EAMCET Syllabus
March 6, 2009 · Print This Article · Email It
CHEMISTRY
ATOMIC STRUCTURE: Characteristics of electron, proton and neutron. Rutherford model of an atom. Nature of electromagnetic radiation. Planck’s quantum theory. Explanation of photo electric effect. Dual behavior of electromagnetic radiation. Features of atomic spectra – Emission and absorption spectra. Characteristics of hydrogen spectrum. Bohr’s theory of the structure of the atom – Postulates, Theory of hydrogen atom, Energy of an electron. Bohr’s explanation of spectral lines. Failure of Bohr’s theory. Wave-particle nature of electron. De Broglie’s hypothesis, Heisenberg’s uncertainty principle. Important features of the quantum mechanical model of an atom – Meaning and significance of wave function. Quantum numbers, concept of orbitals, definition of atomic orbital in terms of quantum Numbers – shapes of s, p and d orbitals, Aufbau principle, Pauli’s exclusion principle and Hund’s rule of maximum multiplicity. Electronic configuration of atoms. Explanation of stability of half filled and completely filled orbitals.
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES: Concept of grouping elements in accordance to their properties – Mendeleef’s Periodic Table. Periodic law – Mendeleef’s classification of elements. Significance of atomic number and electronic configuration as the basis for periodic classification. Classification of elements into s, p, d, f blocks and their main characteristics. Periodic trends in physical and chemical properties of elements: Atomic radii, Ionic radii, Inert gas radii, Ionization energy, Electron gain energy, Electro- negativity, Valency, variation of oxidation states, Electropositivity – Metallic and Non-metallic nature, Nature of Oxides, Diagonal relationship. Variation of atomic radii in inner transition elements.
CHEMICAL BONDING AND MOLECULAR STRUCTURE: Kossel -Lewis approach to chemical bonding. Factors favorable for the formation of ionic bond, energy changes in ionic bond formation. Crystal lattice energy – calculation of lattice energy – Born – Haber cycle. Crystal structures of sodium chloride and Caesium chloride, Coordination number. Properties of ionic compounds. Covalent bond – VSEPR theory – Lewis representation of covalent compounds, Formal charge, geometry of simple molecules. The valence bond approach for the formation of covalent bonds. Directional properties of covalent bond. Properties of covalent bond. Hybridization – different types of hybridization involving s, p and d orbitals. Shapes of simple covalent molecules. Definition of coordinate covalent bond with examples.
STOICHIOMETRY: Laws of chemical combination. Molar mass, concept of equivalent weight with examples. Percentage composition of compounds and calculation of empirical and molecular formulae of compounds. Chemical reactions and equations, Stoichiometry. Oxidation number concept. Balancing of redox reactions by ion electron method and oxidation number method. Types of redox reactions.
STATES OF MATTER: GASES Graham’s law of diffusion, Dalton ’s law of partial pressures, Avogadro’s law. Ideal behavior, empirical derivation of gas equation, ideal gas equation. Kinetic molecular theory of gases. Kinetic gas equation (No derivation) – deduction of gas laws. Distribution of molecular velocities and types of molecular velocities – Average, Root Mean Square and Most Probable Velocity.
SOLUTIONS: Classification of solutions, molarity, normality, molality and mole fraction. Dilute solutions, vapor pressure, Raoult’s law, Limitations of Raoult’s law. Colligative properties – (i) Relative lowering of vapor pressure (ii) Elevation of B.P (iii) Depression in freezing point and their relation to molar mass. Osmosis and osmotic pressure – theory of dilute solutions. Determination of molar mass using colligative properties: Ostwald’s dynamic method, Cottrell’s method, Rast’s method and Berkeley Hartley’s method. Abnormal molecular mass.
