Standard reduction potentials of the half reactions are given below: F_(2)(g)+2e^(-)to2F^(-)(aq),E^(@)=+2.85V Cl_(2)(g)+2e^(-)to2Cl^(-)(aq),E^(@)=+1.36V Br_(2)(s)+2e^(-)to2Br^(-)(aq),E^(@)=+1.06V I_(2)(s)+2e^(-)to2I^(-)(aq),E^(@)=+0.53V The strongest oxidizing and reducing agents respectively are:

Standard reduction potentials of the half reactions are given below:

1.	Standard reduction potentials of the half reactions are given below: F_(2)(g)+2e^(-)to2F^(-)(aq),E^(@)=+2.85V Cl_(2)(g)+2e^(-)to2Cl^(-)(aq),E^(@)=+1.36V Br_(2)(s)+2e^(-)to2Br^(-)(aq),E^(@)=+1.06V I_(2)(s)+2e^(-)to2I^(-)(aq),E^(@)=+0.53V The strongest oxidizing and reducing agents respectively are:
Answer» `Cl_(2) and Br^(-)` `Cl_(2) and I_(2)` `F_(2) and I^(-)` `Br_(2) and Cl^(-)` Solution :Higher the reduction potential, more easily it is reduced and hence STRONGER is the oxidizing agent. `F_(2)` has highest reduction potential. Hence, `F_(2)` is strongest oxidizing agent. CONSIDERING the reverse reaction (oxidation reaction), higher the oxidation potential, more easily it is oxidized and hence stronger is the REDUCING agent. oxidation potential of `I^(-)` ion `(-0.53V)` is highest out of -2.85,-1.36,,-1.06 and -0.53. hence, `I^(-)` is strongest reducing agent.