《無機化學(xué)》針對藥學(xué)類專業(yè)無機化學(xué)的雙語課程，將無機化學(xué)課程的基本內(nèi)容進行精選,結(jié)合國內(nèi)高校教學(xué)實際，刪除原版教材中大量的復(fù)雜、繁瑣及較深奧的部分，力求使之既能體現(xiàn)無機化學(xué)課程的專業(yè)基礎(chǔ)課特色，又可提高學(xué)生的英語應(yīng)用能力。
鑒于醫(yī)藥學(xué)專業(yè)學(xué)生理論與實驗課程并重的特點，全書包含兩大部分：Ⅰ Inorganic Chemistry與Ⅱ Inorganic Chemical Experiments。Part Ⅰ includings thirteen chapters：1 Introduction,2 Structures of Atoms,3 Chemical bonds,4 Thermochemistry,5 Chemical Kinetics,6 Chemical Equilibrium,7 Solutions,8 Solubility Equilibrium,9 AcidBase Equilibria，10 An Introduction to Electrochemistry,11 Chemistry of Coordination Compounds,12 Nonmetals and Semimetals,13 Metals。Part Ⅱ includings three chapters：1 Basic Techniques of Experimental Chemistry,2 Typical Chemical Laboratory Apparatus,3 Experiments。
《無機化學(xué)》可作為高等院校本科藥學(xué)及化學(xué)類相關(guān)專業(yè)的無機化學(xué)雙語教材，也可作為化學(xué)專業(yè)英語課的教材或參考書。
Ⅰ Inorganic Chemistry1
Chapter 1 Introduction2
1.1 Observations and Conclusions3
1.2 The Scientific Method3
1.3 Units of Measurement5
1.4 Advice on Studying Chemistry8
Key Words8
Chapter 2 Structures of Atoms9
2.1 Particles in Atoms10
2.2 The Bohr Model12
2.3 The Wave Theory of Electrons13
2.4 Heisenbergs Uncertainty Principle14
2.5 The Schrdinger Equation14
2.6 Quantum Numbers15
2.7 Shapes of Atomic Orbitals17
2.8 ManyElectron Atoms19
2.9 Valence Electrons24
2.10 The Periodic Table and Electronic Configurations of Atoms24
2.11 The Periodicity of the Properties of Elements and Atomic Structure26
Key Words30
Exercises31
Chapter 3 Chemical bonds33
3.1 Ionic Bonds33
3.2 Covalent Bonds35
3.3 Lewis Dot Symbols and Lewis Structure37
3.4 Sigma and Pi Bonds43
3.5 Bond Polarity44
3.6 Bond Energy, Bond Length and Bond Angle45
3.7 Molecular Geometry47
3.8 The VSEPR Model47
3.9 Hybrid Orbitals51
3.10 Molecular Orbitals56
3.11 Intermolecular Force64
Key Words71
Exercises71
Chapter 4 Thermochemistry74
4.1 First Law of Thermodynamics74
4.2 Enthalpy and Enthalpy Change75
4.3 Hesss Law76
4.4 Entropy and the Second Law of Thermodynamics 79
4.5 Spontaneous Processes and Gibbs Free Energy80
4.6 Temperature and Direction of Spontaneous Change81
4.7 Standard Free Energy of Formation and Standard Free Energy of Reaction82
Key Words83
Exercises83
Chapter 5 Chemical Kinetics85
5.1 Reaction Rates85
5.2 Theories of Reaction Rates 87
5.3 Effect of Concentration on Rate of Reaction89
5.4 Rate and Temperature92
5.5 Catalysis94
Key Words95
Exercises96
Chapter 6 Chemical Equilibrium98
6.1 Concept of Equilibrium98
6.2 Equilibrium Constant98
6.3 Le Chteliers Principle103
Key Words106
Exercises106
Chapter 7 Solutions108
7.1 Ways of Expressing Concentration108
7.2 Colligative Properties113
Key Words124
Exercises125
Chapter 8 Solubility Equilibrium127
8.1 Saturated Solutions and Solubility127
8.2 Solubility Equilibria127
8.3 Factors Affecting Solubility130
8.4 Predicting Precipitation Reaction132
8.5 Selective Precipitation134
8.6 Application of Precipitate on Medicine137
Key Words138
Exercises139
Chapter 9 AcidBase Equilibria141
9.1 Acids and Bases141
9.2 Ion Product of Water143
9.3 Strength of Weak Acids and Bases144
9.4 The pH of Weak Acids and Bases146
9.5 The CommonIon Effect148
9.6 Buffer Solutions150
Key Words153
Exercises153
Chapter 10 An Introduction to Electrochemistry155
10.1 OxidationReduction Reactions155
10.2 Balancing OxidationReduction Equations158
