Carbon is the element forming a diamond’s crystal lattice.
Diamond is a crystalline allotrope of carbon. In its structure, each carbon atom forms strong covalent bonds with four neighboring carbon atoms in a three-dimensional arrangement. This network gives diamond exceptional hardness and makes it one of the best-known natural materials for resisting scratching.
Diamonds form deep within Earth, commonly at depths of roughly 150 to 200 kilometers, where high pressure and temperature allow carbon to crystallize. Volcanic eruptions can carry them toward the surface in rocks called kimberlites. Synthetic diamonds can also be manufactured using high-pressure methods or chemical vapor deposition.
Diamond and graphite are both made only of carbon, but their atomic arrangements differ. Graphite has layered structures that slide easily, making it soft, while diamond’s rigid network makes it hard. Diamond also conducts heat very well but is normally an electrical insulator.