Syllabus

Last revision: July 2002

1. The atom
1.1. Introduction
1.1.1. Counting of nucleons1
1.1.2. Isotopes1
1.2. The hydrogen atom
1.2.1. Concept of energy levels 1
1.2.2. Shape of s-orbitals 1
1.2.3. (7.5) Shape and orientation of p-orbitals 1
1.2.4. (7.6) Shape and orientation of d-orbitals 3
1.2.5. (7.3) Understanding the simplest Schrödinger equation 3
1.2.6. (7.2) Square of the wave function and probability 3
1.2.7. (7.4) Quantum numbers (n, l, ml) 3
1.3. Radioactivity
1.3.1. Types of radioactivity 1
1.3.2. Radioactive decay1
1.3.3. Nuclear reactions2
2. Chemical bonding
2.1. VSEPR - Simple molecular structures with
2.1.1. no more than four electron pairs about central atom 1
2.1.2. with central atom exceeding the "octet rule" 3
2.2. Delocalization and resonance 3
2.3. Hybrid orbital theory 3
2.4. Molecular orbital theory
2.4.1. (7.7) molecular orbital diagram (H2 molecule) 3
2.4.2. (7.8) molecular orbital diagram (N2 and O2 molecules) 3
2.4.3. (7.9) bond orders in O2, O2-, O2+ 3
2.4.4. (7.10) unpaired electrons and paramagnetism 3
3. Chemical calculations
3.1.1. (1.6.1) Balancing equations 1
3.1.2. (1.6.2) Stoichiometric calculations 1
3.1.3. (1.6.3) Mass and volume relations (including density) 1
3.1.4. (1.6.4) Empirical fomula 1
3.1.5. (1.6.5) Avogadro's number 1
3.1.6. (1.6.6) Concentration calculations 1
4. Periodic trends
4.1. Electron configuration
4.1.1. (1.1.4) Pauli exclusion principle 1
4.1.2. (1.1.5) Hund's Rule1
4.1.3. (1.1.1) Main group elements 1
4.1.4. (1.1.2) Transition metal elements 1
4.1.5. (1.1.3) Lanthanide and actinide metals 3
4.2. (1.2.1) Electronegativity 1
4.3. (1.2.2) Electron affinity 2
4.4. (1.2.3) First ionization energy 1
4.5. (1.2.4) Atomic size 1
4.6. (1.2.5) Ion size 1
4.7. (1.2.6) Highest oxidation number 1
5. Inorganic Chemistry
5.1. Introduction
5.1.1. Trends in physical properties of elements (Main groups)
5.1.1.1. (1.3.1) melting point 1
5.1.1.2. (1.3.2) boiling point 1
5.1.1.3. (1.3.3) metal character 1
5.1.1.4. (1.3.4) magnetic properties 3
5.1.1.5. (1.3.7) electrical conductivity 2
5.1.2. (1.5.1) Oxidation number 1
5.1.3. Nomenclature1
5.1.3.1. (1.5.2) main group compounds 1
5.1.3.2. (1.5.3) transition metal compounds 1
5.1.3.3. (1.5.4) simple metal complexes 3
5.2. Groups 1 and 2
5.2.1. (1.9.2) Trend in reactivity of (heavy elements more reactive) 1
5.2.2. Products of reaction with
5.2.2.1. (1.9.1.1) water1
5.2.2.2. halogens1
5.2.2.3. (1.9.9.3) oxygen2
5.2.3. Basicity of oxides1
5.2.4. (1.10.2) Properties of hydrides 3
5.2.5. Other compounds, properties and oxidation states 3
5.3. Groups 13 - 18 and Hydrogen
5.3.1. Binary molecular compounds of hydrogen
5.3.1.1. (1.10.1) Formulae1
5.3.1.2. (1.10.3) Acid-base properties of CH4, NH3, H2O, H2S 1
5.3.1.3. Other properties3
5.3.2. Group 13
5.3.2.1. (1.10.14) The oxidation state of boron and aluminium in their oxides and chlorides is +3 1
5.3.2.2. The acid-base properties of aluminium oxide/hydroxide 2