10.3 Voltaic Cells161
10.4 Standard Cell Electromotive Force164
10.5 Electrochemistry and Thermodynamics171
10.6 Effect of Concentration on Cell EMF172
10.7 Reduction Potential Diagrams of Elements（Latimer Diagrams）174
Key Words177
Exercises177
Chapter 11 Chemistry of Coordination Compounds180
11.1 The History of Coordination Chemistry180
11.2 Formation of Coordination Compound182
11.3 Nomenclature of Coordination Compounds184
11.4 Structure and Isomerism 185
11.5 Coordination Equilibrium in Solution187
11.6 Valence Bond Theory of Coordination Compounds191
11.7 The Crystal Field Theory194
11.8 The Biological Effects of Coordination Compounds199
Key Words200
Exercises201
Chapter 12 Nonmetals and Semimetals203
12.1 General Concepts203
12.2 Hydrogen203
12.3 Boron204
12.4 The Group ⅣA Elements，the Carbon Group Elements205
12.5 The GroupⅤA Elements，the Nitrogen Group Elements208
12.6 The Group ⅥA Elements，the Oxygen Group Elements211
12.7 The Group ⅦA Elements，the Halogens215
12.8 The Group ⅧA Elements，the Noble Gases218
Key Words218
Exercises219
Chapter 13 Metals 220
13.1 The Group IA Elements220
13.2 The Group ⅡA Elements224
13.3 The Group ⅢA Elements229
13.4 A Survey of Transition Metals232
13.5 Chemistry of Some Transition Metals234
Key Words239
Exercises239
Ⅱ Inorganic Chemical Experiments241
Chapter 1 Basic Techniques of Experimental Chemistry242
1.1 Safety242
1.2 Recording Results243
1.3 Weighing243
1.4 Concerning Liquids244
Chapter 2 Typical Chemical Laboratory Apparatus 252
Chapter 3 Experiments254
3.1 Some Elementary Operation254
3.2 AcidBase Titration256
3.3 Electrolyte Solutions259
3.4 Preparation of Officinal Sodium Chloride and Its Purity Examination 262
3.5 OxidationReduction Reactions267
3.6 Coordination Compounds271
3.7 The Halogens275
3.8 Chromium,Manganese and Iron278
3.9 Copper,Silver,Zinc and Mercury283
3.10 Determination of the Ionization Constant of HAc by pH Meter287
3.11 Preparation of Ammonium Iron（Ⅱ）Sulfate291
3.12 Preparation and Content Determination of Zinc Gluconate294
Appendix296
Reference
In science, a theory is a unifying explanation of the general principles of certain phenomena with considerable evidence or facts to support it. Hypotheses that survive many experimental tests of their validity may evolve into theories.
A scientific theory or law represents a hypothesis, or a group of related hypotheses confirmed through repeated experimental tests. Science progresses by cycles of suggested theories and tests by experiment. No matter how elegant a theory is, its predictions must agree with experimental results if we are to believe that it is a valid description of nature. So as soon as a new theory has been suggested, new experiments should be launched to test it. If the experimental results support the theory, it is accepted. If they do not, it must be modified or a new theory invented. Accepted scientific theories and laws become a part of our understanding of the universe and the basis for exploring less well-understood areas of knowledge. In part because of the unavailable necessary technology, probing or disproving a theory can take years, even centuries. For example, it took more than 2000 years to work out atomic theory proposed by Democritus, and ancient Greek philosopher.
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