Understanding advanced physical inorganic chemistry : the learner's approach / Kim Seng Chan and Jeanne Tan.

By:

Chan, Kim Seng

Contributor(s):

Tan, Jeanne

Material type: Text

TextLanguage: English Publication details: Singapore, WS Education, 2020.Edition: Rev. edDescription: xix, 548 p. ; ill. pbk. : 24cmISBN:

9780000989123

Subject(s):

Physical inorganic chemistry

DDC classification:

23 541 CHA

Contents:

Preface v Acknowledgements vii 1 Atomic Structure and the Periodic Table 1 (28) 1.1 The Subatomic Particles of Matter 1 (5) 1.1.1 Behaviour in an electric field/magnetic field 1 (2) 1.1.2 Isotopes 3 (1) 1.1.3 Relative masses of an element 4 (2) 1.2 Orbitals and Quantum Numbers 6 (6) 1.2.1 The nature of electron 6 (4) 1.2.2 Shapes of orbitals 10 (2) 1.3 Electronic Configurations 12 (4) 1.3.1 Rules used in working out electronic configuration 12 (3) 1.3.2 Electronic configuration of transition elements 15 (1) 1.3.3 Anomalous electronic configurations 16 (1) 1.4 Ionisation Energies 16 (6) 1.4.1 Factors influencing the magnitude of ionisation energies 17 (5) 1.5 Periodic Table: Trend in Ionisation Energy 22 (2) 1.6 Periodic Table: Trend in Atomic Radii 24 (5) 2 Chemical Bonding 29 (52) 2.1 Metallic Bonding 29 (2) 2.1.1 Physical properties of metals 30 (1) 2.2 Ionic Bonding (or Electrovalent Bonding) 31 (8) 2.2.1 Guidelines for drawing dot-and-cross diagrams 34 (1) 2.2.2 Physical properties of ionic compounds 35 (4) 2.3 Covalent Bonding 39 (19) 2.3.1 Covalent bond formation 40 (2) 2.3.2 Dative covalent bond (coordinate bond) 42 (2) 2.3.3 Factors affecting strength of covalent bond 44 (2) 2.3.4 Shapes of molecules -- The VSEPR model 46 (6) 2.3.5 Using the Hybridisation Model to understand shape 52 (4) 2.3.6 Delocalised bonding/resonance 56 (2) 2.4 Intermediate Bond Types 58 (4) 2.4.1 Covalent character in ionic bonds 58 (2) 2.4.2 Ionic character in covalent bonds 60 (2) 2.5 Physical Properties of Covalent Compounds 62 (2) 2.5.1 Properties of giant covalent compounds 62 (2) 2.5.2 Properties of simple covalent compounds 64 (1) 2.6 Intermolecular Forces of Attraction 64 (10) 2.6.1 Instantaneous dipole��induced dipole (id��id) interactions 65 (2) 2.6.2 Permanent dipole-permanent dipole (pd��pd) interactions 67 (3) 2.6.3 Hydrogen bonding 70 (4) 2.7 Summary of Chemical Bonding: Putting it all Together 74 (7) 3 Ideal Gas and Gas Laws 81 (28) 3.1 Gas Laws 82 (14) 3.1.1 Boyle's law 82 (1) 3.1.2 Charles' law 83 (1) 3.1.3 Gay-Lussac's law 84 (1) 3.1.4 Avogadro's law 84 (4) 3.1.5 The ideal gas law 88 (2) 3.1.6 Further manipulations of the ideal gas equation 90 (1) 3.1.7 Dalton's Law of Partial Pressure 91 (4) 3.1.8 Types of mathematical problems involving the gas laws 95 (1) 3.2 Kinetic Theory of Gases 96 (13) 3.2.1 Graphical plots representing ideal behaviour 97 (3) 3.2.2 Deviation from ideal gas behaviour 100 (3) 3.2.3 Nature of gas 103 (6) 4 Chemical Thermodynamics 109 (38) 4.1 Energy Changes in Chemical Reactions 110 (25) 4.1.1 Standard enthalpy changes 113 (4) 4.1.2 Calculating enthalpy changes from experimental data 117 (5) 4.1.3 Calculation of enthalpy changes using Hess' Law 122 (1) 4.1.4 Constructing energy cycles 123 (4) 4.1.5 Born��Haber cycle and Hess' law 127 (2) 4.1.6 Constructing Born��Haber cycles 129 (4) 4.1.7 Energetics involving aqueous ionic compounds 133 (2) 4.2 Entropy 135 (12) 4.2.1 What is entropy? 