Question

The hybridisation of carbon in graphite is:

• A. sp.
• B. sp\(^2\).
• C. sp\(^3\).
• D. sp\(^3\)d.

Hint:

In graphite, carbon atoms are sp\(^2\) hybridized, allowing for the formation of strong covalent bonds in a planar structure with delocalized electrons.

Answer 1

The Correct Option is B

Step 1: Understanding hybridization in graphite.
In graphite, each carbon atom is bonded to three other carbon atoms in a plane, forming hexagonal rings. The bonding involves the use of \( sp^2 \) hybrid orbitals, with the remaining p-orbital involved in \( \pi \)-bonding, which accounts for the delocalized electrons in graphite. Step 2: Explanation.
The \(sp^2\) hybridization allows for the formation of three sigma bonds and one pi bond, contributing to the structure of graphite. Step 3: Conclusion.
Thus, the hybridization of carbon in graphite is \(sp^2\).