Atoms and Molecules (i) The concept of atoms having fixed properties in explaining the laws of chemical combination.
(ii) Atomic and isotopic masses and their determinations by spectrometry.
(iii) Chemical equivalents, volumetric calculations in terms of normality. C = 12.00 should be taken as a standard for expressing atomic masses.
(iv) Relative molecular mass and mole. The following methods may be considered for the determination of relative molecular masses for the gases: the molar volume method; Victor Meyer's method.
Atomic Structure
(i) Electrons, Protons and Neutrons as fundamental particles, their charges and masses.
(ii) Rutherford 's nuclear model based on the scattering experiment.
(iii) Bohr's atomic model (No mathematical details are required).
(iv) Atomic structure: wave mechanical model- a simple non mathematical treatment. Quantum numbers; shape, size and orientation of s and p orbitals only. Hund's rule of maximum multiplicity. Pauli's exclusion principle, AUFBAU principle, electronic configuration of elements in terms of s, p, d, f subshells.
Periodic Table
(i) Atomic number (Proton number) as the basis for classification of the elements in the Periodic Table. IUPAC nomenclature for elements with Z> 100.
(ii) Extra nuclear structure as the basis ofperiodicity. Some idea of the following: ionisation potential, electron affinity, atomic radius, atomic volume, electronegativity, etc must be given. The periodicity of electronic structure leading to the periodicity of elements e.g the relative ease of ionisation of elements. (iii) Periodicity of elements with reference to s, p, d and f block elements.
Chemical Bonding
Electrovalent Bond
(i) Electrovalent or ionic bond e.g formation of NaCl, Li 2 O, MgO, CaO, MgF 2, and Na 2 S.
(ii) Factors influencing the formation of ionic bond, e.g electron affinity, lattice energy and electronegativity.
(iii) The relation between the ionic bonding and Periodic Table.
(iv) Variable electrovalency and its causes.
Covalent Bond
(i) Covalent bond, e.g. formation of ammonia, nitrogen, ethene, ethyne, and carbon dioxide.
(ii) Variable valency: chlorine exhibits the valency of 1,3,5 & 7 respectively.
(iii) Deviation from Octet rule and Fajans' rules.
The Gaseous State
(i) The gas laws, kinetic theory treated qualitatively.
(ii) PV = nRT or PV= (W/M)RT and the application of this equation of state.
(iii) Non-ideal behaviour of gases and Van der Waals' equation.
(iv) Dalton 's law, the Avogadro constant, the mole, Graham's law of diffusion, simple numerical problems on the above.
Colloidal Solutions
Preparation and properties of colloids, both lyophilic and lyophobic colloids. Precipitation as evidence that the colloidal particles are charged. Idea of gold number is required, but application of gold number is not required. The importance of large surface area in adsorption should also be appreciated .
Chemical Kinetics
(i) Qualitative treatment of the dependence of reaction rates on: concentration of the reactants, size of the particles, temperature and presence of a catalyst. Catalyst – structure: enzymes and zeolites.
(ii) The concept of energy barrier (it is suggested that some experiments may be devised which may deal with the above mentioned factors).
Chemical Equilibria
(i) Reversible reactions and dynamic equilibrium. The concept of equilibrium constant in terms of concentration or partial pressure to indicate the composition of the equilibrium mixture. The following are the examples: the dissociation of dinitrogen tetroxide, hydrolysis of simple esters, the Contact Process for the manufacture of sulphuric acid, the synthesis of ammonia.
(ii) Le Chatelier's principle and its applications to chemical equilibria.
General Survey of Groups of Elements
General survey of the following groups of elements in the periodic table. It should include the following (a) Occurrence in nature (b) Physical state (c) Type of bonding (d) Nature of oxides, hydroxides, chlorides, hydrides, carbonates, nitrates, sulphates wherever applicable.
(i) p-block elements. 13 th (III A) group- Al, 14 th
(IV A) group - C, allotropes – elementary idea of graphite, fullerenes and diamond, Si, Sn, Pb, 15 th (V A) group – N, P, 16 th (VI A) group O, S, 17 th (VII A) Group – F, Cl, Br, I.
(ii) d- block elements – transition elements e.g. Cu, Ag, Zn, Fe.
(iii) Elements in earth, sea. Mineral wealth of India .
Extraction Properties and Uses of Metals
Only the following metals: Electrolytic reduction: Mg Chemical reduction: Fe; important alloy – steel. Only the chemical principles and reactions are required. Details of the industrial processes are not required.
Redox Reactions
Manufacture, Properties and Uses of the Compounds :
(i) Sodium hydroxide.
(ii) Sodium carbonate.
(iii) Iron (II) Sulphate.
(iv) Magnesium chloride-6-water.
(v) Iron (II) chloride.
(vi) Iron (II) ammonium sulphate-6-water.
(vii) Iron (III) chloride.
(viii) Zinc sulphate-7-water.
Introduction to Organic Chemistry
(i) The unique nature of carbon atom and catenation.
(ii) Classification of organic compounds and homologous series.
(iii) Detection of carbon, hydrogen, sulphur, nitrogen and halogen.
(iv) Estimation of carbon, hydrogen and nitrogen – by Dumas' method.
Hydrocarbons
(i) Alkanes: General methods of preparation, Properties of alkanes with reference to methane and ethane. Petroleum as an industrial source of hydrocarbons.
(ii) Alkenes: general methods of preparation and properties of alkenes.
(iii) Alkynes: methods of preparation (including manufacture), properties and uses of ethyne.
Halide
(i) The nomenclature of aliphatic compounds containing halogen atom.
(ii) Preparation, properties, uses of haloalkanes.
(iii) Correlation of physical properties.
(iv) Preparation, properties, and uses of the following: ethyl bromide, chloroform, iodoform, haloform reaction.
Alcohols
(i) Classification, general formulae, structure and nomenclature.
(ii) General methods of preparation, manufacture, properties and uses of methanol and ethanol
(no details – only outline).
(iii) Manufacture, properties and uses of ethane-1,2 diol, propane-1,2,3 triol (outlineno details).
(iv) Conversions of one alcohol into another may be taken e.g. methanol into ethanol or viceversa.
Applications of Chemicals
(i) In medicine: analgesics, tranquillisers, antiseptics, disinfectants, anti-microbials, anti-fertility drugs, antihistamines, antibiotics, antacids.
(ii) Industry: Dyes- classification with examples – indigo, methyl orange, aniline yellow, alizarine, malachite green. Advanced materials: carbon fibres, ceramics, micro alloys. Detergents: classification, some important examples.
(iii) Space: Rockets propellants- characteristics, chemicals used.
(iv) Food processing: preservatives, artificial sweetening agents, antioxidants and edible colours.
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