0654.C2.4.04 — Describe the properties of ionic compounds: 6 Explain in terms of structure and bonding the (a). high melting points and boiling points prop: past paper questions
Real questions on 0654.c2.4.04 — describe the properties of ionic compounds: 6 explain in terms of structure and bonding the (a). high melting points and boiling points prop
The newest 6 of 6 written questions. Open one to see it on the real paper.
- 0973/41 · October/November 2025 · Q5d[2]
Explain why molten sodium oxide conducts electricity, but solid sodium oxide does not conduct electricity.
See it on the paper → - 0973/41 · May/June 2024 · Q5a(ii)[2]
Lithium chloride has a high melting point of 605 °C. Explain why lithium chloride has a high melting point.
See it on the paper → - 0973/42 · May/June 2023 · Q8e[2]
The element nitrogen is covalently bonded. The melting point of nitrogen is –210 °C. Calcium nitride, Ca 3 N 2 , is an ionic compound. The melting point of calcium nitride is 1195 °C. Explain the difference in melting points in terms of attractive forces.
See it on the paper → - 0973/31 · October/November 2022 · Q11d[1]
Describe the difference in the solubility in water of an ionic compound compared with a covalent compound.
See it on the paper → - 0973/41 · May/June 2021 · Q5b[3]
Chlorine atoms bond together to form the covalent molecule, Cl 2 . Chlorine, Cl 2 , is a gas at room temperature. Chlorine atoms bond with sodium atoms to form the ionic compound sodium chloride, NaCl. Sodium chloride, NaCl, is a solid at room temperature. Explain why chlorine is a gas but sodium chloride is a solid at...
See it on the paper → - 0973/41 · October/November 2019 · Q2c(ii)[2]
The melting point of magnesium nitride is very high. Explain why ionic compounds have high melting points.
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What examiners said
This question proved more difficult for some of the candidates. Often candidates got confused between the covalent bonding between the atoms and the intermolecular forces between covalently bonded molecules. Some candidates were not precise enough in their responses, simply describing strong bonds between ions in an ionic compound without reference to oppositely charged ions. Many candidates were...
— Examiner report, May/June 2023, 0973/42 Q8(e) (Cambridge)
Most candidates were challenged by the need to explain the normal states of chlorine and sodium chloride. The strongest responses made it clear that the forces between molecules of chlorine are weak, and the forces between oppositely charged sodium ions and chloride ions are strong. Marks could not be awarded for referring to the covalent bonds between atoms or molecules, or just referring to the...
— Examiner report, May/June 2021, 0973/41 Q5(b) (Cambridge)
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