1. COVALENT BONDING: ORBITALS Chapter 9

2. Hybridization The mixing of atomic orbitals to form special molecular orbitals for bonding. The atoms are responding as needed to give the minimum energy for the molecule.

3. Molecular Geometry & Hybridization Parent geometry determines the hybridization. Molecular structure is the actual geometry.

4. CH4

5. Energy-level diagram showing the formation of four sp 3 hybrid orbitals.

6. One 2s and three 2p orbitals hybridize to form a new set of sp 3 hybrid orbitals.

7. sp 3 hybrid orbital 4 effective electron pairs. Steric Number 4 tetrahedral geometry. 109.5 o bond angle.

8. The tetrahedral set of four sp 3 orbitals of the carbon atom share one electron each with the four hydrogen atoms to make a methane molecule.

9. The nitrogen atom in ammonia is sp 3 hybridized.

10. 09_164 E 2p 2ss Orbitals in an isolated carbon atom sp 2 Carbon orbitals in ethylene Hybridization 2p An orbital energy-level diagram for sp 2 hybridization.

11. In sp 2 hybridization one p orbital remains unchanged and lies perpendicular to the plane of the hybrid.

12. sp 2 hybrid orbital three effective electron pairs. trigonal planar geometry. 120 o bond angle.

13. Two sp orbitals are formed when one s and one p orbital are hybridized. They are oriented at 180 o to each other.

14. The hybrid orbitals in the CO 2 molecule.

15. sp hybrid orbital two effective electron pairs. linear geometry. 180 o bond angle.

16. The nitrogen molecule forms a triple bond -- one  and two  bonds.

17. dsp 3 hybrid orbitals five effective electron pairs. trigonal bipyramidal geometry. 90 o and 120 o bond angles. hybrid orbitals are not all equivalent as in the other types of hybridization. Phosphorus pentachloride

18. d 2 sp 3 hybrid orbitals six effective electron pairs. octahedral geometry. 90 o bond angles. Sulfur hexafluoride.

19. The relationship of the number of effective pairs, their spatial arrangement, and the hybrid orbitals.

20. The orbitals used to form the bonds in ethylene.

21. Pi and Sigma Bonds sigma (  ) bonds consist of an electron pair shared in the area centered between the atoms. pi (  ) bond bonds occupy the space above and below a line joining the atoms.

22. A carbon-carbon double bond consists of a  bond and a  bond. The  bond is formed from unhybridized p orbitals in the space above and below the  bond.

23. Sigma and pi bonds All single bonds are sigma bonds A double bond is one sigma and one pi bond A triple bond is one sigma and two pi bonds.

24. Pi and Sigma Bonds (  ) bonds allow rotation. (  ) bonds do not allow rotation.

25. The shared electron pair of in ethylene occupies the region directly between the atoms to form a sigma (  ) bond.

26. A sigma (  ) bond centers along the internuclear axis. A pi (  ) bond occupies the space above and below the internuclear axis.

27. Pi and Sigma Bonds  bonds in a molecule are described as being localized.  bonds are considered to be delocalized over the entire molecule.

28. The  bonding system in the benzene molecule.