Question

which would most likely be reduced when combined with cu(s)? click for a reduction potential chart a. zn²⁺ b. mg²⁺ c. au⁺ d. hg

Explanation:

Step1: Recall reduction potential concept

Elements with higher reduction - potential values are more likely to be reduced. Copper has a certain reduction - potential value. We need to compare the reduction - potential values of the given species with that of copper.

Step2: Analyze each option

• Option A: $Zn^{2 + }$ has a lower reduction potential than $Cu$. So, $Zn^{2+}$ is less likely to be reduced by $Cu$.
• Option B: $Mg^{2 + }$ has a very low reduction potential compared to $Cu$. $Mg^{2+}$ is not likely to be reduced by $Cu$.
• Option C: $Au^{+}$ has a higher reduction potential than $Cu$. When $Cu$ is combined with $Au^{+}$, $Au^{+}$ will be reduced to $Au$ and $Cu$ will be oxidized to $Cu^{2+}$.
• Option D: $Hg$ is in its elemental form. For a reduction to occur, we need a species in a higher - oxidation state. Also, $Hg$ has a relatively high reduction potential and is not likely to be reduced further by $Cu$.

Answer:

C. $Au^{+}$