Ethene (C2H4) hybridization


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Samantha Burmester 3H
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Joined: Fri Sep 28, 2018 12:23 am

Ethene (C2H4) hybridization

Postby Samantha Burmester 3H » Mon Nov 19, 2018 11:11 pm

The last example we did in Nov 19th’s lecture was of Ethene.

I don’t understand why in the hybrid orbitals Lavelle put one electron in each of the three orbitals 2sp2 and then one in 2p. Is it because of the carbon interactions? And is the 2p hybridized?

LorenzoDuvergne3I
Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

Re: Ethene (C2H4) hybridization

Postby LorenzoDuvergne3I » Mon Nov 19, 2018 11:18 pm

The 2p is not hybridized. The reason we use the 2p orbital is because the repulsion energy between two electrons is larger than the energy gap between the hybridized orbitals and the 2p orbital. That electron has to go somewhere because carbon has 4 valence electrons. That electron is also the one used to form the pi bond, but I don't know the reason why it is not any other orbital.

Bingcui Guo
Posts: 30
Joined: Fri Sep 28, 2018 12:19 am

Re: Ethene (C2H4) hybridization

Postby Bingcui Guo » Tue Nov 20, 2018 10:02 am

Because the valance electron of carbon atom is four so it originally has 2 in 2s and 2 in sp. The two 2s's energy becomes higher and combine with one electron in p orbital to become sp2 and the left p electron is itself an orbital. You can regard sp2 as 3 orbitals and p as one orbital, with one electron in each orbital


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