137 (1) 4.2.2 Factors affecting entropy of a chemical system 138 (3) 4.2.3 Predicting the spontaneity of a reaction 141 (1) 4.2.4 Relationship between ΔG&theta, &DeltaHtheta, ΔStheta and temperature 142 (5) 5 Reaction Kinetics 147 (50) 5.1 Qualitative Analysis of Reaction Rates 147 (8) 5.1.1 Factors affecting reaction rates 150 (5) 5.2 Quantitative Analysis of Reaction Rates 155 (27) 5.2.1 Rate of reaction 155 (4) 5.2.2 The rate equation (Rate law) 159 (5) 5.2.3 Experimental methods used to determine order of reaction 164 (18) 5.3 Rate Equation and Reaction Mechanism 182 (2) 5.4 Transition State Theory 184 (3) 5.5 Catalysis 187 (10) 5.5.1 Homogeneous catalysis 187 (1) 5.5.2 Heterogeneous catalysis 188 (2) 5.5.3 Autocatalysis 190 (1) 5.5.4 Enzymes (biological catalysts) 191 (6) 6 Chemical Equilibria 197 (34) 6.1 Reversible Reactions 197 (2) 6.2 Equilibrium Systems 199 (1) 6.3 Equilibrium Constants IC, and Kp 200 (11) 6.3.1 Writing Kc or Kp for heterogeneous equilibria 204 (1) 6.3.2 Calculations involving Kc 205 (3) 6.3.3 Calculations involving Kp 208 (3) 6.4 Le Chatelier's Principle 211 (15) 6.4.1 Effect of concentration changes 211 (3) 6.4.2 Effect of pressure changes 214 (6) 6.4.3 Effect of temperature changes 220 (2) 6.4.4 Effect of temperature changes on the value of the equilibrium constant 222 (1) 6.4.5 Effect of catalyst 223 (3) 6.5 The Haber Process 226 (5) 7 Ionic Equilibria 231 (72) 7.1 The Bronsted-Lowry Theory of Acids and Bases 232 (2) 7.2 Conjugate Acid-Base Pairs 234 (1) 7.3 The pH Scale 234 (1) 7.4 The Dissociation Constant of Water, Kw 235 (5) 7.5 Strength of Acids 240 (1) 7.6 Acid Dissociation Constant Ka and pKa 241 (5) 7.7 Strength of Bases 246 (1) 7.8 Base Dissociation Constant Kb and pKb 247 (2) 7.9 Complementary Strengths of a Conjugate Acid-Base Pair 249 (2) 7.10 Hydration and Hydrolysis 251 (5) 7.10.1 Classifying type of salt based on strengths of acid and base that form it 253 (2) 7.10.2 Hydrolysis of high charge density cations 255 (1) 7.11 Buffer Solutions 256 (7) 7.11.1 How does an acidic buffer work 256 (2) 7.11.2 How does an alkaline buffer work 258 (1) 7.11.3 The role of buffer in controlling pH in blood 259 (1) 7.11.4 Calculating pH of buffer solutions 260 (3) 7.12 Acid-Base Indicators 263 (3) 7.13 Acid-Base Titrations 266 (24) 7.13.1 Titration curve of a strong acid-strong base titration 268 (1) 7.13.2 Titration curve of a weak acid-strong base titration 269 (7) 7.13.3 Titration curve of a strong acid��weak base titration 276 (2) 7.13.4 Titration curve of a weak acid��weak base titration 278 (2) 7.13.5 Titration curve of a polybasic acid��strong base titration 280 (1) 7.13.6 Titration curve of a carbonate��strong acid titration (Double-Indicator Method) 281 (5) 7.13.7 Titration curve of a mixture of weak acids strong base titration 286 (2) 7.13.8 Back-titration 288 (2) 7.14 Solubility Product Ksp 290 (13) 7.14.1 Solubility and K8p 291 (2) 7.14.2 Ionic product and Ksp 293 (2) 7.14.3 Common ion effect 295 (2) 7.14.4 Solubility in qualitative analysis 297 (6) 8 Redox Chemistry and Electrochemical Cells 303 (54) 8.1 Rules for Assignment of Oxidation States 307 (3) 8.2 Balancing Redox Equations 310 (3) 8.3 Redox Titrations 313 (5) 8.3.1 Manganate(VII) titrations 314 (1) 8.3.2 Dichromate(VI) titrations 315 (1) 8.3.3 Iodine-thiosulfate titrations 316 (2) 8.4 Redox Reactions and Electricity 318 (20) 8.4.1 Electrode potential 319 (3) 8.4.2 Experimental set-up of half-cells 322 (3) 8.4.3 Information obtained from the standard electrode potential 325 (3) 8.4.4 Describing