Part-1:- Physical chemistry
Unit 1:
Some Basic Concepts in Chemistry
Matter and its nature, Dalton’s atomic theory; Concept of
atom, molecule, element and compound; Physical quantities and their
measurements in Chemistry, precision and accuracy, significant figures,
S.I. Units, dimensional analysis; Laws of chemical combination; Atomic
and molecular masses, mole concept, molar mass, percentage composition,
empirical and molecular formulae; Chemical equations and stoichiometry.
Unit 2:
States of Matter
Classification of matter into solid, liquid and gaseous states:
Gaseous State: Measurable properties of gases; Gas laws -
Boyle’s law, Charle’s law, Graham’s law of diffusion, Avogadro’s law,
Dalton’s law of partial pressure; Concept of Absolute scale of
temperature; Ideal gas equation; Kinetic theory of gases (only
postulates); Concept of average, root mean square and most probable
velocities; Real gases, deviation from Ideal behaviour, compressibility
factor and van der Waals equation.
Liquid State: Properties of liquids - vapour pressure,
viscosity and surface tension and effect of temperature on them
(qualitative treatment only).
Solid State: Classification of solids: molecular, ionic,
covalent and metallic solids, amorphous and crystalline solids
(elementary idea); Bragg’s Law and its applications; Unit cell and
lattices, packing in solids (fcc, bcc and hcp lattices), voids,
calculations involving unit cell parameters, imperfection in solids;
Electrical, magnetic and dielectric properties.
Unit 3:
Atomic Structure
Thomson and Rutherford atomic models and their limitations;
Nature of electromagnetic radiation, photoelectric effect; Spectrum of
hydrogen atom, Bohr model of hydrogen atom - its postulates, derivation
of the relations for energy of the electron and radii of the different
orbits, limitations of Bohr’s model; Dual nature of matter, de-Broglie’s
relationship, Heisenberg uncertainty principle. Elementary ideas of
quantum mechanics, quantum mechanical model of atom, its important
features, concept of atomic orbitals as one electron wave functions;
Variation of Ψ and Ψ2 , with r for 1s and 2s orbitals; various quantum
numbers (principal, angular momentum and magnetic quantum numbers) and
their significance; shapes of s, p and d - orbitals, electron spin and
spin quantum number;
Rules for filling electrons in orbitals – Aufbau Principle,
Pauli’s exclusion principle and Hund’s rule, electronic configuration
of elements, extra stability of half-filled and completely filled
orbitals.
Unit 4:
Chemical Bonding And Molecular Structure
Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.
Covalent Bonding: Concept of Electronegativity, Fajan’s
rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR)
theory and shapes of simple molecules.
Quantum mechanical approach to covalent bonding: Valence
bond theory – Its important features, concept of hybridization involving
s, p and d orbitals; Resonance.
Molecular Orbital Theory - Its important features, LCAOs,
types of molecular orbitals (bonding, antibonding), sigma and pi-bonds,
molecular orbital electronic configurations of homonuclear diatomic
molecules, concept of bond order, bond length and bond energy.
Elementary idea of metallic bonding. Hydrogen bonding and its
applications.
Unit 5:
Chemical Thermodynamics
Fundamentals of thermodynamics: System and surroundings,
extensive and intensive properties, state functions, types of processes.
First law of thermodynamics - Concept of work, heat
internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s
law of constant heat summation; Enthalpies of bond dissociation,
combustion, formation, atomization, sublimation, phase transition,
hydration, ionization and solution.
Second law of thermodynamics- Spontaneity of processes; ΔS
of the universe and ΔG of the system as criteria for spontaneity, ΔGθ
(Standard Gibbs energy change) and equilibrium constant.
Unit 6:
Solutions
Different methods for expressing concentration of solution -
molality, molarity, mole fraction, percentage (by volume and mass
both), vapour pressure of solutions and Raoult’s Law – Ideal and
non-ideal solutions, vapour pressure - composition, plots for ideal and
non-ideal solutions; Colligative properties of dilute solutions-
relative lowering of vapour pressure, depression of freezing point,
elevation of boiling point and osmotic pressure; Determination of
molecular mass using colligative properties; Abnormal value of molar
mass, Van’t Hoff factor and its significance.
