Part II: Chemistry
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1.
States of Matter
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1.1
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Measurement:
Physical quantities and SI units, Dimensional analysis, Precision,
Significant figures.
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1.2
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Chemical reactions: Laws of chemical combination, Dalton’s atomic theory;
Mole concept; Atomic, molecular and molar masses; Percentage composition empirical
& molecular formula; Balanced chemical equations & stoichiometry
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1.3
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Gaseous
state: Gas Laws, Kinetic theory – Maxwell distribution of velocities,
Average, root mean square and most probable velocities and relation to
temperature, Diffusion; Deviation from ideal behaviour – Critical
temperature, Liquefaction of gases, van der Waals equation.
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1.4
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Liquid
state: Vapour pressure, surface tension, viscosity.
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1.5
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Solid
state: Classification; Space lattices & crystal systems; Unit cell –
Cubic & hexagonal systems; Close packing; Crystal structures: Simple AB and AB2 type
ionic crystals, covalent crystals – diamond & graphite, metals.
Imperfections- Point defects, non-stoichiometric crystals; Electrical,
magnetic and dielectric properties; Amorphous solids – qualitative
description.
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2. Atomic Structure
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2.1
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Introduction:
Radioactivity, Subatomic particles; Atomic number, isotopes and isobars, Rutherford’s picture of atom; Hydrogen atom spectrum
and Bohr model.
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2.2
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Quantum mechanics: Wave-particle duality – de Broglie
relation, Uncertainty principle; Hydrogen atom: Quantum numbers and
wavefunctions, atomic orbitals and their shapes (s, p, and d), Spin quantum
number.
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2.3
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Many
electron atoms: Pauli exclusion principle; Aufbau principle and the
electronic configuration of atoms, Hund’s rule.
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2.4
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Periodicity:
Periodic law and the modern periodic table; Types of elements: s, p, d, and f
blocks; Periodic trends: ionization energy, atomic and ionic radii, electron
affinity, electro negativity and valency.
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3.
Chemical Bonding &
Molecular Structure
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3.1
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Ionic
Bond: Lattice Energy and Born-Haber cycle; Covalent character of ionic bonds
and polar character of covalent bond
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3.2
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Molecular
Structure: Lewis picture & resonance structures, VSEPR model &
molecular shapes
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3.3
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Covalent
Bond: Valence Bond Theory- Orbital overlap, Directionality of bonds & hybridization
(s, p & d orbitals only), Resonance; Molecular orbital theory-
Methodology, Orbital energy level diagram, Bond order, Magnetic properties
for homonuclear diatomic species.
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3.4
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Metallic
Bond: Qualitative description.
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3.5
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Intermolecular
Forces: Polarity; Dipole moments; Hydrogen Bond.
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4. Thermodynamics
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4.1
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Basic
Concepts: Systems and surroundings; State functions; Intensive &
Extensive Properties; Zeroth Law and Temperature
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4.2
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First
Law of Thermodynamics: Work, internal energy, heat, enthalpy, heat
capacities; Enthalpies of formation, phase transformation, ionization,
electron gain; Thermochemistry; Hess’s Law. Bond dissociation, combustion,
atomization, sublimation, dilution
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4.3
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Second
Law: Spontaneous and reversible processes; entropy; Gibbs free energy related
to spontaneity and non-mechanical work; Standard free energies of formation,
free energy change and chemical equilibrium
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4.4
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Third
Law: Introduction
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5.
Physical and Chemical Equilibria
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5.1
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Concentration
Units: Mole Fraction, Molarity, and Molality
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5.2
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Solutions: Solubility of solids and
gases in liquids, Vapour Pressure, Raoult’s law, Relative lowering of vapour
pressure, depression in freezing point; elevation in boiling point; osmotic
pressure, determination of molecular mass; solid solutions.
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5.3
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Physical Equilibrium: Equilibria
involving physical changes (solid-liquid, liquid-gas, solid-gas), Surface
chemistry, Adsorption, Physical and Chemical adsorption, Langmuir Isotherm,
Colloids and emulsion, classification, preparation, uses.
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5.4
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Chemical
Equilibria: Equilibrium constants (KP, KC),
Le-Chatelier’s principle.
