1 / 15

Hybridization

Hybridization. A Blending of Orbitals. Methane. CH 4 Sometimes called “natural gas, ” methane is used to heat homes. Shape of Methane. Tetrahedral geometry 109.5 o angle between bonds. Carbon’s atomic orbitals. 4 valence electrons Outermost orbitals: 2s, 2p x , 2p y , 2p z.

searwood
Télécharger la présentation

Hybridization

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Hybridization A Blending of Orbitals

  2. Methane • CH4 • Sometimes called “natural gas, ” methane is used to heat homes.

  3. Shape of Methane • Tetrahedral geometry • 109.5o angle between bonds

  4. Carbon’s atomic orbitals • 4 valence electrons • Outermost orbitals: 2s, 2px, 2py, 2pz

  5. How can this happen?

  6. 2 possibilities • Maybe our quantum mechanical model of atomic orbitals is totally wrong. OR • Maybe carbon is doing something else with its orbitals to form this compound.

  7. Hybridization occurs • A mathematical blending of orbitals • Number of atomic orbitals blended = number of hybrid orbitals produced • Result: Identical orbitals • New shape • New orientation in space

  8. sp3 hybridization • s + px + Py + pz = 4 sp3 orbitals

  9. Sp3 hybridization on carbon • 4 identical sp3 orbitals • 109.5o between orbitals • Tetrahedral orientation

  10. Bonds form when orbitals overlap • Sigma bonds: end to end overlap of orbitals

  11. What happens in ethene? C2H4 • Properties • Double bond between carbons • Trigonal planar geometry around C • 120o bond angles

  12. Sp2 hybridization occurs • S + px + py = 3 sp2 orbitals • 1 unused p orbital left over

  13. Bonding in ethene • Sigma bond: end to end overlap • Pi bond: side to side overlap

  14. Putting ethene together • Carbon-carbon double bond = 1 sigma bond and 1 Pi bond • 4 C-H sigma bonds • Trigonal planar geometry results

  15. What happens in ethyne? • C2H2 • Linear geometry • What type of hybridization is involved? • What hybrid and atomic orbitals can it use? • What types and numbers of bonds are present in the molecule?

More Related