The acidic strength of $$\mathrm{HX}(\mathrm{X}=\mathrm{F}, \mathrm{Cl}, \mathrm{Br}$$ and $\mathrm{I})$ follows the order: $$\mathrm{HF}>\mathrm{HCl}>\mathrm{HBr}>\mathrm{HI}$$.

Fluorine exhibits $-$1 oxidation state whereas other halogens exhibit $+1,+3,+5$ and $+7$ oxidation states also.

The enthalpy of dissociation of $\mathrm{F}_2$ is smaller than that of $\mathrm{Cl}_2$.

Fluorine is stronger oxidising agent than chlorine.