cell components using conventional notation 328 (2) 8.4.5 Calculating standard cell potential 330 (2) 8.4.6 Using Ethetacell to predict feasibility of a reaction 332 (3) 8.4.7 Effect of concentration changes on Ethetacell value 335 (2) 8.4.8 Effect of ligands on Ethetacell value 337 (1) 8.5 Types of Electrochemical Cells 338 (3) 8.6 Electrolysis 341 (16) 8.6.1 Faraday's laws of electrolysis 342 (3) 8.6.2 Selective discharge of ions 345 (2) 8.6.3 Industrial uses of electrolysis 347 (10) 9 The Periodic Table �� Chemical Periodicity 357 (24) 9.1 Atomic Structure and Period 3 Elements 359 (5) 9.1.1 Trend in atomic radius 359 (2) 9.1.2 Trend in ionic radius 361 (1) 9.1.3 Trend in first ionisation energy (1st I.E.) 362 (1) 9.1.4 Trend in electronegativity 363 (1) 9.2 Structure, Bonding and Period 3 Elements 364 (2) 9.2.1 Variation in melting points and boiling points 364 (1) 9.2.2 Variation in electrical conductivity 365 (1) 9.3 Oxides and Chlorides of Period 3 Elements 366 (15) 9.3.1 Oxides of Period 3 elements 369 (4) 9.3.2 Chlorides of Period 3 elements 373 (8) 10 Chemistry of Groups 2 and 7 381 (40) 10.1 Atomic Structure and Group Trends 381 (3) 10.1.1 Trend in atomic radius 381 (1) 10.1.2 Trend in ionic radius 382 (1) 10.1.3 Trend in 1st I.E. 382 (1) 10.1.4 Trend in electron affinity 382 (1) 10.1.5 Trend in electronegativity 383 (1) 10.1.6 Trend in metallic character 383 (1) 10.2 Physical Properties of Group 2 Elements 384 (1) 10.3 Chemical Properties of Group 2 Elements 384 (3) 10.3.1 Reaction with water 386 (1) 10.3.2 Reaction with oxygen 387 (1) 10.4 Thermal Stability of Group 2 Compounds 387 (4) 10.5 Some Uses of Group 2 Elements and Their Compounds 391 (1) 10.6 Properties of Beryllium 391 (3) 10.7 Solubility of Group 2 Compounds 394 (3) 10.8 Physical Properties of Group 7 Elements 397 (3) 10.8.1 Melting point, boiling point and volatility 397 (1) 10.8.2 Colour 398 (1) 10.8.3 Solubility in water 399 (1) 10.8.4 Solubility in organic solvent 399 (1) 10.8.5 Trend in bond energy 400 (1) 10.9 Chemical Properties of Group 7 Elements 400 (9) 10.9.1 Displacement reaction of halogens 402 (1) 10.9.2 Reaction with thiosulfate 403 (3) 10.9.3 Reaction with alkali 406 (2) 10.9.4 Reaction with hydrogen 408 (1) 10.10 Hydrogen Halides 409 (6) 10.10.1 Thermal stability of hydrogen halides 410 (1) 10.10.2 Acidity of hydrogen halides 411 (1) 10.10.3 Reaction of halides with concentrated acid 411 (2) 10.10.4 Distinguishing tests for halide ions 413 (2) 10.11 Industrial Uses and Environmental Impact of Group 7 Elements and Their Compounds 415 (6) 10.11.1 Fluorine and its compounds 415 (1) 10.11.2 Chlorine and its compounds 415 (1) 10.11.3 Bromine and its compounds 415 (6) 11 Introduction to Transition Metals and Their Chemistry 421 (44) 11.1 Writing Electronic Configuration 422 (3) 11.2 Physical Properties of Transition Metals 425 (5) 11.2.1 Trend in atomic radius 425 (1) 11.2.2 Trend in ionic radius 426 (1) 11.2.3 Trend in first ionisation energy 427 (1) 11.2.4 Trend in melting and boiling points 428 (1) 11.2.5 Trend in electrical conductivity 429 (1) 11.2.6 Trend in density 429 (1) 11.3 Chemical Properties of Transition Metals 430 (35) 11.3.1 Variable oxidation states 430 (4) 11.3.2 Catalytic properties 434 (3) 11.3.3 Formation of complexes 437 (7) 11.3.4 The property of colour 444 (7) 11.3.5 Ligand exchange reactions 451 (7) 11.3.6 Selected reactions of some transition metals and their compounds 458 (7) Index 465

