How are the crystal structures of diamond and graphite different?

Diamond and graphite are two distinct allotropes of carbon with significantly different crystal structures:

• Diamond: Features an infinite three-dimensional tetrahedral network. Each carbon atom is covalently bonded to four others at the corners of a tetrahedron, with a bond length of $1.54\times {10}^{-8}$ cm. This rigid, compact structure results in extreme hardness and insulating properties.1
• Graphite: Consists of parallel, two-dimensional sheets of carbon atoms arranged in fused hexagonal rings. Within these layers, the bond distance is $1.42\times {10}^{-8}$ cm. The layers are held together by weak van der Waals forces rather than strong covalent bonds, with an interlayer distance of $3.37\times {10}^{-8}$ cm. This layered structure allows for the material's characteristic softness, lubricity, and electrical conductivity.1

While diamond is a rigid 3D lattice, graphite is a layered structure that can accommodate other molecules between its planes.1