Diamond and graphite are both forms of carbon. Both have giant covalent structures.
The table shows some properties of diamond and graphite.
| Property | Diamond | Graphite |
|---|---|---|
| hardness | very hard | soft and slippery |
| electrical conductivity | does not conduct | conducts |
| melting point | very high | very high |
Describe the structure of diamond.
Explain why diamond is used in the tips of cutting tools.
Graphite is used to make electrodes. Explain why graphite conducts electricity.
Graphite is used as a lubricant. Explain why graphite is slippery.
48 exam-style questions on Edexcel GCSE Chemistry 2.5 Types of substance, covering 2.5.1 Classifying substances by structure and bonding, 2.5.2 Properties of ionic and simple molecular substances, 2.5.3 Giant covalent structures: diamond and graphite, 2.5.4 Fullerenes, graphene and simple polymers, 2.5.5 Properties of metals and non-metals, and 2.5.6 Limitations of bonding models and representations. Each one has a worked solution and a mark scheme showing where the marks go.