When iron (Fe) is placed in a copper sulfate (CuSO4) solution, the blue solution slowly turns light green and the iron is coated with copper.

Question

This equation shows the transfer of electrons during the reaction.
Cu^2+ + Fe -> Cu + Fe^2+
Which best describes what happens during this oxidation-reduction reaction?

A. Iron gives up two electrons and copper accepts two electrons
B. Copper gives up two electrons and iron accepts two electrons
C. Iron gives up one electron and copper accepts one electron
D. Copper gives up one electron and iron accepts one electron

Answer 1

In the given oxidation-reduction reaction, the equation is:

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

In this reaction:

• Iron (Fe) is oxidized, meaning it loses electrons. Specifically, each iron atom loses two electrons to become \(\text{Fe}^{2+}\).
• Copper ions (\(\text{Cu}^{2+}\)) are reduced, meaning they gain electrons to become elemental copper (Cu).

The process can be summarized as follows:

• Iron gives up two electrons: \(\text{Fe} \rightarrow \text{Fe}^{2+} + 2e^-\)
• Copper accepts two electrons: \[\text{Cu}^{2+} + 2e^- \rightarrow \text{Cu}\]

Thus, the correct answer is:

A. Iron gives up two electrons and copper accepts two electrons.