Carbon and silicon both belong to the group 14, but inspite of the stoichiometric similarity, the dioxides, (i.e., carbon dioxide and silicon dioxide), differ in their structures. Comment.

Explanation

Carbon because of its small size and higher electronegatively then silicon forms `ppi-ppi` double bonds with O-atoms to form `CO_(2)` molecule. These molecules of `CO_(2)` are held together by weak van der Waals force of attraction which can be easily overcome by collisions of the moleculs at room temperature. Consequently, `CO_(2)` is a gas.
Silicon, on the other hand, because of its bigger size and electronegativity than carbon has little tendency to form `ppi-ppi` double bonds with O-atoms. Instead, each silicon atom forms four single covalent bonds with O-atoms which are tetrahedrally arranged around it leading to the formation of a three-dimensional network structure. T break these covalent bonds, a large amount of energy is needed and hence `SiO_(2)` is a high melting solid.