BOARD OF INTERMEDIATE EDUCATION,A.P,HYDERABAD

CHAPTERS PERIODS

1. ATOMIC STRUCTURE

1.1 Sub- atomic particles

1.2 Atomic models- Rutherford’s Nuclear model of atom

1.3 Developments to the Bohr’s model of atom

1.3.1 Nature of electromagnetic radiation.

1.3.2 Particle nature of electromagnetic radiation- Planck’s

quantum theory.

1.4 Bohr’s model for Hydrogen atom.

1.4.1 Explanation of line spectrum of hydrogen.

1.4.2 Limitations of Bohr’s model

1.5Quantum mechanical considerations of sub atomic particles.

1.5.1 Dual behaviour of matter.

1.5.2 Heisenberg’s uncertainty principle.

1.6 Quantum mechanical model of an atom. Important

features of Quantum mechanical model of atom.

1.6.1 Orbitals and quantum numbers.

1.6.2 Shapes of atomic orbitals.

1.6.3 Energies of orbitals.

1.6.4 Filling of orbitals in atoms. Aufbau Principle, Pauli’s

exclusion Principle and Hund’s rule of maximum multiplicity.

1.6.5 Electronic configurations of atoms.

1.6.6 Stability of half filled and completely filled orbitals.

2. CLASSIFICATION OF ELEMENTSAND PERIODICITY IN

PROPERTIES

2.1 Need to classify elements

2.2 Genesis of periodic classification.

2.3 Modern periodic law and present form of

the periodic table.

2.4 Nomenclature of elements with atomic number greater

than100

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2.5 Electronic configuration of elements and the periodic

table

2.6 Electronic configuration and types of elements

s,p,d.and f blocks.

2.7.1 Trends in physical properties:

(a) Atomic radius

(b) Ionic radius

(c)Variation of size in inner transition elements.

(d)Ionization enthalpy.

(e) Electron gain enthalpy

(f) Electro negativity.

2.7.2 Periodic trends in chemical properties:

(a) Valence or Oxidation states.

(b) Anomalous properties of second period elements –

diagonal relationship.

2.7.3 Periodic trends and chemical reactivity

3. CHEMICAL BONDING AND MOLECULAR STRUCTURE

3.1 Kossel – Lewis approach to chemical bonding.

3.2 Ionic or electrovalent bond - Factors favourable for the

formation of ionic compounds-Crystal structure of

sodium chloride-General properties of ionic compounds.

3.3 Bond Parameters – bond length, bond angle, and bond

enthalpy, bond order, resonance-Polarity of bonds

dipole moment

3.4 Valence Shell Electron Pair Repulsion (VSEPR) theories.

Predicting the geometry of simple molecules.

3.5 Valence bond theory-Orbital overlap concept-Directional

properties of bonds-overlapping of atomic orbitals

strength of sigma and pi bonds-Factors favouring the

formation of covalent bonds

3.6 Hybridisation- different types of hybridization involving

s, p and d orbitals- shapes of simple covalent molecules.

3.7 Coordinate bond –definition with examples.

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3.8 Molecular orbital theory – Formation of molecular orbitals,

Linear combination of atomic orbitals (LCAO)-conditions for

combination of atomic orbitals - Energy level diagrams for

molecular orbitals -Bonding in some homo nuclear diatomic

molecules- H