Question:
The allotrope of carbon with aromatic character is:
The allotrope of carbon with aromatic character is:
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Buckminsterfullerene \((C_{60})\) is a cage-like carbon allotrope containing delocalized \(\pi\)-electrons.
Updated On: Jun 18, 2026
- Diamond
- Graphite
- Coke
- Fullerene
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The Correct Option is D
Solution and Explanation
Concept:
Aromatic character arises due to delocalization of \(\pi\)-electrons over a cyclic framework. Certain fullerene structures exhibit aromatic behaviour because of extensive electron delocalization.
Step 1: Examine diamond.
Diamond contains only \(sp^3\) hybridized carbon atoms. There are no delocalized \(\pi\)-electrons. Hence diamond is non-aromatic.
Step 2: Examine graphite.
Graphite consists of layered sheets containing delocalized electrons, but it is not classified as an aromatic allotrope.
Step 3: Examine coke.
Coke is an amorphous form of carbon and does not exhibit aromatic character.
Step 4: Examine fullerene.
Fullerenes such as \(C_{60}\) possess conjugated \(\pi\)-electron systems and show aromatic character. Therefore, \[ \boxed{\text{Fullerene}} \]
Step 1: Examine diamond.
Diamond contains only \(sp^3\) hybridized carbon atoms. There are no delocalized \(\pi\)-electrons. Hence diamond is non-aromatic.
Step 2: Examine graphite.
Graphite consists of layered sheets containing delocalized electrons, but it is not classified as an aromatic allotrope.
Step 3: Examine coke.
Coke is an amorphous form of carbon and does not exhibit aromatic character.
Step 4: Examine fullerene.
Fullerenes such as \(C_{60}\) possess conjugated \(\pi\)-electron systems and show aromatic character. Therefore, \[ \boxed{\text{Fullerene}} \]
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