5.3.2.3. Reaction of boron(III) oxide with water 3
5.3.2.4. Reaction of boron(III) chloride with water 3
5.3.2.5. Other compounds, properties and oxidation states 3
5.3.3. Group 14
5.3.3.1. (1.10.14) The oxidation state of Si in its chloride and oxide is +4 1
5.3.3.2. (1.10.16) The +2 and +4 oxidation states of carbon tin and lead, the acid-base and redox properties of the oxides and chlorides 2
5.3.3.3. Other compounds, properties and oxidation states 3
5.3.4. Group 15
5.3.4.1. (1.10.17) Phosphorus(+5) oxide and chloride, and their reaction with water 2
5.3.4.2. Phosphorus(+3) oxide and chloride, and their reaction with water 2
5.3.4.3. Oxides of nitrogen
a (1.10.4) Reaction of NO to form NO2 1
b (1.10.5) Dimerization of NO2 1
c (1.10.6) Reaction of NO2 with water 1
5.3.4.4. Redox properties of
a (1.10.8) HNO3 and nitrates 1
b (1.10.9 and 7) HNO2 and NH2NH2 3
5.3.4.5. (1.10.16) Bi(+5) and Bi(+3) 3
5.3.4.6. Other compounds, properties and oxidation states 3
5.3.5. Group 16
5.3.5.1. (1.10.14) The +4 and +6 oxidation states of sulfur, reaction of their oxides with water, properties of their acids 1
5.3.5.2. (1.10.12) Reaction of thiosulfate anion with I2 3
5.3.5.3. Other compounds, properties and oxidation states 3
5.3.6. Group 17 (Halogens)
5.3.6.1. (1.10.19) Reactivity and oxidant strength decreases from F2 to I2 1
5.3.6.2. Acid-base properties of the hydrogen halides 1
5.3.6.3. (1.10.14) The oxidation state of fluorine in its compounds is -1 1
5.3.6.4. (1.10.14) The -1, +1, +3, +5, +7 oxidation states of chlorine 1
5.3.6.5. Mononuclear oxoanions of chlorine 2
5.3.6.6. (1.10.18) Reactions of halogens with water 3
5.3.6.7. (1.10.14) Reaction of Cl2O and Cl2O7 with water 3
5.3.6.8. Other compounds, properties and oxidation states 3
5.3.7. (1.12.3) Group 183
5.4. Transition elements
5.4.1. (1.11.1) Common oxidation states of common transition metals 1
Cr(+2), Cr(+3) Mn(+2), Mn(+4), Mn(+7) Ag(+1)
Fe(+2), Fe(+3) Co(+2) Zn(+2)
Hg(+1), Hg(+2) Cu(+1), Cu(+2) Ni(+2)
5.4.2. (1.11.2) Colours of ions listed above in aqueous solution 2
5.4.3. (1.11.4) Insolubility of Ag, Hg and Cu don't in HCl 2
5.4.4. (1.11.5) M2+ arising by dissolution of the other metals in HCl 2
5.4.5. (1.11.7) Cr(OH)3 and Zn(OH)2 are amphoteric and the other +2 oxides/hydroxides of the metals listed above are basic 2
5.4.6. (1.11.8) MnO4- and Cr2O72- are strong oxidants in acid solution 1
5.4.7. (1.11.9) pH dependence of products of MnO4- acting as oxidant 2
5.4.8. (1.11.10??) Interconversion between CrO42- and Cr2O72- 3
5.4.9. Other compounds, properties and oxidation states 3
5.5. (1.12.2) Lanthanides and actinides 3
5.6. Coordination chemistry including stereochemistry
5.6.1. (6.2) Definition of coordination number 1
5.6.2. (6.1) Writing equations for complexation reactions given all formulae 1
5.6.3. Formulae of common complex ions
5.6.3.1. Ag(NH3)2+ 1
5.6.3.2. Ag(S2O3)22- 3
5.6.3.3. FeSCN2+3
5.6.3.4. Cu(NH3)42+ 1
5.6.3.5. Other complex ions3
