Question

From emf series, how to decide good oxidant and good reductant​

Answer 1

Answer:

In the electrochemical series the substances are arranged in the decreasing order of electrode potential i.e. decreasing tendency for reduction to occur or power as oxidising agent. The elements at the top of the table have maximum tendency to get reduced and consequently they will act as good oxidising agents.

Answer 2

Answer:

We can measure the standard potentials for a wide variety of chemical substances, some of which are listed in Table P2. These data allow us to compare the oxidative and reductive strengths of a variety of substances. The half-reaction for the standard hydrogen electrode (SHE) lies more than halfway down the list in Table 1 . All reactants that lie below the SHE in the table are stronger oxidants than H+, and all those that lie above the SHE are weaker. The strongest oxidant in the table is F2, with a standard electrode potential of 2.87 V. This high value is consistent with the high electronegativity of fluorine and tells us that fluorine has a stronger tendency to accept electrons (it is a stronger oxidant) than any other element.