Graphite is good conductor of electricity because

Graphite is an allotrope of carbon, consisting of layers of carbon atoms arranged in a hexagonal lattice. Each carbon atom in graphite forms three covalent bonds with neighboring carbon atoms, creating a planar layer. This leaves one electron from each carbon atom free to move.

Why Graphite Conducts Electricity

One key reason why graphite is a good conductor of electricity is the presence of delocalized electrons. In graphite, the fourth electron from each carbon atom is not bound to any specific atom. Instead, these electrons are free to move within the layers. This mobility of electrons allows graphite to conduct electricity effectively.

Moreover, the layered structure of graphite contributes to its conductivity. The layers are held together by weak van der Waals forces, enabling the delocalized electrons to flow within each layer easily. This is why graphite is a good conductor of electricity in a planar direction.

Applications of Graphite’s Electrical Conductivity

Understanding why graphite is a good conductor of electricity has practical implications. Graphite is used in various applications, such as electrodes in batteries and electric arc furnaces, due to its excellent conductivity and stability at high temperatures.