C9.6 Extraction of metals

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Last updated 12:26 AM on 6/12/26
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7 Terms

1
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What is a metal ore?

  • A rock that contains enough of a metal to make it worthwhile extracting

    • Many of them are oxides, making extraction a reduction process

2
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Examples of oxide ores and how they are extracted

  • Iron ore: haematite → blast furnace

  • Aluminium ore: bauxite → electrolysis

3
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What are native metals and some examples?

  • Native metals are very unreactive metals which are found as uncombined elements, since they don’t react easily with other substances

  • Examples: gold and platinum

4
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What is the relation between metals in the reactivity series and their extraction methods?

  • Higher metals in reactivity series = more difficult to extract

    • Metals above carbon must be extracted using electrolysis

    • Metals below carbon can be extracted by heating with carbon or carbon monoxide (blast furnace)

  • Lower metals in reactivity series = easier to obtain

<ul><li><p>Higher metals in reactivity series = more difficult to extract</p><ul><li><p>Metals above carbon must be extracted using electrolysis</p></li><li><p>Metals below carbon can be extracted by heating with carbon or carbon monoxide (blast furnace)</p></li></ul></li><li><p>Lower metals in reactivity series = easier to obtain</p></li></ul><p></p>
5
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Describe what occurs in zone 1 of a blast furnace (include chemical equations)

  • Coke (carbon) burns in the hot air to form carbon dioxide

    • Exothermic reaction which provides heat for the furnace

<ul><li><p>Coke (carbon) burns in the hot air to form carbon dioxide</p><ul><li><p>Exothermic reaction which provides heat for the furnace</p></li></ul></li></ul><p></p>
6
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Describe what occurs in zone 2 of a blast furnace (include chemical equations)

  • At high temperatures, coke reacts with carbon dioxide to form carbon monoxide

    • Main reducing agent in the furnace

<ul><li><p>At high temperatures, coke reacts with carbon dioxide to form carbon monoxide</p><ul><li><p>Main reducing agent in the furnace</p></li></ul></li></ul><p></p>
7
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Describe what occurs in zone 3 of a blast furnace (include chemical equations)

  1. Carbon monoxide reduces the iron (III) oxide to iron

  • Iron extracted by reduction because oxygen is removed from iron (III) oxide

  • Molten iron collects at bottom of furnace and is tapped off

  1. Limestone (calcium carbonate) is added to the furnace to remove impurities in the ore

  • Calcium carbonate in limestone thermally decomposes to form calcium oxide

  1. Calcium oxide formed reacts with silicon dioxide—an impurity in the iron ore—to form calcium silicate

  • This melts and collects as a molten slag floating on top of the molten iron, which is tapped off separately

<ol><li><p>Carbon monoxide reduces the iron (III) oxide to iron</p></li></ol><ul><li><p>Iron extracted by reduction because oxygen is removed from iron (III) oxide</p></li><li><p>Molten iron collects at bottom of furnace and is tapped off</p></li></ul><ol start="2"><li><p>Limestone (calcium carbonate) is added to the furnace to remove impurities in the ore</p></li></ol><ul><li><p>Calcium carbonate in limestone thermally decomposes to form calcium oxide</p></li></ul><ol start="4"><li><p>Calcium oxide formed reacts with silicon dioxide—an impurity in the iron ore—to form calcium silicate</p></li></ol><ul><li><p>This melts and collects as a molten slag floating on top of the molten iron, which is tapped off separately</p></li></ul><p></p>