Define (i) oxidation, (ii) reduction, in terms of electron transfer - Leaving Cert Chemistry - Question (b) - 2014
Question (b)
Define (i) oxidation, (ii) reduction, in terms of electron transfer.
When a zinc rod is dipped into a blue solution of copper(II) sulfate, the following oxidation-r... show full transcript
Worked Solution & Example Answer:Define (i) oxidation, (ii) reduction, in terms of electron transfer - Leaving Cert Chemistry - Question (b) - 2014
Step 1
Define (i) oxidation
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Answer
Oxidation is defined as the loss of electrons from an atom or ion. This process results in an increase in the oxidation state of the substance.
Step 2
Define (ii) reduction
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Answer
Reduction is defined as the gain of electrons by an atom or ion. This process leads to a decrease in the oxidation state of the substance.
Step 3
Identify (iii) the species oxidised
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Answer
The species oxidised in this reaction is Zinc (Zn). It loses two electrons during the reaction.
Step 4
Identify (iv) the species reduced
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Answer
The species reduced is Copper ions (Cu²⁺). They gain two electrons to become elemental copper (Cu).
Step 5
Identify (v) the oxidising agent
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The oxidising agent in this reaction is the Copper ions (Cu²⁺), as they accept electrons from Zinc.
Step 6
Is zinc (Zn) placed above or below copper (Cu) in the electrochemical series?
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Zinc (Zn) is placed above Copper (Cu) in the electrochemical series.
Step 7
Give a reason for your answer.
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Answer
Zinc loses electrons more easily than copper, meaning it is more readily oxidised. The standard electrode potential for zinc is negative, while for copper it is positive, indicating that in an electrochemical cell, electrons flow from zinc to copper through the wire, confirming that zinc is more reactive.
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