🎯 Common Question Types:
- Compare diamond and graphite structures and properties (4-6 marks)
- Explain high melting point of diamond/graphite/SiO₂ (2 marks)
- Explain why graphite conducts but diamond doesn't (2-3 marks)
- Suggest uses based on properties (1-2 marks)
📝 Key Command Words:
- Explain: Reference the bond type (strong covalent), number of bonds per atom, and free electrons
- Compare: State both substances' features side by side
- Suggest: Link properties to real uses (hardness → cutting, conductivity → electrodes)
- Identify: Match properties to structure type
⚠️ Common Mistakes to Avoid:
- Saying diamond "has no electrons" — it has electrons, they're just not free
- Saying graphite is soft because covalent bonds are weak — bonds within layers are strong
- Confusing "high melting point" with "hard" — graphite has a high MP but is soft
- Forgetting SiO₂ is also giant covalent — similar properties to diamond
- Describing fullerenes as giant covalent — they are simple molecules (discrete particles)
This exam tips covers Exam Tips for Giant Covalent Structures within Giant Covalent Structures for GCSE Chemistry. Revise Giant Covalent Structures in Bonding & Structure for GCSE Chemistry with 21 exam-style questions and 21 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 11 of 12 in this topic. Treat this as a marking guide for what examiners are looking for, not just a fact list.
Practice questions for Giant Covalent Structures
Why do giant covalent structures have very high melting points?
Explain why graphite conducts electricity but diamond does not.
Quick recall flashcards
What is graphene?
A single layer of graphite — extremely strong, conducts electricity
What are fullerenes?
Hollow carbon cages (like C₆₀) — used to deliver drugs in medicine