Summary: Written for students taking either the University of Cambridge A-level examinations or the International Baccalaureate examinations, this textbook covers essential topics under both stipulated chemistry syllabi. It is written in such a way as to guide the reader through the understanding and applications of essential chemical concepts by introducing a discourse feature-the asking and answering of questions-that stimulates coherent thinking and hence, elucidates ideas. Based on the Socratic Method, questions are implanted throughout the book to help facilitate the reader's development in forming logical conclusions of concepts. The book helps students to master fundamental chemical concepts in a simple way.

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Preface v
Acknowledgements vii
1 Atomic Structure and the Periodic Table 1 (28)
1.1 The Subatomic Particles of Matter
1 (5)
1.1.1 Behaviour in an electric field/magnetic field
1 (2)
1.1.2 Isotopes
3 (1)
1.1.3 Relative masses of an element
4 (2)
1.2 Orbitals and Quantum Numbers
6 (6)
1.2.1 The nature of electron
6 (4)
1.2.2 Shapes of orbitals
10 (2)
1.3 Electronic Configurations
12 (4)
1.3.1 Rules used in working out electronic configuration
12 (3)
1.3.2 Electronic configuration of transition elements
15 (1)
1.3.3 Anomalous electronic configurations
16 (1)
1.4 Ionisation Energies
16 (6)
1.4.1 Factors influencing the magnitude of ionisation energies
17 (5)
1.5 Periodic Table: Trend in Ionisation Energy
22 (2)
1.6 Periodic Table: Trend in Atomic Radii
24 (5)
2 Chemical Bonding 29 (52)
2.1 Metallic Bonding
29 (2)
2.1.1 Physical properties of metals
30 (1)
2.2 Ionic Bonding (or Electrovalent Bonding)
31 (8)
2.2.1 Guidelines for drawing dot-and-cross diagrams
34 (1)
2.2.2 Physical properties of ionic compounds
35 (4)
2.3 Covalent Bonding
39 (19)
2.3.1 Covalent bond formation
40 (2)
2.3.2 Dative covalent bond (coordinate bond)
42 (2)
2.3.3 Factors affecting strength of covalent bond
44 (2)
2.3.4 Shapes of molecules -- The VSEPR model
46 (6)
2.3.5 Using the Hybridisation Model to understand shape
52 (4)
2.3.6 Delocalised bonding/resonance
56 (2)
2.4 Intermediate Bond Types
58 (4)
2.4.1 Covalent character in ionic bonds
58 (2)
2.4.2 Ionic character in covalent bonds
60 (2)
2.5 Physical Properties of Covalent Compounds
62 (2)
2.5.1 Properties of giant covalent compounds
62 (2)
2.5.2 Properties of simple covalent compounds
64 (1)
2.6 Intermolecular Forces of Attraction
64 (10)
2.6.1 Instantaneous dipole��induced dipole (id��id) interactions
65 (2)
2.6.2 Permanent dipole-permanent dipole (pd��pd) interactions
67 (3)
2.6.3 Hydrogen bonding
70 (4)
2.7 Summary of Chemical Bonding: Putting it all Together
74 (7)
3 Ideal Gas and Gas Laws 81 (28)
3.1 Gas Laws
82 (14)
3.1.1 Boyle's law
82 (1)
3.1.2 Charles' law
83 (1)
3.1.3 Gay-Lussac's law
84 (1)
3.1.4 Avogadro's law
84 (4)
