What allows graphite to conduct electricity?

Graphite is able to conduct electricity due to the presence of delocalised electrons within its structure. In graphite, carbon atoms are arranged in layers, and each carbon atom forms three bonds with other carbon atoms, creating a hexagonal lattice. The fourth outer-shell electron of each carbon atom is not involved in bonding and becomes delocalised. This means that it is free to move throughout the layers of graphite.

These delocalised electrons can carry charge, making graphite an excellent conductor of electricity. When an electric potential is applied, these electrons can flow, allowing graphite to effectively conduct electricity.

The other options do not attribute correct characteristics of graphite related to its electrical conductivity. Ionic bonds are not relevant in this context as graphite primarily forms covalent bonds rather than ionic ones. While graphite does have a high melting point, this property is more related to the strength of the covalent bonds within the lattice structure and not specifically to its ability to conduct electricity. The statement about being composed of liquid molecules is inaccurate because graphite is a solid at room temperature and does not consist of liquid molecules.