What does graphite contain that is similar to metals

It is often confusing why graphite seems to have some metallic properties (conductivity and shiny surface) and some non-metallic properties (brittle). The reason for this is that graphite is composed of carbon which is a non metal and pure carbon in diamonds is an insulator like most non metals. A better way to state the question is “why does graphite a non metal have any metallic properties?”. So the reason is that graphite uses a different conduction mechanism then metals. Metals conduct electricity and heat by the motion of their loosely bound outer electrons. Non metal conduction like that found in graphite and some semiconductors like zinc oxide is caused by electron hoping. The electron hoping mechanism also allows for increased thermal conductivity. This happens in graphite due to the hexagonal planar crystal structure. Graphite is still a non metal but it has a few properties related to it’s electron structure that make it metal like but only in those specific ways. Otherwise graphite is still a non metal so it is brittle and crumbles when you try to shape it.