2F.13 7th Ed


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Summer de Vera 2C
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2F.13 7th Ed

Postby Summer de Vera 2C » Tue Nov 27, 2018 2:32 pm

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?

Emma Scholes 1L
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Re: 2F.13 7th Ed

Postby Emma Scholes 1L » Tue Nov 27, 2018 2:46 pm

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.

Andrewwiner4D
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Re: 2F.13 7th Ed

Postby Andrewwiner4D » Tue Nov 27, 2018 2:54 pm

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.

Schem_student
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Re: 2F.13 7th Ed

Postby Schem_student » Tue Nov 27, 2018 5:03 pm

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.

Summer de Vera 2C
Posts: 65
Joined: Fri Sep 28, 2018 12:16 am

Re: 2F.13 7th Ed

Postby Summer de Vera 2C » Tue Nov 27, 2018 7:34 pm

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!


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