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Hanniel U 2B
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Joined: Fri Sep 28, 2018 12:16 am


Postby Hanniel U 2B » Mon Nov 19, 2018 12:22 pm

During lecture today, C2H4 had a sp^2 hybridization. But when it was expanded, it was 2sp^2 and 2p. I am confused about that.

Jonas Talandis
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

Re: Hybridization

Postby Jonas Talandis » Mon Nov 19, 2018 12:28 pm

Since each C atom only has 3 regions of electron density, and we know that the number of these regions needs to be equal to the number of hybridized orbitals, the resulting hybrid orbitals will be 3 orbitals at the sp2 level. However, since there is one p orbital unaccounted for (there are 3 p orbitals), there is one regular, unhybridized p orbital left over at the 2p energy level. This one will be at 90 degrees, resulting in the side-by-side pi bond mentioned in lecture.

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