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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.

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Hybridization

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  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?

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