3.1.5 The ideal gas law
88 (2)
3.1.6 Further manipulations of the ideal gas equation
90 (1)
3.1.7 Dalton's Law of Partial Pressure
91 (4)
3.1.8 Types of mathematical problems involving the gas laws
95 (1)
3.2 Kinetic Theory of Gases
96 (13)
3.2.1 Graphical plots representing ideal behaviour
97 (3)
3.2.2 Deviation from ideal gas behaviour
100 (3)
3.2.3 Nature of gas
103 (6)
4 Chemical Thermodynamics 109 (38)
4.1 Energy Changes in Chemical Reactions
110 (25)
4.1.1 Standard enthalpy changes
113 (4)
4.1.2 Calculating enthalpy changes from experimental data
117 (5)
4.1.3 Calculation of enthalpy changes using Hess' Law
122 (1)
4.1.4 Constructing energy cycles
123 (4)
4.1.5 Born��Haber cycle and Hess' law
127 (2)
4.1.6 Constructing Born��Haber cycles
129 (4)
4.1.7 Energetics involving aqueous ionic compounds
133 (2)
4.2 Entropy
135 (12)
4.2.1 What is entropy?
137 (1)
4.2.2 Factors affecting entropy of a chemical system
138 (3)
4.2.3 Predicting the spontaneity of a reaction
141 (1)
4.2.4 Relationship between ΔG&theta, &DeltaHtheta, ΔStheta and temperature
142 (5)
5 Reaction Kinetics 147 (50)
5.1 Qualitative Analysis of Reaction Rates
147 (8)
5.1.1 Factors affecting reaction rates
150 (5)
5.2 Quantitative Analysis of Reaction Rates
155 (27)
5.2.1 Rate of reaction
155 (4)
5.2.2 The rate equation (Rate law)
159 (5)
5.2.3 Experimental methods used to determine order of reaction
164 (18)
5.3 Rate Equation and Reaction Mechanism
182 (2)
5.4 Transition State Theory
184 (3)
5.5 Catalysis
187 (10)
5.5.1 Homogeneous catalysis
187 (1)
5.5.2 Heterogeneous catalysis
188 (2)
5.5.3 Autocatalysis
190 (1)
5.5.4 Enzymes (biological catalysts)
191 (6)
6 Chemical Equilibria 197 (34)
6.1 Reversible Reactions
197 (2)
6.2 Equilibrium Systems
199 (1)
6.3 Equilibrium Constants IC, and Kp
200 (11)
6.3.1 Writing Kc or Kp for heterogeneous equilibria
204 (1)
6.3.2 Calculations involving Kc
205 (3)
6.3.3 Calculations involving Kp
208 (3)
6.4 Le Chatelier's Principle
211 (15)
6.4.1 Effect of concentration changes
211 (3)
6.4.2 Effect of pressure changes
214 (6)
6.4.3 Effect of temperature changes
220 (2)
6.4.4 Effect of temperature changes on the value of the equilibrium constant
222 (1)
6.4.5 Effect of catalyst
223 (3)
6.5 The Haber Process
226 (5)
7 Ionic Equilibria 231 (72)
7.1 The Bronsted-Lowry Theory of Acids and Bases
232 (2)
7.2 Conjugate Acid-Base Pairs
234 (1)
7.3 The pH Scale
234 (1)
7.4 The Dissociation Constant of Water, Kw
235 (5)
7.5 Strength of Acids
240 (1)
7.6 Acid Dissociation Constant Ka and pKa
241 (5)
7.7 Strength of Bases
246 (1)
7.8 Base Dissociation Constant Kb and pKb
247 (2)
7.9 Complementary Strengths of a Conjugate Acid-Base Pair
249 (2)
7.10 Hydration and Hydrolysis
251 (5)
7.10.1 Classifying type of salt based on strengths of acid and base that form it
253 (2)
7.10.2 Hydrolysis of high charge density cations
255 (1)
7.11 Buffer Solutions
256 (7)
