes 187
7.3.1 Solubility Product 187
7.3.2 Solubility Product Rules 189
Exercises 195
Chapter 8 Applied Electrochemistry 197
8.1 Voltaic Cell and Cell Diagram 197
8.1.1 Voltaic Cell 197
8.1.2 Electrode, Cell Reaction and Cell Diagram 199
8.2 Generation, Determination, Influencing Factors and Application of Electrode Potential 201
8.2.1 Generation of Electrode Potential: Electric Double Layer Theory 202
8.2.2 Measurement of Standard Electrode Potential 203
8.2.3 Nernst Equation: Effect of Concentration on Electrode Potential 208
8.2.4 Application of Electrode Potential and EMF 211
8.3 Electrolytic Cell 216
8.3.1 Composition and Electrode Reaction of Electrolytic Cells 216
8.3.2 Main Factors Affecting Electrode Reaction 217
8.3.3 Decomposition Voltage and over Voltage 221
8.3.4 General Law of Electrolytic Products 224
8.3.5 Application of Electrolysis 225
8.4 Chemical Power Supply 228
8.4.1 Classification of Chemical Power Sources 228
8.4.2 Electromotive Force, Open Circuit Voltage and Working Voltage of Chemical Power Supply 228
8.4.3 Voltaic Cells 229
8.4.4 Secondary Battery 231
8.4.5 Fuel Cells 232
8.4.6 Environmental Pollution Caused by Chemical Power Supply and
Its Treatment Measures 236
Exercises 238
Chapter 9 Corrosion and Material Protection 242
9.1 Principle and Rate of Metal Corrosion 242
9.1.1 Principle of Electrochemical Corrosion 243
9.1.2 Polarization of Corrosion Battery and Factors Affecting Corrosion Rate 244
9.2 Main Methods to Prevent Metal Corrosion 248
9.2.1 Improve the Anticorrosion Performance of Metal 248
9.2.2 The Use of Various Protective Layers 249
9.2.3 Corrosion Inhibitor Method 249
9.2.4 Electrochemical Protection 250
9.3 Protection of Polymer Materials 251
9.3.1 Influence Mechanism of Environmental Factors 252
9.3.2 Anti-aging Measures 255
9.4 Electronic Packaging Materials 257
9.4.1 Main Performance Requirements for Electronic Packaging Materials 257
9.4.2 Commonly Used Electronic Packaging Materials 258
9.4.3 Preparation Method of Metal-based Composite Electronic Packaging Materials 261
Exercises 262
Chapter 10 Metal Coordination Compound 263
10.1 Basic Concepts and Nomenclature 264
10.1.1 Coordinate Bonds and Coordination Compounds 264
10.1.2 Composition and Type of Complexes 264
10.1.3 Ligands 266
10.1.4 Naming Coordination Compounds 268
10.2 Complex Ion Equilibria 270
10.2.1 Dissociation Balance and Equilibrium Constant of Complex Ion 270
10.2.2 The Coordination Equilibria 272
10.3 The Chemical Bond Theory in Coordination Compounds 275
10.3.1 Valence Bond Theory 275
10.3.2 Crystal Field Theory (CFT) 278
10.4 Applications of Coordination Chemistry 283
10.4.1 Nitrogenase (Nitrogen Fixation) 283
10.4.2 Cisplatin: A Cancer-fighting Drug 284
10.4.3 Sequestering Metal Ions 285
10.4.4 Photosynthesis 286
10.4.5 Metalloprotein and Metalloenzyme 287
Exercises 290
Appendix 291
Ⅰ Some Basic Constants of Physics and Chemistry 291
Ⅱ Thermodynamic Properties of Substances at 298.15K 291
Ⅲ Dissociation Equilibrium Constants of Weak Electrolytes in Water at 298.15K 295
Ⅳ Solubility Product of Common Insoluble Electrolytes 297
Ⅴ Standard Electrode (Reduction) Potentials at 298.15K 298
Ⅵ Saturated Vapor Pressure of Water at Different Temperatures 302
Ⅶ Ground-state Electron Configurations 305
References 307
riodic Table of the Elements 308
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