Unit 7:
Equilibrium
Meaning of equilibrium, concept of dynamic equilibrium.
Equilibria involving physical processes: Solid-liquid,
liquid - gas and solid – gas equilibria, Henry’s law, General
characteristics of equilibrium involving physical processes.
Equilibria involving chemical processes: Law of chemical
equilibrium, equilibrium constants (Kp and Kc) and their significance,
significance of ΔG and ΔG
Θ in chemical equilibria, factors
affecting equilibrium concentration, pressure, temperature, effect of
catalyst; Le Chatelier’s principle.
Ionic equilibrium: Weak and strong electrolytes, ionization
of electrolytes, various concepts of acids and bases (Arrhenius,
Bronsted - Lowry and Lewis) and their ionization, acid - base equilibria
(including multistage ionization) and ionization constants, ionization
of water, pH scale, common ion effect, hydrolysis of salts and pH of
their solutions, solubility of sparingly soluble salts and solubility
products, buffer solutions.
Unit 8:
Redox Reactions And Electrochemistry
Electronic concepts of oxidation and reduction, redox
reactions, oxidation number, rules for assigning oxidation number,
balancing of redox reactions. Electrolytic and metallic conduction,
conductance in electrolytic solutions, specific and molar conductivities
and their variation with concentration: Kohlrausch’s law and its
applications.
Electrochemical cells - Electrolytic and Galvanic cells,
different types of electrodes, electrode potentials including standard
electrode potential, half - cell and cell reactions, emf of a Galvanic
cell and its measurement; Nernst equation and its applications;
Relationship between cell potential and Gibbs’ energy change; Dry cell
and lead accumulator; Fuel cells.
Unit 9:
Chemical Kinetics
Rate of a chemical reaction, factors affecting the rate of
reactions: concentration, temperature, pressure and catalyst; elementary
and complex reactions, order and molecularity of reactions, rate law,
rate constant and its units, differential and integral forms of zero and
first order reactions, their characteristics and half - lives, effect
of temperature on rate of reactions – Arrhenius theory, activation
energy and its calculation, collision theory of bimolecular gaseous
reactions (no derivation).
Unit 10:
Surface Chemistry
Absorption- Physisorption and chemisorption and their
characteristics, factors affecting absorption of gases on solids-
Freundlich and Langmuir absorption isotherms, absorption from solutions.
Colloidal state - distinction among true solutions,
colloids and suspensions, classification of colloids - lyophilic,
lyophobic; multi molecular, macromolecular and associated colloids
(micelles), preparation and properties of colloids - Tyndall effect,
Brownian movement, electrophoresis, dialysis, coagulation and
flocculation; Emulsions and their characteristics.
Part-2: Inorganic Chemistry
Unit 11:
Classification Of Elements And Periodicity In Properties
Modern periodic law and present form of the periodic
table, s, p, d and f block elements, periodic trends in properties of
elements atomic and ionic radii, ionization enthalpy, electron gain
enthalpy, valence, oxidation states and chemical reactivity.
Unit 12:
General Principles And Processes Of Isolation Of Metals
Modes of occurrence of elements in nature, minerals, ores;
Steps involved in the extraction of metals - concentration, reduction
(chemical and electrolytic methods) and refining with special reference
to the extraction of Al, Cu, Zn and Fe; Thermodynamic and
electrochemical principles involved in the extraction of metals.
Unit 13:
Hydrogen
Position of hydrogen in periodic table, isotopes,
preparation, properties and uses of hydrogen; Physical and chemical
properties of water and heavy water; Structure, preparation, reactions
and uses of hydrogen peroxide; Hydrogen as a fuel.
Unit 14:
S - Block Elements (Alkali And Alkaline Earth Metals)
Group - 1 and 2 Elements
General introduction, electronic configuration and general
trends in physical and chemical properties of elements, anomalous
properties of the first element of each group, diagonal relationships.
Preparation and properties of some important compounds- sodium carbonate
and sodium hydroxide; Industrial uses of lime, limestone, Plaster of
Paris and cement; Biological significance of Na, K, Mg and Ca.
