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無機(jī)及分析化學(xué)(郭明)(英文版) 讀者對(duì)象:本教材適用于本科高等院校化學(xué)、應(yīng)用化學(xué)、化工、輕工、水產(chǎn)、醫(yī)學(xué)、材料、生物、醫(yī)藥、環(huán)境、地質(zhì)、農(nóng)林等相關(guān)專業(yè)的化學(xué)基礎(chǔ)課程英語教學(xué)和雙語教學(xué),也可用于各類院校同等基礎(chǔ)各相關(guān)專業(yè)留學(xué)生的師生教學(xué)和教學(xué)參考。
《Inorganic & Analytical Chemistry》可共十七章,其中介紹了無機(jī)化學(xué)的基本知識(shí),如物質(zhì)結(jié)構(gòu)、分散體系、化學(xué)反應(yīng)速率、化學(xué)平衡、非金屬元素和金屬元素等;化學(xué)分析的四大滴定法及其相關(guān)理論和應(yīng)用,如酸堿滴定法、重量分析法、沉淀滴定法、配位滴定法和氧化還原滴定法等。
《Inorganic & Analytical Chemistry》可作為應(yīng)用型本科院校化學(xué)、應(yīng)用化學(xué)、化工、輕工、材料、生物、醫(yī)藥、環(huán)境、地質(zhì)、農(nóng)林等專業(yè)的教材及考研參考書,也可供相關(guān)專業(yè)的科技人員與分析測(cè)試工作者使用,也可作為自學(xué)者的閱讀參考。
郭明,男,浙江農(nóng)林大學(xué),教 授,1996年碩士研究生畢業(yè)于中科院長春應(yīng)用化學(xué)研究所,分析化學(xué)專業(yè);2004年博士研究生畢業(yè)于浙江大學(xué),物理化學(xué)專業(yè)(化學(xué)生物學(xué)); 2005-2007年于中國林科院林產(chǎn)化學(xué)工業(yè)研究所開展博士后工作,林產(chǎn)化工專業(yè)(生物質(zhì)材料方向)。2007-2010年于浙江中醫(yī)藥大學(xué)開展博士后工作,藥理學(xué)專業(yè)。
主持并完成國家自然科學(xué)基金項(xiàng)目兩項(xiàng);主持并完成中國博士后科學(xué)基金項(xiàng)目一項(xiàng)(一等資助);主持并完成省部級(jí)科研項(xiàng)目4項(xiàng);主持并完成廳局級(jí)科研項(xiàng)目3項(xiàng)。作為參加者參與國家、省部級(jí)項(xiàng)目多項(xiàng)。 發(fā)表論文120余篇,SCI/EI收錄40篇(第*一作者27篇)。授權(quán)專利41項(xiàng),其中授權(quán)發(fā)明專利6項(xiàng)。獲省科技進(jìn)步三等獎(jiǎng)一項(xiàng)(排序第*一)。 長期從事結(jié)構(gòu)化學(xué)、儀器分析、有機(jī)化學(xué)等課程的教學(xué)任務(wù)。
Chapter1 Dispersion system 1
1.1 Solution 2 1.1.1 Amount-of-substances and its units 2 1.1.2 Concentration of amount-of-substance 3 1.1.3 Amount-of-substance fraction 3 1.1.4 Molality 3 1.1.5 Mass fraction 4 1.2 General properties of dilute solution 4 1.2.1 Colligative properties 4 1.2.2 The vapour pressure of the solution decreases 4 1.2.3 Boiling point rise of solution 6 1.2.4 The freezing point of the solution decreases 7 1.2.5 Osmotic pressure of solution 9 1.3 Electrolyte solution 11 1.3.1 Electrolyte solution 11 1.3.2 Dissociation degree 11 1.3.3 Deviation of electrolyte colligative property 12 1.3.4 Introduction of strong electrolyte solution theory 12 1.3.5 Activity, activity coefficient and ionic strength 13 1.4 Colloidal solution 14 1.4.1 Dispersion degree and specific surface 14 1.4.2 Surface energy 15 1.4.3 Adsorption of gases by solids 15 1.4.4 Adsorption of solids in solution 16 1.4.5 Properties of sol 18 1.4.6 Causes of charged sol particles 21 1.4.7 Micelle structure 21 1.4.8 Stability and condensation of sol 22 1.4.9 Comparison of polymer solution and sol 24 Exercises 25 Chapter2 Fundamentals of chemical thermodynamics 27 2.1 Basic Concepts 27 2.1.1 System and environment 27 2.1.2 State and state function 27 2.1.3 Process and path 28 2.1.4 Heat and work 28 2.1.5 Internal energy 28 2.2 Thermal effect of chemical reaction 29 2.2.1 The first law of thermodynamics 29 2.2.2 Concepts of reaction heat at constant volume, reaction heat at constant pressure and enthalpy 29 2.2.3 Thermochemical equation 31 2.2.4 Hess’s Law 31 2.2.5 Formation enthalpy 33 2.3 Entropy and entropy increase principle 34 2.3.1 Spontaneity of chemical reactions 34 2.3.2 Entropy 35 2.3.3 Standard molar entropy 36 2.4 Gibbs function and chemical reaction direction 38 2.4.1 Gibbs function 38 2.4.2 Standard generated Gibbs