Eduqas GCSE Chemistry
Eduqas GCSE Chemistry 6 Reactivity Series and Extraction of Metals Exam Questions
Free Eduqas GCSE Chemistry revision for 6 Reactivity Series and Extraction of Metals: what you need to know, common mistakes and exam-style questions with answers. Covers the reactivity series, displacement and redox reactions, extraction of iron and aluminium, electrolysis of molten and aqueous compounds and electroplating.
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About Eduqas GCSE Chemistry 6 Reactivity Series and Extraction of Metals
This Eduqas GCSE Chemistry topic uses the reactivity series to explain how metals react and how they are extracted from their ores. You learn displacement reactions, oxidation and reduction in terms of oxygen and electrons, extraction of iron by reduction with carbon in the blast furnace, and extraction of aluminium by electrolysis. Electrolysis of molten and aqueous solutions, half equations and electroplating are central, along with metal properties and tests for metal ions using sodium hydroxide. It builds on ions and bonding (topic 5) and links to corrosion (topic 11). Examiners often ask you to predict electrolysis products and write half equations, and to explain why aluminium needs electrolysis.
What you need to know
- Reactivity series Potassium, sodium, calcium, magnesium, aluminium, (carbon), zinc, iron, (hydrogen), copper, silver, gold. A more reactive metal displaces a less reactive metal from its compound. SP6A: relative reactivities of metals through displacement reactions.
- Oxidation and reduction Oxidation is gain of oxygen or loss of electrons; reduction is loss of oxygen or gain of electrons. In Mg + CuSO4 → MgSO4 + Cu, magnesium is oxidised and copper ions are reduced.
- Extracting iron Metals less reactive than carbon are extracted by heating with carbon. In the blast furnace, coke burns to form carbon monoxide, which reduces iron(III) oxide: Fe2O3 + 3CO → 2Fe + 3CO2. Limestone removes impurities as slag.
- Extracting aluminium Aluminium is more reactive than carbon so it is extracted by electrolysis of aluminium oxide dissolved in molten cryolite, which lowers the operating temperature. Aluminium forms at the cathode and oxygen at the anode, which burns the carbon anodes away.
- Electrolysis of solutions Positive ions move to the cathode and negative ions to the anode. In aqueous solutions, hydrogen forms at the cathode unless the metal is less reactive than hydrogen; oxygen forms at the anode unless halide ions are present. Half equations: Cu2+ + 2e- → Cu; 2Cl- → Cl2 + 2e-. SP6B: electrolysis of aqueous solutions and electroplating.
- Tests for metal ions Add sodium hydroxide solution: Cu2+ gives a blue precipitate, Fe2+ green, Fe3+ orange-brown. Aluminium, calcium and magnesium give white precipitates; aluminium hydroxide dissolves in excess.
Common mistakes in 6 Reactivity Series and Extraction of Metals
- Saying the cathode is positive. In electrolysis the cathode is negative and attracts positive ions.
- Predicting sodium at the cathode in electrolysis of sodium chloride solution. Sodium is more reactive than hydrogen, so hydrogen is produced.
- Writing half equations with electrons on the wrong side. Reduction at the cathode gains electrons; oxidation at the anode loses electrons.
- Saying aluminium is extracted by electrolysis because it is expensive. It is extracted by electrolysis because it is more reactive than carbon.
- Saying carbon reduces iron oxide directly in the blast furnace equation. The main reducing agent is carbon monoxide.
Try three 6 Reactivity Series and Extraction of Metals exam-style questions
1. Calculate the maximum mass of iron produced from 320 g of iron(III) oxide. Fe2O3 + 3CO → 2Fe + 3CO2 (Ar: Fe = 56, O = 16) (3 marks)
Show the mark scheme answer
Mr Fe2O3 = 160 so moles = 320 / 160 = 2.0 mol; moles Fe = 2 x 2.0 = 4.0 mol; mass = 4.0 x 56 = 224 g.
2. Name the products at each electrode when copper(II) sulfate solution is electrolysed with inert electrodes, and write the half equation at the cathode. (3 marks)
Show the mark scheme answer
Cathode: copper; anode: oxygen; Cu2+ + 2e- → Cu.
3. Explain why aluminium oxide is dissolved in molten cryolite during electrolysis. (2 marks)
Show the mark scheme answer
It lowers the melting point / operating temperature; so less energy is needed, which reduces costs.
6 Reactivity Series and Extraction of Metals FAQs
What does Eduqas GCSE Chemistry 6 Reactivity Series and Extraction of Metals cover?
It covers the reactivity series and displacement, oxidation and reduction, extraction of iron and aluminium, electrolysis of molten and aqueous compounds, electroplating and tests for metal ions.
Which paper is 6 Reactivity Series and Extraction of Metals examined in?
It is examined in Component 1: Concepts in Chemistry (2 hours 15 minutes, 120 marks). Component 2: Applications in Chemistry can also test it through practical contexts and an unseen article.
How do I predict electrolysis products in Eduqas GCSE Chemistry 6 Reactivity Series and Extraction of Metals?
For a molten compound, the metal forms at the cathode and the non-metal at the anode. For a solution, compare the metal with hydrogen at the cathode, and check for halide ions at the anode; if there are none, oxygen is produced.
