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.

What type of hybridization is present in the carbon atoms of graphite?

• sp3

• dsp2

• sp2

• sp

What is the separation distance between the layers in graphite?

• 3.35 angstroms

• 5.5 angstroms

• 2.5 angstroms

• 4.0 angstroms

Why is graphite a good conductor of electricity?

• Due to the presence of free protons

• Due to its dense structure

• Because of its sp3 hybridization

• Because the fourth electron is delocalized

What type of bond is formed by the overlap of 2p orbitals in graphite?

• Hydrogen bond

• Pi bond

• Ionic bond

• Sigma bond

In which application is graphite used to slow down neutrons?

• Pencil leads

• Lubricants

• Nuclear reactors

• Electrodes