function 39 2.4.3 Relationship between ΔG and temperature 40 Exercises 41 Chapter3 Chemical reaction rate and chemical equilibrium 43 3.1 Chemical reaction rate 43 3.1.1 Reaction rate 43 3.1.2 Mass action law and rate equation 46 3.1.3 Rate theory of chemical reaction 51 3.2 Catalyst 54 3.2.1 Definition of catalyst 54 3.2.2 Principle and method of catalysis 54 3.3 Reversible reaction and chemical equilibrium 56 3.3.1 Reversible reaction 56 3.3.2 Equilibrium constant 57 3.3.3 Relationship between standard equilibrium constant and Gibbs free energy 59 3.3.4 Multiple equilibrium rules 62 3.3.5 The movement of chemical equilibrium 63 Exercises 65 Chapter4 The Structure of the Chemical Substance 69 4.1 Quantum mechanical models of atom 69 4.1.1 Wave-particle duality of microscopic particles 69 4.1.2 Heisenberg uncertainty relationship 70 4.1.3 Wave functions and atomic orbitals 71 4.1.4 Electron cloud and radial distribution 72 4.2 Motion state of extranuclear electrons 74 4.2.1 Four quantum numbers 74 4.2.2 Electron arrangement outside the nucleus 76 4.3 Electron layer of atoms and periodic table of elements 82 4.3.1 Electron layer structure and period 82 4.3.2 Periodicity of element properties 83 4.4 Covalent bond 86 4.4.1 Valence bond theory 87 4.4.2 Hybrid orbital theory 92 4.5 Intermolecular forces and hydrogen bonds 97 4.6 Crystal structure 101 4.6.1 Crystal characteristics 101 4.6.2 Types of crystals 102 Exercises 105 Chapter5 Chemical analysis 108 5.1 Overview of Analytical Chemistry 108 5.1.1 Tasks and functions of Analytical Chemistry 108 5.1.2 Classification of analytical methods 109 5.1.3 General steps of quantitative analysis 111 5.2 Errors in quantitative analysis 115 5.2.1 Sources and classification of errors 116 5.2.2 Expression of error 117 5.2.3 Methods to improve the accuracy of analysis results 122 5.2.4 Data processing of analysis results 123 5.3 Significant figures and operation rules 129 5.3.1 Significant figures 129 5.3.2 Rounding off of significant figures 130 5.3.3 Operation rules of significant numbers 130 5.4 Titration analysis 132 5.4.1 Overview of titration analysis 132 5.4.2 Classification of titration analysis 132 5.4.3 Conditions and methods of titration reaction 133 5.4.4 Standard solution and reference material 134 5.4.5 Calculation in titration analysis 136 Exercises 138 Chapter6 Acid-base reaction balance and acid-base titration 141 6.1 Acid base proton theory 141 6.1.1 Definition of acid base 141 6.1.2 The conjugate relationship of acid and alkali and the common appearance of acid base pair 142 6.1.3 Essence of acid-base reaction 143 6.1.4 Proton self-transfer of water and pH value of solution 145 6.2 Acid base balance 146 6.2.1 Treatment method of acid-base balance in solution 146 6.2.2 Dissociation equilibrium of weak acid and weak base in solution 148 6.2.3 Same ion effect and salt effect 149 6.3 Calculation of concentration in acid-base balance 150 6.3.1 Calculation of pH value of acid-base solution 150 6.3.2 Distribution of acid-base components in aqueous solution 157 6.4 Acid base buffer solution 161 6.4.1 Buffering principle 162 6.4.2 Calculation of pH value of buffer solution 162 6.4.3 