1. Chemical Bonding - HL

2. Predict the shape and bond angles for species with five and six negative charge centers using VSEPR theory.
Expanded valence shell
Promote s electron to d shell
Form bond to small, electronegative elements such as F, O, Cl

3. PF5 5 Charge centers trigonal bipyramidal

4. SF4 5 charge centers Saw-horse

5. ICl3 5 charge centers T-shaped

6. XeF2 5 charge centers Linear

7. SF6 6 charge centers Octahedral

8. BrF 6 charge centers square pyramid5

9. XeF4 6 charge centers square planar

10. 14.2.1 Describe sigma and pi bonds
A sigma bond is a bond where the electron density is concentrated along the intranuclear axis
A pi bond is a bond where the electron density is concentrated on either side of an imaginary line joining the 2 nuclei (the intranuclear axis)

12. Explain hybridization in terms of the mixing of atomic orbitals to form new orbitals for bonding.
identify and explain the relationships between Lewis structures, molecular shapes and types of hybridization (sp; sp2; sp3)

15. SP3 hybridization

16. SP2 hybridization

20. Hybridization in NH3?
Hybridization in BF3?

21. Hybridization Summary
Number of regions of electron density
Hybridization of central atom
Shape
Examples 1
Unhybridized
Linear
H-H H-Cl 2 sp
HCCH O=C=O 3
sp2
Triangular planar
H2C=CH2 BF3 4
sp3
tetrahedral
CH4 NH3 H2O

22. Resonance structures

24. Delocalized electrons