Question

What is the hybridization of carbon atoms in fullerene?
A.$s{p^3}$
B.$sp$
C.$s{p^2}$
D.$ds{p^3}$

Answer 1

Hint: At first think about the definition of hybridization of carbon atoms. Carbon atoms usually form bonds by mixing different orbitals and can contribute to the formation of different structures and properties.

Complete step by step answer:
The hybridization in carbon atoms is divided into three types. They are $sp,s{p^2}$ and $s{p^3}$ hybridization.
Coming to the question Fullerene is an allotrope of carbon whose molecule consists of carbon atoms connected by single and double bonds in order to form a closed structure with fused rings of five to seven atoms. Fullerenes are informally denoted by the empirical formula ${C_n}$, where n is the number of carbon atoms. Allotropy is the property of an element to exist in more than one physical form having similar chemical properties but different physical properties. Carbon exists in both crystalline and amorphous allotropic forms.
Diamond, graphite and fullerene are crystalline allotropes of carbon. Fullerene has a curved structure and it is called Buckminsterfullerene (${C_{60}}$). It has a similar structure to graphite.
Fullerenes are stable but they are least reactive. Fullerenes are cage-like molecules and have a shape like a soccer ball. It contains a $20$ six membered ring fused with a six or seven membered ring. The carbon atoms in fullerene are $s{p^2}$ hybridized and due to its structure it is in between the diamond and graphite.
So the answer is C.

Note:
Don’t get confused with the terminology. Diamond exhibits hardness and high dispersion of light. Graphene has high electron mobility. In fullerenes carbon takes the form of a hollow sphere, ellipsoid or tube.