SECTION: A
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, ?? and ??2, concept of atomic orbitals as one
electron wave functions; Variation of ?? and ??2 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 STRUCURE
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; DS of the universe and DG of
the system as criteria for spontaneity, Dgo (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 characterics of equilibrium involving physical processes.
Equilibria involving chemical processes:
Law of chemical equilibrium, equilibrium constants (Kp and Kc) and
their significance, significance of DG and DGo 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, Br??nsted – 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.
Eectrolytic 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
Adsorption- Physisorption and
chemisorption and their characteristics, factors affecting adsorption of
gases on solids – Freundlich and Langmuir adsorption isotherms,
adsorption 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.
SECTION – B
INORGANIC CHEMISTRY
UNIT 11: CLASSIFICATON OF ELEMENTS AND PERIODICITY IN PROPERTIES
Modem 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, (PCl3, PCl5); 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,
ionization enthalpy, oxidation states, atomic radii, colour, catalytic
behaviour, magnetic properties, complex formation, interstitial
compounds, alloy formation; Preparation, properties and uses of K2 Cr2 O7 and KMnO4 .
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, co-ordination number, denticity, chelation;
IUPAC nomenclature of mononuclear co-ordination 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.
SECTION-C
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.
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, antifertility
drugs, antibiotics, antacids, antihistamins – their meaning and common
examples.
Chemicals in food – Preservatives, artificial sweetening agents – common examples. Cleansing agents – Soaps and detergents, cleansing action.
Chemicals in food – Preservatives, artificial sweetening agents – common examples. Cleansing agents – Soaps and detergents, cleansing action.
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 excercises – 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:
1. Enthalpy of solution of CuSO4
2. Enthalpy of neutralization of strong acid and strong base.
3. Preparation of lyophilic and lyophobic sols.
4. Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.
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