Final answer:
A lower position on the table of standard reduction potentials indicates a stronger tendency for the reactant to be oxidized. which has the weakest oxidizing power in the given set, is the hardest to reduce and thus the easiest to oxidize.
Step-by-step explanation:
The table of standard reduction potentials is a tool used to predict the spontaneity of redox reactions and understand the behavior of reactants and products in these reactions. A lower position on this table, which corresponds to a more negative reduction potential, indicates a stronger tendency for the reactant to lose electrons, or, in other words, to be oxidized. Therefore, the correct answer to the question is (c) Reactant to be oxidized.
When assessing oxidizing agents, the strength is determined by how easily they can gain electrons, which is reflected by a higher (or more positive) reduction potential. Conversely, substances with lower (or more negative) reduction potentials will be weaker oxidizing agents and are more inclined to lose electrons, hence they are more readily oxidized. To illustrate, if we have compounds like permanganate, dichromate, and titanium dioxide, the one with the largest reduction potential is the strongest oxidizer. In contrast, a species like titanium dioxide, which has the weakest oxidizing power in the given set, is the hardest to reduce and thus the easiest to oxidize.