Unit 1: Some Basic Concepts of Chemistry | - General Introduction: Importance and scope of chemistry
- Historical approach to particulate nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
- Atomic and molecular masses. percentage composition and empirical and molecular formula; mole concept and molar mass;chemical reactions, stoichiometry and calculations based on stoichiometry.
|
Unit 2: Structure of Atom | - Discovery of electron, proton and neutron; atomic number, isotopes and isobars. Thompson’s model and its limitations, Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, rules for filling electrons in orbitals - Aufbau principle, Pauli exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half filled and completely filled orbitals, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals.
|
Unit 3: Classification of Elements and Periodicity in Properties | - Significance of classification, brief history of the development of periodic table, periodic trends in properties of elements –atomic radii, ionic radii, inert gas radii, modern periodic law and the present form of periodic table, ionization enthalpy, electron gain enthalpy, electronegativity, valence. Nomenclature of elements with atomic number greater than 100.
|
Unit 4: Chemical Bonding and Molecular Structure | - VSEPR theory, concept of hybridization involving s, p and d orbitals and shapes of some simple molecules, and molecular orbital theory of homonuclear diatomic molecules (qualitative idea only). Hydrogen bond, Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules.
|
Unit 5: States of Matter: Gases and Liquids | - Three states of matter, intermolecular interactions, Boyle’s law, Charle’s law, Gay Lussac’s law, Avogadro’s law, ideal behaviour, empirical derivation of gas equation, Avogadro number, ideal gas equation, types of bonding, melting and boiling points, role of gas laws in elucidating the concept of the molecule. Kinetic energy and molecular speeds (elementary idea), deviation from ideal behaviour, liquefaction of gases, critical temperature.
- Liquid State – Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).
|
Unit 6: Thermodynamics | - Concepts of system, types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions
- First law of thermodynamics – internal energy and enthalpy, heat capacity and specific heat, measurement of ΔU and ΔH, ionization, solution and dilution,Hess’s law of constant heat summation, enthalpy of: bond dissociation, combustion, formation, atomization, sublimation, phase transition
- Introduction of entropy as a state function, Second law of thermodynamics, criteria for equilibrium, Gibbs energy change for spontaneous and non-spontaneous process.
- Third law of thermodynamics –Brief introduction.
|
Unit 7: Equilibrium | - Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, Hydrolysis of salts (elementary idea), , buffer solutions, Henderson equation, solubility product, common ion effect (with illustrative examples), equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle; ionic equilibrium – ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of polybasic acids, acid strength, concept of pH.
|
Unit 8: Redox Reactions | - Concept of oxidation and reduction, redox reactions, oxidation number, applications of redox reactions, balancing redox reactions in terms of loss and gain of electrons and change in oxidation numbers.
|
Unit 9: Hydrogen | - Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties and uses of hydrogen; hydrides – ionic, covalent and interstitial, use and structure; hydrogen as a fuel, physical and chemical properties of water, heavy water; hydrogen peroxide-preparation, reactions.
|
Unit 10: s- Block Elements (Alkali and Alkaline earth metals) | - Group 1 and Group 2 elements: General introduction, electronic configuration, occurrence, anomalous properties of the first element of each group, diagonal relationship, trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii).
- Preparation and Properties of Some Important Compounds: Sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogencarbonate, biological importance of sodium and potassium
- CaO, CaCO3, and industrial use of lime and limestone, biological importance of Mg and Ca
|
Unit 11: Some p-Block Elements | - General Introduction to p-Block Elements
- Group 13 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, Bronophysical and chemical properties, some important compounds: borax, boric acids, boron hydrides, trends in chemical reactivity, anomalous properties of first element of the group. Aluminium: uses reactions with acids and alkalies.
- Group 14 elements: General introduction, electronic configuration, occurrence, variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first element. Carbon - catenation, allotropic forms, physical and chemical properties; uses of some important compounds: oxides.
- Important compounds of silicon and a few uses: silicon tetrachloride, silicones, silicates and zeolites, their uses.
|
Unit 12: Organic Chemistry – Some Basic Principles and Techniques | - General introduction, methods of purification, qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds.
- Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation.
- Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions
|
Unit 13: Hydrocarbons | - Classification of Hydrocarbons. Aliphatic Hydrocarbons:
- Alkanes – Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis.
- Alkynes – Nomenclature, structure of triple bond (ethyne), acidic character of alkynes, addition reaction of - hydrogen, halogens, hydrogen halides and water, physical properties, methods of preparation, chemical reactions.
- Alkenes– Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, ozonolysis, oxidation, mechanism of electrophilic addition, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect).
- Aromatic hydrocarbons – Introduction, IUPAC nomenclature; Benzene: resonance, aromaticity; chemical properties: mechanism of electrophilic substitution – nitration sulphonation, halogenation, Friedel Craft’s alkylation and acylation; directive influence of functional group in mono-substituted benzene; carcinogenicity and toxicity.
|
Unit 14: Environmental Chemistry | - Environmental pollution – Air, water and soil pollution, chemical reactions in atmosphere, smogs, major atmospheric pollutants; acid rain, ozone and its reactions, effects of depletion of ozone layer, strategy for control of environmental pollution, greenhouse effect and global warming – pollution due to industrial wastes; green chemistry as an alternative tool for reducing pollution.
|
