Unit 1 : Some basic concepts in Chemistry
Importance of Chemistry, physical quantities and their measurement in Chemistry, SI Units, uncertainty in measurements and use of significant figures, Unit and dimensional analysis, Matter and its nature, laws of chemical combinations, atomic, and molecular, masses mole concept, molar masses, percentage composition and molecular formula, chemical stoichiometry.
Unit 2 : States of Matter
Three states of matter, gaseous state, gas laws ( Boyle’s Law and Charles Law ), Avogadro’s Law, Grahams’ Law of diffusion, Dalton’s law of partial pressure, ideal gas equation, Kinetic theory of gases, real gases and deviation from ideal behaviour, van der Waals’ equation, liquefaction of gases and critical points, Intermolecular Forces; liquids and solids.
Unit 3 : Atomic Structure
Earlier atomic models ( Thomson’s and Rutherford ), Emission Spectrum of Hydrogen Atom, Bohr’s model, of hydrogen atom, Limitations of Bohr’s model, dual nature of matter and radiation, Heisenberg uncertainty principle, quantum mechanical model of atom ( Quantum designation of atomic orbitals and electron energy in terms of principal, angular momentum and magnetic quantum numbers ), electronic spin and spin quantum numbers, Pauli’s exclusion principle, general idea of screening ( constants ) of outer electrons by inner electrons in an atom, Aufbau principle, Hund’s rule, atomic orbitals and their pictorial representation, electronic configurations of elements.
Unit 4 : Classification of elements and periodicity in properties
Need and genesis of classification of elements ( from Doebereiner to Mendeleev ), Modern periodic law and present form of periodic table, Nomenclature of elements with atomic number > 100, electronic configurations of elements and periodic table, electronic configuration and types of elements and s, p, d and f blocks, periodic trends in properties of elements ( atomic size, ionization enthalpy, electron gain enthalpy, valence / oxidation states and chemical reactivity ).
Unit 5 : Chemical Energetics
Some basic concepts in thermodynamics, first law of thermodynamics, heat capacity, measurement of DU and DH, calorimetry, standard enthalpy changes, thermochemical equations, enthalpy changes during phase transformations, Hess’s Law, standard enthalpies of formation, bond enthalpies and calculations based on them.
Unit 6 : Chemical Bonding
Kossel – Lewis approach to chemical bond formation, ionic bonds, covalent bonds, polarity of bonds and concept of electronegativity, valence shell electron pair repulsion ( VSEPR ) theory, shapes of simple molecules, valence bond theory, hybridization involving s, p and d orbitals and shapes of molecules s and p bonds; Molecular orbital theory involving homounclear diatomic molecules; Hydrogen – bonding.
Unit 7 : Equilibrium
Equilibrium in physical and chemical processes
Equilibrium in physical and chemical processes, dynamic equilibrium, law of chemical equilibrium and equilibrium constant, homogeneous equilibrium, heterogenous equilibrium, application of equilibrium constants, Relationship between reaction quotient Q, equilibrium constant, K and Gibbs’ energy G; factors affecting equilibrium – Le Chateliar’s Principle.
Ionic Equilibrium
Acids, Bases and Salts and their ionization, weak and strong electrolytes degree of ionization and ionization constants, concept of pH, ionic product of water, buffer solution, common ion effect, solubility of sparingly soluble salts and solubility products.
Unit 8 : Redox Reactions
Electronic concepts of reduction – oxidation, redox reactions, oxidation number, balancing of redox reactions.
Unit 9 : Solid State Chemistry
Classification of solids based on different binding forces : molecular, ionic, covalent and metallic solids, amorphous and crystalline solids; unit cells in two dimensional and three dimensional lattices, calculation of density of a unit cell, packing in solids, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.
Unit 10 : Chemical Thermodynamics
Spontaneous processes, energy and spontaneity, entropy and second law of thermodynamics, concept of absolute entropy, Gibbs energy and spontaneity, Gibbs energy change and equilibrium constant.
Unit 11 : Solutions
Types of solutions, different units for expressing concentration of solution, mole fraction, percentage ( by volume and mass both ), definitions of dilute solutions, vapour pressure of solutions and Raoult’s Law, Colligative properties, lowering of vapour pressure, depression of freezing point, elevation of boiling points and osmotic pressure, determination of molecular masses using colligative properties, abnormal values of molecular masses, van’t Hoff factor. simple numerical problems.
