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Ⅰ Inorganic Chemistry 1

Chapter 1　Introduction 2

1.1　Observations and Conclusions 3

1.2　The Scientific Method 3

1.3 Units of Measurement 5

1.4　Advice on Studying Chemistry 8

Key Words 8

Chapter 2　Structures of Atoms 9

2.1　Particles in Atoms 10

2.2　The Bohr Model 12

2.3　The Wave Theory of Electrons 13

2.4　Heisenberg's Uncertainty Principle 14

2.5　The Schr？dinger Equation 14

2.6 Quantum Numbers 15

2.7 Shapes of Atomic Orbitals 17

2.8·Many-Electron Atoms 19

2.9 Valence Electrons 24

2.10 The Periodic Table and Electronic Configurations of Atoms 24

2.11 The Periodicity of the Properties of Elements and Atomic Structure 26

Key Words 30

Exercises 31

Chapter 3　Chemical bonds 33

3.1　Ionic Bonds 33

3.2 Covalent Bonds 35

3.3　Lewis Dot Symbols and Lewis Structure 37

3.4　Sigma and Pi Bonds 43

3.5　Bond Polarity 44

3.6　Bond Energy，Bond Length and Bond Angle 45

3.7　Molecular Geometry 47

3.8　The VSEPR Model 47

3.9　Hybrid Orbitals 51

3.10　Molecular Orbitals 56

3.11 Intermolecular Force 64

Key Words 71

Exercises 71

Chapter 4　Thermochemistry 74

4.1　First Law of Thermodynamics 74

4.2　Enthalpy and Enthalpy Change 75

4.3　Hess's Law 76

4.4 Entropy and the Second Law of Thermodynamics 79

4.5 Spontaneous Processes and Gibbs Free Energy 80

4.6 Temperature and Direction of Spontaneous Change 81

4.7 Standard Free Energy of Formation and Standard Free Energy of Reaction 82

Key Words 83

Exercises 83

Chapter 5　Chemical Kinetics 85

5.1 Reaction Rates 85

5.2　Theories of Reaction Rates 87

5.3　Effect of Concentration on Rate of Reaction 89

5.4　Rate and Temperature 92

5.5　Catalysis 94

Key Words 95

Exercises 96

Chapter 6　Chemical Equilibrium 98

6.1 Concept of Equilibrium 98

6.2　Equilibrium Constant 98

6.3　Le Ch？telier's Principle 103

Key Words 106

Exercises 106

Chapter 7　Solutions 108

7.1　Ways of Expressing Concentration 108

7.2　Colligative Properties 113

Key Words 124

Exercises 125

Chapter 8　Solubility Equilibrium 127

8.1　Saturated Solutions and Solubility 127

8.2　Solubility Equilibria 127

8.3 Factors Affecting Solubility 130

8.4　Predicting Precipitation Reaction 132

8.5 Selective Precipitation 134

8.6　Application of Precipitate on Medicine 137

Key Words 138

Exercises 139

Chapter 9　Acid-Base Equilibria 141

9.1　Acids and Bases 141

9.2　Ion Product of Water 143

9.3 Strength of Weak Acids and Bases 144

9.4　The pH of Weak Acids and Bases 146

9.5　The Common-Ion Effect 148

9.6　Buffer Solutions 150

Key Words 153

Exercises 153

Chapter 10　An Introduction to Electrochemistry 155

10.1 Oxidation-Reduction Reactions 155

10.2　Balancing Oxidation-Reduction Equations 158

10.3　Voltaic Cells 161

10.4　Standard Cell Electromotive Force 164

10.5 Electrochemistry and Thermodynamics 171

10.6　Effect of Concentration on Cell EMF 172

10.7 Reduction Potential Diagrams of Elements(Latimer Diagrams) 174

Key Words 177

Exercises 177

Chapter 11　Chemistry of Coordination Compounds 180

11.1　The History of Coordination Chemistry 180

11.2 Formation of Coordination Compound 182

11.3 Nomenclature of Coordination Compounds 184

11.4 Structure and Isomerism 185

11.5　Coordination Equilibrium in Solution 187

11.6　Valence Bond Theory of Coordination Compounds 191

11.7　The Crystal Field Theory 194

11.8　The Biological Effects of Coordination Compounds 199

Key Words 200

Exercises 201

Chapter 12 Nonmetals and Semimetals 203

12.1　General Concepts 203

12.2　Hydrogen 203

12.3 Boron 204

12.4　The Group Ⅳ A Elements,the Carbon Group Elements 205

12.5　The Group Ⅴ A Elements,the Nitrogen Group Elements 208

12.6 The Group Ⅵ A Elements,the Oxygen Group Elements 211

12.7 The Group Ⅶ A Elements,the Halogens 215

12.8 The Group Ⅷ A Elements,the Noble Gases 218

Key Words 218

Exercises 219

Chapter 13 Metals 220

13.1 The Group IA Elements 220

13.2 The Group Ⅱ A Elements 224

13.3 The Group Ⅲ A Elements 229

13.4 A Survey of Transition Metals 232

13.5 Chemistry of Some Transition Metals 234

Key Words 239

Exercises 239

Ⅱ Inorganic Chemical Experiments 241

Chapter 1 Basic Techniques of Experimental Chemistry 242

1.1 Safety 242

1.2 Recording Results 243

1.3 Weighing 243

1.4 Concerning Liquids 244

Chapter 2 Typical Chemical Laboratory Apparatus 252

Chapter 3 Experiments 254

3.1 Some Elementary Operation 254

3.2 Acid-Base Titration 256

3.3 Electrolyte Solutions 259

3.4 Preparation of Officinal Sodium Chloride and Its Purity Examination 262

3.5 Oxidation-Reduction Reactions 267

3.6 Coordination Compounds 271

3.7 The Halogens 275

3.8 Chromium,Manganese and Iron 278

3.9 Copper,Silver,Zinc and Mercury 283

3.10 Determination of the Ionization Constant of HAc by pH Meter 287

3.11 Preparation of Ammonium Iron（Ⅱ）Sulfate 291

3.12 Preparation and Content Determination of Zinc Gluconate 294

Appendix 296

Reference 308