Here is an electrode reaction.
$C u \to C u^{2 +} (C u p p e r i o n s) + 2 e^{-}$
In which electrode the reaction is taking place? Is this reaction oxidation or reduction?

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Solution

The reaction which involves the loss of electrons is Oxidation and after oxidation, a positively charged species will be formed.
The loss of electrons or oxidation is happening on the electrode Anode.
While that reduction or gain of electrons is happening on the electrode Cathode.
The reaction here happening is loss of electrons and positively charged copper ions are forming so the reaction is oxidation.
$C u \to C u^{2 +} (C u p p e r i o n s) + 2 e^{-}$
Hence, The reaction is taking place at Anode and the reaction is an oxidation process.

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Q. (a) Here is an electrode reaction:
Cu → Cu²⁺ + 2e.
At which electrode (anode or cathode) would such a reaction take place? Is this an example of oxidation?
(b) A solution contains magnesium ions (Mg²⁺), iron (II) ions (Fe²⁺) and copper ions (Cu²⁺). On passing an electric current through this solution which ions will be the first to be discharged at the cathode? Write the equation for the cathode reaction.
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(a) Here is an electrode reaction :

$C u \to C u^{2 +} + 2 e^{-}$ . At which electrode (anode or cathode) would such a reaction take place? Is this an example of oxidation or reduction ?

(b) A solution contains magnesium ions $(M g^{2 +})$ , iron (II) ions $F e^{2 +}$ and copper ions $C u^{2 +}$ . On passing an electric current through this solution, which ions will be the first to be discharged at the cathode? Write the equation for the cathode reaction.