Question

A diamond is an example of this type of solid.
A. Amorphous solid
B. ionic solid
C. Metallic solid
D. Network covalent solid

Answer 1

Hint: Solids are substances having a rigid and definite mass, shape and volume. Solids can be classified according to the intermolecular forces in them. Amorphous solids consist of short range order, while crystalline solids have a long range order. Diamond is an allotrope of carbon and has carbon units attached in its structure.

Complete answer:
Solids are the substances having strong intermolecular forces, rigid with definite shape and mass. Among them crystalline solids have a definite long range order while amorphous solids are smooth with short range orders.
We have diamond, which is an allotrope of carbon. Diamond consists of a three – dimensional network of carbon atoms attached to each other. Since carbon atoms have properties for catenation, they form covalent bonds with each other in a 3 – D frame network. Therefore diamond is termed as a network covalent solid.
Due to this diamond is the hardest substance with high boiling and melting point and is a poor conductor. The intermolecular covalent bonds make it hard.
Hence, diamond is an example of network covalent solid.

So option D is correct.

Note:
Amorphous solids have a short range order example, chalk, Teflon etc. The ionic solids contain ionic bonds that are formed by the transfer of valence electrons, example, NaCl, KCl, CaO, etc. The metallic solids consist of metallic bonding; they are hard malleable and ductile, for example, iron, copper, silver, etc.