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5.5
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Ionic
Equilibria: Strong and Weak electrolytes, Acids and Bases (Arrhenius, Lewis,
Lowry and Bronsted) and their dissociation; Ionization of Water; pH; Buffer
solutions; Acid-base titrations; Hydrolysis; Solubility Product of Sparingly
Soluble Salts; Common Ion Effect.
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5.6
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Factors
Affecting Equilibria: Concentration, Temperature, Pressure, Catalysts,
Significance of DG
and DG0 in Chemical Equilibria.
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6. Electrochemistry
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6.1
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Redox Reactions: Oxidation-reduction
reactions (electron transfer concept); Oxidation number; Balancing of redox
reactions; Electrochemical cells and cell reactions; Electrode potentials;
EMF of Galvanic cells; Nernst equation; Factors affecting the electrode potential;
Gibbs energy change and cell potential; Secondary cells; Fuel cells;
Corrosion and its prevention.
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6.2
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Electrolytic Conduction: Electrolytic
Conductance; Specific and molar conductivities; Kolhrausch’s Law and its
application, Faraday’s laws of electrolysis; Coulometer; Electrode potential
and electrolysis, Commercial production of the chemicals, NaOH, Na, Al, Cl2 & F2.
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7.
Chemical Kinetics
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7.1
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Aspects
of Kinetics: Rate and Rate expression of a reaction; Rate constant; Order and
molecularity of the reaction; Integrated rate expressions and half life for
zero and first order reactions.
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7.2
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Factor
Affecting the Rate of the Reactions: Concentration of the reactants, size of
particles; Temperature dependence of rate constant; Activation energy; Catalysis,
Surface catalysis, enzymes, zeolites; Factors affecting rate of collisions between
molecules.
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7.3
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Mechanism
of Reaction: Elementary reactions; Complex reactions; Reactions involving
two/three steps only.
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8.
Hydrogen
and s-block elements
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8.1
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Hydrogen:
Element: unique position in periodic table, occurrence, isotopes; Dihydrogen:
preparation, properties, reactions, and uses; Molecular, saline, interstitial
hydrides; Water: Properties; Structure and aggregation of water molecules;
Heavy water; Hydrogen peroxide; Hydrogen as a fuel.
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8.2
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s-block
elements: Abundance and occurrence;
Anomalous properties of the first elements in each group; diagonal
relationships.
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8.3
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Alkali
metals: Lithium, sodium and potassium: occurrence, extraction, reactivity,
and electrode potentials; Biological importance; Reactions with oxygen,
hydrogen, halogens and liquid ammonia; Basic nature of oxides and hydroxides;
Halides; Properties and uses of compounds such as NaCl, Na2CO3,
NaHCO3, NaOH, KCl, and KOH.
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8.4
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Alkaline
earth metals: Magnesium and calcium: Occurrence, extraction, reactivity and
electrode potentials; Reactions with non-metals; Solubility and thermal
stability of oxo salts; Biological importance; Properties and uses of
important compounds such as CaO, Ca(OH)2, plaster of Paris, MgSO4,
MgCl2, CaCO3, and CaSO4; Lime and limestone,
cement.
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9.
p-
d- and f-block elements
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9.1
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General:
Abundance, distribution, physical and chemical properties, isolation and uses
of elements; Trends in chemical reactivity of elements of a group;.
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9.2
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Group
13 elements: Boron; Properties and uses of borax, boric acid, boron hydrides
& halides. Reaction of aluminum with acids and alkalis;
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9.3
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Group
14 elements: Carbon: Uses, Allotropes (graphite, diamond, fullerenes),
oxides, halides and sulphides, carbides; Silicon: Silica, silicates,
silicone, silicon tetrachloride, Zeolites.
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9.4
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Group
15 elements: Dinitrogen; Reactivity and uses of nitrogen and its compounds;
Industrial and biological nitrogen fixation; Ammonia: Haber’s process, properties
and reactions; Oxides of nitrogen and their structures; Ostwald’s process of
nitric acid production; Fertilizers –
NPK type; Production of phosphorus; Allotropes of phosphorus;
Preparation, structure and properties of hydrides, oxides, oxoacids and
halides of phosphorus.
