Answer:
Fe - oxidized, reducing agent
Cu - reduced, oxidizing agent
Explanation:
We are given the following reaction:
2Fe + 3CuCl₂ →2FeCl3 + 3Cu
We want to figure out which element is oxidized and which one is reduced. Furthermore, we want to figure out which substance would be the oxidizing agent, and which one would be the reducing agent.
Remember that if a substance is being oxidized, it is also the reducing agent. The same goes for the substance being reduced; it is also the oxidizing agent.
Recall that in order to figure out which element is oxidized or reduced, we need to look at the changes in their oxidation numbers. If an element's oxidation number increases, then it is oxidized, but if it decreases, it is reduced.
In order to help us, remember that any element by itself will always have an oxidation number of 0, and halogens usually have an oxidation number of -1. In a compound, the total sum of the oxidation numbers will equal the charge. Similarly, ions always have the same oxidation number as their charge.
Based on the rules, for the left side of the equation, we can determine that:
For the right side of the equation, we can determine that:
Notice how Fe's number increased. This means that Fe is oxidized. It is also the reducing agent.
Furthermore, notice how Cu's oxidation number went down. This means that Cu is reduced, and is therefore the oxidizing agent.