REVISION OF SYLLABUS
Subject –CHEMISTRY –I (w.e.f. 2012-13)
1.1 
Sub- atomic particles
Sub- atomic particles
1.2 Atomic models- Rutherford’s Nuclear model of atom
1.3 Developments to the Bohr’s model of atom
1.3.1 Nature of electromagnetic radiation.
1.3.2 Particle nature of electromagnetic
radiation- Planck’s quantum theory.
1.4 Bohr’s model for Hydrogen atom.
1.4.1 Explanation of line spectrum of hydrogen.
1.4.2 Limitations of Bohr’s model
1.5Quantum
mechanical considerations of sub atomic
particles.
1.5.1 Dual behaviour of matter.
1.5.2 Heisenberg’s uncertainty principle.
1.6 Quantum mechanical model of an
atom. Important features of Quantum mechanical model of atom.
1.6.1 Orbitals and quantum numbers.
1.6.2 Shapes of atomic orbitals.
1.6.3 Energies of orbitals.
1.6.4
Filling
of orbitals in atoms. Aufbau Principle, Pauli’s exclusion Principle and Hund’s
rule of maximum multiplicity.
1.6.5 Electronic configurations of atoms.
1.6.6 Stability of half filled and completely filled orbitals.
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2. CLASSIFICATION OF ELEMENTSAND PERIODICITY IN
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PROPERTIES
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2.1
Need to classify elements
2.2
Genesis of periodic classification.
2.3
Modern
periodic law and present form of the periodic table.
2.4
Nomenclature
of elements with atomic number greater than100
2.6
Electronic
configuration and types of elements s,p,d.and f blocks.
2.7.1
Trends in physical properties:
(a) Atomic radius
(b) Ionic radius
(c)Variation
of size in inner transition elements.
(d)Ionization
enthalpy.
(e) Electron gain enthalpy
(f) Electro negativity.
2.7.2 Periodic trends in chemical properties:
(a) Valence or Oxidation states.
(b) Anomalous properties of second period
elements – diagonal relationship.
2.7.3 Periodic trends and chemical reactivity
3. CHEMICAL BONDING AND MOLECULAR STRUCTURE
3.1
Kossel
– Lewis approach to chemical bonding.
3.2
Ionic
or electrovalent bond - Factors favourable for the formation of ionic
compounds-Crystal structure of
sodium
chloride-General properties of ionic compounds.
3.3
Bond
Parameters – bond length, bond angle, and bond enthalpy, bond order,
resonance-Polarity of bonds dipole moment
3.4 Valence Shell Electron Pair Repulsion
(VSEPR) theories. Predicting the geometry of simple molecules.
3.5
Valence
bond theory-Orbital overlap concept-Directional properties of bonds-overlapping
of atomic orbitals strength of sigma and pi bonds-Factors favouring the
formation of covalent bonds
3.6
Hybridisation-
different types of hybridization involving s, p and d orbitals- shapes of
simple covalent molecules.
3.7 Coordinate bond –definition with examples.
3.8 Molecular orbital theory –
Formation of molecular orbitals, Linear combination of atomic orbitals
(LCAO)-conditions for combination of atomic orbitals - Energy level diagrams
for molecular orbitals -Bonding in some homo nuclear diatomic molecules- H ,He
,Li ,B ,C ,N ,and O
3.9
Hydrogen
bonding-cause of formation of hydrogen bond-Types of hydrogen bonds-inter and
intra molecular-General properties of hydrogen bonds.
4.
STATES OF MATTER: GASES AND LIQUIDS
4.1
Intermolecular
forces
4.2 Thermal Energy
4.3 Intermolecular forces Vs Thermal interactions.
4.4 The Gaseous State.
4.5 The Gas Laws
4.6 Ideal gas equation.
4.7
Graham’s
law of diffusion – Dalton’s Law of partial pressures.
4.8 Kinetic molecular theory of gases.
4.9
Kinetic
gas equation of an ideal gas (No derivation) deduction of gas laws from Kinetic
gas equation.
4.10 Distribution of molecular speeds –
rms, average and most probable speeds-Kinetic energy of gas molecules.
4.11 Behaviour of real gases – Deviation
from Ideal gas behaviour – Compressibility factor Vs Pressure diagrams of real
gases.
4.12 Liquefaction of gases
4.13 Liquid State – Properties of Liquids
in terms of Inter molecular interactions – Vapour pressure, Viscosity and
Surface tension (Qualitative idea only. No mathematical
derivation)
5.
STOICHIOMETRY
5.1 Some Basic Concepts – Properties of
matter – uncertainty in Measurement-significant figures, dimensional analysis.
5.2 Laws of Chemical Combinations – Law
of Conservation of Mass, Law of Definite Proportions, Law of Multiple
Proportions, Gay Lussac’s Law of Gaseous Volumes, Dalton’s Atomic Theory,
Avogadro Law, Principles, Examples.
5.3 Atomic and molecular masses- mole
concept and molar mass concept of equivalent weight.
5.4 Percentage composition of compounds
and calculations of empirical and molecular formulae of compounds.
