1.AtomicStructure: Idea of de Broglie matter wave, Heisenberg uncertainty principle, atomic orbitals, Schrödinger wave equation, significance of Y and Y2,Quantum numbers, radial and angular wave functions and probability distribution curves, shapes of s, p, d orbitals, effective nuclear charge.
2.Periodic Properties: Trends in periodic table and applications in predicting and explaining the physical and chemical behaviors. Atomic and ionic radii, ionization energy, electron affinity and electro negativity.
3.Chemical Bonding :Valence bond theory and its limitations, directional characteristics of covalent bond, various types of hybridization and shapes of simple inorganic molecules and ions, Valence shell electron pair repulsion (VSEPR) theory and its applications to NH3, H3O+, SF4, ClF3, ICl2- and H2O. MO theory, homonuclear and heteronuclear (CO and NO) diatomic molecules,multicenter bonding in electron deficient molecules, bond strength and bond energy, percentage ionic character, from dipole moment and electro negativity difference. Weak interactions, Hydrogen bonding, van der Waal forces.
4.Ionic Solids : Concept and properties of ionic bond and structure of ionic compounds, radius ratio effect and coordination number, limitation of radius ratio rule, lattice defects, semiconductors, lattice energy and Born – Haber cycle, Solvation energy and solubility of ionic solids, polarizing power and Polarizability of ions, Fajan’s rule. Metallic bond – free electron, valence bond theory.
5.Chemistry of Nobel gases: Chemical properties of the Nobel gases, chemistry of Xenon, structure and bonding in xenon compounds.
Paper - II
General Organic Chemistry-I
15 Hrs (1 Hrs/week)
1.Structure and Bonding:
Hybridization, bond length and bond angles, bond energy, localized and delocalized chemical bond, inclusion compounds, clathrates, charge transfer complexes, resonance, hyper-conjugation, aromaticity, inductive and field effects, hydrogen bonding.
2.Mechanism of Organic reactions:
Curved arrow notations, drawing electron movement with arrows, half-headed and double-headed arrows, homolytic and heterolytic bond breaking.
Types of reagents – electrophilic and nucleophilic. Types of organic reactions, reactive intermediates – carbocations, carbanians, free radicals, carbenes, arynes and nitrenes (with examples)
Concept of isomerism, types of isomerism, optical isomerism. Elements of symmetry, chirality, enantiomers, chiral and achiral molecules with two stereogenic centers,diastereomers, threo and erythro diastereomers, meso compounds, resolution, inversion, retention and recemization. Relative and absolute configuration and sequence rules. R S system of nomenclature.
Paper –III: General Physical Chemistry-I
15 Hrs (1 Hrs/week)
1.Mathematical Concept :
Logarithmic relations, curve sketching, linear graphs and calculation of slopes, differentiation of functions likeXn , ex, sin x, log x; maxima and minima, partial differentiation and reciprocacity relations. Integration of some useful/relevant functions; permutations and combinations, factorials. Probability.
2.Computers: introduction to computers, different components of a computer, hardware and software, Input – Output devices, binary numbers and binary arithmetic. Introduction to computer languages, Programming, operating system.
3.Gaseous states :
Vander Waals equation of state, the isotherms of van der Waal equation, relationship between critical constants and van der Waal constants. The law of corresponding states, reduced equation of state.
Root mean square velocity, average and most probable velocities. Qualitative discussion of the Maxwell’s distribution of molecular velocities, collision number, mean free path and collision diameter, liquefaction of gases based on Joule – Thomson effect.
5.Liquid State :
Intermolecular forces, structure of liquids (a qualitative description). Structural differences between solids, liquids and gases.
Liquid crystals, difference between liquid crystals, solid and liquids. Classification, structure of nematic and cholestric phases. Thermography and seven segment cell.
General Chemistry-I Practical Exercise
30 Hrs (2 Hrs/week)
·Calibration of fractional weights, balance and knowledge of volumetric measurement apparatus and measurement units.
·Preparation of standard solutions and their verification (maximum two examples).
·Semi micro analysis – Anion and cation analysis,
·Separation and identification of cations from Group I, II, III, IV, V and VI on the basis of solubility of their Chlorides, Hydroxides, Sulphides, Carbonates, Phosphates etc. salts.
·Detection of elements – Nitrogen, Sulphur and halogens.
·Standardization of thermometers and determination of melting points
·Determination of boiling points.
·Mixed melting point determination.
·Purification of organic compounds: sublimation, crystallization and distillation.
·Chemical kinetics – hydrolysis of methyl acetate/ ethyl acetate catalyzed by H+ ions
·Effect of strength of acids on hydrolysis of ester
·Preparation of arsenius sulphides sol. A comparative account of mono, di and tri-valent ions during coagulation
·Surface tension determination
·Percentage composition of binary mixtures by surface tension.