Exploring Graphite's Unique Structure

Graphite is a two-dimensional structure where each carbon atom is bonded to three others via sigma bonds, forming a planar hexagonal lattice. The layers are held together by van der Waals forces, making graphite slippery. The fourth electron in each carbon atom is delocalized, allowing graphite to conduct electricity. Graphite's 2P orbitals overlap to form Π bonds. It is used as a lubricant, in pencil leads, and as a moderator in nuclear reactors to slow down neutrons.

Explain how the delocalized electrons in graphite contribute to its electrical conductivity.

What is the role of graphite in nuclear reactors?