Diamond, graphite and buckminsterfullerene, C₆₀, are all made only of carbon atoms.
The table shows information about them.
| Form of carbon | Description of structure | What happens when heated | Conducts electricity? |
|---|---|---|---|
| diamond | each carbon atom is covalently bonded to four other carbon atoms in a giant 3D structure | does not melt below 3500 °C | no |
| graphite | each carbon atom is covalently bonded to three other carbon atoms in flat layers of hexagons | does not melt below 3600 °C | yes |
| buckminsterfullerene | molecules of 60 carbon atoms, each shaped like a hollow ball | turns into a gas at about 600 °C | no |
Explain the differences in the properties shown in the table.
Use ideas about structure and bonding.
Diamond is used on the tips of drills for cutting rock.
Explain why diamond is suitable for this use.
Graphene is a single layer of graphite. Graphene is used in some flexible touch screens.
Suggest two properties of graphene that make it suitable for this use. Explain each property in terms of its structure and bonding.
60 exam-style questions on OCR GCSE Chemistry 2.3 Properties of materials, covering 2.3.1 Carbon bonding and the variety of organic compounds, 2.3.2 Diamond, graphite, fullerenes and graphene, 2.3.3 Bond strength, changes of state and predicting states, 2.3.4 Bulk properties and types of bonding, and 2.3.5 Nanoparticles: scale, surface area, uses and risks. Each one has a worked solution and a mark scheme showing where the marks go.