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2F.13 7th Ed

Posted: Tue Nov 27, 2018 2:32 pm
by Summer de Vera 2C
Hi! For 2F.13, why is the hybridization of CH2 and CH sp2? Because there are each 4 areas of e- density surrounding the molecules, shouldn't the hybridization be sp3?

Re: 2F.13 7th Ed

Posted: Tue Nov 27, 2018 2:46 pm
by Emma Scholes 1L
The hybridization of CH2 and CH are sp2 because there are only three areas of electron density surrounding them. The C in CH2 has one bond connecting each of the two hydrogens and a double bond connecting it to the other carbon. The C in CH has one bond connecting it to the hydrogen, one double bond connecting to a carbon, and one single bond connecting to the other carbon.

Re: 2F.13 7th Ed

Posted: Tue Nov 27, 2018 2:54 pm
by Andrewwiner4D
There are three areas of electron concentration. Total valence electrons for CH2 is 6. Each hydrogen has one bond and there is one lone pair. The bent shape will give you an SP2 hybridization.

Re: 2F.13 7th Ed

Posted: Tue Nov 27, 2018 5:03 pm
by Schem_student
I got confused by this one too! Just think about hybridization labels of central atoms in terms of amount of atoms bonded not if they are double or single bonds. Therefore there are only 3 atoms bonded around C so it would be sp2.

Re: 2F.13 7th Ed

Posted: Tue Nov 27, 2018 7:34 pm
by Summer de Vera 2C
Schem_student wrote:I got confused by this one too! Just think about hybridization labels of central atoms in terms of amount of atoms bonded not if they are double or single bonds. Therefore there are only 3 atoms bonded around C so it would be sp2.

I think this is what I was getting confused by. Thank you!