Strongly electropositive metals, e.g. aluminium and sodium, are extracted from their ores by electrolysis. Chemical methods can be used to extract other metals, e.g.... show full transcript
Worked Solution & Example Answer:Strongly electropositive metals, e.g - Leaving Cert Chemistry - Question B - 2021
Step 1
Explain the underlined term.
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Answer
Electrolysis is a process that uses electricity to break down a chemical (substance) to cause a chemical reaction.
Step 2
Why must the aluminium oxide be molten?
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Answer
In molten form, ions are free to move, which is essential for conduction during electrolysis.
Step 3
Write balanced equations for the reactions that occur at the graphite electrodes, and for the overall reaction, during the electrolysis of aluminium oxide.
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Identify the chemical method used to extract iron from iron ore.
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Answer
Reduction is used, typically involving carbon monoxide, with a reaction in a blast furnace.
Step 5
Suggest a reason why strongly electropositive metals were not isolated before 1800.
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Before 1800, there was no electricity or the necessary techniques to isolate these highly reactive metals because they were too difficult to reduce.
Step 6
Refer to the electrochemical series to explain why only some metals are found free in nature.
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Answer
Metals lower down in the electrochemical series are more difficult to oxidise, making them less reactive. Those at the bottom are generally found as free metals.
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