Comparative Inorganic Chemistry (eBook)

Front Cover 
1 
Comparative Inorganic Chemistry 4
Copyright Page 5
Table of Contents 6
Preface to the first edition 8
Preface to the second edition 10
Preface to the third edition 12
Chapter 1. The development of fundamental ideas in 19th century chemistry 16
Science and chemistry 16
The purification and identification of substances in the laboratory 17
Atoms: classical arguments for their existence 17
Molecules: classical arguments for their existence 20
The Kinetic Theory 24
Electrolytes, ions and electrons 25
Chapter 2. The properties of elements and the structure of their atoms 27
The method of study 27
Classification of the elements in the 19th century 
27 
Mendeléeff and Lothar Meyer 28
Mendeléeff's Periodic Law 30
The divisible atom 31
The atomic nucleus 33
The structure of the atom 35
The determination of atomic masses by the mass spectrometer 37
Nuclear reactions 39
Artificial radioactivity and nuclear transmutations 40
Nuclear fusion 41
Nuclear power 41
Hazards of nuclear power and processing 42
The detection of radioactivity 42
Radioactive isotopes 43
Chapter 3. The properties of elements and the electronic configuration of their atoms 44
The discovery of Argon and its significance 44
The classification of the elements in the 20th century 46
The Periodic Law 51
Atomic orbitals and quantum numbers 54
The 's, p, d, f blocks' of elements 57
Quantitative evidence for assigning electronic configurations to atoms 
57 
Successive ionization energies and electronic configuration 
59 
Electron affinity 59
Exchange energy 61
Using the long form of the Periodic Table 62
Further predictions using the Periodic Table—the transuranium elements 63
Chapter 4. The electronic theory of valency and the periodic classification 65
Simple definitions of valency 65
The development of the concept of valency 65
The periodicity of valency 66
The basic assumptions of the electronic theory 67
The ionic bond and the formation of ions 67
Anions of oxoacids 71
The hydration of ions 71
The solid structure of ionic compounds 73
The covalent bond and the formation of molecules 73
Covalency achieved by donation: the co-ionic bond 76
The bonding in complex ions 80
A note on formulae 81
The positions occupied by metals and non-metals in the Periodic Table 81
Chapter 5. Bonding and the structures displayed by elements and their compounds 84
The general physical properties of compounds related to bond type 84
The shapes of simple inorganic molecules 86
Atomic and ionic (including metallic) radii 89
van der Waals' radii 92
The transition from ionic to covalent bond type 93
Electronegativity 94
Dipole moments 95
The Theory of Resonance 96
Fajans' Rules 97
Lattice energy and crystal energy 99
The Born-Haber thermochemical cycle 100
Lattice energy and the solubility of ionic compounds 102
Physical properties of the elements in relation to their structures and to their positions in the Periodic Table 103
Semiconductors 105
Chapter 6. Crystallization and the crystalline state 107
The characteristics of crystals, their structure and bonding 107
Allotropy, polymorphism and isomorphism 120
An examination of some allotropic systems 122
Isomorphism 126
Chapter 7. Oxidation, reduction and electrochemical processes 129
Oxidation and reduction 129
Electrode potentials and redox potentials 131
Some examples of oxidation and reduction 135
Oxidation number and valency 139
The action at electrodes during electrolysis 141
The electrochemical series and the properties of metals 145
Chapter 8. The principles governing the extraction of elements 148
The nature of the problem 148
The smelting of oxides 151
Oxidation as a means of isolating some elements 152
The application of electrolysis inextraction processes 152
Other problems to be studied 153
An outline of extraction methods 153
