C1a Rocks and Metals

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C1a Rocks and Metals

2.2 Extracting Iron

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Learning objectives

Understand which metals can be extracted using carbon

Be able to describe how a blast furnace works

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What do you understand?

How would you rate yourself when thinking about extraction of metals?

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The Reactivity

Series

potassium

sodium

calcium

magnesium

aluminium

zinc

iron

copper

gold

(carbon)

Increasing reactivity

Metals above carbon must be extracted using electrolysis.

Metals below carbon

can be extracted from the ore by reduction using carbon, coke, or charcoal.

Gold and silver often do not need to

be extracted. They occur native.

The reactivity of a metal determines the method of extraction.

lead

silver

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Iron age

Iron – 2nd most common metal in the Earth’s crust

Found as haematite

Iron (III) oxide (Fe2O3)

Sand

Can be obtained using a blast furnace

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Reduction of iron ore

carbon + oxygen  carbon dioxide

Carbon dioxide + carbon  carbon monoxide

Carbon monoxide + iron oxide  iron + carbon dioxide

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Removing impurities

Calcium carbonate  calcium oxide + carbon dioxide

Calcium oxide + silicon dioxide  calcium silicate

This is called SLAG

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Summary of the process

Iron is not found naturally, but in Iron Ore

We can extract iron form iron ore using a Blast Furnace

Using chemistry we can produce pure iron

Limestone (CaCO3) is used to remove impurities

Coke/Carbon gives us the high temperature we need for the reactions to take place

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Learning outcomes

Why can some metals be extracted using carbon when some can’t?

What do we use to extract iron?

How does a blast furnace work?

What chemical reactions take place?

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Extraction of Iron