Properties of Metals Exam Questions
Practice IGCSE Chemistry exam questions on properties of metals. Covers physical and chemical properties, metallic bonding links to properties, comparing metals with non-metals, and choosing metals for specific uses with mark schemes and examiner notes.
Published by IGCSEChemistry.com.my
Chemistry teaching team: K. S. Tan (15+ years teaching IGCSE Chemistry) and Ms Yash (10+ years teaching IGCSE Chemistry) and Ms Kartini (15+ years teaching IGCSE Chemistry).
Mapped to Cambridge IGCSE Chemistry 0620 (2026–2028). Last updated 2026-08-19.
These questions cover properties of metals. Write full answers before checking.
Question 1 (4 marks, Core)
State four physical properties typical of metals.
Mark scheme
Any four from:
- Good conductors of electricity [1]
- Good conductors of heat [1]
- Malleable (can be hammered into shape) [1]
- Ductile (can be drawn into wires) [1]
- High melting and boiling points (generally) [1]
- Shiny/lustrous appearance [1]
- High density (generally) [1]
Examiner note: “Strong” is too vague — use specific terms like malleable, ductile, hard. State “good conductors of electricity AND heat” as two separate properties for 2 marks.
Question 2 (3 marks, Supplement)
Use the metallic bonding model to explain why metals are:
(a) Good conductors of electricity. (1)
(b) Malleable. (1)
(c) Good conductors of heat. (1)
Mark scheme
(a) Metals have delocalised/free electrons that can move through the structure, carrying charge [1]
(b) Layers of metal ions can slide over each other without breaking the metallic bond, because the delocalised electrons continue to hold the structure together [1]
(c) Delocalised electrons gain kinetic energy when heated and transfer it rapidly through the metal by colliding with other electrons and ions [1]
Examiner note: All three explanations must reference delocalised electrons. Simply saying “metals have free electrons” without linking this to the property does not earn the mark.
Question 3 (3 marks, Core)
The table shows some properties of four elements.
| Element | Melting point (degC) | Electrical conductivity | Appearance |
|---|---|---|---|
| A | 1085 | High | Shiny, orange-brown |
| B | -7 | None | Yellow-green gas |
| C | 1538 | High | Shiny, grey |
| D | 44 | None | Yellow solid |
(a) Which elements are metals? (1)
(b) Which elements are non-metals? (1)
(c) Identify element A and element B. (1)
Mark scheme
(a) A and C [1]
(b) B and D [1]
(c) A = copper; B = chlorine [1]
Examiner note: Metals typically have high melting points, conduct electricity, and are shiny. Non-metals have lower melting points, do not conduct, and may be gases. The specific descriptions help with identification.
Question 4 (3 marks, Core)
Explain why copper is used for electrical wiring and aluminium is used for overhead power cables.
Mark scheme
- Copper is an excellent conductor of electricity [1] and is ductile (can be drawn into thin wires) [1]
- Aluminium is also a good conductor and is used for overhead cables because it has a much lower density than copper, so the cables are lighter and need less support [1]
Examiner note: This is a “choosing metals for uses” question. You must link the property to the use. Copper is better at conducting but heavier. Aluminium is lighter — important for long overhead spans.
Question 5 (4 marks, Core)
Compare the general properties of metals and non-metals. Complete the table.
| Property | Metals | Non-metals |
|---|---|---|
| State at room temp | Mostly ? | Mostly ? |
| Melting point | Generally ? | Generally ? |
| Electrical conductivity | ? | ? |
| Type of oxide | ? | ? |
Mark scheme
| Property | Metals | Non-metals |
|---|---|---|
| State at room temp | Mostly solid (except mercury) [1] | Mostly gases or solids; bromine is a liquid |
| Melting point | Generally high [1] | Generally low |
| Conductivity | Good conductors [1] (except graphite as a non-metal conductor) | Poor conductors / insulators |
| Oxide type | Basic (or amphoteric) [1] | Acidic (or neutral) |
Examiner note: Mercury is the only metal that is liquid at room temperature. Graphite (a form of carbon) is the main exception among non-metals — it conducts electricity due to delocalised electrons.
Question 6 (2 marks, Core)
Explain why metals are used to make saucepans.
Mark scheme
- Metals are good thermal conductors, so heat transfers quickly from the heat source through the pan to the food [1]
- Metals have high melting points, so they do not melt or deform at cooking temperatures [1]
Examiner note: Additional points could include: metals are malleable (can be shaped into a pan), strong (do not break when dropped). Stainless steel is commonly used because it also resists corrosion.
Question 7 (3 marks, Supplement)
Explain why most metals have high melting points, but mercury has a very low melting point (-39 degC).
Mark scheme
- Most metals have strong metallic bonds — strong electrostatic attraction between positive ions and the sea of delocalised electrons requires a lot of energy to overcome [1]
- Mercury has unusually weak metallic bonding [1]
- This is because mercury’s electron configuration results in very poor overlap of orbitals and weaker delocalisation, leading to weaker metallic bonds and a low melting point [1]
Examiner note: At IGCSE level, it is acceptable to say mercury has “weaker metallic bonds” without the detailed quantum explanation. The important point is that the general rule (high melting point) has exceptions, and these exceptions are explained by differences in bonding strength.
What to revise if you scored below 5
If you struggled to link properties to metallic bonding, memorise the three key explanations: conductivity = delocalised electrons move; malleability = layers slide; thermal conductivity = electrons transfer KE. Revisit the properties of metals notes.
Studying this yourself? Tutoring arrangements are normally made by a parent or guardian. Message us for the details to share with them, or send them this page.