5.6.4. (6.5) Ligand field theory (eg and t2g terms, high and low spin) 3
5.6.5. Stereochemistry
5.6.5.1. (6.7) cis and trans 3
5.6.5.2. enantiomers3
5.7. Selected industrial processes
5.7.1. (1.12.1) Preparation of H2SO4 1
5.7.2. (1.12.1) Preparation of NH3 1
5.7.3. (1.12.1) Preparation of Na2CO3 2
5.7.4. (1.12.1) Preparation of Cl2 and NaOH 2
5.7.5. Preparation of HNO3 2
6. Physical chemistry
6.1. Gases
6.1.1. (2.7.1) Ideal gas law 1
6.1.2. (2.7.2) van der Waal's gas law 3
6.1.3. (2.7.3) definition of partial pressure 2
6.1.4. Dalton's Law3
6.2. Thermodynamics
6.2.1. First Law
6.2.1.1. (2.5.1) Concept of system and surroundings 2
6.2.1.2. (2.5.2) Energy, heat and work 2
6.2.2. Enthalpy
6.2.2.1. (2.5.3) Relationship between internal energy and enthalpy 3
6.2.2.2. (2.5.4) Definition of heat capacity 2
6.2.2.3. (2.5.5) Difference between Cp and Cv (ideal gas only) 3
6.2.2.4. (2.5.6) That enthalpy is a state property (Hess's Law) 2
6.2.2.5. (2.5.7) Born-Haber cycle for ionic compounds 3
6.2.2.6. (2.5.9) Use of standard formation enthalpies 2
6.2.2.7. (2.5.10) Enthalpies of solution and solvation 3
6.2.2.8. (2.5.11) Bond enthalpies (definition and use) 2
6.2.3. Second Law (Entropy and Free Energy)
6.2.3.1. (2.6.1) Entropy definition (dq/T) 3
6.2.3.2. (2.6.2) Entropy and disorder 2
6.2.3.3. (2.6.3) Entropy definition (S = k ln W) 3
6.2.3.4. (2.6.4) Free energy definition (DG = DH - TDS) 3
6.2.3.5. (2.6.5) Using DG to predict direction of natural change 3
6.2.3.6. (2.1.5) Relationship of DG0 and equilibrium constant K 3
6.3. Equilibrium
6.3.1. Acid-base
6.3.1.1. (2.2.1) Arrhenius definitions of acids and bases 1
6.3.1.2. (2.2.2) Brønsted-Lowry definitions, 1
6.3.1.3. (2.2.2) conjugate acids and bases 1
6.3.1.4. (2.2.3) pH definition 1
6.3.1.5. (2.2.4) Kw definition 1
6.3.1.6. (2.2.5) Ka as a measure of acid and base strength 1
6.3.1.7. (2.2.6) Acidity or basicity of ions 1
6.3.1.8. (2.2.9) Calculation of pH from pKa(weak acid) 1
6.3.1.9. (5.4) Calculation of pH of a simple buffer solution 2
6.3.2. Gas phase
6.3.2.1. (2.1.4) Equilibrium constant in partial pressures 3
6.3.2.2. (2.1.3) Relating Kp and Kc 3
6.3.3. Solubility
6.3.3.1. (2.2.7) Solubility constant (product) definition (Ks) 2
6.3.3.2. (2.2.8) Calculation of solubility in water from Ks 2
6.3.4. Compleximetric
6.3.4.1. (6.4) Complex formation constant (definition) 3
6.3.4.2. Problems involving compleximetric equilibria 3
6.3.4.3. (7.12) Lewis acids and bases 3
6.3.4.4. (7.13) Hard and soft Lewis acids and bases 3
6.3.5. Phase
6.3.5.1. (2.7.4) Temperature dependence of vapour pressure 3
6.3.5.2. (2.7.5) Clausius-Clapeyron equation 3
6.3.5.3. Single component phase diagrams
a (2.7.6) triple point3
b (2.7.7) critical point) 3
6.3.5.4. liquid-vapour system
a (2.7.9) ideal and nonideal systems 3
b (2.7.8) diagram3
c (2.7.9) use in fractional distillation 3
6.3.5.5. (2.7.11) Henry's Law3
6.3.5.6. (2.7.12) Raoult's Law 3
