(A): The carbon- carbon bond lengths in benzene molecule are 1.54 $\overset{°}{A}$ and 1.34 $\overset{°}{A}$ .
(R): Benzene has delocalized pi-bonds.

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Both A and R are true. R is not the correct explanation of A

A is true but R is false

Both A and R are true and R is correct explanation of A

A is false but R is true

answer is D.

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Detailed Solution

X-ray data indicates that all the six C—C bond lengths are of the same order (1.39 $\overset{°}{A}$ ), which is intermediate between C— C single bond (1.54 $\overset{°}{A}$ ) and C—C double bond (1.33 $\overset{°}{A}$ ).
This is due to the delocalization of pi electrons in the molecule, creating a ring of electron density above and below the plane of carbon atoms.
The delocalization of electrons makes the bonds stronger, leading to a bond length of 1.39 Å, which is intermediate between the length of a single bond (1.54 Å) and a double bond (1.33 Å).
Thus, A is false but R is true.

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