*describe the number and relative energies of the s, p and d orbitals for the principal quantum numbers 1, 2 and 3 and also the 4s and 4p orbitals.
*describe the shapes of s and p orbitals
explain and use the term ionisation energy (energy required to remove outermost electron to infinity in gas phase).
(i) The shapes of simple molecules
*explain the shapes of, and bond angles in, molecules by using the qualitative model of electron-pair repulsion (including lone pairs), using as simple examples: BF3 (trigonal); CO2 (linear); CH4 (tetrahedral); NH3 (pyramidal); H2O (non-linear); SF6 (octahedral)
*describe covalent bonding in terms of orbital overlap, giving σ and π bonds
(e) *explain the shape of, and bond angles in, the ethane (edit: they are 109.5), ethene ( edit: 122 HC=C and 117 HCH) and benzene (edit: 120 degrees each).molecules in terms of σ and π bonds (see also Section 10.1)
state the basic assumptions of the kinetic theory as applied to an ideal gas the conditions necessary for a gas to approach ideal behaviour (deviates from Ideal behavior due to high pressure, low temperature leading to molecules turning into liquid, molecules are heavy, molecules are attractive)
Define
I Enthalpy changes: ∆H of formation, combustion, hydration, solution, neutralisation and atomisation; bond energy; lattice energy; electron affinity.
construct and interpret a reaction pathway diagram, in terms of the enthalpy change of the reaction and of the activation energy (see Section 8)
*state Le Chatelier’s Principle (the principle that if any change is imposed on a system that is in equilibrium then the system tends to adjust to a new equilibrium counteracting the change).
deduce expressions for equilibrium constants in terms of partial pressures, Kp (
http://www.chemguide.co.uk/physical/equilibria/kp.html)
show understanding of, and use the Brønsted-Lowry theory of acids and bases (proton donator is acid, proton acceptor is base).
*show understanding, including reference to the Boltzmann distribution
interpret this catalytic effect in terms of the Boltzmann distribution
describe the reactions, if any, of the elements with oxygen (to give Na2O; MgO; Al2O3; P4O10; SO2; SO3), chlorine (to give NaCl; MgCl2; Al2Cl6; SiCl4; PCl5), and water (Na and Mg only)
describe the thermal decomposition of the GROUP II nitrates and carbonate
describe and explain the relative thermal stabilities of the GROUP VII hydride
describe and explain the reactions of halide ions with
(i) aqueous silver ions followed by aqueous ammonia
(ii) concentrated sulfuric acid
describe and interpret in terms of changes of oxidation number the reaction of chlorine with cold, and with hot, aqueous sodium hydroxide (Cold: NaOH + NaOCl), (Hot: NaCL + NaClO3)
Explain Flu Gas desulphurization (Use of Calcium Carbonate to form Calcium Sulphite + CO2)
*describe the mechanism of free-radical substitution at methyl groups with particular reference to the initiation, propagation and termination reactions
describe the chemistry of alkenes as exemplified, where relevant, by the following reactions of ethene:
(i) *addition of hydrogen, steam, hydrogen halides and halogens
(ii) *oxidation by cold, dilute, acidified manganate(VII) ions to form the diol
(iii) oxidation by hot, concentrated, acidified manganate(VII) ions leading to the rupture of the carbon-to-carbon double bond
in order to determine the position of alkene linkages in larger molecules the following nucleophilic substitution reactions of bromoethane: hydrolysis; formation of nitriles; formation of primary amines by reaction with ammonia
(ii) the elimination of hydrogen bromide from 2-bromopropane
Reaction of Alcohols with Sodium
Describe the reduction of aldehydes and ketones e.g. using NaBH4
describe the use of 2,4-dinitrophenylhydrazine (2,4-DNPH) reagent to detect the presence of carbonyl compounds
describe the formation of carboxylic acids from alcohols, aldehydes and nitriles
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