1.2 Rutherford_model
1.3.2
Particle nature of electromagnetic radiation- Planck’s
quantum
theory.
1.4
Bohr’s model for Hydrogen atom.
1.4.2
Limitations of Bohr’s model
1.5.1Dual behaviour of matter.
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.
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
2.5
Electronic configuration of elements and the periodic
table
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
(b)
Anomalous properties of second period elements –
diagonal
relationship.
2.7.3
Periodic trends and chemical reactivity
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
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
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
molecular
interactions – Vapour pressure, Viscosity and
Surface
tension (Qualitative idea only. No mathematical
derivation)
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,
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.
6.1
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.
7.1
Equilibrium in Physical process.
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.
7.6
Applications of Equilibrium constant.
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
7.9
Ionic Equilibrium in solutions.
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.
8.
HYDROGEN AND ITS COMPOUNDS
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.
9.
THE s – BLOCK ELEMENTS
(ALKALI
AND ALKALINE EARTH METALS)
Group
1 Elements
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 &
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.
12.1
Definition of terms: Air, Water and Soil Pollutions.
12.2
Environmental Pollution
12.3
Atmospheric pollution; Tropospheric Pollution; Gaseous
Air
Pollutants (Oxides of Sulphur
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
13.1
General introduction.
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.
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
Oxidation,
Isomerisation, Aromatization, reaction with
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.