Allotropes of Carbon

Question 1

Properties of Diamond?

Answer 1

1. Diamond has a giant covalent structure, made up of carbon atoms that each form four covalent bonds. This makes diamond very hard.
2. These strong covalent bonds take a lot of energy to break, and give diamond a very high melting point.
3. It doesn’t conduct electricity because it has no free electrons or ions.

Question 2

Properties of Graphite?

Answer 2

1. In graphite, each carbon atom only forms three covalent bonds, creating sheets of carbon atoms arranged into haxagons.
2. There aren’t any covalent bonds between the layers - they’re only held together weakly, so they’re free to slide over each other. This makes graphite soft and slippery (can be used as a lubricant)
3. Graphite has a high melting point - the covalent bonds in the layers require a lot of energy to break.
4. Only three of carbons outer shell electrons are used in covalent bonds, so each carbon atom has an electron that is delocalised. This means graphite conducts electricity and thermal energy.

Question 3

What are fullurenes?

Answer 3

1. Fullerenes are molecules of carbon shaped like closed tubes or hollow balls.
2. They’re mainly made up of carbon atoms arranged in haxagons, but also contain pentagons or heptagons.

Question 4

Uses of Fullurenes?

Answer 4

1. Fullurenes can be used to cage other molecules. The fullurene structure forms around another atom or molecule, which is then trapped inside. This could be used to deliver a drug into the body.
2. Fullerenes make good lubricants.
3. Fullurenes have a huge surface area so they make good industrial catalysts.
4. Fullurenes can form nanotubes.