Questions: Identify the species that is oxidized and the species that is reduced in the reaction. (Choose one) ∇ is oxidized and (Choose one) ∇ is reduced.

Transcript text: Identify the species that is oxidized and the species that is reduced in the reaction. (Choose one) $\boldsymbol{\nabla}$ is oxidized and (Choose one) $\boldsymbol{\nabla}$ is reduced.

Solution

Solution Steps

Step 1: Identify Oxidation and Reduction

In a redox reaction, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. We need to determine which species loses electrons and which gains electrons.

Step 2: Analyze the Reaction

The given reaction is:

\[ \mathrm{Fe} + \mathrm{Cu}^{2+} \rightarrow \mathrm{Fe}^{2+} + \mathrm{Cu} \]

Iron (Fe) starts as a neutral atom and becomes $\mathrm{Fe}^{2+}$. This indicates that Fe loses 2 electrons, so it is oxidized.
Copper (Cu}^{2+}\) starts as $\mathrm{Cu}^{2+}$ and becomes neutral Cu. This indicates that $\mathrm{Cu}^{2+}$ gains 2 electrons, so it is reduced.