Who this is for: Cambridge IGCSE Chemistry (0620) students who want extraction of metals — blast furnace, electrolysis and choosing a reduction method — to become a clear process map instead of disconnected diagrams.
What query it owns: how to understand and revise extraction of metals in Cambridge IGCSE Chemistry.
Why this is safe: this page owns the extraction of metals revision-guide angle, while Tutopiya’s Extraction Of Metals subtopic page owns the learning resource and the free Extraction Of Metals quiz owns the practice.

Extraction of metals is how useful metals are obtained from their ores. Cambridge IGCSE Chemistry (0620) tests the blast furnace for iron, electrolysis for aluminium, and the principle that more reactive metals need stronger extraction methods. This guide walks through each process, the equations examiners expect, and how reactivity decides the method.

Key takeaways

• Metals are extracted from ores — naturally occurring compounds (usually oxides or sulfides).
• Less reactive metals (below carbon) are reduced by carbon or carbon monoxide.
• Iron is extracted in the blast furnace using coke (carbon), limestone and haematite (Fe₂O₃).
• Aluminium is extracted by electrolysis of molten aluminium oxide — too reactive for carbon reduction.
• Electrolysis uses large amounts of electricity; the anode is carbon and must be replaced.

What is extraction of metals in Cambridge IGCSE Chemistry?

Extraction of metals is the industrial process of obtaining a pure metal from its ore by chemical reduction or electrolysis. In Cambridge IGCSE Chemistry, you describe the blast furnace and aluminium electrolysis, write key equations, and explain why different metals need different methods based on their position in the reactivity series.

Read the full notes on Tutopiya’s Extraction Of Metals subtopic page before attempting questions.

The core processes you must master

Metal	Method	Key materials / conditions	Main equation idea
Iron	Blast furnace	Coke, limestone, haematite, hot air	Fe₂O₃ + 3CO → 2Fe + 3CO₂
Aluminium	Electrolysis	Molten Al₂O₃ in cryolite; carbon electrodes	Al³⁺ + 3e⁻ → Al at cathode
Copper (low grade)	Electrolysis or displacement	From solution or scrap purification	Cu²⁺ + 2e⁻ → Cu
Zinc / below carbon	Carbon reduction	Heated with coke	Oxide + C → metal + CO/CO₂

How to answer extraction questions — step by step

1. Identify the metal and its approximate position in the reactivity series.
2. Choose the method — carbon reduction vs electrolysis.
3. Name raw materials — for iron: coke, limestone, haematite.
4. Write balanced equations for reduction steps.
5. State a purpose — e.g. limestone removes impurities as slag (CaSiO₃).
6. For electrolysis, identify anode and cathode products.

Test yourself with the free Extraction Of Metals quiz.

Blast furnace vs electrolysis: which process applies?

Situation	Process to describe	Typical signal words
Iron production	Blast furnace	”haematite”, “coke”, “slag”, “limestone”
Aluminium production	Electrolysis of molten oxide	”cryolite”, “carbon anode”, “cathode”
Method choice	Reactivity vs carbon	”why aluminium cannot be reduced by carbon”
Environmental	CO₂ from blast furnace	”environmental impact of iron extraction”

Extraction of metals in past-paper wording: command words that matter

Command word / phrase	What the question wants	Typical extraction stem
Describe	Process steps or conditions	”Describe how iron is extracted in the blast furnace.”
Write an equation	Balanced chemical equation	”Write an equation for the reduction of iron(III) oxide.”
Explain	Why a method is used	”Explain why aluminium is extracted by electrolysis.”
State	Named material or product	”State the purpose of limestone in the blast furnace.”

Worked exam-style stems (how to answer the wording)

1. “State the purpose of limestone in the blast furnace.” Limestone decomposes to calcium oxide, which reacts with sand (silicon dioxide) to form slag (calcium silicate) that removes impurities. Reward: slag formation linked to impurity removal.
2. “Explain why aluminium is extracted by electrolysis and not by carbon.” Aluminium is more reactive than carbon — carbon cannot reduce aluminium oxide. Reward: reactivity comparison with carbon.
3. “Write an equation for the reduction of iron(III) oxide by carbon monoxide.” Fe₂O₃ + 3CO → 2Fe + 3CO₂. Reward: balanced equation with CO as reducing agent.

When you can recognise the wording instantly, work through the Extraction Of Metals quiz and Reactivity Series.

How extraction connects to the rest of the course

Extraction links to the Reactivity Series, Redox and electrolysis in acids/bases. The Cambridge IGCSE Chemistry resource hub links all units.

Common mistakes students make

• Saying carbon reduces aluminium — aluminium is above carbon in reactivity.
• Confusing coke (carbon) with coal — coke is the fuel/reductant in the blast furnace.
• Forgetting limestone’s role — removes impurities as slag, not fuel.
• Writing electrolysis equations with water present — aluminium extraction uses molten oxide.
• Omitting that carbon anodes burn away in aluminium electrolysis (CO₂ formed).

When you need more support

If blast furnace or electrolysis diagrams keep losing marks, work through the Extraction Of Metals quiz, then get focused help from a Cambridge IGCSE Chemistry tutor.

Frequently asked questions

Why is cryolite used in aluminium extraction? It lowers the melting point of aluminium oxide, reducing energy costs and allowing the oxide to conduct when molten.

What is slag in the blast furnace? Calcium silicate formed when calcium oxide reacts with sand — it floats on molten iron and is removed as waste.

Can iron be extracted by electrolysis at IGCSE level? The syllabus focuses on blast furnace extraction for iron; electrolysis is the key method for aluminium.

How do I revise extraction of metals effectively? Learn one process at a time with equations and raw materials, then take the Extraction Of Metals quiz before mixing iron and aluminium questions.

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