Chemistry Grade 11
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6.3 Ionization Energy,Electron Affinity and Electronegativity
6.3.1 Ionization Energy
6.3.1.1 Factors Influencing the Ionization Energies
6.3.1.2 Variation of Ionization Energy in the Periodic Table
6.3.1.3 Higher Ionization Energies
6.3.2 Electron Affinity
6.3.2.1 Factors Influencing the Electron Affinity
6.3.2.2 Variation in the Periodic Table
6.3.3 Electronegativity
6.3.3.1 Variation of Electronegativities in Periodic Table
6.4 TYPES OF BONDS
6.4.1 Lewis Concept
6.4.1.1 (i) Ionic Bond
6.4.1.2 (ii) Covalent Bond (electron pair bond)
6.4.1.2.1 Non-Polar Covalent Bonds
6.4.1.2.2 Polar Covalent Bonds
6.4.1.3 iii) Coordinate Covalent Bond
6.4.2 MODERN THEORIES OF COVALENT BOND
6.4.3 VALENCE SHELL ELECTRON PAIR REPULSION THEORY
6.4.3.2 Postulates of VSEPR Theory
6.4.3.2.1 Molecules Containing Two Electron Pairs (AB<sub>2</sub> type)
6.4.3.2.2 Molecules Containing Three Electron Pairs ? (AB<sub>3</sub> type:)
6.4.3.2.3 (iii) Molecules Containing Four Electron Pairs (AB<sub>4</sub>- Type:)
6.4.4 Valence Bond Theory (VBT)
6.4.5 Atomic Orbital Hybridization and Shapes of Molecules
6.4.5.1 (i) sp<sup>3</sup> Hybridization
6.4.5.2 (b) Ammonia
6.4.5.3 (c) Water, H<sub>2</sub>0
6.4.5.4 (ii) sp<sup>2</sup>- Hybridization
6.4.5.5 Bonding and Structure of Boron Trifluoride and Ethene
6.4.5.6 Bonding and Structure of Beryllium Dichloride and Ethyne
6.4.6 Molecular Orbital Theory
6.4.6.1 Head on Approach
6.4.6.2 Relative Energies of the Molecular Orbitals
6.4.6.3 Molecular Orbital Structures of Some Diatomic Molecules
6.4.6.4 (i) Helium, He<sub>2</sub>
6.4.6.5 (ii) Nitrogen, N<sub>2</sub>
6.4.6.6 (iii) Oxygen, O<sub>2</sub>