Units | Topics |
Section A – Physical Chemistry |
Some Basic Concepts in Chemistry | Matter and its nature, Dalton's atomic theory; the concept of the atom, molecule, element, and compound;laws of chemical combination; atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae; chemical equations and stoichiometry. |
Atomic Structure | nature of electromagnetic radiation, photoelectric effect; spectrum of hydrogen atom, Bohr model of hydrogen atom - its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr's model; dual nature of matter, de-Broglie's relationship, heisenberg uncertainty principle. Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; variation of t|/ and \|/2 with r for Is and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number; rules for filling electrons in orbitals - aufbau principle, Pauli's exclusion principle and Hund's rule, electronic configuration of elements, extra stability of half-filled and filled orbitals. |
Chemical Bonding and Molecular Structure | Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds. Ionic Bonding: formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy. Covalent Bonding: concept of electronegativity, Fajan's rule, dipole moment; valence shell electron pair repulsion (VSEPR) theory and shapes of simple molecules. Quantum mechanical approach to covalent bonding: valence bond theory - its important features, concept of hybridization involving s, p and d orbitals; resonance. Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, concept of bond order, bond length and bond energy, elementary idea of metallic bonding, hydrogen bonding and its applications. |
Chemical Thermodynamics | Fundamentals of thermodynamics: system and surroundings, extensive and intensive properties, state functions, types of processes. First law of thermodynamics - concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess's law of constant heat summation; enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution. Second law of thermodynamics: spontaneity of processes; AS of the universe and AG of the system as criteria for spontaneity, AG" (Standard Gibbs energy change) and equilibrium constant. |
Solutions | Different methods for expressing concentration of solution - molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of solutions and Raoult's Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non-ideal solutions; colligative properties of dilute solutions - relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; determination of molecular mass using colligative properties; abnormal value of molar mass, van't hoff factor and its significance. |
Equilibrium | Meaning of equilibrium, concept of dynamic equilibrium, equilibria involving physical processes: solid -liquid, liquid - gas and solid - gas equilibria, Henry's law, general characteristics of equilibrium involving physical processes. Equilibria involving chemical processes: law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of AG and AG" in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier's principle. Ionic equilibrium: weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, bronsted - Lowry and Lewis) and their ionization, acid - base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions. |
Redox Reactions and Electro-chemistry | Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions. Electrolytic and metallic conduction, conductance in electrolytic solutions, molar conductivities and their variation with concentration: kohlrausch's law and its applications. Electrochemical cells - electrolytic and galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half - cell and cell reactions, emf of a galvanic cell and its measurement; nernst equation and its applications; relationship between cell potential and Gibbs' energy change; dry cell and lead accumulator; fuel cells. |
Chemical Kinetics | Rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure and catalyst; elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first order reactions, their characteristics and half -lives, effect of temperature on rate of reactions -Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation). |
Section B – Inorganic Chemistry |
Classification of Elements and Periodicity in Properties | Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity. |
P- Block Elements | Group -13 to Group 18 elements General Introduction: electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group. |
d - and f - Block Elements | Transition Elements General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the first row transition elements -physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; preparation, properties and uses of K2 Cr, O7 and KmnO4. Inner Transition Elements Lanthanoids - electronic configuration, oxidation states and lanthanoid contraction. Actinoids - electronic configuration and oxidation states. |
Co-ordination Compounds | Introduction to co-ordination compounds, Werner's theory; ligands, co-ordination number, denticity, chelation; IUPAC nomenclature of mononuclear coordination compounds, isomerism; Bonding-Valence bond approach and basic ideas of crystal field theory, colour and magnetic properties; Importance of coordination compounds (in qualitative analysis, extraction of metals and in biological systems). |
Section C – Organic Chemistry |
Purification and Characterization of Organic Compounds | Purification - crystallization, sublimation, distillation, differential extraction and chromatography - principles and their applications. Qualitative analysis - detection of nitrogen, sulphur, phosphorus and halogens. Quantitative analysis (basic principles only)- estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus, calculations of empirical formula and molecular formula; numerical problems in organic quantitative analysis. |
Some Basic Principles of Organic Chemistry | Tetravalency of carbon; shapes of simple molecules -hybridization (s and p); classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen and sulphur; homologous series; Isomerism - structural and stereoisomerism. Nomenclature (Trivial and IUPAC) Covalent bond fission - homolytic and heterolytic: free radicals, carbocations and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles. Electronic displacement in a covalent bond - inductive effect, electromeric effect, resonance and hyperconjugation. Common types of organic reactions- substitution, addition, elimination and rearrangement. |
Hydrocarbons | Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions. Alkanes - Conformations: sawhorse and newman projections of ethane; mechanism of halogenation of alkanes. Alkenes - geometrical isomerism; mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff s and peroxide effect); ozonolysis and polymerization. Alkynes - acidic character; addition of hydrogen, halogens, water and hydrogen halides; polymerization. Aromatic hydrocarbons - nomenclature, benzene -structure and aromaticity; mechanism of electrophilic substitution: halogenation, nitration, Friedel - Craft's alkylation and acylation, directive influence of functional group in mono-substituted benzene. |
Organic Compounds Containing Halogens | General methods of preparation, properties and reactions; nature of C-X bond; mechanisms of substitution reactions. Uses, environmental effects of chloroform, iodoform freons and DDT. |
Organic Compounds Containing Oxygen | General methods of preparation, properties, reactions and uses. Alcohols, Phenols and Ethers Alcohols: identification of primary, secondary and tertiary alcohols; mechanism of dehydration. Phenols: acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reitner - Tiemann reaction. Ethers: structure. Aldehyde and Ketones: Nature of carbonyl group; nucleophilic addition to >C=0 group, relative reactivities of aldehydes and ketones; Important reactions such as - nucleophilic addition reactions (addition of HCN, NH, and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of a-hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between aldehydes and ketones, carboxylic acids. Acidic strength and factors affecting it. |
Organic Compounds Containing Nitrogen | General methods of preparation, properties, reactions and uses. Amines: nomenclature, classification, structure, basic character and identification of primary, secondary and tertiary amines and their basic character. Diazonium Salts: importance in synthetic organic chemistry. |
Biomolecules | General introduction and importance of biomolecules. Carbohydrates - classification: aldoses and ketoses; monosaccharides (glucose and fructose) and constituent monosaccharides of oligosaccharides (sucrose, lactose and maltose). Proteins - elementary Idea of a-amino acids, peptide bond, polypeptides; proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes. Vitamins - classification and functions. Nucleic Acids - chemical constitution of DNA and RNA. Biological functions of nucleic acids. |
Principles Related to Practical Chemistry | Detection of extra elements (N,S, halogens) in organic compounds; detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds. • Chemistry involved in the preparation of the following: Inorganic compounds: Mohr's salt, potash alum. Organic compounds: acetanilide, p nitroacetanilide, aniline yellow, iodoform. •Chemistry involved in the titrimetric exercises -Acids bases and the use of indicators, oxalic-acid vs KMnO,, Mohr's salt vs KMnO,. •Chemical principles involved in the qualitative salt analysis: Cations - Pb2+, Cu!+, Af,+, Fe1+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, nh;. Anions- CO,", S2~, SO4", NO", NO~2, Cf, Br", I" . (Insoluble salts excluded). •Chemical principles involved in the following experiments: 1. Enthalpy of solution of CuSO4 2. Enthalpy of neutralization of strong acid and strong base. 3. Preparation of lyophilic and lyophobic sols. 4. Kinetic study of the reaction of iodide ion with hydrogen peroxide at room temperature. |
