For 3-D Structure of Diamond Molecular Structure using Jsmol
Graphite is one of the allotropes of carbon. (See also allotropes of carbon.) Unlike diamond, graphite is a conductor, and can be used, for instance, as the material in the electrodes of an electrical arc lamp.
The pi orbital electrons delocalized across the hexagonal atomic sheets of carbon contribute the graphite's conductivity. In an oriented piece of graphite, conductivity parallel to these sheets is greater than that perpendicular to these sheets.
The loose coupling among the sheets in graphite contributes to another industrially important property -- graphite powder is used as a dry lubricant. Recent studies suggest that an effect called superlubricity can also account for this effect. Graphite is also used in pencils.
Associated minerals include quartz, calcite, micas, iron meteorites and tourmalines.
Other characteristics: thin flakes are flexible but inelastic, mineral can leave black marks on hands and paper, conducts electricity. In graphite the effect superlubricity also takes place
Best field indicators are softness, luster, density and streak.
The unit cell dimensions are a = b = 2.456 Å, c = 6.694 Å. The carbon-carbon bond length in the bulk form is 1.418 Å, and the interlayer spacing is c/2 = 3.347 Å.