Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?

Verified step by step guidance

1. insert step 1: Understand the concept of oxidation and reduction. Oxidation involves the loss of electrons, while reduction involves the gain of electrons.
2. insert step 2: Refer to the standard reduction potential table. Metals with lower reduction potentials can be oxidized by ions of metals with higher reduction potentials.
3. insert step 3: Identify the standard reduction potentials for Mn^{2+} and Mg^{2+}. Mn^{2+} has a higher reduction potential than Mg^{2+}.
4. insert step 4: Determine which metals have reduction potentials between Mn^{2+} and Mg^{2+}. These metals can be oxidized by Mn^{2+} but not by Mg^{2+}.
5. insert step 5: Select a metal from the list identified in step 4 that fits the criteria of being oxidized by Mn^{2+} but not by Mg^{2+}.

Key Concepts

Oxidation and Reduction

Oxidation refers to the loss of electrons by a substance, while reduction is the gain of electrons. In a redox reaction, one species is oxidized and another is reduced. Understanding these processes is crucial for determining which metals can be oxidized by specific ions, as it involves comparing their relative tendencies to lose electrons.

Electrochemical Series

The electrochemical series is a list of elements arranged by their standard electrode potentials. 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, as a metal can only be oxidized by an ion that has a higher reduction potential.

Metal Reactivity

Metal reactivity refers to how readily a metal can lose electrons and undergo oxidation. This property varies among metals, with alkali metals being highly reactive and noble metals being less so. In the context of the question, identifying the reactivity of the metals involved will clarify which can be oxidized by Mn2+ but not by Mg2+.