AQA · GCSE · Chemistry
Course version: 8462 · Version from Sept 2018
In graphite, each carbon atom forms three covalent bonds with three other…
Full specification wording
Graphite: In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers.
Graphite is a giant covalent structure of carbon.
Checked against the AQA 8462 specification (opens in a new tab) on .
- Point 1 of 4
- 4 key terms
Study notes
From the checked teaching notes for this specification point.
The idea
Graphite is a giant covalent structure of carbon. Each carbon atom bonds covalently to three other carbon atoms, leaving one outer electron per atom not used in bonding. The bonded atoms arrange into flat layers of hexagonal rings, like a honeycomb. Within a layer, each carbon has three single covalent bonds, so the layer is a continuous two-dimensional network. Between layers there are no covalent bonds; the layers are held together only by weak intermolecular forces. This explains why graphite is soft and slippery: the layers can slide over one another because the forces between them are weak, even though the covalent bonds within each layer are strong.
For example: This sliding allows graphite to be used as a lubricant and in pencil leads.
What earns the marks
- States that each carbon atom forms three covalent bonds to three other carbon atoms.
- Describes the layers as hexagonal rings or a honeycomb arrangement.
- States that there are no covalent bonds between the layers.
- Explains that weak forces between layers allow them to slide, making graphite soft and slippery.
- Contrasts strong covalent bonds within layers with weak forces between layers.
Common mistakes and how to put them right
Saying each carbon atom forms four covalent bonds in graphite.
Put it right by stating three covalent bonds per carbon atom.
Saying there are covalent bonds between the layers.
Put it right by stating there are no covalent bonds between layers, only weak forces.
Saying graphite is soft because its covalent bonds are weak.
Put it right by stating the covalent bonds within layers are strong and it is the weak forces between layers that allow sliding.
Exam tips
- Use the phrase layers of hexagonal rings when describing the structure.
- State clearly that there are no covalent bonds between the layers before explaining sliding.
- Contrast strong covalent bonds within a layer with weak forces between layers to explain softness.
Try the lesson
The start of the Graphite: In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers. lesson, made from checked teaching notes for this specification point.
Have a go first
How many covalent bonds does each carbon atom form in graphite?
Listen
Graphite is a giant covalent structure of carbon. Each carbon atom bonds covalently to three other carbon atoms, leaving one outer electron per atom not used in bonding. The bonded atoms arrange into flat layers of hexagonal rings, like a honeycomb. Within a layer, each carbon has three single covalent bonds, so the layer is a continuous two-dimensional network. Between layers there are no covalent bonds; the layers are held together only by weak intermolecular forces. This explains why graphite is soft and slippery: the layers can slide over one another because the forces between them are weak, even though the covalent bonds within each layer are strong. For example, this sliding allows graphite to be used as a lubricant and in pencil leads. A strong answer earns marks for these points. States that each carbon atom forms three covalent bonds to three other carbon atoms. Describes the layers as hexagonal rings or a honeycomb arrangement. States that there are no covalent bonds between the layers. Explains that weak forces between layers allow them to slide, making graphite soft and slippery. A common slip: Saying each carbon atom forms four covalent bonds in graphite. Instead, stating three covalent bonds per carbon atom. Exam tip: Use the phrase layers of hexagonal rings when describing the structure.
Key words
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Giant covalent structures
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Covalent bonding
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Layered structures
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Structure-property relationships
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See every definition
- Giant covalent structures
- Graphite is a giant covalent structure of carbon, in which each carbon atom bonds covalently to three other carbon atoms.
- Covalent bonding
- Within a layer, each carbon has three single covalent bonds, so the layer is a continuous two-dimensional network.
- Layered structures
- The bonded atoms arrange into flat layers of hexagonal rings, like a honeycomb, with no covalent bonds between the layers.
- Structure-property relationships
- Weak forces between layers allow them to slide, making graphite soft and slippery, even though the covalent bonds within each layer are strong.
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