Buffer capacity and buffer range 163 6.4.4 Preparation of buffer solution 164 6.5 Acid base indicator 165 6.5.1 Discoloration principle of acid base indicator 165 6.5.2 Discoloration range of acid-base indicator 166 6.5.3 Main factors affecting the range of acid-base indicator 168 6.5.4 Mixed indicators 169 6.6 Basic principle of acid base titration 170 6.6.1 Mutual titration of strong acid and strong base 171 6.6.2 Titration of single weak acid (base) with strong base (acid) 174 6.6.3 Titration of polybasic acids and bases 178 6.7 Application of acid base titration 182 6.7.1 Preparation and calibration of acid base standard solution 182 6.7.2 Application examples 184 Exercises 187 Chapter7 Precipitation dissolution equilibrium and precipitation analysis 191 7.1 Solubility product constant and solubility product rule 191 7.1.1 Solubility 191 7.1.2 Solubility product constant 191 7.1.3 Conversion between solubility product and solubility 193 7.1.4 Common ion effect and salt effect 194 7.1.5 Rule of solubility product 195 7.2 Application of solubility product rule 196 7.2.1 Formation of precipitation 196 7.2.2 Fractional precipitation 198 7.2.3 Dissolution of precipitates 199 7.2.4 Transformation of precipitation 202 7.3 Precipitation titration method 203 7.3.1 Overview of precipitation titration 203 7.3.2 Determination of end point by precipitation titration 204 7.4 Gravimetric method 208 7.4.1 Overview of precipitation gravimetric analysis 208 7.4.2 Factors affecting precipitation purity 209 7.4.3 Selection of precipitation conditions 210 7.4.4 Filtration and washing of precipitates 211 7.4.5 Drying or burning of precipitates 212 7.4.6 Calculation of analysis results 212 Exercises 212 Chapter8 Redox Reaction Balance and Redox Titration 214 8.1 The basic concept of redox reaction 214 8.1.1 Oxidation number 214 8.1.2 Redox reaction 215 8.1.3 Redox half reaction and redox electric pairs 217 8.2 Balancing redox reaction equation 217 8.2.1 Oxidation number method 217 8.2.2 Ion-electron method 218 8.3 Galvanic cell and electrode potential 220 8.3.1 Galvanic cell and redox reaction 220 8.3.2 Electrode potential 222 8.3.3 Theoretical calculation of electrode potential (the relationship between electromotive force and ΔrGm) 225 8.4 Factors affecting electrode potential and application of electrode potential 227 8.4.1 Nernst equation and its application 227 8.4.2 Factors affecting electrode potential 229 8.5 Element potential diagram and its application 232 8.5.1 Element potential diagram 232 8.5.2 Application of element potential diagrams 232 8.6 Redox titration 234 8.6.1 Overview 234 8.6.2 Redox titration curve 239 8.6.3 Redox titration indicator 242 8.7 Redox titration method in common use 244 8.7.1 Potassium permanganate method 245 8.7.2 Potassium dichromate method 248 8.7.3 Iodometry 251 Exercises 255 Chapter9 Coordination Reaction Equilibrium and Coordination Titration 261 9.1 Composition and nomenclature of coordination compound 261 9.1.1 Composition of coordination compound 261 9.1.2 Nomenclature of coordination compound 263 9.2 Valence bond theory of coordination compound 265 9.2.1 Valence bond theory 265 9.2.2 Crystal field