If diamonds and graphite are both made of the element carbon, then why are they so different? It's all in the atomic structure. The atoms in graphite are arranged in layers and the carbon atoms within each layer are connected by strong covalent bonds. However, only weak forces exist between the layers. Imagine graphite to be a stack of paper. It is very difficult to go through the stack perpendicularly, but very easy to slice through horizontally. By contrast, the bonding of carbon atoms in the crystal lattice of diamond has perfect tetrahedral symmetry. Each atom is bonded to four other atoms in an equal 3-dimensional way, rather than only in layers. This creates an incredibly strong structural bond in all directions providing diamond with its superior hardness and other properties…