PHYSICAL CHEMISTRY

UNIT 1: Some Basic Concepts in Chemistry

• Matter and its nature, Dalton’s atomic theory: concept of atoms, molecule, element, and compound:
• Laws of chemical combination;  Atomic and molecular masses, mole concept and molar mass; percentage composition and empirical and molecular formula;
• Chemical equations and stoichiometry.

UNIT 2: Atomic Structure

• Nature of electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom. Bohr model of a hydrogen atom – its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitation of Bohr’s model; Dual nature of matter, de Broglie’s relationship, Heisenberg uncertainty principle.
• Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features. Concept of  atomic orbital as one-electron wave functions: Variation of  Ψ  and  Ψ2  with r for 1s 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 exclusion principles and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.

UNIT 3: Chemical Bonding and Molecular Structure

• Kossel – Lewis approach to chemical bond formation, the 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, the 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, the concept of bond order, bond length, and bond energy.
• Elementary idea of metallic bonding. Hydrogen bonding and its applications.

UNIT 4: Chemical Thermodynamics

• Fundamentals of thermodynamics: system and surroundings, extensive and intensive properties’ state functions, types of processes.
• The 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.
• The second law of thermodynamics – Spontaneity of processes:  ∆S of the universe and ∆G  of the system as criteria for spontaneity. ∆G°  (Standard Gibbs energy change) and equilibrium constant.

UNIT 5: Solutions

• Different methods for expressing the concentration of solution – molarity, molarity, mole fraction. percentage (by volume and mass both), the 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 – a relative lowering of vapour pressure, depression of freezing point, the 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.

UNIT 6: Equilibrium

• Meaning of equilibrium, the 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.
• Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc  ) and their significance, the significance of ∆G and ∆G°  in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the 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, the solubility of sparingly soluble salts and solubility products, buffer solutions.

UNIT 7: Redox Reactions and Electrochemistry 

• Electronics 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, electrodes 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.

UNIT 8: 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, the effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of biomolecular gaseous reactions ( no derivation ).

INORGANIC CHEMISTRY

UNIT 9: Classification of Elements and Periodicity in Properties

• Modern 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 enthakpy, electron gain enthalpy. valence, oxidation states, and chemical reactivity.

UNIT 10: 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.

UNIT 11: d – and f- Block Elements

• Inner Transition Elements
• Lanthanoids- Electronic configuration, oxidation states, and lanthanoids contraction.
• Antinoids- Electronics configurationand oxidation states.

UNIT 12: Co-ordination Compounds

• Introduction to Coordination compounds. Werner’s theory; ligands, coordination 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 co-ordination compounds (in qualitative analysis, extraction of metals and in biological systems).

ORGANIC CHEMISTRY

UNIT 13: Purification and Characterisation 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 principle only) – Estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus.
• Calculations of empirical formulae and molecular formulae: Numerical problems in organic quantitative analysis.

UNIT 14: 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 carbocation 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. 

UNIT 15: 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 (Markownikoffs 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 the functional group in mono- substituted benzene.

UNIT 16: 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.

UNIT 17: 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. Reimer – Tiemann reaction.
• Ethers: Structure.
• Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones; Important reactions such as – Nucleophilic addition reactions (addition of HCN. NH3 and its derivatives), Grignard reagent; oxidation: reduction (wolf Kishner and Clemmensen); the acidity of œ- hydrogen. aldol condensation cannizzaro reaction. Haloform reaction, Chemical tests to distinguish between aldehydes and Ketones’
• Carboxylic Acids 
• Acidic strength and factors affecting it.

UNIT 18: 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.

UNIT 19: 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 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.
• Hormones (General introduction)

UNIT 20: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY

Detection of extra elements (Nitrogen, Sulphur, halogens) in organic compounds; Detection of the following functional groups; hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones) carboxyl, and amino groups in organic compounds.

• The chemistry involved in the preparation of the following: Inorganic compounds; Mohr’s salt, potash alum. Organic compounds: Acetanilide, p-nitro acetanilide, aniline yellow, iodoform.
• The chemistry involved in the titrimetric exercises – Acids, bases, and the use of indicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4
• Chemical principles involved in the qualitative salt analysis:

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 ions with hydrogen peroxide at room temperature.