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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Bob Bobson on October 06, 2004, 10:56:11 AM

Title: hybridization of orbitals
Post by: Bob Bobson on October 06, 2004, 10:56:11 AM

My textbook says that pi bonds generally do not hybridize.  What I want to know is why don't they?  Is it just a fact that is accepted by experimental evidence or is there some concept that could be better understood?  Thanks.

Title: Re:hybridization of orbitals
Post by: Demotivator on October 06, 2004, 11:12:47 AM

Hybridization is a reconfiguring/mixing of atomic orbitals that occurs to produce maximum bonding overlap. This is important in sigma bond formation. But with pi bonds, the atomic orbitals already happen to be "optimally" oriented for maximum overlap and therefore do not gain from hybridization.
Mathematically, p orbitals have + and - phases above and below the plane. When mixed with S orbitals (+ phase), the opposite phase lobe gets almost wiped out while the other lobe gets enhanced. That's good for sigma bonding, but not good for pi bonding which needs both ends above and below the plane.