The allotropes of carbon include a variety of structures that include three-dimensional tetrahedral lattices, planes of hexagonal rings, cylindrical tubes of hexagonal rings, and spheres of five- and six-membered rings. Similar shapes of network covalent atomic solids are possible with carbon nitride, boron, and pure silicon (e.g., silicene is a graphene-like allotrope of pure silicon). In contrast, silicates exist as either highly ordered or amorphous (more random) three-dimensional lattices. What could explain why there are there no naturally occurring sheets, stacked sheets, cylindrical tubes, or spheres of network covalent atomic solids composed of silicon and oxygen (SiO2)? Would pure silicate structures make good lubricants or good electrical conductors? Answer these questions by completing the statements below.

SiO2 has a peculiar nature. It isn't very reactive. It has a very high melting point. grinding wheels. It is difficult to deform or melt it and its related compounds because its polar covalent (Si–C or Si–O) bonds must be broken, and this requires a large input of energy. It also does not contain any hydrogen, thus it cannot act as a Brønsted–Lowry acid. While not soluble in water, it dissloves in hot concentrated alkali or fused hydroxide.

Silicon metal is made from the reaction of silica (silicon dioxide, SiO2) and carbon materials like coke, coal and wood chips. Silica is typically received in the form of metallurgical grade gravel.

Silicates can be used as solid lubricants, lubricant additives in engine oil, as fume silica grease, rubber materials, waterproofing materials, and caulks.

Fused Silica has extremely good dielectric and insulating properties. For these reasons it is used as an inert, low expansion filler material for epoxy resins in electronic circuits as an insulator.