Diamond, Graphite, Fullerenes, Carbon Nano-tubes and Graphene

Diamond, Graphite, Fullerenes, Carbon Nano-tubes and Graphene

Diamond

• Formed entirely of carbon atoms each bonded to four other carbon atoms in a tetrahedral structure
• The strong covalent bonds and the rigid structure make diamond extremely hard
• Lacks free electrons so it does not conduct electricity
• High melting and boiling points due to the strong covalent bonds which need a large amount of energy to be broken

Graphite

• Each carbon atom is bonded to three other carbon atoms, forming hexagonal layers
• Layers are held together by weak forces allowing them to slide over each other, making graphite slippery
• One electron from each carbon atom is delocalized, allowing graphite to conduct electricity and heat

Fullerenes

• Made up of carbon atoms arranged in hexagons and pentagons
• They are hollow and can be used to ‘cage’ other molecules
• Can form nanotubes which are conductive due to delocalized electrons

Carbon Nanotubes

• Hexagonal arrangement of carbon atoms but in cylindrical structures
• Strong covalent bonds make them extremely strong and lightweight
• Conduct electricity and are used in electronics

Graphene

• A single layer of graphite - very thin but extremely strong
• Excellent conductor of heat and electricity due to delocalized electrons
• High elasticity despite its strength