Chemistry Syllabus
Physical chemistry
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.
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.
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).
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.
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.
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.
Chemical kinetics: Rates of
chemical reactions; Order of reactions; Rate constant; First order reactions;
Temperature dependence of rate constant (Arrhenius equation).
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.
Solutions: Raoult’s law;
Molecular weight determination from lowering of vapour pressure, elevation of
boiling point and depression of freezing point.
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).
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.
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.
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.
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).
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.
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).
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
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.
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.
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.
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.
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).
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.
Properties and uses of some important
polymers: Natural rubber, cellulose, nylon, teflon and PVC.
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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