Question
Explain the resonance structures of benzene using the orbital overlap concept.
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Answer
The structure of benzene can be better explained by the orbital overlap concept,
$i.$ All six carbon atoms in benzene are $sp^2$ hybridized. Two $sp^2$ hybrid orbitals of each carbon atom overlap and form carbon$-$carbon sigma $(\sigma)$ bond and the remaining third $sp^2$ hybrid orbital of each carbon overlaps with $s$ orbital of a hydrogen atom to form six $C – H$ sigma bonds.
$ii.$ The unhybridized $p$ orbitals of carbon atoms overlap laterally forming $\pi$ bonds. There are two possibilities of forming three $\pi$ bonds by overlap of $p$ orbitals of $C_1 – C_2, C_3 – C_4, C_5 – C_6$ or $C_2 – C_3, C_4 – C_5, C_6 – C_1,$ respectively, as shown in the following figure. Both the structures are equally probable.
According to resonance theory, these are two resonance structures of benzene.
$i.$ All six carbon atoms in benzene are $sp^2$ hybridized. Two $sp^2$ hybrid orbitals of each carbon atom overlap and form carbon$-$carbon sigma $(\sigma)$ bond and the remaining third $sp^2$ hybrid orbital of each carbon overlaps with $s$ orbital of a hydrogen atom to form six $C – H$ sigma bonds.
$ii.$ The unhybridized $p$ orbitals of carbon atoms overlap laterally forming $\pi$ bonds. There are two possibilities of forming three $\pi$ bonds by overlap of $p$ orbitals of $C_1 – C_2, C_3 – C_4, C_5 – C_6$ or $C_2 – C_3, C_4 – C_5, C_6 – C_1,$ respectively, as shown in the following figure. Both the structures are equally probable.
According to resonance theory, these are two resonance structures of benzene.
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