AQA · Chemistry · 8462
GCSE Chemistry (AQA): Diamond & Graphite
Topic 2 — Bonding, Structure & Properties of Matter. Generated from the caption track of Cognito's lesson video "GCSE Chemistry - Diamond & Graphite - Structure | Properties (2027/28 exams)"; each card deep-links to the moment in the video it came from. Lesson 2.08 of Cognito's AQA GCSE Combined Science (Trilogy) and Chemistry course (Higher tier), filed under AQA Chemistry 8462. Teaching by Cognito — https://cognitoedu.org/coursesubtopic/c2-gcse-aqa-h-c_2.08.
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What is an allotrope?
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A different structural form of the same element in the same physical state, e.g. diamond and graphite are both solid carbon.
In graphite the carbon atoms are arranged into ? that form large flat sheets.
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hexagons
Why does each carbon atom in graphite have a delocalised electron?
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Carbon can form four bonds but uses only three in graphite, leaving one spare electron free to move.
How many carbon atoms is each carbon bonded to in graphite?
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Three.
Why does diamond not conduct electricity?
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It has no free electrons or ions that can move around — all four outer electrons of each carbon are used in bonding.
Why does diamond have a very high melting point?
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Its many strong covalent bonds in a giant lattice require a large amount of energy to break.
Why can graphite conduct electricity and heat?
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It has delocalised electrons that are free to move through the structure.
Why does graphite have a high melting point despite the weak forces between its layers?
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Within each layer the carbon atoms are held by strong covalent bonds, which need lots of energy to break.
What are fullerenes?
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Carbon structures such as spheres and tubes built from graphene-like layers.
How many carbon atoms is each carbon bonded to in diamond?
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Four — the maximum number of covalent bonds carbon can make.
Why is graphite soft and slippery?
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Its layers have no covalent bonds between them and are only weakly held together, so they can slide over one another.
A single layer of graphite is known as ?.
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graphene
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