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Why does graphite conduct electricity?

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A labeled diagram of the periodic table entry for carbon, showing its atomic number 6, symbol C, electron configuration, atomic weight range, solid physical state, hexagonal crystal structure, and weakly acidic oxide properties. Color coding and icons indicate it is a nonmetal, solid at room temperature, with hexagonal structure and weak acidity. — carbon Carbon and its properties.

Graphite conducts electricity due to its unique crystal structure, which consists of parallel, stacked layers of carbon atoms arranged in fused hexagonal rings.12

Within each layer, the carbon atoms are covalently bonded, a structure interpreted as involving complete π-bonding. This arrangement allows for the movement of electrons within the plane of the sheets, which facilitates electrical conductivity. Because the bonding between these layers is very weak—attributed to van der Waals forces—the structure is anisotropic, meaning its electrical conductivity is significantly higher along the plane of the sheets than perpendicular to them.13