2. 1 s orbital

3. 2 Bonding between two s orbitals This is called a sigma (  ) bond.

4. 3 note: the amount of overlap that gives the lowest energy (most stable)

5. 4 p orbitals Family portrait

6. 5  (sigma) bonds s-s overlap s-p overlap p-p overlap

7. 6 p orbitals again

8. 7  bond (2 overlapping regions form 1 bond) What would be the effect of the orbitals rotating independently?

9. 8 Enter Hybridization The geometries and the angles don’t match orbital shapes.

10. 9 Bring in the mathematicians!

11. 10 Orbitals are combined to form hybrids. s + p + p = sp 2 1/3 s and 2/3 p in character

12. 11 sp 2 again

13. 12 sp 2 (trigonal planar)  (sigma) bonds  bond

14. 13 1/2  bond Find the  bonds the other 1/2 

15. 14 p-orbital left over after hybidization

16. 15

17. 16 sp 3 hybridization 1/4 s and 3/4 p

18. 17 sp 3

19. 18

20. 19

21. 20 H-C  C-H How many sigma (  ) bonds are in this molecule? How many pi (  ) bonds are in this molecule? Hybridization??

22. 21

23. 22

24. 23

25. 24 BeF 2 Hybridization?

26. 25

27. 26 Hybridization?

28. 27

29. 28

30. 29