By which of the following reason layers of carbon atoms in graphite are held together?

CONCEPT:

Layers of Carbon Atoms in Graphite

• Graphite is composed of layers of carbon atoms arranged in a hexagonal lattice structure.
• Within each layer, the carbon atoms are bonded through strong covalent bonds.
• However, the layers themselves are held together by weak intermolecular forces known as van der Waals forces.

EXPLANATION:

• The bonding in graphite can be explained as follows:
  • Each carbon atom in a graphite layer forms covalent bonds with three neighboring carbon atoms, creating a planar hexagonal structure.
  • These covalent bonds are strong and responsible for the structural integrity of the individual layers.
  • Between adjacent layers, there are no covalent bonds; instead, the layers are held together by weak van der Waals forces.

• Van der Waals forces are weak intermolecular forces arising due to temporary dipoles in atoms or molecules. These forces allow the layers to slide over each other, giving graphite its characteristic lubricating property.

Therefore, the layers of carbon atoms in graphite are held together by van der Waals forces.