Question

Graphite is an example of

• A. Covalent solid
• B. Metallic solid
• C. Ionic solid
• D. None of these

Answer 1

The correct option is A

Covalent solid

Explanation of correct answer:

Option (A) Covalent solid

Covalent solid:

• Covalent bonds are formed between atoms by equal sharing of electrons.
• Graphite is the crystalline allotropes of carbon and it has a layered structure.
• In graphite, all carbons are attached to one another through a nonpolar bond due to the same electronegativity of carbon atoms, and this non-polar bond between the carbon atoms in graphite is called a covalent bond.
• Due to the strong network of covalent bonds, they have high melting points.
• Example: Diamond, graphite, fullerenes.
• Hence option A is correct.

Explanation of incorrect answer:

Option (B) Metallic solid

• Metallic solids are composed of metal cations held together by a delocalized sea of valence electrons.
• Because of their mobile electrons, metallic solids are good conductors of heat and electricity.
• Example: Copper ($\mathrm{Cu}$), Zinc ($\mathrm{Zn}$)
• Hence option B is incorrect.

Option (C) Ionic solid

• Ionic solids are composed of cations and anions held together by electrostatic forces.
• Due to the strength of these strong interactions, ionic solids are hard, brittle, and have high melting points.
• Example: Sodium chloride ($\mathrm{NaCl}$), Zinc oxide($\mathrm{ZnO}$)
• Hence option C is incorrect.

Option (D) None of these

• Option A Covalent solid is correct.
• Hence option D is incorrect.

Therefore, graphite is an example of a covalent solid, option (A) is the correct answer.