Chapter 9. The extraction and uses of typical elements 157
The Presentation 157
Group I: Lithium, sodium and potassium 157
Group II: Beryllium, magnesium and calcium 158
Group III: Boron and aluminium 160
Group IV: Carbon, silicon, germanium, tin and lead 163
Group V: Nitrogen, phosphorus, arsenic, antimony and bismuth 167
Group VI: Oxygen and sulphur 170
Group VII: Fluorine, chlorine, bromine and iodine 171
Chapter 10. The extraction and uses of transition and associated metals 174
The metals, their physical properties and value 174
Elements 22-28 inclusive (Ti – Ni) of electronic configuration (Ar), (3d)2–8 (4s)2(1) 175
Element 40 (Zr) of electronic configuration (Kr), (Ad)2 (5s)2 181
Elements 29,47 and 79 (Cu, Ag and Au, respectively) of outer electronic configurations (3d)10 (4s)1, (4d)10 (5s)1 and (5d)10 (6s)1 181
Elements 30, 48 and 80 (Zn, Cd and Hg, respectively) of outer electronic configurations (3d)10 (4s)2, (4d)10 (5s )2 and (5d)10(6s)2 185
Chapter 11. Industrial alloys 188
The need for alloys 188
The nature of solid phases in alloy production 188
Alloys based on copper 189
The coinage alloys 190
Light alloys based on aluminium, magnesium, titanium and beryllium 190
Alloys developed for resistance to chemical attack 191
Heat-resisting alloys 192
Alloys developed for electrical resistance and electrical heating 192
Type metals and master pattern alloys 194
Fusible alloys and solders 194
Bearing metal 194
Magnetic alloys 194
Miscellaneous alloys of interest 194
The production of steel 195
Industrial pollution 197
Corrosion of iron and steel 197
Chapter 12. Commercial processes based on air, water, petroleum and coal 198
The liquefaction and fractionation of air 198
Chemicals from coal: coal gas 201
Town gas from petroleum 204
The commercial production of ammonia and nitrogen compounds 204
Chapter 13. The industrial production of sulphuric acid 213
The paramount importance of sulphuric acid 213
Sulphur dioxide 214
Sulphuric acid 215
Chapter 14. Chemicals from salt: the alkali industry 219
A brief history of alkali production 219
The occurrence of brine and rock salt 221
Soda (sodium carbonate): the Ammonia-Soda process 221
Caustic soda (sodium hydroxide): the Lime-Soda (Gossage) process 223
Refined sodium hydrogencarbonate (sodium bicarbonate) 224
Sodium silicates 224
Uses of the major alkali products 224
Electrolysis of sodium chloride 225
Potassium compounds produced electrolytically 230
Applications of the elements produced by the electrolysis of sodium chloride 230
Chapter 15. Hydrogen, the hydrides and water 232
Hydrogen 232
The hydrides 233
Hydride type and the Periodic Table 234
The hydrogen cation, H+ 235
The hydrogen bond 235
Reactions in which hydrogen is liberated 236
The industrial production of hydrogen 238
The reactions of hydrogen 239
Monatomic hydrogen 240
A summary of the uses of hydrogen 240
Hydrogen oxide: water 240
Water supplies 243
The reactions of water 246
The structure of water and hydration 247
Deuterium compounds 249
The general properties of acids, bases and salts in relation to water 250
Salt hydrolysis 256
Chapter 16. Oxygen, oxides and peroxides 258
Oxygen 258
Oxides 260
Oxide type, oxidation state and the Periodic Table 262
Reactions in which oxygen is liberated 264
The reactions of oxygen 265
A summary of methods used to prepareoxides 267
Photosynthesis 268
Respiration 268
The uses of oxygen 269
The allotropy of oxygen: ozone (trioxygen) 269
The preparation of ozone 270
The reactions of ozone 270
The formula of ozone 271
The detection and estimation of ozone 272
Hydrogen peroxide 272
The formula and structure of hydrogen peroxide 274
The preparation of hydrogen peroxide 274
The commercial production of hydrogen peroxide 275
The reactions of hydrogen peroxide solution 276
The detection and estimation of hydrogen peroxide 277
The uses of hydrogen peroxide 278
