Giant Covalent Structures Quiz
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5 questions, one answer each
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1. How many covalent bonds does each carbon atom form in diamond?
- A. 2
- B. 3
- C. 4
- D. 6
2. Why does graphite conduct electricity?
- A. It contains free-moving ions
- B. Each carbon atom has one delocalised electron that is free to move
- C. Its layers are held together by metallic bonds
- D. Graphite is not actually covalently bonded
3. Why do giant covalent structures like diamond have very high melting points?
- A. They contain weak intermolecular forces only
- B. All atoms are linked by strong covalent bonds throughout the structure
- C. They are made of small, separate molecules
- D. They contain free ions that resist melting
4. A substance is hard, has a very high melting point, and does not conduct electricity. What is it most likely to be?
- A. Graphite
- B. Diamond
- C. A simple molecular substance
- D. A metal
5. Graphite and diamond are both giant covalent structures made only of carbon, but graphite conducts electricity and is soft, while diamond does not conduct and is extremely hard. Which explanation accounts for both differences?
- A. Graphite has weaker covalent bonds than diamond
- B. Graphite atoms form three bonds each in layers with delocalised electrons and no bonds between layers, while diamond atoms form four bonds each in a fully bonded 3D network
- C. Diamond contains metallic bonding while graphite does not
- D. Graphite is a mixture of carbon and other elements, unlike pure diamond