Why are halogens strong oxidising agents?

Explanation

Due to low bond dissociation enthalpy, high electronegativity and large negative electron gain enthalpy halogens have a strong tendency to accept electrons and thus get reduced.
`X+e^(-)toX’`
As a result, halogens act as strong oxidizing agents. Their oxidizing power, however, decreases from`F_(2)`to`I_(2)` la as is evident from their electrode potentials:
`E_(r_(2)//F)^(0)=+2.87VE_(CI_(2)//CI)=+11.36V`
`E_(Br_(2)//Br^(-))=+1.09 `and `E_(I_(2)//I^(-))=+0.54V`
Thus, `F_(2)` is the strongest while `l_(2)` is the weaker oxidizing agent.