CHAPTER 4 :CHEMICAL BONDING

Lecture 1

a) Describe the formation of the following bonds using Lewis dot symbol.

i. Ionic or electrovalent bond

ii. Covalent bond

iii. Dative or coordinate bond

(b) Draw Lewis structure of covalent species with single, double and triple bonds.

(c) Compare the bond length between single, double and triple bonds.

(d) Determine the formal charge and the most plausible Lewis structure.

(e) Explain the exception to the octet rule: incomplete octet, expanded octet and odd number electrons.

(h) Explain the concept of resonance using appropriate examples.

Lecture 2

(a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR)

(b) Draw the basic molecular shapes: linear, trigonal planar, tetrahedral, trigonal bipyramidal and octahedral.

(c) Predict and explain the shapes of molecule and bond angles in a given species.

Lecture 3

At the end of the lesson the students should be able to:

    • Describe a hybridization process.

    • Draw and explain hybrid orbital sp3.

    • Use hybrid orbitals to explain bond formation in selected molecules.