Graphite has a giant covalent (macromolecular) structure and is a good electrical conductor, whereas buckminsterfullerene ($C_{60}$) has a simple molecular structure and is a poor electrical conductor because its delocalised electrons are restricted within individual molecules.

Both graphite and buckminsterfullerene ($C_{60}$) have giant covalent structures, but buckminsterfullerene has a higher sublimation point due to the strength of its spherical covalent network.

In graphite, each carbon atom is covalently bonded to three other carbon atoms, whereas in buckminsterfullerene ($C_{60}$), each carbon atom is covalently bonded to four other carbon atoms, leaving no delocalised electrons.

Graphite has a simple molecular structure held together by weak intermolecular forces, whereas buckminsterfullerene ($C_{60}$) forms a giant covalent lattice with no intermolecular forces.