6.3.5.7. (2.7.13) Deviation from Raoult's Law 3
6.3.5.8. (2.7.14) Boiling point elevation 3
6.3.5.9. (2.7.15) Freezing point depression 3
6.3.5.10. (2.7.16) Osmotic pressure 3
6.3.5.11. (2.7.17) Partition coefficient 3
6.3.5.12. (2.7.18) Solvent extraction 3
6.3.6. Multiple
6.3.6.1. (2.2.11) Calculation of pH for multiprotic acids 3
6.3.6.2. (2.2.12) Calculation of pH for weak acid mixtures 3
6.4. Electrochemistry
6.4.1. (2.3.1) Electromotive force (definition) 1
6.4.2. (2.3.2) First kind electrodes 1
6.4.3. (2.3.3) Standard electrode potential 1
6.4.4. (2.3.4) Nernst equation 3
6.4.5. (2.3.5) Second kind electrodes 3
6.4.6. (2.3.6) Relationship between DG and electromotive force 3
7. Chemical kinetics (Homogeneous reactions)
7.1. Introduction
7.1.1. (2.4.1) Factors affecting reaction rate 1
7.1.2. (2.4.15) Reaction coordinates and the basic idea of a transition state 1
7.2. Rate law
7.2.1. (2.4.2) Differential rate law 2
7.2.2. (2.4.4) Concept of reaction order 2
7.2.3. (2.4.3) Rate constant definition 2
7.2.4. First order reactions
7.2.4.1. (2.4.5) Dependence of concentration on time 3
7.2.4.2. (2.4.6) Concept of half life 3
7.2.4.3. (2.4.7) Relationship between half life and rate constant 3
7.2.4.4. (2.4.11) Calculation of first order rate constant from
a Differential rate law 3
b Integrated rate law3
7.2.4.5. (2.4.12) Rate constant for second and third order reactions 3
7.3. Reaction mechanisms
7.3.1. (2.4.9) Concept of molecularity 3
7.3.2. (2.4.8) Rate-determining step 3
7.3.3. (2.4.14) Basic concepts of collision theory 3
7.3.4. (2.4.16) Opposing parallel and consecutive reactions 3
7.3.5. Arrhenius's law
7.3.5.1. (2.4.10) Definition of activation energy 3
7.3.5.2. (2.4.13) Calculation of activation energy 3
8. Spectroscopy
8.1. UV/visible
8.1.1. (8.1.1) Identification of aromatic compound 3
8.1.2. (8.1.2) Identification of chromophore 3
8.1.3. (3.11.10) Dyes: colour vs structure 3
8.1.4. (5.9) Beer's Law3
8.2. Infrared
8.2.1. (8.3.1) Interpretation using a table of frequencies 3
8.2.2. (8.3.2) Recognition of hydrogen bonds 3
8.3. x-Ray
8.3.1. (8.5.1) Bragg's Law3
8.3.2. Concept of
8.3.2.1. (8.5.3) coordination number 3
8.3.2.2. (8.5.1) unit cell3
8.3.3. Solid structures
8.3.3.1. (8.5.5) NaCl3
8.3.3.2. (8.5.6) CsCl3
8.3.3.3. (8.5.7) metals3
8.4. NMR
8.4.1. General Concepts
8.4.1.1. (8.4.2.) chemical shift 3
8.4.1.2. (8.4.2) spin-spin coupling and coupling constants 3
8.4.1.3. integration3
8.4.2. (8.4.1) Interpretation of a simple 1H spectrum (like ethanol) 3
8.4.3. (8.4.4) Identification of o- and p-disubstituted benzene 3
8.4.4. (8.4.5 +) Interpretation of simple spectra of 13C (proton decoupled) and other spin ½ nuclei 3
8.5. Mass spectrometry
8.5.1.1. (8.1.1) Recognition of molecular ion 3
8.5.1.2. (8.1.2) Recognition of fragments with the help of a table 3
8.5.1.3. (8.2.3) Recognition of typical isotope distribution 3
9. Organic Chemistry
9.1. Introduction
9.1.1. (3.1.1) Alkane naming (IUPAC) 1