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9.5
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Group
16 elements: Isolation and chemical
reactivity of dioxygen; Acidic, basic and amphoteric oxides; Preparation,
structure and properties of ozone; Allotropes of sulphur; Production of
sulphur and sulphuric acid; Structure and properties of oxides, oxoacids,
hydrides and halides of sulphur.
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9.6
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Group
17 and group 18 elements: Structure and properties of hydrides, oxides,
oxoacids of chlorine; Inter halogen compounds; Bleaching Powder; Preparation,
structure and reactions of xenon fluorides, oxides, and oxoacids.
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9.7
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d-Block
elements: General trends in the chemistry of first row transition elements;
Metallic character; Oxidation state; Ionic radii; Catalytic properties;
Magnetic properties; Interstitial compounds; Occurrence and extraction of
iron, copper, silver, zinc, and mercury; Alloy formation; Steel and some
important alloys; preparation and properties of CuSO4, K2Cr2O7,
KMnO4, Mercury halides; Silver nitrate and silver halides;
Photography.
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9.8
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f-Block
elements: Lanthanoids and actinoids; Oxidation states and chemical reactivity
of lanthanoids compounds; Lanthanide contraction; Comparison of actinoids and
lanthanoids.
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9.9
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Coordination
Compounds: Coordination number; Ligands; Werner’s coordination theory; IUPAC
nomenclature; Application and importance of coordination compounds (in
qualitative analysis, extraction of metals and biological systems e.g.
chlorophyll, vitamin B12, and hemoglobin); Bonding: Valence-bond approach,
Crystal field theory (qualitative); Stability constants; Shapes, color and
magnetic properties; Isomerism including stereoisomerisms; Organometallic
compounds.
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10.
Principles
of Organic Chemistry and Hydrocarbons
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10.1
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Classification: Based on functional groups, trivial and
IUPAC nomenclature.
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10.2
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Electronic
displacement in a covalent bond:
Inductive, resonance effects, and hyperconjugation; free radicals;
carbocations, carbanions, nucleophiles and electrophiles; types of organic
reactions.
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10.3
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Alkanes
and cycloalkanes: Structural isomerism
and general properties.
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10.4
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Alkenes
and alkynes: General methods of preparation and reactions, physical
properties, electrophilic and free radical additions, acidic character of
alkynes and (1,2 and 1,4) addition to dienes.
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10.5
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Aromatic
hydrocarbons: Sources; Properties; Isomerism; Resonance delocalization;
polynuclear hydrocarbons; mechanism of electrophilic substitution reaction,
directive influence and effect of substituents on reactivity.
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10.6
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Haloalkanes
and haloarenes: Physical properties, chemical reactions. Uses and
environmental effects; di, tri, tetrachloromethanes, iodoform, freon and DDT.
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10.7
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Petroleum:
Composition and refining, uses of petrochemicals.
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11. Stereochemistry
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11.1
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Introduction:
Chiral molecules; Optical activity; Polarimetry; R,S and D,L configurations;
Fischer projections; Enantiomerism; Racemates; Diastereomerism and meso
structures.
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11.2
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Conformations:
Ethane conformations; Newman and Sawhorse projections.
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11.3
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Geometrical
isomerism in alkenes
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12.
Organic
Compounds with Functional Groups Containing Oxygen and Nitrogen
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12.1
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General:
Electronic structure, important methods of preparation, important reactions
and physical properties of alcohols, phenols, ethers, aldehydes, ketones,
carboxylic acids, nitro compounds, amines, diazonium salts, cyanides and
isocyanides.
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12.2
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Specific:
Effect of substituents on alpha-carbon on acid strength, comparative
reactivity of acid derivatives, basic character of amines methods of
preparation, and their separation, importance of diazonium salts in synthetic
organic chemistry.
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13. Biological , Industrial and
Environmental chemistry
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13.1
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The Cell:
Concept of cell and energy cycle.
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13.2
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Carbohydrates: Classification; Monosaccharides; Structures
of pentoses and hexoses; Anomeric carbon; Mutarotation; Simple chemical
reactions of glucose, Disaccharides: reducing and non-reducing sugars –
sucrose, maltose and lactose; Polysaccharides: elementary idea of structures
of starch, cellulose and glycogen.
