Physical chemistry
Unit 1:
General topics
Concept of atoms and molecules; Dalton’s atomic theory;
Mole concept; Chemical formulae; Balanced chemical equations;
Calculations (based on mole concept) involving common
oxidation-reduction, neutralisation, and displacement reactions;
Concentration in terms of mole fraction, molarity, molality and
normality.
Unit 2:
Gaseous and liquid states
Absolute scale of temperature, ideal gas equation;
Deviation from ideality, van der Waals equation; Kinetic theory of
gases, average, root mean square and most probable velocities and their
relation with temperature; Law of partial pressures; Vapour pressure;
Diffusion of gases.
Unit 3:
Atomic structure and chemical bonding
Bohr model, spectrum of hydrogen atom, quantum numbers;
Wave-particle duality, de Broglie hypothesis; Uncertainty principle;
Qualitative quantum mechanical picture of hydrogen atom, shapes of s, p
and d orbitals; Electronic configurations of elements (up to atomic
number 36); Aufbau principle; Pauli’s exclusion principle and Hund’s
rule; Orbital overlap and covalent bond; Hybridisation involving s, p
and d orbitals only; Orbital energy diagrams for homonuclear diatomic
species; Hydrogen bond; Polarity in molecules, dipole moment
(qualitative aspects only); VSEPR model and shapes of molecules (linear,
angular, triangular, square planar, pyramidal, square pyramidal,
trigonal bipyramidal, tetrahedral and octahedral).
Unit 4:
Energetics
First law of thermodynamics; Internal energy, work and
heat, pressure-volume work; Enthalpy, Hess’s law; Heat of reaction,
fusion and vapourization; Second law of thermodynamics; Entropy; Free
energy; Criterion of spontaneity.
Unit 5:
Chemical equilibrium
Law of mass action; Equilibrium constant, Le Chatelier’s
principle (effect of concentration, temperature and pressure);
Significance of ΔG and ΔG° in chemical equilibrium; Solubility product,
common ion effect, pH and buffer solutions; Acids and bases (Bronsted
and Lewis concepts); Hydrolysis of salts.
Unit 6:
Electrochemistry
Electrochemical cells and cell reactions; Standard
electrode potentials; Nernst equation and its relation to ΔG;
Electrochemical series, emf of galvanic cells; Faraday’s laws of
electrolysis; Electrolytic conductance, specific, equivalent and molar
conductivity, Kohlrausch’s law; Concentration cells.
Unit 7:
Chemical kinetics
Rates of chemical reactions; Order of reactions; Rate
constant; First order reactions; Temperature dependence of rate constant
(Arrhenius equation).
Unit 8:
Solid state
Classification of solids, crystalline state, seven crystal
systems (cell parameters a, b, c, α, β, γ), close packed structure of
solids (cubic), packing in fcc, bcc and hcp lattices; Nearest
neighbours, ionic radii, simple ionic compounds, point defects.
Unit 9:
Solutions
Raoult’s law; Molecular weight determination from lowering
of vapour pressure, elevation of boiling point and depression of
freezing point.
Unit 10:
Surface chemistry
Elementary concepts of adsorption (excluding adsorption
isotherms); Colloids: types, methods of preparation and general
properties; Elementary ideas of emulsions, surfactants and micelles
(only definitions and examples).
Unit 11:
Nuclear chemistry
Radioactivity: isotopes and isobars; Properties of α, β and
γ rays; Kinetics of radioactive decay (decay series excluded), carbon
dating; Stability of nuclei with respect to proton-neutron ratio; Brief
discussion on fission and fusion reactions.
Unit 12:
Inorganic Chemistry
Isolation/preparation and properties of the following
non-metals: Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and
halogens; Properties of allotropes of carbon (only diamond and
graphite), phosphorus and sulphur.
Unit 13:
Preparation and properties of the following compounds
Oxides, peroxides, hydroxides, carbonates, bicarbonates,
chlorides and sulphates of sodium, potassium, magnesium and calcium;
Boron: diborane, boric acid and borax; Aluminium: alumina, aluminium
chloride and alums; Carbon: oxides and oxyacid (carbonic acid); Silicon:
silicones, silicates and silicon carbide; Nitrogen: oxides, oxyacids
and ammonia; Phosphorus: oxides, oxyacids (phosphorus acid, phosphoric
acid) and phosphine; Oxygen: ozone and hydrogen peroxide; Sulphur:
hydrogen sulphide, oxides, sulphurous acid, sulphuric acid and sodium
thiosulphate; Halogens: hydrohalic acids, oxides and oxyacids of
chlorine, bleaching powder; Xenon fluorides.
