The strong bonds between carbon atoms in graphite are covalent bonds, specifically strong covalent sigma bonds within each layer.

Quick Scoop

  • In graphite, each carbon atom bonds to three neighboring carbons using strong covalent bonds, forming hexagonal rings in flat layers.
  • These in‑plane bonds are sigma-type covalent bonds arising from sp2sp^2sp2 hybridization of the carbon atoms.
  • The layers themselves are held together only by weak intermolecular (van der Waals) forces, which is why graphite is soft and slippery even though the in‑layer covalent bonds are very strong.

Answer for exams: covalent bonds (strong covalent sigma bonds between carbon atoms in each layer).