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13.3
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Proteins:
Amino acids; Peptide bond; Polypeptides; Primary structure of proteins;
Simple idea of secondary , tertiary and quarternary structures of proteins;
Denaturation of proteins and enzymes.
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13.4
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Nucleic
Acids: Types of nucleic acids; Primary building blocks of nucleic acids
(chemical composition of DNA & RNA); Primary structure of DNA and its
double helix; Replication; Transcription and protein synthesis; Genetic code.
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13.5
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Vitamins: Classification, structure,
functions in biosystems; Hormones
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13.6
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Polymers:
Classification of polymers; General methods of polymerization; Molecular mass
of polymers; Biopolymers and biodegradable polymers; Free radical, cationic
and anionic addition polymerizations; Copolymerization: Natural rubber;
Vulcanization of rubber; Synthetic rubbers. Condensation polymers.
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13.7
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Pollution: Environmental pollutants; soil, water and
air pollution; Chemical reactions in atmosphere; Smog; Major atmospheric
pollutants; Acid rain; Ozone and its reactions; Depletion of ozone layer and
its effects; Industrial air pollution; Green house effect and global warming;
Green Chemistry.
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13.8
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Chemicals
in medicine, health-care and food: Analgesics, Tranquilizers, antiseptics,
disinfectants, anti-microbials, anti-fertility drugs, antihistamines,
antibiotics, antacids; Preservatives, artificial sweetening agents,
antioxidants, soaps and detergents.
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14.
Theoretical
Principles of Experimental Chemistry
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14.1
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Volumetric Analysis: Principles; Standard solutions of
sodium carbonate and oxalic acid; Acid-base titrations; Redox reactions involving
KI, H2SO4, Na2SO3, Na2S2O3and
H2S; Potassium permanganate in acidic, basic and neutral media;
Titrations of oxalic acid, ferrous ammonium sulphate with KMnO4, K2
Cr2O7/Na2S2O3,
Cu(II)/Na2S2O3.
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14.2
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Qualitative
analysis of Inorganic Salts: Principles in the determination of the cations
Pb2+, Cu2+, As3+, Mn2+, Zn2+,
Co2+, Ca2+, Sr2+, Ba2+, Mg2+,
NH4+, Fe3+, Ni2+ and the anions
CO32-, S2-, SO42-, SO32-,
NO2-, NO3-, Cl-, Br-,
I-, PO43-, CH3COO-, C2O42-.
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14.3
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Physical Chemistry Experiments: preparation and crystallization
of alum, copper sulphate, ferrous sulphate, double salt of alum and ferrous
sulphate, potassium ferric sulphate; Temperature vs. solubility; pH
measurements; Lyophilic and lyophobic sols; Dialysis; Role of emulsifying
agents in emulsification. Equilibrium
studies involving (i) ferric and
thiocyanate ions (ii) [Co(H2O)6]2+ and
chloride ions; Enthalpy determination for (i) strong acid vs. strong base
neutralization reaction (ii) hydrogen bonding interaction between acetone and
chloroform; Rates of the reaction between (i) sodium thiosulphate and
hydrochloric acid, (ii) potassium iodate and sodium sulphite (iii) iodide vs.
hydrogen peroxide, concentration and
temperature effects in these reactions.
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14.4
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Purification Methods: Filtration, crystallization,
sublimation, distillation, differential extraction, and chromatography.
Principles of melting point and boiling point determination; principles of
paper chromatographic separation – Rf values.
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14.5
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Qualitative Analysis of Organic Compounds: Detection of
nitrogen, sulphur, phosphorous and halogens; Detection of carbohydrates, fats
and proteins in foodstuff; Detection of alcoholic, phenolic, aldehydic,
ketonic, carboxylic, amino groups and unsaturation.
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14.6
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Quantitative Analysis of Organic Compounds: Basic
principles for the quantitative estimation of carbon, hydrogen, nitrogen,
halogen, sulphur and phosphorous; Molecular mass determination by silver salt
and chloroplatinate salt methods; Calculations of empirical and molecular
formulae.
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14.7
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Principles of Organic Chemistry Experiments: Preparation of iodoform, acetanilide,
p-nitro acetanilide, di-benzayl acetone, aniline yellow, beta-naphthol;
Preparation of acetylene and study of its acidic character.
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