Unit 14:
Transition elements (3d series):
Definition, general characteristics, oxidation states and
their stabilities, colour (excluding the details of electronic
transitions) and calculation of spin-only magnetic moment; Coordination
compounds: nomenclature of mononuclear coordination compounds, cis-trans
and ionisation isomerisms, hybridization and geometries of mononuclear
coordination compounds (linear, tetrahedral, square planar and
octahedral).
Unit 15:
Preparation and properties of the following compounds:
Oxides and chlorides of tin and lead; Oxides, chlorides and
sulphates of Fe2+, Cu2+ and Zn2+; Potassium permanganate, potassium
dichromate, silver oxide, silver nitrate, silver thiosulphate.Ores and minerals: Commonly occurring ores and minerals of iron, copper, tin, lead, magnesium, aluminium, zinc and silver.
Unit 16:
Extractive metallurgy
Chemical principles and reactions only (industrial details
excluded); Carbon reduction method (iron and tin); Self reduction method
(copper and lead); Electrolytic reduction method (magnesium and
aluminium); Cyanide process (silver and gold).
Unit 17:
Principles of qualitative analysis:
Groups I to V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+,
Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and Mg2+); Nitrate, halides
(excluding fluoride), sulphate and sulphide.
Organic chemistry
Unit 18:
Concepts
Hybridisation of carbon; Sigma and pi-bonds; Shapes of
simple organic molecules; Structural and geometrical isomerism; Optical
isomerism of compounds containing up to two
asymmetric centres, (R,S and E,Z nomenclature excluded); IUPAC
nomenclature of simple organic compounds (only hydrocarbons,
mono-functional and bi-functional compounds); Conformations of ethane
and butane (Newman projections); Resonance and hyperconjugation;
Keto-enol tautomerism; Determination of empirical and molecular formulae
of simple compounds (only combustion method); Hydrogen bonds:
definition and their effects on physical properties of alcohols and
carboxylic acids; Inductive and resonance effects on acidity and
basicity of organic acids and bases; Polarity and inductive effects in
alkyl halides; Reactive intermediates produced during homolytic and
heterolytic bond cleavage; Formation, structure and stability of
carbocations, carbanions and free radicals.
Unit 19:
Preparation, properties and reactions of alkanes:
Homologous series, physical properties of alkanes (melting
points, boiling points and density); Combustion and halogenation of
alkanes; Preparation of alkanes by Wurtz reaction and decarboxylation
reactions.
Unit 20:
Preparation, properties and reactions of alkenes and alkynes:
Physical properties of alkenes and alkynes (boiling points,
density and dipole moments); Acidity of alkynes; Acid catalysed
hydration of alkenes and alkynes (excluding the stereochemistry of
addition and elimination); Reactions of alkenes with KMnO4 and ozone;
Reduction of alkenes and alkynes; Preparation of alkenes and alkynes by
elimination reactions; Electrophilic addition reactions of alkenes with
X2, HX, HOX (X=halogen) and H2O; Addition reactions of alkynes; Metal
acetylides.
Unit 21:
Reactions of benzene:
Structure and aromaticity; Electrophilic substitution
reactions: halogenation, nitration, sulphonation, Friedel-Crafts
alkylation and acylation; Effect of o-, m- and p-directing groups in
monosubstituted benzenes.
Unit 22:
Phenols:
Acidity, electrophilic substitution reactions
(halogenation, nitration and sulphonation); Reimer-Tieman reaction,
Kolbe reaction.Characteristic reactions of the following (including those mentioned above): Alkyl halides: rearrangement reactions of alkyl carbocation, Grignard reactions, nucleophilic substitution reactions; Alcohols: esterification, dehydration and oxidation, reaction with sodium, phosphorus halides, ZnCl2/concentrated HCl, conversion of alcohols into aldehydes and ketones; Ethers:Preparation by Williamson’s Synthesis; Aldehydes and Ketones: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Perkin reaction; Cannizzaro reaction; haloform reaction and nucleophilic addition reactions (Grignard addition); Carboxylic acids: formation of esters, acid chlorides and amides, ester hydrolysis; Amines: basicity of substituted anilines and aliphatic amines, preparation from nitro compounds, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts; carbylamine reaction; Haloarenes: nucleophilic aromatic substitution in haloarenes and substituted haloarenes (excluding Benzyne mechanism and Cine substitution).
Unit 23:
Carbohydrates:
Classification; mono- and di-saccharides (glucose and
sucrose); Oxidation, reduction, glycoside formation and hydrolysis of
sucrose.Amino acids and peptides: General structure (only primary structure for peptides) and physical properties.
Unit 24:
Properties and uses of some important polymers:
Natural rubber, cellulose, nylon, teflon and PVC.
Unit 25:
Practical organic chemistry:
Detection of elements (N, S, halogens); Detection and
identification of the following functional groups: hydroxyl (alcoholic
and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino and
nitro; Chemical methods of separation of mono-functional organic
compounds from binary mixtures.
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