1. Ch 9 – Covalent Bonding: Orbitals

2. VSEPR Model VSEPR – valence shell electron pair repulsion model
Is useful in predicting the geometries of covalently bonded molecules
The structure around a given atom is determined principally by minimizing electron-pair repulsions

3. Hybridization
Some atoms combine orbitals so they can move electrons around and have more electrons available for bonding.
This is called hybridization.

4. sp3 Hybridization
The s orbital and the three p orbitals combine to create 4 equal energy orbitals. Each hybrid orbital is ¼ s and ¾ p character.

5. With all orbitals being equidistant at 109
With all orbitals being equidistant at 109.5o, the result is a tetrahedral shape.

6. sp2 Hybridization
The s orbital and two p orbitals combine to create 3 equal energy orbitals. Each hybrid orbital is 1/3 s and 2/3 p character.

7. The result are 3 hybrid orbitals and 1 unchanged orbital.

8. The resulting shape is trigonal planar with 120o bond angles.

9. sp Hybridization
The s orbital and one p orbital combine to create 2 equal energy orbitals. Each hybrid orbital is ½ s and ½ p character. There are two unchanged p orbitals.

10. The resulting shape is linear with 180o bond angles.

11. dsp3 hybridization
The key is having 5 pair of electrons around the central atom. They can be shared or unshared and the bond angles are 120o from side to side and 90o between top and bottom.
90o
120o

12. Trigonal bipyramidal
1 pair of d orbital electrons, 1 pair of s orbital electrons and 3 pair of p orbital electrons are hybridized.

13. d2sp3 hybridization
The key is having 6 pair of electrons around the central atom. They can be shared or unshared and the bond angles are all 90o

14. Octahedral
2 pair of d orbital electrons, 1 pair of s orbital electrons and 3 pair of p orbital electrons are hybridized.