Diamond
A solid is one of the three basic states of the matter. Intermolecular attraction forces are stronger in solids compared to liquids and gases i.e., in solids the atoms are tightly bound to each other. Due to this solids are hard and structurally rigid. Due to their resistance to change they can not be compressed easily.
Solids have definite shape and volume. They neither flow, nor diffuse. They can be further divided into two major types:
Crystalline solids:
The constituents (atoms, ions, or molecules) of these solids are arranged in a regular pattern forming a crystalline lattice.
e.g: Diamond, Sugar crystal, Rocks, Snowflakes etc.
Glass and quartz both, consist of silicon dioxide. However, the molecule in quartz form an orderly crystalline
network, while those in glass do not.
Amorphous solids:
These solids are characterized by irregular shape as the atoms in them have no regular pattern of arrangement. Hence, they are
also called non-crystalline solids.
e.g: Glass, Gels, Paraffin, Wax etc.
The atoms in a solid can have variety of bonding. For e.g. NaCl have ionic bonding due to attraction between Na+ and Cl− ions, whereas the atoms in diamond are bound to each other through strong covalent bonds.
Diamond is the hardest substance. It is non malleable, non ductile mineral that shows very less reactivity because of its compact crystalline structure.
On heating, some solids can be converted into liquids or gases. Heating provides the energy that is sufficient to overcome the strong attraction forces among the atoms in a solid. Hence, atoms move a little further apart. On cooling, the atoms once again come closer to each other due to decrease in motion and resume their former shape.