Transition Elements Exam Questions
Practice IGCSE Chemistry exam questions on transition elements. Covers properties of transition metals, variable oxidation states, coloured compounds, catalytic activity, and comparisons with Group 1 metals 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 transition elements. Write full answers before checking.
Question 1 (4 marks, Core)
State four characteristic properties of transition metals that distinguish them from Group 1 metals.
Mark scheme
Any four from:
- They have variable oxidation states / can form ions with different charges (e.g. Fe2+ and Fe3+) [1]
- They form coloured compounds [1]
- They are useful as catalysts [1]
- They have higher melting points than Group 1 metals [1]
- They have higher densities than Group 1 metals [1]
- They are harder and stronger than Group 1 metals [1]
Examiner note: Each property must be clearly stated. “They are different from Group 1 metals” is not a property. Give specific examples where possible: iron is used as a catalyst in the Haber process; copper compounds are blue/green.
Question 2 (3 marks, Core)
Give one example of each of the following:
(a) A transition metal used as a catalyst, naming the process. (1)
(b) A coloured transition metal compound, stating its colour. (1)
(c) A transition metal with two different oxidation states, naming both compounds. (1)
Mark scheme
(a) Iron in the Haber process / vanadium(V) oxide in the Contact process / nickel in hydrogenation / manganese dioxide in decomposition of hydrogen peroxide [1]
(b) Copper sulfate (blue) / iron(III) oxide (red-brown) / potassium dichromate (orange) / potassium manganate(VII) (purple) [1]
(c) Iron: Fe2+ (iron(II), e.g. FeSO4 — green) and Fe3+ (iron(III), e.g. FeCl3 — yellow-brown) [1] OR: Copper: Cu+ (copper(I)) and Cu2+ (copper(II)) [1]
Examiner note: Transition metals form ions with different charges because they can lose different numbers of electrons. The Roman numeral in the name indicates the charge: iron(II) = Fe2+, iron(III) = Fe3+.
Question 3 (4 marks, Core)
Compare the properties of iron (a transition metal) with sodium (a Group 1 metal).
| Property | Iron | Sodium |
|---|---|---|
| Melting point | ? | 98 degC |
| Density | ? | 0.97 g/cm3 |
| Hardness | ? | Very soft |
| Reaction with water | ? | Vigorous |
Complete the table for iron. (4)
Mark scheme
| Property | Iron |
|---|---|
| Melting point | 1538 degC (much higher) [1] |
| Density | 7.87 g/cm3 (much higher) [1] |
| Hardness | Hard [1] |
| Reaction with water | Reacts slowly / only with steam, not cold water [1] |
Examiner note: Transition metals are “typical” metals — hard, dense, high melting point, and less reactive. Group 1 metals are unusual — soft, low density, low melting point, and very reactive. This contrast is a common exam question.
Question 4 (3 marks, Supplement)
Explain what is meant by variable oxidation states and give two examples of transition metals showing this property.
Mark scheme
- Variable oxidation states means that the element can form ions with different positive charges / can lose different numbers of electrons [1]
- Example 1: Iron can form Fe2+ (iron(II)) and Fe3+ (iron(III)) [1]
- Example 2: Copper can form Cu+ (copper(I)) and Cu2+ (copper(II)) / manganese can have oxidation states +2, +4, +7 [1]
Examiner note: Group 1 and Group 2 metals always form ions with the same charge (1+ and 2+ respectively). Transition metals are different because they have more complex electron configurations that allow them to lose different numbers of electrons.
Question 5 (2 marks, Core)
Explain why transition metals are widely used in construction and engineering, whereas Group 1 metals are not.
Mark scheme
- Transition metals are hard, strong, and have high melting points, making them suitable for structural use [1]
- Group 1 metals are too soft (can be cut with a knife), have low melting points, and are too reactive (react with air and water) to be used in construction [1]
Examiner note: Iron and steel (iron alloy) are the most commonly used structural metals. Sodium and potassium would be useless for construction — they would react with moisture in the air and corrode instantly.
Question 6 (3 marks, Supplement)
The colour of a transition metal compound can be used to identify it. State the colour of:
(a) Copper(II) sulfate solution (1)
(b) Iron(II) sulfate solution (1)
(c) Iron(III) chloride solution (1)
Mark scheme
(a) Blue [1]
(b) Pale green [1]
(c) Yellow / yellow-brown [1]
Examiner note: These colours are due to the transition metal ions: Cu2+ = blue, Fe2+ = pale green, Fe3+ = yellow/brown. These are frequently tested and must be memorised. The colour depends on the oxidation state — Fe2+ and Fe3+ give different colours.
Question 7 (3 marks, Core)
A student heats copper to form copper oxide, then iron to form iron oxide. The copper oxide is black and the iron oxide is red-brown.
(a) Write equations for both reactions. (2)
(b) Explain what these coloured products tell us about copper and iron. (1)
Mark scheme
(a) 2Cu + O2 → 2CuO [1] 4Fe + 3O2 → 2Fe2O3 [1]
(b) The coloured oxides confirm that copper and iron are transition metals, which characteristically form coloured compounds [1]
Examiner note: Group 1 and Group 2 metal oxides are white (e.g. Na2O, MgO, CaO). Coloured oxides are a distinctive feature of transition metals.
What to revise if you scored below 5
If transition metal properties were difficult to recall, make a list of four key properties with one example each. If colours were mixed up, make flashcards for Cu2+ (blue), Fe2+ (pale green), and Fe3+ (yellow/brown). Revisit the transition elements notes.
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