It is formed when each carbon atom is covalently bonded with three other carbon atoms.
Often forms tubular molecules(nanotubes) or spherical structures (Buckminister fullerene-C60 i.e 60 carbon atoms forms a ball)
Weak intermolecular forces having low melting points.
Weak forces makes them soft + slippery (Lubricant)
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Graphene
It is not a simple molecule
Consists of a sheet of carbon with no fixed formula.
Sheet is one atom thick--making it very light
covalently bonded--making it extremely strong
Allows electrons to freely move across its surface--making it a good electrical conductor
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Graphite
Giant molecular covalent structure
3D networks of carbons covalently bonded
Each carbon atom is covalently bonded with 3 carbon atoms forming a hexagonal sheet
sheets are held together by weak forces of attraction allowing the layers to slide past each other-- making it a good lubricant(soft/slippery)
Layered stucture--so not all of the electrons are covalently bonded. Delocalised electrons are free to move to carry electron--conducts electricity--used as electrodes
High melting points due to strong covalent bonds
Cheap and very unreactive
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diamond
Giant molecular covalent structure
3D rigid network of carbon atoms in a tetrahedral arrangement
Each carbon atom is covalently bonded with 4 other carbon atoms
Strong covalent bonds having high melting points
No charged particles/delocalised electrons so it is a good elecrical insulator
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