7.11.1 How does an acidic buffer work
256 (2)
7.11.2 How does an alkaline buffer work
258 (1)
7.11.3 The role of buffer in controlling pH in blood
259 (1)
7.11.4 Calculating pH of buffer solutions
260 (3)
7.12 Acid-Base Indicators
263 (3)
7.13 Acid-Base Titrations
266 (24)
7.13.1 Titration curve of a strong acid-strong base titration
268 (1)
7.13.2 Titration curve of a weak acid-strong base titration
269 (7)
7.13.3 Titration curve of a strong acid��weak base titration
276 (2)
7.13.4 Titration curve of a weak acid��weak base titration
278 (2)
7.13.5 Titration curve of a polybasic acid��strong base titration
280 (1)
7.13.6 Titration curve of a carbonate��strong acid titration (Double-Indicator Method)
281 (5)
7.13.7 Titration curve of a mixture of weak acids strong base titration
286 (2)
7.13.8 Back-titration
288 (2)
7.14 Solubility Product Ksp
290 (13)
7.14.1 Solubility and K8p
291 (2)
7.14.2 Ionic product and Ksp
293 (2)
7.14.3 Common ion effect
295 (2)
7.14.4 Solubility in qualitative analysis
297 (6)
8 Redox Chemistry and Electrochemical Cells 303 (54)
8.1 Rules for Assignment of Oxidation States
307 (3)
8.2 Balancing Redox Equations
310 (3)
8.3 Redox Titrations
313 (5)
8.3.1 Manganate(VII) titrations
314 (1)
8.3.2 Dichromate(VI) titrations
315 (1)
8.3.3 Iodine-thiosulfate titrations
316 (2)
8.4 Redox Reactions and Electricity
318 (20)
8.4.1 Electrode potential
319 (3)
8.4.2 Experimental set-up of half-cells
322 (3)
8.4.3 Information obtained from the standard electrode potential
325 (3)
8.4.4 Describing cell components using conventional notation
328 (2)
8.4.5 Calculating standard cell potential
330 (2)
8.4.6 Using Ethetacell to predict feasibility of a reaction
332 (3)
8.4.7 Effect of concentration changes on Ethetacell value
335 (2)
8.4.8 Effect of ligands on Ethetacell value
337 (1)
8.5 Types of Electrochemical Cells
338 (3)
8.6 Electrolysis
341 (16)
8.6.1 Faraday's laws of electrolysis
342 (3)
8.6.2 Selective discharge of ions
345 (2)
8.6.3 Industrial uses of electrolysis
347 (10)
9 The Periodic Table �� Chemical Periodicity 357 (24)
9.1 Atomic Structure and Period 3 Elements
359 (5)
9.1.1 Trend in atomic radius
359 (2)
9.1.2 Trend in ionic radius
361 (1)
9.1.3 Trend in first ionisation energy (1st I.E.)
362 (1)
9.1.4 Trend in electronegativity
363 (1)
9.2 Structure, Bonding and Period 3 Elements
364 (2)
9.2.1 Variation in melting points and boiling points
364 (1)
9.2.2 Variation in electrical conductivity
365 (1)
9.3 Oxides and Chlorides of Period 3 Elements
366 (15)
9.3.1 Oxides of Period 3 elements
369 (4)
9.3.2 Chlorides of Period 3 elements
373 (8)
10 Chemistry of Groups 2 and 7 381 (40)
10.1 Atomic Structure and Group Trends
381 (3)
10.1.1 Trend in atomic radius
381 (1)
10.1.2 Trend in ionic radius
382 (1)
10.1.3 Trend in 1st I.E.
382 (1)
10.1.4 Trend in electron affinity
382 (1)
10.1.5 Trend in electronegativity
383 (1)