5.5 Stoichiometry and stoichiometric calculations.
5.6 Methods of Expressing concentrations
of solutions-mass percent, mole fraction, molarity, molality and normality.
5.7 Redox reactions-classical idea of
redox reactions, oxidation and reduction reactions-redox reactions in terms of
electron transfer.
5.8 Oxidation number concept.
5.9 Types of Redox reactions-combination,
decomposition, displacement. and disproportionation reactions
5.10 Balancing of redox reactions –
oxidation number method Half reaction (ion-electron) method.
5.11 Redox reactions in Titrimetry.
6. THERMODYNAMICS
6.1
Thermodynamic Terms.
6.1.1 The system and the
surroundings. 6.1.2. Types of systems and surroundings.
6.1.3 The state of the system.
6.1.4 The Internal Energy as a State Function.
(a) Work (b) Heat (c) The general case, the first law of
Thermodynamics.
6.2
Applications.
6.2.1 Work
6.2.2 Enthalpy, H- a useful new state function
6.2.3 Extensive and intensive properties.
6.2.4 Heat capacity
6.2.5 The relationship between CP and Cv.
6.3 Measurement of U
and H: Calorimetry
6.4 Enthalpy change, r H of reactions – reaction Enthalpy
(a) Standard enthalpy of reactions.
(b) Enthalpy changes during
transformations.
(c) Standard enthalpy of formation.
(d) Thermo chemical equations.
(e) Hess’s law of constant Heat
summation.
6.5 Enthalpies for different types of reactions.
(a) Standard enthalpy of combustion ( c HO )
(b) Enthalpy of atomization ( a Hø),
phase transition, sublimation and ionization.
(c) Bond Enthalpy (
bond Hø )
(d) Enthalpy of solution (
sol Hø ) and dilution.
6.6 Spontaneity.
(a) Is decrease in enthalpy a criterion for spontaneity?
(b) Entropy and spontaneity, *the second
law of thermodynamics.
(c) Gibbs Energy and spontaneity.
6.7 Gibbs Energy change and equilibrium.
6.8 Absolute entropy and the third law of thermodynamics.
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7. CHEMICAL EQUILIBRIUM AND ACIDS-BASES
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7.1 Equilibrium in Physical process.
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7.2 Equilibrium in chemical process – Dynamic Equilibrium
7.3 Law of chemical Equilibrium - Law of
mass action and Equilibrium constant.
7.4 Homogeneous Equilibria, Equilibrium
constant in gaseous systems. Relationship between KP and Kc
7.5 Heterogeneous Equilibria.
7.7 Relationship between Equilibrium constant K, reaction
quotient
Q and Gibbs energy G.
7.8 Factors affecting
Equilibria.-Le-chatlieprinciple application to industrial synthesis of Ammonia
and Sulphur trioxide.
7.9 Ionic Equilibrium in solutions.
7.10 Acids, bases and salts- Arrhenius,
Bronsted-Lowry and Lewis concepts of acids and bases.
7.11 Ionisation of Acids and Bases
–Ionisation constant of water and it’s ionic product- pH scale-ionisation
constants of weak acids-ionisation of weak bases-relation between
Ka and Kb-Di and poly basic acids and
di and poly acidic Bases-Factors affecting acid strength-Common ion effect in
the ionization of acids and bases-Hydrolysis of salts and pH of their
solutions.
7.12
Buffer
solutions-designing of buffer solution-Preparation of Acidic buffer
7.13
Solubility
Equilibria of sparingly soluble salts. Solubility product constant Common ion
effect on solubility of Ionic salts.
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8. HYDROGEN AND ITS COMPOUNDS
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8.1 Position of hydrogen in the periodic table.
8.2 Dihydrogen-Occurance and Isotopes.
8.3 Preparation of Dihydrogen
8.4 Properties of Dihydrogen
8.5 Hydrides: Ionic, covalent, and non-stiochiometric
hydrides.
8.6 Water: Physical properties; structure
of water, ice. Chemical properties of water; hard and soft water Temporary and
permanent hardness of water
8.7
Hydrogen
peroxide: Preparation; Physical properties; structure and chemical properties;
storage and uses.
8.8 Heavy Water
8.9 Hydrogen as a fuel.
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(ALKALI AND ALKALINE EARTH METALS)
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Group 1 Elements
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9.1 Alkali metals; Electronic configurations;
Atomic
and Ionic radii; Ionization enthalpy; Hydration enthalpy; Physical properties;
Chemical properties; Uses
9.2 General characteristics of the
compounds of the alkali metals: Oxides; Halides; Salts of Oxy Acids.
9.3 Anomalous properties of Lithium:
Differences and similarities with
other alkali metals. Diagonal relationship; similarities between Lithium and
Magnesium.
9.4 Some important compounds of Sodium:
Sodium Carbonate; Sodium Chloride; Sodium Hydroxide;
Sodium hydrogen carbonate.
