1. Starter Complete the full electronic configuration of: 1)Ti 2)Br 3)Cl - 4)Ca 2+ 5)Fe 3+ 6)Co 3+

2. Covalent bonding L.O.: Describe a covalent bond as a shared pair of electrons. Describe single and multiple covalent bonding. Use dot-and-cross diagrams to represent covalent bonding. Describe dative covalent (coordinate) bonding. Use dot-and-cross diagrams to represent covalent bonding

3. Octet rule.

4. A covalent is a bond formed by a shared pair of electrons.

5. Covalent bond formation in H 2

6. Covalent bonding in Cl 2

7. Covalent bonding in H 2 O, NH 3 and CH 4

8. Draw dot-and-cross diagrams for: a) Cl 2 b) HCl c) SiF 4 d) SCl 2

12. Q2, page 55.

13. Dative covalent bonding in NH 4 + A dative covalent bond is a shared pair of electrons which has been provided by one of the bonding atoms only.

14. The ammonium ion

15. The oxonium ion

16. Dot-and-cross diagram of BF 3

17. Dot-and-cross diagram of SF 6

18. Expansion of the octet: o unpaired electrons pair up o The maximum number of electrons that can pair up is equivalent to the number of electrons in the outer shell.

19. Qs 1&2, page 57.