Unit 15:
P - Block Elements
Group - 13 to Group 18 Elements
General Introduction: Electronic configuration and general
trends in physical and chemical properties of elements across the
periods and down the groups; unique behaviour of the first element in
each group. Groupwise study of the p – block elements.
Group – 13
Preparation, properties and uses of boron and aluminium;
properties of boric acid, diborane, boron trifluoride, aluminium
chloride and alums.
Group – 14
Allotropes of carbon, tendency for catenation; Structure & properties of silicates, and zeolites.
Group – 15
Properties and uses of nitrogen and phosphorus; Allotrophic
forms of phosphorus; Preparation, properties, structure and uses of
ammonia, nitric acid, phosphine and phosphorus halides, (PCl
3, PCl
5); Structures of oxides and oxoacids of phosphorus.
Group – 16
Preparation, properties, structures and uses of ozone;
Allotropic forms of sulphur; Preparation, properties, structures and
uses of sulphuric acid (including its industrial preparation);
Structures of oxoacids of sulphur.
Group – 17
Preparation, properties and uses of hydrochloric acid;
Trends in the acidic nature of hydrogen halides; Structures of
Interhalogen compounds and oxides and oxoacids of halogens.
Group – 18
Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.
Unit 16:
d – and f – Block Elements
Transition Elements
General introduction, electronic configuration, occurrence
and characteristics, general trends in properties of the first row
transition elements - physical properties, ionizationenthalpy, oxidation
states, atomic radii, colour, catalytic behaviour, magnetic
properties,complex formation, interstitial compounds, alloy formation;
Preparation, properties and uses of K
2Cr
2O
7 and KmnO
4.
Inner Transition Elements
Lanthanoids - Electronic configuration, oxidation states and lanthanoid contraction.
Actinoids - Electronic configuration and oxidation states.
Unit 17:
Co-Ordination Compounds
Introduction to co-ordination compounds, Werner’s theory;
ligands, coordination number, denticity, chelation; IUPAC nomenclature
of mononuclear coordination compounds, isomerism; Bonding-Valence bond
approach and basic ideas of Crystal field theory, colour and magnetic
properties; Importance of co-ordination compounds (in qualitative
analysis, extraction of metals and in biological systems).
Unit 18:
Environmental Chemistry
Environmental pollution - Atmospheric, water and soil. Atmospheric pollution - Tropospheric and Stratospheric
Tropospheric pollutants – Gaseous pollutants: Oxides of
carbon, nitrogen and sulphur, hydrocarbons; their sources, harmful
effects and prevention; Green house effect and Global warming; Acid
rain;
Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects and prevention.
Stratospheric pollution- Formation and breakdown of ozone, depletion of ozone layer - its mechanism and effects.
Water Pollution - Major pollutants such as, pathogens,
organic wastes and chemical pollutants; their harmful effects and
prevention.
Soil pollution - Major pollutants such as: Pesticides
(insecticides, herbicides and fungicides), their harmful effects and
prevention. Strategies to control environmental pollution.
Part-3: Organic Chemistry
Unit 19:
Purification And Characterisation Of Organic Compounds
Purification-Crystallization, sublimation, distillation,
differential extraction and chromatography - principles and their
applications.
Qualitative analysis - Detection of nitrogen, sulphur, phosphorus and halogens.
Quantitative analysis (basic principles only) - Estimation
of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus.
Calculations of empirical formulae and molecular formulae; Numerical
problems in organic quantitative analysis.
Unit 20:
Some Basic Principles Of Organic Chemistry
Tetravalency of carbon; Shapes of simple molecules -
hybridization (s and p); Classification of organic compounds based on
functional groups: - C = C - , - C h C – and those containing halogens,
oxygen, nitrogen and sulphur; Homologous series; Isomerism -structural
and stereoisomerism.
Nomenclature (Trivial and IUPAC) Covalent bond fission -
Homolytic and heterolytic: free radicals, carbocations and carbanions;
stability of carbocations and free radicals, electrophiles and
nucleophiles.
Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance and hyperconjugation.
