Allotropes of Carbon
- Created by: ElizabethStudies
- Created on: 21-01-20 17:25
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- Allotropes of Carbon
- Diamond is very hard.
- Diamond has a giant covalent structure, made up of carbon atoms that each form 4 covalent bonds.
- Diamond has a high melting and boiling point because of the strong covalent bonds.
- It doesn't conduct electricity because it has no free electrons or ions.
- Graphite contains sheets of hexagons.
- Each carbon atom forms three covalent bonds.
- There are not any covalent bonds between the layers so they are free to move over each other. This makes graphite soft and slippery.
- The covalent bonds need lots of energy to break so graphite has got a high melting and boiling point.
- Graphite conducts electricity and thermal energy because only three out of carbons four outer electrons so each carbon atom has one electron that is delocalised.
- Graphene is one layer of graphite.
- Graphene is a sheet of carbon atoms joined together in hexagons. The sheet is just one atom thick, making it a 2 - dimensional compound.
- The network of covalent bonds make it very strong and it is also incredibly light.
- It contains delocalised electrons so can conduct electricity.
- Fullerenes form spheres and tubes.
- Fullerenes are molecules of carbon.
- Fullerenes can be used to 'cage' other molecules - the fullerene structure forms around another atom or molecule. This could be used to deliver a drug into the body.
- Fullerenes have a huge surface area, so they can help in making industrial catalysts.
- Diamond is very hard.
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