Standard reduction potentails of the half reactions are given below:
`F_(2)(g)+2e^(-) rarr 2F^(-)(aq.),, E^(ɵ)= +2.87`
`Cl_(2)(g)+2e^(-) rarr 2Cl^(-)(aq.),, E^(ɵ)= +1.36 V`
`Br_(2)(g)+2e^(-) rarr 2Br^(-)(aq.),, E^(ɵ)= +1.09 V`
`I_(2)(s)+2e^(-) rarr 2l^(-)(aq.),, E^(ɵ)= +0.54 V`
The strongest oxidizing and reducing agents respectively are:

Options

A. `Cl_(2)` and `Br^(-)`
B. `Cl_(2)` and `I_(2)`
C. `F_(2)` and `I^(-)`
D. `Br_(2)` and `Cl^(-)`

Answer

C

Explanation

Higher the reduction potential more easily it is reduced and hence stronger is the oxidising agent. `F_(2)` has highest reduction potential. `therefore F_(2)` is the strongest oxidising agent. Considering the reverse reaction (oxidiation reactions). higher the oxidiation potential more easily it is oxidised and hence stronger is the reducing agent.
Oxidation potential `1(-0.53V)` is highest out of 2.85,-1.36,-1.36 and 0. 53, Hence I is the strongest reducing agent.