1. Co-ordinate Covalent Bonds and Resonance Structures

2. Co-ordinate Covalent Bond A covalent bond is formed by two atoms sharing a pair of electrons. The atoms are held together because the electron pair is attracted by both of the nuclei. In a simple covalent bond, each atom supplies one electron to the bond - but that doesn't have to be the case. A co-ordinate bond is a covalent bond (a shared pair of electrons) in which both electrons come from the same atom.

3. Example: NH 4 +

4. Rules for molecules with an overall charge: 1.When figuring out the number of electrons available (ie. counting the valence electrons), add or subtract electrons as indicated by the charge. 2.Create the Lewis structure the same as always 3. Put [square] brackets around the structure 4. Write the charge as a superscript

5. Do you remember polyatomic ions? FormulaNameFormulaName NH 4 + /NH 3 Ammonium/Ammonia CrO 4 -2 Chromate C2H3O2-C2H3O2- AcetateCr 2 O 7 -2 Dichromate CH 3 COO - AcetateMnO 4 - Permanganate CN - CyanideMnO 4 -2 Manganate CO 3 -2 CarbonateNO 2 - Nitrite HCO 3 - BicarbonateNO 3 - Nitrate C 2 O 4 -2 OxalateOH - Hydroxide ClO - HypochloritePO 4 -3 Phosphate ClO 2 - ChloriteSCN - Thiocyanate ClO 3 - ChlorateSO 3 -2 Sulfite ClO 4 - PerchlorateSO 4 -2 Sulfate S 2 O 3 -2 ThiosulfateHSO 4 - Hydrogen sulfate BrO - HypobromiteIO 3 - Iodate AsO 2 -3 ArseniteSeO 4 -2 Selenate BrO 3 - BromateHSO 3 - Hydrogen sulfite

6. Try it: CO 3 -2 C: 4 e -, O: 6 x 3 e -, (-2): e - = total 24 e -O C O

7. Try it: CO 3 -2 C: 4 e -, O: 6 x 3 e -, (-2): e - = total 24 e -O C O

8. Try it: CO 3 -2 C: 4 e -, O: 6 x 3 e -, (-2): e - = total 24 e -O C O

9. Try it: CO 3 -2 O OOCOOOCO All 24 e- have been used, buy C does NOT have a complete octet….. Need to make a double bond….Does it matter which O it makes the double bond with?

10. Try it: CO 3 -2 O OOCOOOCO The bond can go here but it could also go between the C and either of the other Os

11. Finished Product CCC -2

12. Resonance Structures The Lewis structure for CO 3 shows two different types of bonds, single and double. Double bonds also have a shorter bond length, the distance between the nuclei of the two atoms in the bond, than single bonds do. Thus, if the above Lewis structure for nitrate were correct, the carbonate ion would have one bond that is shorter and stronger than the other two. This is not the case. All three of the bonds in the carbonate ion are the same strength and the same length. Interestingly, the behaviour of the bonds suggests they are longer than double bonds and shorter than single bonds. They are also stronger than single bonds but not as strong as double bonds.

13. Resonance Structures (2) So the carbonate ion would actually 3 bonds, with the bond lengths between the characteristic single and double bond lengths The important points to remember about resonance forms are:  The molecule is not rapidly oscillating between different discrete forms  There is only one form of the each molecule, we need to draw two (or more) Lewis structures because a single structure is insufficient to describe the real structure

14. Drawing them: Expressing resonance when drawing Lewis structures is done by drawing each of the possible resonance forms and placing double-headed arrows between them

15. Carbonate ion: CCC -2

16. Try these: 1.O 3 2.NO 3 -1 3.HCO 2 -1 4.CN -1 5.SO 3 2- 6. BrO -1 7. PO 4 3- 8. IO 3 -1 9. CHO 2 -1 10. NO 2 +1