The hybridized state of carbon in diamond, graphite, fullerene and acetylene are:a)sp3, sp2, sp, sp2b)sp3, sp2, sp2, spc)sp3, sp2, sp3, spd)sp3, sp2, sp, spCorrect answer is option 'B'. Can you explain this answer?

Question

Answer

In diamond there is one carbon attached to 3 carbon tetrahedraly, in graphite there is hexagonal layer structure so SP2 same in Fullerence. but in acetylene there is triple bond between C and C.

Answer

For acetylene 2sigma bond therefore hybridisation is sp
for Diamond 4 valency is filled therefore hybridisation is sp 3
For graphite one p orbital electron is free so it's hybridisation is sp2

for fullerene is like of graphite it is also sp2 hybridised

Answer

Hybridization of Carbon in Diamond, Graphite, Fullerene, and Acetylene

To understand the hybridization state of carbon in diamond, graphite, fullerene, and acetylene, we need to consider the bonding and molecular structures of these compounds.

Diamond:
- Diamond is a three-dimensional network solid composed entirely of carbon atoms.
- Each carbon atom in diamond is covalently bonded to four neighboring carbon atoms, resulting in a tetrahedral arrangement.
- The carbon-carbon bonds in diamond are formed by the overlap of sp3 hybrid orbitals.
- Hence, the hybridization state of carbon in diamond is sp3.

Graphite:
- Graphite is composed of layers of carbon atoms arranged in a hexagonal lattice.
- Within each layer, each carbon atom is covalently bonded to three neighboring carbon atoms, resulting in a trigonal planar arrangement.
- The carbon-carbon bonds in graphite are formed by the overlap of sp2 hybrid orbitals.
- Hence, the hybridization state of carbon in graphite is sp2.

Fullerene:
- Fullerene is a hollow cage-like molecule composed of carbon atoms arranged in a spherical or cylindrical structure.
- The carbon atoms in fullerene are connected by both single and double bonds.
- Each carbon atom in fullerene is covalently bonded to three neighboring carbon atoms, resulting in a trigonal planar arrangement.
- The carbon-carbon bonds in fullerene are formed by the overlap of sp2 hybrid orbitals.
- Hence, the hybridization state of carbon in fullerene is sp2.

Acetylene:
- Acetylene, also known as ethyne, is a linear molecule composed of two carbon atoms and two hydrogen atoms.
- Each carbon atom in acetylene is covalently bonded to one hydrogen atom and one neighboring carbon atom, resulting in a linear arrangement.
- The carbon-carbon triple bond in acetylene is formed by the overlap of sp hybrid orbitals.
- Hence, the hybridization state of carbon in acetylene is sp.

Summary:
- The hybridization state of carbon in diamond is sp3.
- The hybridization state of carbon in graphite is sp2.
- The hybridization state of carbon in fullerene is sp2.
- The hybridization state of carbon in acetylene is sp.
- Therefore, the correct answer is option 'B' (sp3, sp2, sp2, sp).

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