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Jammu Kashmir BPEE Common Entrance Test 2018 Chemistry Syllabus – Page 2
UNIT 1 : CHEMICAL ARITHMETIC & ATOMIC STRUCTURE ( Marks : 03 )
Laws of chemical combination, Mole concept ( numericals ) Percentage composition, Chemical reactions, Stoichiometry and calculations based on stoichiometry.
Atomic structure : Bohr‘s model of Hydrogen atom, Quantum numbers, Pauli‘s exclusion principle, Hund‘s rule and Aufbau principle. Heisenberg‘s uncertainty principle, de – Broglie wave equation and its significance.
UNIT 2 : CHEMICAL EQUILIBRIUM ( Marks : 04 )
Law of mass action, Le – Chatelier‘s principle, and its application to physical and chemical equilibria. Ionisation of weak electrolytes ( Ostwald‘s dilution law )
Acids and bases : Acid base equilibria. Bronsted – Lowry and Lewis concept, of acids and bases. Ionic product of water. pH and pOH scales, pKa & pKb values, Solubility product, Buffer solutions Common ion effect, Hydrolysis
UNIT 3 : CHEMICAL KINETICS ( Marks : 02 )
Rate of chemical reaction, Average and instantaneous rate, Factors effecting rate of reaction, Order and molecularity of reaction, Integrated rate equation and Half – life period ( for zero and first order ) reaction, Activation energy and Arrhenius equation.
UNIT 4 : SOLUTIONS ( Marks : 02 )
Vapour pressure, Raoult‘s law, Ideal and Non – ideal solutions, Colligative properties. Determination of molecular mass of non – volatile solutes through colligative properties. Abnormal molecular masses and Van‘t Hoff Factor.
UNIT 5 : CHEMICAL THERMODYNAMICS ( Marks : 04 )
Energy changes taking place during chemical reactions, Internal Energy and Enthalpy changes, Enthalpy of combustion, Solution and Neutralization. Hess‘s Law ( Numerical problems ) Laws of thermodynamics – first, second & third, Concepts of Entropy and Free energy, Spontaneity of a chemical reaction and Thermodynamic equilibrium.
UNIT 6 : REDOX REACTIONS AND ELECTROCHEMISTRY ( Marks : 03 )
Dependence of electrode and cell potential on concentration ( Nernst Equation ), Electrode potential as a criteria for product formation in electrolysis. E.M.F. of Galvanic cell, Relationship between free energy change and E.M.F. of a cell. Definition and units of Equivalent, Molar and Specific conductivity.
UNIT 7 : SOLID STATE & STATES OF MATTER ( Marks : 04 )
Boyle‘s Law, Charle‘s law, Dalton‘s law of partial pressure, Graham‘s law of diffusion of gases. Causes of deviation from ideal behaviour, ideal gas equation and nature of oR‘, Vander Waal‘s equation, surface tension and viscosity of liquids.
Crystalline and amorphous solids, Crystal lattice, Crystal types, Packing efficiency, calculation of density of unit cell, Number of atoms per unit cell in a cubic cell. Co – ordination number, Stoichiometric defects: Schottky, Frenkel and interstitial.
Properties of solids : Electrical, Magnetic & Dielectric.
UNIT 8 : SURFACE CHEMISTRY ( Marks : 02 )
Freundlich Adsorption isotherm, preparation of colloidal solutions by physical and chemical method. Electrical properties ( cataphoresis, electroosmosis, coagulation and protective colloids ) Homogeneous and Heterogeneous Catalysis.
UNIT 9 : PERIODIC PROPERTIES ( Marks : 02 )
Classification of elements as s, p, d, and f block elements. Variation of Ionization energy, Electron affinity, Electronegativity, Atomic and Ionic radii along the period and down the group in the periodic table.
UNIT 10 : CHEMICAL BONDING AND MOLECULAR STRUCTURE ( Marks : 04 )
Types of chemical bonds, Ionic & covalent bonds, Bond parameters, Quantum theory of covalent bond, pi and sigma bonds, Hybridization involving s, p and d-orbitals, Dipole moments and hydrogen bond. VSEPR: Shapes of simple molecules ( H2O, NH3, SO2, CO2, PCl3, PCl5, CIF3, BF3, SF4, XeF2, XeF4 ). Molecular orbital theory: Energy Levels and M.O. diagrams of H2, H2 +,He2, O2, O2-2 ,O1-2,O22- & F2. Bond order and its significance.