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Chemistry
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
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
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 K2Cr 2O7 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
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, 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.
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 KMnO4USTIFY" style="margin-bottom: 0in">
• 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
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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