Unit 12 : Chemical Kinetics
Rate of chemical reactions, factors, affecting rates of reactions – concentration, temperature and catalyst, order and molecularity of reactions, rate law and rate constant, differential and integral forms of first order reaction, half – life ( only zero and first order ) characteristics of first order reaction, effect of temperature on reactions, Arrhenius theory – activation energy, collision theory of reaction rate ( no derivation ).
Unit 13 : Electrochemistry
Conductance in electrolytic solutions, specific and molar conductivity, variation of conductivity with concentration, Kohlrausch’s law, electrolysis and laws of electrolysis ( elementary idea ), electrolytic and galvanic cells, emf. of a cell, standard electrode potential, Nernst equation, concentration cell, fuel cells, cell potential and Gibbs energy, dry cell and lead accumulator.
Unit 14 : Surface Chemistry
Adsorption – physisorption and chemisorption, factors affecting adsorption of gases on solids, catalysis, homogeneous and heterogeneous activity and selectivity, enzyme catalysis, colloidal state, distinction between true solutions, colloids and suspensions; lyophillic, lyophobic, multimolecular and macromolecular colloids, properties of colloids, Tyndal effect, Brownian movement, electrophoresis, coagulation, emulsions – type of emulsions.
Unit 15 : Hydrogen
Position of hydrogen in periodic table, isotopes of hydrogen, heavy water, hydrogen peroxide – preparation, reactions and structures; hydrides and their classification.
Unit 16 : s – Block Elements ( Alkali and Alkaline Earth metals ):
Group 1 and Group 2 elements
Electronic configurations and general trends in physical and chemical properties, anomalous properties of the first element of each group, diagonal relationship.
Preparation and properties of some important compounds, sodium carbonate, sodium hydroxide, sodium hydrogen carbonate and industrial uses of lime and limestone, biological significance of Na, K, Mg and Ca.
Unit 17 : General principles and processes of isolation of elements
Principles and methods of extraction – concentration, reduction, ( chemical and electrolytic methods ), and refining.
Importance of Chemistry, physical quantities and their measurement in Chemistry, SI Units, uncertainty in measurements and use of significant figures, Unit and dimensional analysis, Matter and its nature, laws of chemical combinations, atomic, and molecular, masses mole concept, molar masses, percentage composition and molecular formula, chemical stoichiometry.
Unit 2 : States of Matter
Three states of matter, gaseous state, gas laws ( Boyle’s Law and Charles Law ), Avogadro’s Law, Grahams’ Law of diffusion, Dalton’s law of partial pressure, ideal gas equation, Kinetic theory of gases, real gases and deviation from ideal behaviour, van der Waals’ equation, liquefaction of gases and critical points, Intermolecular Forces; liquids and solids.
Unit 3 : Atomic Structure
Earlier atomic models ( Thomson’s and Rutherford ), Emission Spectrum of Hydrogen Atom, Bohr’s model, of hydrogen atom, Limitations of Bohr’s model, dual nature of matter and radiation, Heisenberg uncertainty principle, quantum mechanical model of atom ( Quantum designation of atomic orbitals and electron energy in terms of principal, angular momentum and magnetic quantum numbers ), electronic spin and spin quantum numbers, Pauli’s exclusion principle, general idea of screening ( constants ) of outer electrons by inner electrons in an atom, Aufbau principle, Hund’s rule, atomic orbitals and their pictorial representation, electronic configurations of elements.
Unit 4 : Classification of elements and periodicity in properties
Need and genesis of classification of elements ( from Doebereiner to Mendeleev ), Modern periodic law and present form of periodic table, Nomenclature of elements with atomic number > 100, electronic configurations of elements and periodic table, electronic configuration and types of elements and s, p, d and f blocks, periodic trends in properties of elements ( atomic size, ionization enthalpy, electron gain enthalpy, valence / oxidation states and chemical reactivity ).
Unit 5 : Chemical Energetics
Some basic concepts in thermodynamics, first law of thermodynamics, heat capacity, measurement of DU and DH, calorimetry, standard enthalpy changes, thermochemical equations, enthalpy changes during phase transformations, Hess’s Law, standard enthalpies of formation, bond enthalpies and calculations based on them.
