Allotropes of Carbon

Question 1

What is an allotrope?

Answer 1

Different structural forms of the same element

Question 2

Name the 4 Allotropes of carbon

Answer 2

Diamond
Graphite
Graphene
Fullerenes

Question 3

Diamond:

Answer 3

Each carbon atom in a Diamond has 4 covalent bonds.

They have a rigid structure (very hard)

High melting and boiling points because of the strong covalent bond between the atoms so a lot of energy is needed to overcome these bonds.

Cannot conduct electricity as there is no free election or ions to move

Question 4

Graphite:

Answer 4

Each carbon atom only has three covalent bonds

Can conduct electricity because they have delocalised that can carry charge around the structure

Structured in hexagonal layers
and these layers are held with weak intermolecular forces between them.

The layers can move past each other making Graphite a good lubricating material.

High melting and boiling points because of strong covalent bonds as more energy is needed to break the bonds in the layers.

Can conduct electricity as three out of the four electrons are held with covalent bonds so there is one delocalized electron left which can carry charge in the structure.

Question 5

Graphene:

Answer 5

A single hexagonal layer of Graphite that is only one atom thick

Very strong because of the covalent bonds in the layers

Graphene is very light

Can also conduct electricity because of the delocalized electrons in the layers

Used in electronics

Question 6

Fullerenes

Answer 6

Hollow molecules of carbon are shaped in tubes and balls.

Question 7

Examples of Fullerenes

Answer 7

Buckminsterfullerene
Nanotubes

Question 8

Uses of Fullerenes

Answer 8

Medicine
Catalysts
Strengthening materials
Electronics
Lubricant