Final answer:
The question asks to determine the strongest reducing agent among given options, including elemental and ionic forms of metals like magnesium and aluminum. Mg(s) stands out as the strongest reducing agent based on its position in the electrochemical series, which is confirmed by examples where magnesium is involved in reduction-oxidation reactions, solidifying its role as a reducing agent.
option e is the correct
Step-by-step explanation:
To determine which of the following is the strongest reducing agent:
- Al³⁺(aq)
- Mg²⁺(aq)
- Zn(s)
- Al(s)
- Mg(s)
We must consider which of them will more easily donate electrons. Since reducing agents undergo oxidation themselves, we look for the species that is most easily oxidized. In general, solid metals have greater reducing ability compared to their ions in aqueous solution, because ions are already in a higher oxidation state and require more energy to donate electrons.
Comparing the solid metals, we know from electrochemical series that Mg (s) is a stronger reducing agent than Al (s) and Zn (s). Therefore, Mg(s) is the strongest reducing agent among the given options.
In the provided reactions, we see agents like Mg and Al acting as reducing agents, confirming their tendencies to donate electrons:
- Mg(s) + NiCl₂ (aq) → MgCl2(aq) + Ni(s)
- F₂ (g) + 2Au(s) → 6F⁻ (aq) + 2Au³⁺ (aq), where Lithium (Li) is mentioned as the strongest reducing agent known.
Magnesium is specifically noted to be produced at the cathode during electrolysis, indicating its role as a reducing agent in this context.