书名：General Chemistry（王欣）（普通化学）  
定价：88.0  
ISBN：9787122413659  
作者：王欣、耿旺昌 等 编  
版次：第1版  
出版时间：2022-09  

内容提要：  
General Chemistry（《普通化学》）根据我国高等院校工科专业学生对化学学习的需求及特点编写而成。书中从物质结构出发，阐明组成物质的原子及分子结构及其作用力，结合热力学、动力学、溶液、电化学、配位化学等基本化学原理，探讨当今迅速发展的材料、能源、环境、信息、国防等工程领域中的一些化学应用问题。本书内容精而不简，通用性强，注重可靠性、规范性的同时体现先进性和创新性。 本书可作为高等院校各工科专业的全英文或双语化学基础课教学用书，也可供自学者、工程技术人员参考使用。  



作者简介：  
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目录：  
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  

Periodic Table of the Elements 308