Diamond:
* Crystal Structure: Face-centered cubic (FCC)
* Bonding: Covalent bonds between all carbon atoms, forming a strong, rigid 3D network.
* Properties: Hardest known natural material, high refractive index, excellent thermal conductor.
Graphite:
* Crystal Structure: Hexagonal layered structure. Each layer is composed of hexagonal rings of carbon atoms connected by covalent bonds. The layers are held together by weak van der Waals forces.
* Bonding: Covalent bonds within each layer, van der Waals forces between layers.
* Properties: Soft, slippery, good electrical conductor, used in pencils, lubricants, and electrodes.
Graphene:
* Crystal Structure: Single layer of graphite, a 2D honeycomb lattice of carbon atoms.
* Bonding: Covalent bonds between carbon atoms.
* Properties: Extremely strong and thin, excellent electrical and thermal conductor, transparent, used in electronics, composites, and energy storage.
Fullerene (Buckminsterfullerene):
* Crystal Structure: Spherical or ellipsoidal molecules composed of 60 or more carbon atoms arranged in a network of pentagons and hexagons.
* Bonding: Covalent bonds between carbon atoms.
* Properties: Unique molecular structure, potential applications in medicine, electronics, and materials science.
Carbon Nanotubes:
* Crystal Structure: Cylindrical structures composed of rolled-up sheets of graphene.
* Bonding: Covalent bonds between carbon atoms.
* Properties: High tensile strength, high electrical and thermal conductivity, used in composites, electronics, and energy storage.
Other Crystal Structures:
* Lonsdaleite (Hexagonal Diamond): A rare form of diamond with a hexagonal crystal structure.
* Carbon Nanofoam: A 3D network of interconnected carbon nanotubes with a low density.
* Diamondoid: A family of molecules with a diamond-like structure.
These are just a few examples of the diverse crystal structures that carbon can form, highlighting its versatility and importance in materials science.
