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JEE Advanced NIC |
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Re: JEE Advanced NIC
JEE Main & Advanced syllabus is a list of topics and sub-topics that are specifically and solely specified by the Central Board of Secondary Education (CBSE). The Syllabus of Indian Institutes of Technology-Joint Entrance Examination (IIT-JEE) (Advanced) is as follows: CHEMISTRY Physical chemistry General topics Concept of atoms and molecules; Daltons atomic theory; Mole concept; Chemical formulae; Balanced chemical equations; Calculations (based on mole concept) involving common oxidation-reduction, neutralisation, and displacement reactions; Concentration in terms of mole fraction, molarity, molality and normality. Gaseous and liquid states Absolute scale of temperature, ideal gas equation; Deviation from ideality, van der Waals equation; Kinetic theory of gases, average, root mean square and most probable velocities and their relation with temperature; Law of partial pressures; Vapour pressure; Diffusion of gases. Atomic structure and chemical bonding Bohr model, spectrum of hydrogen atom, quantum numbers; Wave-particle duality, de Broglie hypothesis; Uncertainty principle; Qualitative quantum mechanical picture of hydrogen atom, shapes of s, p and d orbitals; Electronic configurations of elements (up to atomic number 36); Aufbau principle; Paulis exclusion principle and Hunds rule; Orbital overlap and covalent bond; Hybridisation involving s, p and d orbitals only; Orbital energy diagrams for homonuclear diatomic species; Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects only); VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, trigonal bipyramidal, tetrahedral and octahedral). Energetics First law of thermodynamics; Internal energy, work and heat, pressure-volume work; Enthalpy, Hesss law; Heat of reaction, fusion and vapourization; Second law of thermodynamics; Entropy; Free energy; Criterion of spontaneity. Chemical equilibrium Law of mass action; Equilibrium constant, Le Chateliers principle (effect of concentration, temperature and pressure); Significance of ΔG and ΔG0 in chemical equilibrium; Solubility product, common ion effect, pH and buffer solutions; Acids and bases (Bronsted and Lewis concepts); Hydrolysis of salts. Electrochemistry Electrochemical cells and cell reactions; Standard electrode potentials; Nernst equation and its relation to ΔG; Electrochemical series, emf of galvanic cells; Faradays laws of electrolysis; Electrolytic conductance, specific, equivalent and molar conductivity, Kohlrauschs law; Concentration cells. Chemical kinetics Rates of chemical reactions; Order of reactions; Rate constant; First order reactions; Temperature dependence of rate constant (Arrhenius equation). Solid state Classification of solids, crystalline state, seven crystal systems (cell parameters a, b, c, , , ), close packed structure of solids (cubic), packing in fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic compounds, point defects. Solutions Raoults law; Molecular weight determination from lowering of vapour pressure, elevation of boiling point and depression of freezing point Surface chemistry Elementary concepts of adsorption (excluding adsorption isotherms); Colloids: types, methods of preparation and general properties; Elementary ideas of emulsions, surfactants and micelles (only definitions and examples). Nuclear chemistry Radioactivity: isotopes and isobars; Properties of , and rays; Kinetics of radioactive decay (decay series excluded), carbon dating; Stability of nuclei with respect to proton-neutron ratio; Brief discussion on fission and fusion reactions. |
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