Which of the following substances will oxidize Sn(s) to Sn^2+?
a) Cu(s)
b) Cl2(g)
c)Cl-(g)
d) Mg(s)
e) Cu^2+(aq)
f) Mg^2+(aq)
To determine which substance will oxidize Sn(s) to Sn^2+, we need to understand the concept of oxidation and reduction reactions.
In an oxidation-reduction (redox) reaction, oxidation refers to the loss of electrons by a species, while reduction refers to the gain of electrons by a species. The substance that causes another substance to undergo oxidation is called an oxidizing agent. In this case, we are looking for the substance that can oxidize Sn(s) to Sn^2+.
To determine which substance can cause Sn(s) to undergo oxidation, we need to look at the reduction potentials (or reduction potentials) of the substances. A substance with a higher reduction potential than Sn(s) would be able to oxidize Sn(s) to Sn^2+.
Let's go through the given options and compare their reduction potentials to Sn(s):
a) Cu(s): The reduction potential of Cu(s) is higher than Sn(s). Therefore, Cu(s) can oxidize Sn(s) to Sn^2+.
b) Cl2(g): Cl2(g) is not an option for oxidizing Sn(s) to Sn^2+ because its reduction potential is lower than that of Sn(s).
c) Cl-(g): Cl-(g) is not an option for oxidizing Sn(s) to Sn^2+ as it is already in its reduced state (has gained an electron).
d) Mg(s): The reduction potential of Mg(s) is higher than Sn(s). Therefore, Mg(s) can oxidize Sn(s) to Sn^2+.
e) Cu^2+(aq): Cu^2+(aq) cannot oxidize Sn(s) to Sn^2+ as it is in its reduced state and has a lower reduction potential than Sn(s).
f) Mg^2+(aq): Mg^2+(aq) cannot oxidize Sn(s) to Sn^2+ as it is in its reduced state and has a lower reduction potential than Sn(s).
Therefore, the substances that can oxidize Sn(s) to Sn^2+ are Cu(s) and Mg(s) (options a and d).