AQA · Chemistry · 8462
GCSE Chemistry: Graphite
Bonding, structure, and the properties of matter · AQA GCSE Chemistry (8462), specification point 4.2.3.2. Cards are generated from the exam board's own specification for "Graphite", and every card links back to the page it came from. Specification © AQA — used with attribution.
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How many covalent bonds does each carbon atom form in graphite?
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Three, each to another carbon atom.
In graphite, the carbon atoms are arranged in layers of ? rings.
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hexagonal
What type of bonding exists between the layers in graphite?
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None — there are no covalent bonds between the layers, only weak intermolecular forces.
How many electrons per carbon atom are delocalised in graphite?
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One.
Why does graphite conduct electricity?
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Each carbon atom has one delocalised electron, and these electrons are free to move through the structure and carry charge.
Why is graphite soft and slippery?
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There are no covalent bonds between the layers, so the layers can slide over each other easily.
In what way is graphite similar to metals?
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Both have delocalised electrons, which is why both conduct electricity.
Why does graphite have a very high melting point?
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Many strong covalent bonds between carbon atoms within the layers must be broken, which needs a lot of energy.
Why does each carbon atom in graphite have a delocalised electron?
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Carbon has four outer electrons but only forms three covalent bonds in graphite, leaving one electron delocalised.
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