Why are the N, O, and C ALL sp2 hybridized here? At the top, N has 1 lone pair a

Question

Why are the N, O, and C ALL sp2 hybridized here?

At the top, N has 1 lone pair and 3 bonds, making it sp3 hybrized. In structure C, I understand HERE that the N is now sp2 hybridized with the bonds, but now O is now sp3 hybridized with 3 lone pairs and one bond, so how are they all sp2 hybridized? Thanks.

lution ere is a reasonable contributing structure (C), which places a double bond tween the carbon and the nitrogen. Therefore, all three atoms are sp. This ans that the lone pair on N is in a 2p orbital A. B.

Explanation / Answer

look at the structure A dont try with structure B and structure C

yes your assumtion is correct

if nitrogen is having one lone pair and three sigma bonds it must be in SP3

but this rule will be applicable only if the lone pair in the nitrogen should not be in conjugation

but here the lone pair in nitrogen is in conjugation this can involve in resonence only if it is present in unhybridised P orbital and this is possible if the nitrogen is in sp2 hybridisation

i will give the another example

take the cyclo hexyl amine in this lone pair on the nitrogen doesnt involve any conjugation so nitrogen is in SP3 hybridisation

where as in aniline the lone pair of electrons on the nitrogen involve in resonence so the nitrogen is in SP2 hybridisation

comming top the oxygen and C in both casesw one Pi bond is there so both are in SP2 hybridisation

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