Choose the correct statements about allotropes of carbon
I. Graphite has layered structure
II. Buckminster fullerene is not aromatic in nature
III. The distance between two adjacent layers in graphite is 141.5 pm
IV. The hybridization of carbons in graphite and Buckminster fullerene is same
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Remember the key features of carbon allotropes:
Diamond: sp$^3$ hybridized, tetrahedral, 3D network, very hard.
Graphite: sp$^2$ hybridized, planar layers, conductive, soft.
Fullerene: sp$^2$ hybridized (approximately), cage-like structures.
The distance between layers in graphite (~335 pm) is much larger than the bond length within the layers (~142 pm).
I. Graphite has layered structure:
Graphite consists of planar layers of carbon atoms arranged in hexagonal rings.
Within each layer, carbon atoms are held by strong covalent bonds, and the layers are held together by weak van der Waals forces.
This statement is correct.
II. Buckminster fullerene is not aromatic in nature:
Buckminsterfullerene (C$_{60}$) has fused five- and six-membered rings.
Although it has delocalized pi electrons, its curved structure prevents continuous planar overlap required for aromaticity according to H��ckel's rule.
This statement is correct.
III. The distance between two adjacent layers in graphite is 141.5 pm:
The C-C bond length within the layers is ~141.5 pm, but the interlayer distance is ~335 pm.
Therefore, this statement is incorrect.
IV. The hybridization of carbons in graphite and Buckminster fullerene is same:
In graphite, carbon is sp$^2$ hybridized, bonded to three atoms in a planar arrangement.
In Buckminsterfullerene, each carbon is bonded to three carbons in a curved structure, giving predominantly sp$^2$ character with some distortion.
Strictly speaking, the hybridization is not identical due to curvature.
This statement is incorrect.
