Common Misconceptions
Part of Giant Covalent Structures · GCSE GCSE Chemistry revision
This common misconceptions covers Common Misconceptions 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 8 of 12 in this topic. Use this common misconceptions to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 8 of 12
Practice
21 questions
Recall
21 flashcards
⚠️ Common Misconceptions
Misconception 1: "Graphite has no covalent bonds — it's held together by weak forces"
Graphite has very strong covalent bonds — WITHIN each layer. The hexagonal sheets are held together by covalent bonds just as strong as in diamond. The weak forces are only BETWEEN the layers. This is why graphite has a very high melting point (you must break those strong intralayer bonds) but is still soft (the layers slide easily past each other).
Misconception 2: "Diamond conducts electricity because it's very pure carbon"
Purity is irrelevant to conductivity. Diamond doesn't conduct because ALL its outer electrons are locked in covalent bonds — none are free to move. Conductivity requires mobile charge carriers (free electrons or ions). Diamond has none.
Misconception 3: "Fullerenes are giant covalent structures"
Fullerenes (like C₆₀) are actually simple molecular structures — they consist of discrete, finite molecules with a fixed number of carbon atoms. They are NOT giant structures. Fullerene molecules have weak intermolecular forces between them, which is why they have relatively low melting points compared to diamond and graphite.
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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.
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