Bonding & StructureKey Facts

Key Facts to Memorise

Part of Giant Covalent Structures · GCSE GCSE Chemistry revision

This key facts covers Key Facts to Memorise 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 7 of 12 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.

Topic position

Section 7 of 12

Practice

21 questions

Recall

21 flashcards

📌 Key Facts to Memorise

Giant covalent structures = atoms connected by covalent bonds extending in all directions
No molecules — the whole solid is one giant structure
Very high melting points — many strong covalent bonds must be broken
Diamond: 4 bonds per C, very hard, doesn't conduct, transparent
Graphite: 3 bonds per C, soft layers, CONDUCTS (free electrons), black
Why graphite conducts: 1 free electron per carbon can move along layers
Why graphite is soft: weak forces between layers allow them to slide
Silicon dioxide: similar to diamond structure, very hard, high MP, doesn't conduct

Quick Check: Why do diamond and graphite both have very high melting points, even though graphite is soft?

Keep building this topic

Read this section alongside the surrounding pages in Giant Covalent Structures. That gives you the full topic sequence instead of a single isolated revision point.

Key Definitions Common Misconceptions Diamond Structure — Click to Explore Graphite Structure — Layered Giant Covalent

Practice Questions for Giant Covalent Structures

Why do giant covalent structures have very high melting points?

A. They contain ionic bonds that are difficult to break
B. They contain weak forces between separate molecules
C. They contain delocalised electrons that require a lot of energy to remove
D. They contain many strong covalent bonds that require a lot of energy to break

1 markfoundation

Explain why graphite conducts electricity but diamond does not.

3 marksstandard

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

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Key Definitions

Common Misconceptions