Unit 21:
Hydrocarbons
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions.
Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes.
Alkenes - Geometrical isomerism; Mechanism of electrophilic
addition: addition of hydrogen, halogens, water, hydrogen halides
(Markownikoff’s and peroxide effect); Ozonolysis and polymerization.
Alkynes - Acidic character; Addition of hydrogen, halogens, water and hydrogen halides; Polymerization.
Aromatic hydrocarbons - Nomenclature, benzene - structure
and aromaticity; Mechanism of electrophilic substitution: halogenation,
nitration, Friedel – Craft’s alkylation and acylation, directive
influence of functional group in mono-substituted benzene.
Unit 22:
Organic Compounds Containing Halogens
General methods of preparation, properties and reactions;
Nature of C-X bond; Mechanisms of substitution reactions, Uses;
Environmental effects of chloroform & iodoform.
Unit 23:
Organic Compounds Containing Oxygen
General methods of preparation, properties, reactions and uses.
Alcohols, Phenols And Ethers Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution
reactions: halogenation, nitration and sulphonation, Reimer - Tiemann
reaction.
Ethers: Structure.
Aldehyde and Ketones: Nature of carbonyl group;
Nucleophilic addition to >C=O group, relative reactivities of
aldehydes and ketones; Important reactions such as – Nucleophilic
addition reactions (addition of HCN, NH3 and its derivatives), Grignard
reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of
- hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction;
Chemical tests to distinguish between aldehydes and Ketones.
Carboxylic Acids: Acidic strength and factors affecting it.
Unit 24:
Organic Compounds Containing Nitrogen
General methods of preparation, properties, reactions and
uses. Amines: Nomenclature, classification, structure, basic character
and identification of primary, secondary and tertiary amines and their
basic character. Diazonium Salts: Importance in synthetic organic
chemistry.
Unit 25:
Polymers
General introduction and classification of polymers,
general methods of polymerization addition and condensation,
copolymerization; Natural and synthetic rubber and vulcanization; some
important polymers with emphasis on their monomers and uses - polythene,
nylon, polyester and bakelite.
Unit 26:
Biomolecules
General introduction and importance of biomolecules.
Carbohydrates - Classification: aldoses and ketoses;
monosaccharides (glucose and fructose) and constituent monosaccharides
of oligosacchorides (sucrose, lactose and maltose).
Proteins - Elementary Idea of - amino acids, peptide bond,
polypeptides; Proteins: primary, secondary, tertiary and quaternary
structure (qualitative idea only), denaturation of proteins, enzymes.
Vitamins - Classification and functions.
Nucleic Acids - Chemical constitution of DNA and RNA. Biological functions of nucleic acids.
Unit 27:
Chemistry In Everyday Life
Chemicals in medicines - Analgesics, tranquilizers,
antiseptics, disinfectants, antimicrobials, anti-fertility drugs,
antibiotics, antacids, anti-histamins – their meaning and common
examples.
Chemicals in food - Preservatives, artificial sweetening agents - common examples.
Cleansing agents - Soaps and detergents, cleansing action.
Section B
Practical Component having 20% weightage:
Unit 28:
Principles Related To Practical Chemistry
- Detection of extra elements (N, S, halogens) in organic
compounds; Detection of the following functional groups: hydroxyl
(alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and
amino groups in organic compounds.
- Chemistry involved in the preparation of the following:
Inorganic compounds: Mohr’s salt, potash alum. Organic compounds:
Acetanilide, pnitroacetanilide, aniline yellow, iodoform.
- Chemistry involved in the titrimetric exercises - Acids
bases and the use of indicators, oxalic-acid vs KMnO4, Mohr’s salt vs
KMnO4
- Chemical principles involved in the qualitative salt analysis:
- Cations - Pb2+ , Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+.
- Anions- CO3 2-, S2-, SO4 2-, NO2-, NO3-, CI -, Br, I.
- (Insoluble salts excluded).
- Chemical principles involved in the following experiments:
- Enthalpy of solution of CuSO4
- Enthalpy of neutralization of strong acid and strong base.
- Preparation of lyophilic and lyophobic sols.
- Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.
