Multiple Choice
Which of the following metals will react with a solution of copper(II) sulfate, based on the activity series?
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6. Chemical Quantities & Aqueous Reactions
Activity Series
Multiple Choice
Which of the following ions is the strongest oxidizing agent according to the activity series?
A
Zn^{2+}
B
Ag^{+}
C
Cu^{2+}
D
Fe^{3+}
Verified step by step guidance1
Understand that an oxidizing agent is a species that gains electrons (is reduced) during a redox reaction. The stronger the oxidizing agent, the more readily it accepts electrons.
Recall that the activity series ranks metals and their ions based on their tendency to be reduced or oxidized. Ions higher in the activity series are stronger oxidizing agents because they more easily gain electrons.
Identify the standard reduction potentials for each ion: \(\mathrm{Zn^{2+}}\), \(\mathrm{Ag^{+}}\), \(\mathrm{Cu^{2+}}\), and \(\mathrm{Fe^{3+}}\). The ion with the highest (most positive) standard reduction potential is the strongest oxidizing agent.
Compare the standard reduction potentials: for example, \(\mathrm{Ag^{+} + e^{-} \rightarrow Ag}\) has a higher reduction potential than \(\mathrm{Zn^{2+} + 2e^{-} \rightarrow Zn}\), \(\mathrm{Cu^{2+} + 2e^{-} \rightarrow Cu}\), and \(\mathrm{Fe^{3+} + e^{-} \rightarrow Fe^{2+}}\).
Conclude that the ion with the highest standard reduction potential (in this case, \(\mathrm{Ag^{+}}\)) is the strongest oxidizing agent according to the activity series.
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