2. Section 8.4 – Molecular Shapes
Summarize the VSEPR bonding theory.
Predict the shape of, and the bond angles in, a molecule.
Define hybridization.

3. VSEPR Theory
Valence
Shell
Electron
Pair
Repulsion

4. VSEPR Theory (Continued)
Used to determine molecular shape.
Shared and unshared pairs of electrons repel each other to minimize repulsion.
Electron pairs located as far apart as possible from each other.

5. Hybridization
Hybridization – atomic orbitals mix and form new, identical, hybrid orbitals.
Single, double, and triple bonds occupy only one hybrid orbital.

6. Hybridization (Cont.)

7. Hybridization (Cont.)

8. Hybridization (Cont.)

9. Hybridization (Cont.)

10. Assessment
The two lone pairs of electrons on a water molecule do what to the bond angle between the hydrogen atoms and the oxygen atom?
A. They attract the hydrogen atoms and increase the angle greater than 109.5°.
B. They occupy more space and squeeze the hydrogen atoms closer together.
C. They do no affect the bond angle.
D. They create resonance structures with more than one correct angle.

11. Assessment
The two lone pairs of electrons on a water molecule do what to the bond angle between the hydrogen atoms and the oxygen atom?
B. They occupy more space and squeeze the hydrogen atoms closer together.

12. Assessment The sp3 hybrid orbital in CH4 has what shape? A. linear
B. trigonal planar
C. tetrahedral
D. octahedral

13. Assessment The sp3 hybrid orbital in CH4 has what shape?
C. tetrahedral

14. Assignment – Pg. 264, Problems 56-59
Determine the molecular shape, bond angle, and hybrid orbitals for each molecule:
56. BF3
57. OCl2
58. BeF2
59. CF4