Allotropes of Carbon: Diamond, Graphite and Buckminster Fullerene

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  • Created by: kamna03
  • Created on: 11-03-18 15:25

Diamond

A diamond is a giant molecule of carbon atoms.

Diamonds are colourless transparent. They sparkle and reflect light – they're sparkly which makes them convinent for use in jewelry.

Diamond is extremely hard and has a high melting point. For this reason it's very useful in cutting tools. The cutting edges of discs used to cut bricks and concrete  have diamond tipped ends. Heavy-duty drill bits, like those used for oil extraction to drill through rocks, are made with diamonds so that they stay sharp for longer.

Diamond is insoluble in water and it does not conduct electricity.

Every atom in a diamond is bonded to others by four strong covalent bonds leaving no free electrons and no ions. That's why diamond does not conduct electricity. The bonding also explains the hardness of diamond and its high melting point. A lot of energy would be needed to separate atoms so strongly bonded together. At the end of the document is a picture of the structure of diamond.

Graphite

Graphite is formed from carbon atoms in layers.

Graphite is black, shiny and opaque . It's also a material that slides easily.. It's used in pencil…

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