1. -Understand how the absence or presence of lone pairs of electrons affects the geometry of a molecule -Know what the various geometries are and how to predict them -Understand the concept of orbital hybridization and how it changes the bonding in an atom such as carbon (NEXT LECTURE)

2. The arrangement of atoms within a given molecule. ( Section 8.3 232-236 in your textbook) Valence Shell Electron Pair Repulsion = VSEPR

3. Assumption: Electron pairs repulse each other Consequences 1)This repulsion of electron pairs causes them to orientate as far from each other as possible. 2)Atom centers also want to be as far apart as possible

5. 2 Bonding pairs 0 lone pairs AX 2

6. .. 2 Bonding pairs 2 lone pairs :AX 2 :

7. 3 Bonding Pairs 0 lone pairs AX 3

8. 3 bonding pairs One lone pair :AX 3

9. 4 bonding pairs 0 lone pairs AX 4

10. Summary of Five Main Geometries Linear Formula= AX 2 Bent Formula = : AX 2 : Trigonal Planar Formula = AX 3 Trigonal Pyramidal Formula = : AX 3 Tetrahedral Formula = AX 4 Note: A –represents the central atom X – represents the attached atom

11. 5 cards in your packet … one for each geometry. As a group, use your whiteboards to draw the Lewis dot structure for each one of your compound cards. Once you have the Lewis Dot structure, use it as a guide to construct a model of the compound. I will walk around and check your Lewis Dot structures and models. Create a group sheet to record those Lewis Dot structures/models that you are having trouble with. We will have cool down that you will hand in today (exit slip)

12. Groupwork norm I will also be assessing …. Every student contributes when every student feels safe to make mistakes in the group. What the fudge?! DON’T JUDGE!

13. Hybridization

14. The electron structure of a carbon atom can be written as: Based on this model, we would predict that carbon atoms should form two covalent bonds??!!

15. Instead carbon atoms almost always form 4 bonds. Why???? Hybridization

16. hybridization 1 s + 3 p = 4 sp 3 (All 4 orbitals are now equal at the 2nd energy level) Regular Carbon Aufbau Diagram Hybridized Carbon Aufbau Diagram

17. Electrons must be distributed among the new orbitals. Since these hybrid orbitals are equal in energy, the electrons must distributed according to Hund’s Rule.

18. 4 sp 3 orbitals

19. 4 sp 3 orbitals bond with 4 hydrogen atoms - methane sp 3 carbon Overlap here is known as sigma bond

20. sp 2 hybridization

21. sp 2 hybridization carbon double bond - ethene

22. sp hybridization

23. sp hybridization carbon triple bond - acetylene

24. 234-236 in your text discusses these examples