9.1.2. Trends in boiling points of
9.1.2.1. (3.1.3) alkanes with structure 1
9.1.2.2. (3.7.1) alcohols vs ethers due to hydrogen-bonding 1
9.1.3. (3.3.1, 3.4.1) Geometry at singly, doubly, and triply bonded carbon 1
9.1.4. Identification of common functional groups 1
9.1.5. Isomerism of alkenes
9.1.5.1. (3.3.2) cis-trans 1
9.1.5.2. (3.3.2) E/Z 3
9.1.6. Enantiomers
9.1.6.1. (3.10.3.14) Optical activity 2
9.1.6.2. (3.10.3.14) R/S nomenclature 3
9.2. Reactivity
9.2.1. Alkanes
9.2.1.1. reaction with halogens
a (3.1.4.1) products1
b (3.1.4.2) free radical mechanism (initiation, termination) 2
9.2.1.2. Cycloalkanes
a (3.2.1) names2
b (3.2.2) Strain in small rings 3
c (3.2.3) chair/boat conformations of cyclohexane 3
9.2.2. Alkenes
9.2.2.1. (3.3.3.1) Products from Br2, HBr and H2O/H+ 1
9.2.2.2. (3.3.3.2) Markownikoff's rule 2
9.2.2.3. (3.3.3.3) Mechanism involving carbocation intermediates 3
9.2.2.4. (3.3.3.4) Relative stability of carbocations 3
9.2.2.5. (3.3.3.5) 1,4 addition to dienes 3
9.2.3. Alkynes
9.2.3.1. (3.4.2) Acidity relative to alkenes 3
9.2.3.2. (3.4.3) Differences in chemical properties from alkenes
9.2.4. Benzene
9.2.4.1. (3.5.1) formula1
9.2.4.2. (3.5.2 and 3) stabilization by resonance 1
9.2.4.3. electrophilic substitution (nitration, halogenation)
a (3.5.9) directing effect of first substituent 3
b (3.5.8) effect of first substituent on reactivity 3
c (3.5.10) explanation of substituent effects 3
9.2.5. Halogen compounds
9.2.5.1. Nomenclature of monofunctional 1
9.2.5.2. (3.6.1) Substitution reactions
a giving alcohols3
b (3.6.2) in which halogen is exchanged 3
c (3.6.3) reactivity
iprimary vs secondary vs tertiary 3
ii(3.6.6) aliphatic vs aromatic 3
d (3.6.4) SN1 and SN2 mechanisms 3
9.2.5.3. Elimination reactions 2
9.2.5.4. (3.6.5) Competition of elimination and substitution 2
9.2.6. Alcohols
9.2.6.1. Nomenclature of monofunctional 1
9.2.6.2. (3.7.1) Comparison of acidity of alcohols and phenols 2
9.2.6.3. (3.7.2) Dehydration to alkenes 1
9.2.6.4. Esters with inorganic acid 2
9.2.6.5. Oxidation reactions1
9.2.7. Adehydes and ketones
9.2.7.1. Nomenclature of monofunctional 1
9.2.7.2. Oxidation of aldehydes 1
9.2.7.3. Reduction to alcohols (LiAlH4, NaBH4) 3
9.2.7.4. Keto/enol tautomerism 3
9.2.7.5. Nucleophilic addition reactions with
a HCN3
b RNH2 (R = alkyl, HO, NH2) 3
c enolate anions (aldol condensation) 3
d alcohols to form acetals/ketals 3
e Grignard reagents3
9.2.8. Carboxylic acids and their derivatives
9.2.8.1. Nomenclature of carboxylic acids and their derivatives (esters, acid halides, amides) 2
9.2.8.2. Acidity strength related to inductive effects 3
9.2.8.3. Preparation of carboxylic acids by hydrolysis of
a esters (including soaps) 1
b amides2
c nitriles3
9.2.8.4. Reaction of carboxylic acids
a with alcohols to form esters 1
b to form acid chlorides 3
c to form anhydrides3
9.2.8.5. Reaction of acid chlorides to form amides 3
9.2.8.6. Mechanism of esterification 3
