-R effect in benzene causes anti-aromaticity?

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The discussion centers on the -R effect of groups like NO2 in benzene, specifically how it affects the π electron count and stability. The introduction of the nitro group leads to the formation of a double bond between nitrogen and carbon, resulting in a positive charge at the ortho and para positions. This creates a scenario where resonance structures suggest a planar ring with four π electrons, which would classify it as anti-aromatic and thus unstable. However, participants argue that the canonical forms actually maintain six π electrons in a non-cyclic conjugated system, contradicting the anti-aromatic classification. The conversation seeks clarity on the apparent contradiction between resonance stability and the anti-aromatic nature of the system.
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Consider any -R effect showing group like NO2 in place of anyone of the hydrogen of the benzene ring, here we get nitrobenzene.

We know that after showing -R effect a double bond will be formed between N and C and one of the π bond will no longer be present in the ring and it's place will be taken by + charge on ortho and para position which will be in conjugation with the remaining two π bonds in the ring as can be seen from the diagram below.

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However the problem is that, in the canonical forms after resonance there will be 4 π electrons in a planar conjugated ring, which by definition is anti aromatic. But this should not be true because we know that resonance increases stability but anti aromatic hydrocarbons are unstable.

Can anyone give an explanation for the same.
 
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None of the canonical forms has a ring of 4 pi electrons. They have six pi electrons in a non-cyclic conjugated system (including the C=N bond).
 

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