Chemistry›Giant Covalent Structures
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C2 · BondingAQA GCSE Chemistry · 8462 (Triple)

Giant Covalent Structures

Diamond, graphite, graphene, silicon dioxide — structures and properties. Higher tier material science.

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Diamond and graphite samples side by side, both allotropes of carbon
Wikimedia Commons, CC BY-SA 3.0Diamond and graphite - both giant covalent structures of carbon
CognitoGiant covalent structures — diamond, graphite, graphene
Key facts & methods

Diamond — fill in the table

PropertyDetail
Bonding
Properties
Uses

Graphite — fill in the table

PropertyDetail
Bonding
Properties
Uses

Graphene — fill in the table

PropertyDetail
Structure
Properties
Potential uses

Silicon dioxide (SiO₂) — fill in the table

PropertyDetail
Bonding
Properties
Occurrence & uses
Compare to diamond
Exam questions — 4 questions · 10 marks · AQA 8462 style
⚡ Show all working — the AI marks against the AQA mark scheme. Method marks awarded for correct working even if the final answer is wrong.
1 markDiamond vs graphiteAQA 8462 style

Why can graphite conduct electricity but diamond cannot?

A Graphite has a higher melting point than diamond
B Graphite contains one delocalised electron per carbon atom that is free to move and carry charge; diamond has all electrons in covalent bonds
C Diamond is made of a different type of carbon than graphite
D Graphite is an ionic compound
3 marksWhy is diamond hard?AQA 8462 P1 style

Explain why diamond is one of the hardest naturally occurring materials. Refer to its structure and bonding. (3 marks)

Hint: Structure: giant covalent, 3D network. Each C bonded to 4 others. All bonds are strong covalent bonds that would need to be broken. Link to hardness.
+30 XP
1 markGraphene propertiesAQA 8462 style

Which of the following is NOT a property of graphene?

A Excellent electrical conductor
B Extremely strong for its mass
C Does not conduct electricity because all electrons are in covalent bonds
D Only one atom thick (a single layer of graphite)
4 marksCompare allotropesAQA 8462 style

Diamond and graphite are both allotropes of carbon. Compare their structures and explain why graphite is used as a lubricant but diamond is used as a cutting tool. (4 marks)

Hint: Two structures → two properties → two uses. Be explicit about why each structure gives each property.
+40 XP
Quick recall flashcards

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