9.5 Biological importance of Sodium and Potassium.
Group 2 Elements:
9.6 Alkaline earth elements; Electronic
configuration; Ionization enthalpy; Hydration enthalpy; Physical properties,
Chemical properties; Uses.
9.7 General characteristics of compounds of the Alkaline Earth
Metals:
Oxides, hydroxides, halides, salts of Oxyacids
(Carbonates;
Sulphates and Nitrates).
9.8 Anomalous behavior of Beryllium; its
diagonal relationship with Aluminum.
9.9 Some important compounds of calcium:
Preparation
and uses of Calcium Oxide ; Calcium Hydroxide; Calcium Carbonate;Plaster of
Paris; Cement. 9.10 Biological importance of Calcium and Magnesium.
10. P- BLOCK ELEMENTS GROUP 13 ( BORON
FAMILY)
10.1
General introduction – Electronic configuration, Atomic
radii, Ionization enthalpy, Electro negativity; Physical &
General introduction – Electronic configuration, Atomic
radii, Ionization enthalpy, Electro negativity; Physical &
Chemical
properties.
10.2 Important trends and anomalous properties of boron.
10.3
Some
important compounds of boron – Borax, Ortho boric acid,diborane.
10.4 Uses of boron, aluminium and their compounds.
11. p-BLOCK ELEMENTS - GROUP 14 ( CARBON
FAMILY)
11.1
General
introduction - Electronic configuration, Atomic radii, Ionization enthalpy,
Electro negativity; Physical & Chemical properties.
11.2 Important trends and anomalous properties of carbon.
11.3 Allotropes of carbon.
11.4 Uses of carbon.
11.5
Some
important compounds of carbon and silicon – carbonmonoxide, carbon
dioxide,Silica, silicones, silicates and zeolites.
12. ENVIRONMENTAL CHEMISTRY
12.1 Definition of terms: Air, Water and Soil Pollutions.
12.2 Environmental Pollution
12.3
Atmospheric
pollution; Tropospheric Pollution; Gaseous Air Pollutants (Oxides of Sulphur;
Oxides of Nitrogen; Hydro Carbons; Oxides of Carbon (CO; CO2).
Global warming and Green house
effect.
12.4 Acid Rain- Particulate Pollutants- Smog.
12.5
Stratospheric
Pollution: Formation and breakdown of Ozone- Ozone hole- effects of depletion
of the Ozone layer.
12.6 Water Pollution: Causes of Water
Pollution; International standards for drinking water.
12.7 Soil Pollution: Pesticides, Industrial Wastes.
12.8 Strategies to control environmental
pollution- waste Management- collection and disposal.
12.9 Green Chemistry: Green chemistry in
day-to-day life; Dry cleaning of clothes; Bleaching of paper; Synthesis of
chemicals
13. ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES
AND
TECHNIQUES AND HYDROCARBONS
13.2 Tetravalency of Carbon: shapes of organic compounds.
13.3 Structural representations of organic compounds.
13.4 Classification of organic compounds.
13.5 Nomenclature of organic compounds.
13.6 Isomerism.
13.7
Fundamental
concepts in organic reaction mechanisms. 13.7.1 Fission of covalent bond.
13.7.2 Nucleophiles and electrophiles.
13.7.3 Electron movements in organic
reactions. 13.7.4 Electron displacement effects in covalent bonds. 13.7.5 Types
of Organic reactions.
13.8 Methods of purification of organic compounds.
13.9 Qualitative elemental analysis of organic compounds.
13.10 Quantitative elemental analysis of organic compounds.
HYDROCARBONS
13.11 Classification of Hydrocarbons.
13.12
Alkanes
– Nomenclature, isomerism (structural and conformations of ethane only)
13.12.1 Preparation of alkanes
13.12.2
Properties
– Physical properties and chemical Reactivity, Substitution reactions –
Halogenation(free radical mechanism), Combustion, Controlled
steam
and Pyrolysis.
13.13 Alkenes- Nomenclature, structure of ethane, Isomerism
(structural
and geometrical).
13.13.1 Methods of preparation.
13.13.2
Properties-
Physical and chemical reactions: Addition of Hydrogen, halogen, water,
sulphuric acid, Hydrogen
halides
(Mechanism- ionic and peroxide effect,
Markovnikov’s
, antiMarkovnikov’s or Kharasch
effect).
Oxidation, Ozonolysis and Polymerization.
13.14
Alkynes
– Nomenclature and isomerism,
structure of acetylene. Methods of preparation of acetylene.
13.14.1
Physical
properties, Chemical reactions- acidic character of acetylene, addition
reactions- of hydrogen, Halogen, Hydrogen halides and water. Polymerization.
13.15 Aromatic
Hydrocarbons: Nomenclature and
isomerism.Structure of benzene, Resonance and aromaticity.
13.15.1
Preparation
of benzene. Physical properties. Chemical properties: Mechanism of electrophilic
substitution. Electrophilic substitution reactions- Nitration, Sulphonation,
Halogenation, Friedel-Craft’ alkylation and acylation.
13.15.2
Directive
influence of functional groups in mono substituted benzene, Carcinogenicity and
toxicity.