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Chris Tai 1B
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Joined: Sat Aug 24, 2019 12:16 am


Postby Chris Tai 1B » Wed Nov 27, 2019 8:11 pm

Consider the bonding in H2C=CHCHO. (a) Draw the most important Lewis structure. Include all nonzero formal charges. (b) Identify the composition of the bonds and the hybridization of each lone pair—for example, by writing sigma(H1s,C2sp^2 ).

for part b, why is the sigma bond sigma(C2sp,O2p^2) while the pi bond is pi(C2p,O2p)? Where did the hybridized orbital of 2sp^2 for carbon go? (same question for oxygen)

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Joined: Thu Jul 25, 2019 12:15 am

Re: 2.45

Postby 205296774 » Thu Nov 28, 2019 1:57 pm

The answer for the sigma bond between C-O is sigma( C 2sp2, O 2sp2). This is the case because both the carbon and oxygen have three regions of electron density (C - 2 single bonds and 1 double bond) (O- 2 lone pairs and 1 double bond). Pi bonds are p-orbitals overlapping (not s-orbitals) so it will always be 2p. 

Hope this helps!

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