theory 267 9.3 Coordination equilibrium 268 9.3.1 Coordination equilibrium constant 268 9.3.2 Movement of coordination equilibrium 271 9.4 Chelate 278 9.4.1 Definition of chelates 278 9.4.2 Chelating agent 278 9.4.3 Chelate effect 279 9.5 The complexes of EDTA with metal ions and the stable 280 9.5.1 EDTA dissociation equilibrium 280 9.5.2 The characteristics of the chelate of EDTA and metal ions 281 9.5.3 Main factors affecting the stability of EDTA complexes 282 9.5.4 Conditional stability constants of EDTA complexes 284 9.6 Coordination titration 285 9.6.1 Coordination titration curve 285 9.6.2 The condition of accurately titrating a metal 287 9.6.3 Acidity range of coordination titration 287 9.7 Metal indicator 289 9.7.1 Principle of action of metal indicator 289 9.7.2 Requirements for metal indicator 290 9.7.3 Common metal indicators 290 9.7.4 Selection of metal indicator 291 9.7.5 Problems that should be paid attention to during the use of metal indicator 291 9.8 Classification of coordination titration and elimination of interfering ions 292 9.8.1 Classification of coordination titration 292 9.8.2 Elimination of titration interference 293 9.9 Application of coordination titration 295 9.9.1 Preparation and calibration of EDTA standard solution 295 9.9.2 Application examples 296 Exercises 297 Chapter 10 Brief Content of Elemental Chemistry 300 10.1 Halogen 300 10.1.1 Overview 300 10.1.2 Halogen elements 301 10.1.3 Hydrogen halides and hydrohalides 302 10.1.4 Halide 303 10.1.5 Oxyacids and salts of halogens 303 10.2 Oxygen 305 10.2.1 Oxygen and ozone 305 10.2.2 Hydrogen peroxide 306 10.3 Nitrogen and phosphorus 307 10.3.1 Nitrogen and its important compounds 307 10.3.2 Important compounds of phosphorus 309 10.4 Copper, silver, zinc, cadmium and mercury 311 10.4.1 Important compounds of copper and silver 312 10.4.2 Important compounds of zinc, cadmium and mercury 313 10.5 Chromium, molybdenum and manganese 314 10.5.1 Chromium and molybdenum compounds 315 10.5.2 Manganese compounds 316 10.6 Iron and cobalt 317 10.6.1 Iron compounds 317 10.6.2 Cobalt compounds 318 Exercises 319 Chapter 11 Spectrophotometric method 320 11.1 Selective absorption of light by substances 320 11.1.1 Electromagnetic spectrum 320 11.1.2 The interaction between light and matter 321 11.1.3 Adsorption curve 322 11.1.4 Characteristics of spectrophotometry 323 11.2 Law of absorption of light 324 11.2.1 Lambert-Beer’s law 324 11.2.2 Molar absorptivity 325 11.2.3 The reason for deviating from Lambert-Beer’s law 326 11.3 Spectrophotometer 328 11.4 Color reaction and selection of color conditions 330 11.4.1 Selection of chromogenic reaction 331 11.4.2 Selection of chromogenic conditions 331 11.5 Selection of conditions for absorbance determination 333 11.5.1 Selection of absorbing light range 333 11.5.2 Selection of reference solution 335 11.5.3 Interference and elimination methods 335 11.6 Application of spectrophotometry 336 11.6.1 Determination of single component 336 11.6.2 Multicomponent quantitative method 337 11.6.3 Differential spectrophotometry 338 Exercises 339 References 342 The appendix 343
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