Hybridization

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Hybridization

• A Blending of Orbitals

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Methane

• CH4
• Sometimes called natural gas, methane is used
  to heat homes.

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Shape of Methane

• Tetrahedral geometry
• 109.5o angle between bonds

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Carbons atomic orbitals

• 4 valence electrons
• Outermost orbitals 2s, 2px, 2py, 2pz

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How can this happen?
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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.

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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

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sp3 hybridization

• s px Py pz 4 sp3 orbitals

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Sp3 hybridization on carbon

• 4 identical sp3 orbitals
• 109.5o between orbitals
• Tetrahedral orientation

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Bonds form when orbitals overlap

• Sigma bonds end to end overlap of orbitals

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What happens in ethene?

• C2H4
• Properties
• Double bond between carbons
• Trigonal planar geometry around C
• 120o bond angles

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Sp2 hybridization occurs

• S px py 3 sp2 orbitals
• 1 unused p orbital left over

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Bonding in ethene

• Sigma bond end to end overlap
• Pi bond side to side overlap

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Putting ethene together

• Carbon-carbon double bond 1 sigma bond and 1
  Pi bond
• 4 C-H sigma bonds
• Trigonal planar
• geometry results

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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?