⚡ Topic 2.7: Metallic Bonding
Past Paper Practice (Papers 2 & 4)
Cambridge IGCSE Chemistry 0620 (2026-2028)
📋 Examination Instructions
• Total Marks: 42 marks
• Recommended Time: 50 minutes
• Structure:
→ Section A: Definitions & Structure (5 questions)
→ Section B: Malleability (5 questions)
→ Section C: Electrical & Thermal Conductivity (5 questions)
• Command Words: Describe, Explain, State, Suggest, Compare
• ⚠️ Mark Scheme Rules: Use Cambridge keywords. Vague answers = 0 marks.
Section A: Definitions & Structure (10 marks)
Describe the structure of metallic bonding.
A student states: "Metals contain atoms held together by strong forces." Explain what is incorrect about this statement and provide the correct description.
State the origin of the delocalised electrons in sodium metal.
Magnesium has a higher melting point than sodium. Suggest why magnesium has stronger metallic bonding than sodium.
Describe the arrangement of particles in a metal.
Section B: Malleability (13 marks)
Copper can be hammered into thin sheets without breaking. Explain why metals like copper are malleable.
The diagram shows the structure of a metal before and after force is applied. [Before: Regular layers of positive ions] [After: Layers shifted but still intact] Use the diagram to explain why the metal does not shatter when the force is applied.
A blacksmith heats iron and then hammers it into the shape of a horseshoe. Explain why heating makes the iron easier to shape.
Aluminium is used to make aircraft bodies because it is both strong and malleable. State what is meant by the term "malleable".
Compare the malleability of metals with the brittleness of ionic compounds. Explain the difference in terms of structure and bonding.
Section C: Conductivity (19 marks)
Explain why copper is used for electrical wiring.
A student tests the electrical conductivity of solid magnesium and molten magnesium. Both conduct electricity. Explain why, in terms of particles, both forms conduct.
The table shows the electrical conductivity of three substances: | Substance | Conductivity | |-----------|-------------| | Copper | Good | | Graphite | Good | | Diamond | Poor | All three are made of non-metal elements (or contain non-metals). Copper is a metal. Explain, in terms of bonding and structure, why copper and graphite conduct but diamond does not.
Explain why metals are good conductors of heat.
A student connects a battery to a piece of copper wire and measures the current. (a) State what happens to the delocalised electrons when the battery is connected. [2] (b) The student heats the copper wire. The current decreases slightly. Suggest why heating the metal reduces its electrical conductivity. [3]
🎯 Examination Summary
⚠️ EXAMINER WARNING: The most common mistake is forgetting that metals contain IONS (not atoms) and that the metallic bond is NOT BROKEN when layers slide. Always use Cambridge keywords: "delocalised", "electrostatic attraction", "positive ions".
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