Which metal can be oxidized with an Sn²⁺ solution but not with an Fe²⁺ solution?

Verified step by step guidance

1. Identify the standard reduction potentials (E°) for Sn2+/Sn and Fe2+/Fe from a standard reduction potential table.
2. Understand that a metal can be oxidized by an ion if the ion has a higher reduction potential than the metal's corresponding ion.
3. Compare the reduction potential of Sn2+ with the reduction potential of the metal in question to determine if Sn2+ can oxidize the metal.
4. Similarly, compare the reduction potential of Fe2+ with the reduction potential of the metal in question to determine if Fe2+ can oxidize the metal.
5. Find a metal whose corresponding ion has a reduction potential between those of Sn2+ and Fe2+, indicating that it can be oxidized by Sn2+ but not by Fe2+.

Key Concepts

Oxidation and Reduction

Oxidation refers to the loss of electrons by a substance, while reduction is the gain of electrons. In redox reactions, one species is oxidized and another is reduced. Understanding these processes is crucial for determining which metals can be oxidized by specific ions, as the ability of a metal to be oxidized depends on its position in the electrochemical series.

Electrochemical Series

The electrochemical series is a list of metals and their standard electrode potentials, which indicates their tendency to be oxidized or reduced. Metals higher in the series are more easily oxidized than those lower down. This series helps predict which metals can be oxidized by certain ions, such as Sn2+ and Fe2+, based on their relative positions.

Metal Reactivity

Metal reactivity refers to how readily a metal can lose electrons and undergo oxidation. More reactive metals can displace less reactive metals from their compounds in solution. In the context of the question, identifying a metal that can be oxidized by Sn2+ but not by Fe2+ requires understanding the reactivity of the metals involved and their respective positions in the electrochemical series.