Which of the following trends indicates the weakest oxidizing agent from a table of standard electrode potentials?

The trend that indicates the weakest oxidizing agent corresponds to the lowest positive electrode potential. Oxidizing agents are substances that can accept electrons and, therefore, undergo reduction. The strength of an oxidizing agent is determined by its standard electrode potential, with higher values indicating a greater tendency to gain electrons and be reduced.

In the context of standard electrode potentials, a lower positive value reveals a weaker ability to accept electrons compared to those with higher values. Thus, an oxidizing agent with the lowest positive electrode potential demonstrates a weaker oxidizing capability because it is less favorable for it to undergo reduction compared to other species with higher potentials. As a result, it will not effectively drive oxidation reactions forward when compared to stronger oxidizing agents.

Therefore, identifying the lowest positive electrode potential directly correlates with finding the weakest oxidizing agent among a given set.