10.1.6 Trend in metallic character
383 (1)
10.2 Physical Properties of Group 2 Elements
384 (1)
10.3 Chemical Properties of Group 2 Elements
384 (3)
10.3.1 Reaction with water
386 (1)
10.3.2 Reaction with oxygen
387 (1)
10.4 Thermal Stability of Group 2 Compounds
387 (4)
10.5 Some Uses of Group 2 Elements and Their Compounds
391 (1)
10.6 Properties of Beryllium
391 (3)
10.7 Solubility of Group 2 Compounds
394 (3)
10.8 Physical Properties of Group 7 Elements
397 (3)
10.8.1 Melting point, boiling point and volatility
397 (1)
10.8.2 Colour
398 (1)
10.8.3 Solubility in water
399 (1)
10.8.4 Solubility in organic solvent
399 (1)
10.8.5 Trend in bond energy
400 (1)
10.9 Chemical Properties of Group 7 Elements
400 (9)
10.9.1 Displacement reaction of halogens
402 (1)
10.9.2 Reaction with thiosulfate
403 (3)
10.9.3 Reaction with alkali
406 (2)
10.9.4 Reaction with hydrogen
408 (1)
10.10 Hydrogen Halides
409 (6)
10.10.1 Thermal stability of hydrogen halides
410 (1)
10.10.2 Acidity of hydrogen halides
411 (1)
10.10.3 Reaction of halides with concentrated acid
411 (2)
10.10.4 Distinguishing tests for halide ions
413 (2)
10.11 Industrial Uses and Environmental Impact of Group 7 Elements and Their Compounds
415 (6)
10.11.1 Fluorine and its compounds
415 (1)
10.11.2 Chlorine and its compounds
415 (1)
10.11.3 Bromine and its compounds
415 (6)
11 Introduction to Transition Metals and Their Chemistry 421 (44)
11.1 Writing Electronic Configuration
422 (3)
11.2 Physical Properties of Transition Metals
425 (5)
11.2.1 Trend in atomic radius
425 (1)
11.2.2 Trend in ionic radius
426 (1)
11.2.3 Trend in first ionisation energy
427 (1)
11.2.4 Trend in melting and boiling points
428 (1)
11.2.5 Trend in electrical conductivity
429 (1)
11.2.6 Trend in density
429 (1)
11.3 Chemical Properties of Transition Metals
430 (35)
11.3.1 Variable oxidation states
430 (4)
11.3.2 Catalytic properties
434 (3)
11.3.3 Formation of complexes
437 (7)
11.3.4 The property of colour
444 (7)
11.3.5 Ligand exchange reactions
451 (7)
11.3.6 Selected reactions of some transition metals and their compounds
458 (7)
Index 465

Written for students taking either the University of Cambridge A-level examinations or the International Baccalaureate examinations, this textbook covers essential topics under both stipulated chemistry syllabi. It is written in such a way as to guide the reader through the understanding and applications of essential chemical concepts by introducing a discourse feature-the asking and answering of questions-that stimulates coherent thinking and hence, elucidates ideas. Based on the Socratic Method, questions are implanted throughout the book to help facilitate the reader's development in forming logical conclusions of concepts. The book helps students to master fundamental chemical concepts in a simple way.

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