1. 6-5 Molecular Geometry

2. VSEPR Theory VSEPR theory – states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible Shared pairs are oriented as far away from each other as possible

3. VSEPR Theory VSEPR and Unshared Electron Pairs – lone pair occupies space around the atom just as the bonding pairs do

4. Hybridization Hybridization – the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies What does hybridization mean???

5. Ex. of hybridization… Methane, CH 4, C __ __ __ __ __ 1s 2s 2p How does carbon form four equivalent, tetrahedrally arranged covalent bonds by orbital overlap with four other atoms?

6. Ex. of hybridization… Methane, CH 4, undergoes hybridization C __ __ __ __ __ 1s sp 3 Hybrid orbitals- orbitals of equal energy produced by the combination of two or more orbitals on the same atom

7. Intermolecular Forces Intermolecular forces – the forces of attraction between molecules vary in strength but are generally weaker than bonds that join atoms in molecules, ions in ionic compounds, or metal atoms in solid metals

8. Hydrogen Bonding Hydrogen bonding- hydrogen atom is bonded to a highly electronegative atom, that group is attracted to other nearby molecules Hydrogen bonds are usually represented by dotted lines connecting the hydrogen-bonded hydrogen