Extraction of metals
Cambridge IGCSE Chemistry (0620) · Unit 9: Metals · 8 flashcards
Extraction of metals is topic 9.3 in the Cambridge IGCSE Chemistry (0620) syllabus , positioned in Unit 9 — Metals , alongside Properties of metals, Reactivity series and Uses of metals. In one line: An alloy is a mixture of a metal with other elements. These elements can be other metals or non-metals. Alloys are often harder and stronger than pure metals.
This topic is examined in Paper 1 (multiple-choice) and Papers 3/4 (theory), plus Paper 5 or Paper 6 (practical / alternative to practical).
The deck below contains 8 flashcards — 2 definitions, 3 key concepts and 3 identification cards — covering the precise wording mark schemes reward. Use the 2 definition cards to lock down command-word answers (define, state), then move on to the concept and application cards to handle explain, describe and compare questions.
An alloy
An alloy is a mixture of a metal with other elements. These elements can be other metals or non-metals. Alloys are often harder and stronger than pure metals.
What the Cambridge 0620 syllabus says
2026-2028 syllabus, in our wordsWhat the syllabus expects you to be able to do in this topic, in plain English. Match the command word (Describe, Explain, State, etc.) in your answer to score full marks. For the exact wording, see the official syllabus (PDF).
- Describe Describe how easy or hard it is to get a metal from its ore, and link this to where the metal is in the reactivity series.
- Describe Describe how iron is extracted from hematite in a blast furnace, covering only: burning carbon (coke) to give heat and form carbon dioxide; carbon dioxide being reduced to carbon monoxide; carbon monoxide reducing iron(III) oxide; limestone (calcium carbonate) breaking down on heating (thermal decomposition) to give calcium oxide; and slag forming. You do not need symbol equations here.
- State State that aluminium's main ore is bauxite and that electrolysis is used to extract the metal.
- State State, as symbol equations, how iron is extracted from hematite: C + O₂ → CO₂; C + CO₂ → 2CO; Fe₂O₃ + 3CO → 2Fe + 3CO₂; CaCO₃ → CaO + CO₂; CaO + SiO₂ → CaSiO₃. Supplement
- Describe Describe how aluminium is extracted from purified bauxite (aluminium oxide), including what cryolite does, why the carbon anodes must be replaced regularly, and the electrode reactions with their ionic half-equations. Details of how bauxite is purified are not required. Supplement
What is an alloy?
An alloy is a mixture of a metal with other elements. These elements can be other metals or non-metals. Alloys are often harder and stronger than pure metals.
Give an example of an alloy containing copper, and its constituent element.
Brass is an alloy made from copper and zinc. By mixing copper and zinc, you create a material more suitable for some applications than pure copper.
Give an example of an alloy containing iron, and its constituent elements.
Stainless steel is an alloy made from iron, chromium, nickel, and carbon. The addition of these elements makes it resistant to rusting.
Why are alloys often more useful than pure metals?
Alloys are often harder and stronger than the pure metals they are composed of. This makes them more suitable for certain applications.
Explain why alloys are harder and stronger than pure metals in terms of their structure.
Alloys have atoms of different sizes disrupting the regular arrangement of atoms. This means the layers of atoms can no longer easily slide over each other, making the alloy harder and stronger. The different sized atoms prevent easy movement.
Explain the purpose of adding chromium to steel to make stainless steel.
The chromium reacts with oxygen to form a thin layer of chromium oxide on the surface of the steel. This layer protects the iron from rusting (oxidation).
Describe one specific use of stainless steel and explain why it is suitable for that use.
Stainless steel is used in cutlery because of its hardness and resistance to rusting. The hardness means it can withstand repeated use, and resistance to rusting ensures it stays clean and hygienic.
Name one property that alloys have over their pure metal counterparts
Alloys are often stronger and harder than their pure metal counterparts. This makes them useful in a variety of different applications
Key Questions: Extraction of metals
What is an alloy?
An alloy is a mixture of a metal with other elements. These elements can be other metals or non-metals. Alloys are often harder and stronger than pure metals.
Name one property that alloys have over their pure metal counterparts
Alloys are often stronger and harder than their pure metal counterparts. This makes them useful in a variety of different applications
Tips to avoid common mistakes in Extraction of metals
- ● Metals BELOW carbon in the reactivity series can be extracted from their oxides using carbon; metals ABOVE carbon need electrolysis.
- ● Consider both what a metal does and does not react with to gauge its reactivity.
- ● Learn common applications: aluminium is used where lightness and corrosion resistance are key, stainless steel for its strength and resistance to rust.
- ● Create a table summarizing the reactions of common metals (Ca, Mg, Zn, Fe, Cu) with water, steam, and dilute acids, linking it to the metal reactivity series.
- ● Relate metal extraction method to reactivity: electrolysis (most reactive), carbon reduction (intermediate), native state (least reactive).
More topics in Unit 9 — Metals
Extraction of metals sits alongside these Chemistry decks in the same syllabus unit. Each uses the same spaced-repetition system, so progress in one informs the next.
Cambridge syllabus keywords to use in your answers
These are the official Cambridge 0620 terms tagged to this section. Mark schemes credit responses that use the exact term — weave them into your answers verbatim rather than paraphrasing.
Key terms covered in this Extraction of metals deck
Every term below is defined in the flashcards above. Use the list as a quick recall test before your exam — if you can't define one of these in your own words, flip back to that card.
Related Chemistry guides
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