Unit 6 : Chemical Bonding
Kossel – Lewis approach to chemical bond formation, ionic bonds, covalent bonds, polarity of bonds and concept of electronegativity, valence shell electron pair repulsion ( VSEPR ) theory, shapes of simple molecules, valence bond theory, hybridization involving s, p and d orbitals and shapes of molecules s and p bonds; Molecular orbital theory involving homounclear diatomic molecules; Hydrogen – bonding.
Unit 7 : Equilibrium
Equilibrium in physical and chemical processes
Equilibrium in physical and chemical processes, dynamic equilibrium, law of chemical equilibrium and equilibrium constant, homogeneous equilibrium, heterogenous equilibrium, application of equilibrium constants, Relationship between reaction quotient Q, equilibrium constant, K and Gibbs’ energy G; factors affecting equilibrium – Le Chateliar’s Principle.
Ionic Equilibrium
Acids, Bases and Salts and their ionization, weak and strong electrolytes degree of ionization and ionization constants, concept of pH, ionic product of water, buffer solution, common ion effect, solubility of sparingly soluble salts and solubility products.
Unit 8 : Redox Reactions
Electronic concepts of reduction – oxidation, redox reactions, oxidation number, balancing of redox reactions.
Unit 9 : Solid State Chemistry
Classification of solids based on different binding forces : molecular, ionic, covalent and metallic solids, amorphous and crystalline solids; unit cells in two dimensional and three dimensional lattices, calculation of density of a unit cell, packing in solids, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.
Unit 10 : Chemical Thermodynamics
Spontaneous processes, energy and spontaneity, entropy and second law of thermodynamics, concept of absolute entropy, Gibbs energy and spontaneity, Gibbs energy change and equilibrium constant.
Unit 11 : Solutions
Types of solutions, different units for expressing concentration of solution, mole fraction, percentage ( by volume and mass both ), definitions of dilute solutions, vapour pressure of solutions and Raoult’s Law, Colligative properties, lowering of vapour pressure, depression of freezing point, elevation of boiling points and osmotic pressure, determination of molecular masses using colligative properties, abnormal values of molecular masses, van’t Hoff factor. simple numerical problems.
Unit 12 : Chemical Kinetics
Rate of chemical reactions, factors, affecting rates of reactions – concentration, temperature and catalyst, order and molecularity of reactions, rate law and rate constant, differential and integral forms of first order reaction, half – life ( only zero and first order ) characteristics of first order reaction, effect of temperature on reactions, Arrhenius theory – activation energy, collision theory of reaction rate ( no derivation ).
Unit 13 : Electrochemistry
Conductance in electrolytic solutions, specific and molar conductivity, variation of conductivity with concentration, Kohlrausch’s law, electrolysis and laws of electrolysis ( elementary idea ), electrolytic and galvanic cells, emf. of a cell, standard electrode potential, Nernst equation, concentration cell, fuel cells, cell potential and Gibbs energy, dry cell and lead accumulator.
Unit 14 : Surface Chemistry
Adsorption – physisorption and chemisorption, factors affecting adsorption of gases on solids, catalysis, homogeneous and heterogeneous activity and selectivity, enzyme catalysis, colloidal state, distinction between true solutions, colloids and suspensions; lyophillic, lyophobic, multimolecular and macromolecular colloids, properties of colloids, Tyndal effect, Brownian movement, electrophoresis, coagulation, emulsions – type of emulsions.
Unit 15 : Hydrogen
Position of hydrogen in periodic table, isotopes of hydrogen, heavy water, hydrogen peroxide – preparation, reactions and structures; hydrides and their classification.
Unit 16 : s – Block Elements ( Alkali and Alkaline Earth metals ):
Group 1 and Group 2 elements
Electronic configurations and general trends in physical and chemical properties, anomalous properties of the first element of each group, diagonal relationship.
Preparation and properties of some important compounds, sodium carbonate, sodium hydroxide, sodium hydrogen carbonate and industrial uses of lime and limestone, biological significance of Na, K, Mg and Ca.
Unit 17 : General principles and processes of isolation of elements
Principles and methods of extraction – concentration, reduction, ( chemical and electrolytic methods ), and refining.