Chapter 17. Group I: the alkali metals 280
Lithium, sodium, potassium, rubidium and caesium 280
The hydrides, oxides and hydroxides 285
Important salts formed by the alkali metals 288
Group V: nitrogen, phosphorus 291
Group VI (excluding oxygen): sulphur 294
Group VII: halogens 297
Qualitative tests for the ions of lithium, sodium and potassium 298
Chapter 18. Group II: the alkaline-earth metals 300
Beryllium, magnesium, calcium,strontium and barium 300
The metals, except beryllium 305
The hydrides, oxides and hydroxides 307
Important salts formed by the alkaline-earth metals 309
Group V: nitrogen, phosphorus 311
Group VI (excluding oxygen): sulphur 312
Group VII: halogens 314
Qualitative tests for ions of the alkaline-earth metals 316
Chapter 19. Group III: the boron group 318
Boron and aluminium 318
Boron, the boric acids and borates 321
Aluminium and its important compounds 322
Chapter 20. Group IV: the carbon group 329
Carbon, silicon, germanium, tin and lead 329
The elements 336
Carbides and suicides 338
Dioxides, monoxides and oxoacids/hydroxides 340
Disulphides, monosulphides and thiosalts 349
Halides 351
Salts of the oxoacids 355
Carbon, silicon, germanium, tin and lead 329
The elements 336
Carbides and silicides 338
Dioxides, monoxides and oxoacids/hydroxides 340
Disulphides, monosulphides and thiosalts 349
Halides 351
Salts of the oxoacids 355
Qualitative and quantitative analysis for tin and lead and their compounds 357
Miscellaneous inorganic compounds containing cyano (—C=N) and carbonyl (C=O) groups 358
The elements 336
Carbides and silicides 338
Dioxides, monoxides and oxoacids/hydroxides 340
Chapter 21. Group V: the nitrogen group 362
Nitrogen, phosphorus, arsenic antimony and bismuth 362
The elements 370
Nitrides 372
Hydrides and related compounds 373
Oxides and oxoacids/hydroxides 378
Sulphides 393
Halides, halides of oxoradicals and oxide halides 395
Salts of the oxoacids 398
Qualitative and quantitative analysis for arsenic, antimony and bismuth in their compounds 398
Chapter 22. Group VI: sulphur 401
The unusual nature of sulphur 401
Oxygen and sulphur in relation to other elements of Group VI (p block): oxygen, sulphur, selenium and tellurium 401
Sulphur 404
Chapter 23. Group VII: the halogens 418
Fluorine, chlorine, bromine and iodine 418
A laboratory introduction to the halogens 424
The laboratory preparations of chlorine, bromine and iodine 425
A comparison of the reactions of chlorine, bromine and iodine showing the progressive gradation of properties 426
The laboratory preparation of hydrogen chloride, bromide and iodide 430
A comparison of the reactions of hydrogen chloride, bromide and iodide 431
The action of water on halides 433
The distinctive character of fluorine, hydrogen fluoride and fluorides 436
Halogen and halide aspects of qualitative and quantitative analysis 442
The principal oxides of the halogens, their oxoacids and salts 445
The oxoacids of chlorine and their salts 447
Chapter 24. Period 4: transition and associated elements 457
The first transition series 457
Comparing the 3d elements 460
Scandium 467
Titanium 467
Vanadium 468
Chromium 469
Complexes of Cr° and CrIII 473
Manganese 474
Iron 477
Complexes of Feo, FeII and FeIII 483
Cobalt 484
Complexes of CoII and CoIII 486
Nickel 487
Complexes of Ni° and NiII 490
Copper 491
Complexes of CuI and CuII 497
Zinc 498
Complexes of ZnII 500
Chapter 25. Period 5: silver 502
The element, its character and uses 502
Ag1: silver(i) compounds (formerly sometimes called argentous compounds) 503
The laboratory importance of silver nitrate 506
Photography and silver compounds 509
Chapter 26. Period 6: mercury 511
The element and its oxidation states 511
Hg(l): dimercury(I) compounds and their reactions 514
Hg(II): mercury(II) compounds and their reactions 515
Examination questions 519
Answers to numerical and problem sections 559
Index 561