Question:
The hybridization of elements present in Fullerene and graphite are respectively:
The hybridization of elements present in Fullerene and graphite are respectively:
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In graphite and fullerene, each carbon atom is bonded to three other carbon atoms, so the carbon atoms are \(sp^2\) hybridised.
Updated On: Jun 26, 2026
- \(sp^3,\ sp^2\)
- \(sp^2,\ sp^2\)
- \(sp,\ sp^2\)
- \(sp^2,\ sp\)
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The Correct Option is B
Solution and Explanation
Step 1: Hybridization in fullerene.
Fullerene is an allotrope of carbon.
In fullerene, each carbon atom is bonded to three other carbon atoms.
Therefore, each carbon forms three sigma bonds and has one unhybridized \(p\)-orbital.
Hence, carbon in fullerene is \[ sp^2 \] hybridised.
Step 2: Hybridization in graphite.
Graphite consists of layers of carbon atoms arranged in hexagonal sheets.
Each carbon atom in graphite is bonded to three other carbon atoms by sigma bonds.
The fourth electron remains in an unhybridized \(p\)-orbital and participates in delocalized \(\pi\)-bonding.
Thus, carbon in graphite is also \[ sp^2 \] hybridised.
Step 3: Final conclusion.
Therefore, the hybridization in fullerene and graphite respectively is \[ \boxed{sp^2,\ sp^2} \] Hence, the correct option is \[ \boxed{(2)} \]
Fullerene is an allotrope of carbon.
In fullerene, each carbon atom is bonded to three other carbon atoms.
Therefore, each carbon forms three sigma bonds and has one unhybridized \(p\)-orbital.
Hence, carbon in fullerene is \[ sp^2 \] hybridised.
Step 2: Hybridization in graphite.
Graphite consists of layers of carbon atoms arranged in hexagonal sheets.
Each carbon atom in graphite is bonded to three other carbon atoms by sigma bonds.
The fourth electron remains in an unhybridized \(p\)-orbital and participates in delocalized \(\pi\)-bonding.
Thus, carbon in graphite is also \[ sp^2 \] hybridised.
Step 3: Final conclusion.
Therefore, the hybridization in fullerene and graphite respectively is \[ \boxed{sp^2,\ sp^2} \] Hence, the correct option is \[ \boxed{(2)} \]
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