SECTION: A<\/p>\n
PHYSICAL CHEMISTRY<\/strong><\/p>\n <\/p>\n UNIT 1: SOME BASIC CONCEPTS IN CHEMISTRY<\/strong><\/p>\n Matter and its nature, Dalton\u2019s atomic theory; Concept of atom, molecule, element and compound; Physical quantities and their measurements in Chemistry, precision and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular\u00a0<\/p>\n formulae; Chemical equations and stoichiometry.<\/p>\n <\/p>\n UNIT 2: STATES OF MATTER\u00a0<\/strong><\/p>\n Classification of matter into solid, liquid and gaseous states.\u00a0Gaseous State:<\/p>\n Measurable properties of gases; Gas laws – Boyle\u2019s law, Charle\u2019s law, Graham\u2019s law of diffusion, Avogadro\u2019s law, Dalton\u2019s law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation; Kinetic theory of gases (only postulates); Concept of average, root mean square and most probable velocities; Real gases, deviation from Ideal behaviour, compressibility factor and van der Waals equation.<\/p>\n Liquid State:<\/strong><\/p>\n Properties of liquids – vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).\u00a0<\/p>\n Solid State:<\/strong><\/p>\n Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Bragg\u2019s Law and its applications; Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, imperfection in solids; Electrical, magnetic and dielectric properties.<\/p>\n UNIT 3: ATOMIC STRUCTURE<\/strong><\/p>\n Thomson and Rutherford atomic models and their limitations; Nature of\u00a0electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom,\u00a0Bohr model of hydrogen atom – its postulates, derivation of the relations for\u00a0energy of the electron and radii of the different orbits, limitations of Bohr\u2019s\u00a0model; Dual nature of matter, de-Broglie\u2019s relationship, Heisenberg uncertainty\u00a0principle. Elementary ideas of quantum mechanics, quantum mechanical model\u00a0<\/p>\n of atom, its important features, ?? and ??2, concept of atomic orbitals as one electron wave functions; Variation of ?? and ??2 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 \u2013 aufbau principle, Pauli\u2019s exclusion principle and Hund\u2019s rule, electronic configuration of\u00a0 <\/p>\n UNIT 4: CHEMICAL BONDING AND MOLECULAR STRUCURE<\/strong><\/p>\n Kossel – Lewis approach to chemical bond formation, concept of ionic and\u00a0covalent bonds.<\/p>\n Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.\u00a0<\/p>\n Covalent Bonding:<\/p>\n Concept of electronegativity, Fajan\u2019s 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.<\/p>\n 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.<\/p>\n UNIT 5: CHEMICAL THERMODYNAMICS<\/strong><\/p>\n Fundamentals of thermodynamics: System and surroundings, extensive and\u00a0intensive properties, state functions, types of processes.<\/p>\n First law of thermodynamics – Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess\u2019s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution.<\/p>\n Second law of thermodynamics; Spontaneity of processes; DS of the universe and DG of the system as criteria for spontaneity, Dgo (Standard Gibbs energy change) and equilibrium constant.<\/p>\n UNIT 6: SOLUTIONS<\/strong><\/p>\n Different methods for expressing concentration of solution – molality, molarity,\u00a0mole fraction, percentage (by volume and mass both), vapour pressure of\u00a0solutions and Raoult\u2019s Law \u2013 Ideal and non-ideal solutions, vapour pressure –\u00a0composition, plots for ideal and non-ideal solutions; Colligative properties of\u00a0dilute solutions – relative lowering of vapour pressure, depression of freezing\u00a0point, elevation of boiling point and osmotic pressure; Determination of\u00a0molecular mass using colligative properties; Abnormal value of molar mass,\u00a0van\u2019t Hoff factor and its significance.<\/p>\n <\/p>\n UNIT 7: EQUILIBRIUM<\/strong><\/p>\n Meaning of equilibrium, concept of dynamic equilibrium.\u00a0Equilibria involving physical processes: Solid -liquid, liquid – gas and solid \u2013 gas\u00a0equilibria, Henry\u2019s law, general characterics of equilibrium involving physical\u00a0processes.<\/p>\n Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of DG and DGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier\u2019s principle.<\/p>\n Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Br??nsted – 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.<\/p>\n UNIT 8: REDOX REACTIONS AND ELECTROCHEMISTRY<\/strong><\/p>\n Electronic concepts of oxidation and reduction, redox reactions, oxidation\u00a0number, rules for assigning oxidation number, balancing of redox reactions.Eectrolytic and metallic conduction, conductance in electrolytic solutions,\u00a0specific and molar conductivities and their variation with concentration:\u00a0Kohlrausch\u2019s law and its applications.\u00a0<\/p>\n 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\u2019 energy change; Dry cell and lead accumulator; Fuel cells.<\/p>\n <\/p>\n UNIT 9 : CHEMICAL KINETICS\u00a0<\/strong><\/p>\n Rate of a chemical reaction, factors affecting the rate of reactions:\u00a0concentration, temperature, pressure and catalyst; elementary and complex\u00a0reactions, order and molecularity of reactions, rate law, rate constant and its\u00a0units, differential and integral forms of zero and first order reactions, their\u00a0characteristics and half – lives, effect of temperature on rate of reactions \u2013\u00a0Arrhenius theory, activation energy and its calculation, collision theory of\u00a0bimolecular gaseous reactions (no derivation).<\/p>\n <\/p>\n UNIT-10 : SURFACE CHEMISTRY<\/strong><\/p>\n Adsorption- Physisorption and chemisorption and their characteristics, factors\u00a0affecting adsorption of gases on solids – Freundlich and Langmuir adsorption\u00a0isotherms, adsorption from solutions.\u00a0Colloidal state – distinction among true solutions, colloids and suspensions,\u00a0classification of colloids – lyophilic, lyophobic; multi molecular, macromolecular\u00a0and associated colloids (micelles), preparation and properties of colloids –\u00a0Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation and\u00a0flocculation; Emulsions and their characteristics.<\/p>\n","protected":false},"excerpt":{"rendered":" AIEEE CHEMISTRY SYLLABUS SECTION: A PHYSICAL CHEMISTRY UNIT 1: SOME BASIC CONCEPTS IN CHEMISTRY Matter and its nature, Dalton\u2019s atomic theory; Concept of atom, molecule, element and compound; Physical quantities and their measurements in Chemistry, precision and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, … Read more<\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"fifu_image_url":"","fifu_image_alt":""},"categories":[1],"tags":[1956,26],"amp_enabled":true,"_links":{"self":[{"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/posts\/13415"}],"collection":[{"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/comments?post=13415"}],"version-history":[{"count":0,"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/posts\/13415\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/media?parent=13415"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/categories?post=13415"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.kopykitab.com\/blog\/wp-json\/wp\/v2\/tags?post=13415"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\nelements, extra stability of half-filled and completely filled orbitals.<\/p>\n