When iron (Fe

Question

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

This equation shows the transfer of electrons during the reaction.

Cu2++Fe→Cu+Fe2+

Which best describes what happens during this oxidation-reduction reaction?

(1 point)
Responses

Copper gives up two electrons and iron accepts two electrons.
Copper gives up two electrons and iron accepts two electrons.

Copper gives up one electron and iron accepts one electron.
Copper gives up one electron and iron accepts one electron.

Iron gives up one electron and copper accepts one electron.
Iron gives up one electron and copper accepts one electron.

Iron gives up two electrons and copper accepts two electrons.

Answer 1

In the given oxidation-reduction reaction between iron (Fe) and copper ions (Cu²⁺ in CuSO₄), here's what happens:

1. Oxidation: Iron (Fe) is oxidized, meaning it loses electrons. In this case, iron loses two electrons to form Fe²⁺.
2. Reduction: Copper ions (Cu²⁺) are reduced, meaning they gain electrons. Each Cu²⁺ ion gains two electrons to form neutral copper (Cu).

The reaction can be summarized as follows:

• Iron (Fe) → Fe²⁺ + 2e⁻ (Iron is oxidized)
• Cu²⁺ + 2e⁻ → Cu (Copper is reduced)

Based on the description of the electron transfer:

• Iron gives up two electrons (which leads to the formation of Fe²⁺).
• Copper accepts two electrons (which leads to the formation of Cu).

Therefore, the best description of what happens during this oxidation-reduction reaction is:

Iron gives up two electrons and copper accepts two electrons.