9.2.8.7. Multifunctional acids (hydroxyacids, ketoacids) 3
9.2.8.8. Polycarboxylic acids3
9.2.9. Amines
9.2.9.1. Nomenclature
a simple amines1
b recognition of primary, secondary, tertiary 1
9.2.9.2. Basicity
a As a property of an amine 1
b Comparison of basicity of aliphatic and aromatic 3
c Comparison of basicity of amines and amides 3
d Preparation of amines
i from halides3
iifrom aromatic nitro compounds 3
iii from amides (by hydrolysis) 3
9.2.9.3. Diazotization
a of aliphatic amines3
b of aromatic amines3
10. Polymers
10.1. Synthetic
10.1.1. Addition polymers
10.1.1.1. polystyrene2
10.1.1.2. polyethene1
10.1.1.3. chain mechanism of formation 2
10.1.2. Condensation polymers
10.1.2.1. polyesters2
10.1.2.2. polyamides2
10.1.3. Silicones3
10.1.4. Concept of cross-linking and its affect on properties 3
10.2. Natural
10.2.1. Silicates3
10.2.2. Rubber3
11. Biochemistry
11.1. Carbohydrates
11.1.1. Glucose and fructose
11.1.1.1. chain formulae1
11.1.1.2. Fischer projections2
11.1.1.3. Haworth formulae3
11.1.2. Difference between starch and cellulose 2
11.1.3. Difference between a- and b- D glucose 2
11.2. Fats
11.2.1. Structure of fats in relationship to properties 2
11.2.2. Formula of glycerol1
11.3. Nitrogen-containing Compounds of Biological Importance
11.3.1. Amino acids
11.3.1.1. Ionic structure1
11.3.1.2. Isoelectric point3
11.3.1.3. 20 amino acids (classification with structures provided) 2
11.3.1.4. Separation by electrophoresis 3
11.3.1.5. The peptide linkage1
11.3.2. Proteins
11.3.2.1. Primary structure1
11.3.2.2. -S-S- bridges3
11.3.2.3. Sequence analysis3
11.3.2.4. Secondary structure3
11.3.2.5. Details of a helix structure 3
11.3.2.6. Tertiary structure3
11.3.2.7. Denaturation (change in pH, temperature, metals, ethanol) 2
11.3.3. Nuclei Acids and Protein Synthesis
11.3.3.1. Pyrimidine and purine 3
11.3.3.2. Nucleosides and nucleotides 3
11.3.3.3. Formulae of pyrimidine and purine bases 3
11.3.3.4. Difference between ribose and 2-deoxyribose 3
11.3.3.5. Base combination CG and AT (hydrogen-bonding) 3
11.3.3.6. Difference between DNA and RNA 3
11.3.3.7. Difference between mRNA and tRNA 3
11.4. Enzymes
11.4.1.1. General properties, active centers 3
11.4.1.2. Nomenclature, kinetics, coenzymes, function of ATP 3
12. Analytical chemistry
12.1. Titrations
12.1.1. acid-base
12.1.1.1. (5.2) Titration curve; pH (strong and weak acid) 2
12.1.1.2. (5.1) Choice of indicators for acidimetry 2
12.1.2. (5.3) Redox titration 3
12.2. Qualitative analysis
12.2.1. Ions (Inorganic)
12.2.1.1. (5.5) Identification of Ag+, Ba2+, Cl-, SO42- 2
12.2.1.2. Identification of other anions and cations 3
12.2.2. Organic functional groups
12.2.2.1. (3.7.7) Lucas reagent (1°, 2°, 3° alcohols) 3
12.2.2.2. (3.7.6) Iodoform reaction 3
12.2.2.3. (3.11.4) Identification of primary, secondary, tertiary, quarternary amines in the laboratory 3
12.3. (2.7.19) Chromatographic methods of separation 3

 

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