a
\(F _2\) is the strongest oxidizing agent in the whole periodic table. The order of oxidizing power depends on the reduction potential, which depends on factors like Hydration enthalpy, enthalpy of atomization, and electron affinity. Combining all these factors and checking with experimental values leads to the well-known order of oxidizing power of halogens:

Here are the standard reduction potentials of all the halogens:

\(F _2 \rightarrow 2.87\)

\(Cl _2 \rightarrow 1.36\)

\(Br _2 \rightarrow 1.07\)

\(I _2 \rightarrow 0.54\)

\(F _2\) has high hydration energy and low bond dissociation energy of all and that is why it is the strongest oxidizing agent of all.