1. Chapter 9 Valence Bond
Theory

2. Valence Bond Theory Related to Lewis Dot Structures
Bonding electron pairs and lone pairs
Explains bonding in molecules with multiple atoms
Bonds are formed by overlap of atomic orbitals (s, p and d)

5. Sigma bond (s) – a single covalent bond resulting from the overlap of two orbitals.
The electron density of the two bonding electrons is between the atoms

6. Valence Bond Theory Orbitals overlap to form bonds
Two electrons are used to form bonds
Bonding electrons are found in the region between atoms

7. Orbital Hybridization
Bonding with more than two atoms
Hybrid orbitals result from the mixing
of s, p and d orbitals
The number of hybrid orbitals is equal to the number of atomic orbitals that are mixed

8. Set of Hybrid Orbitals
sp – results from mixing an s orbital with one p orbital
sp2 – mixing an s orbital with two p orbitals
sp3 – mixing an s orbital with three p orbitals

9. Bonding with more than two atoms

11. BF3

12. NH3

13. H2O

14. CH3CH3

15. Stop