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Among the following which is the strongest oxidizing agent?
A
$Cl_2$
B
$F_2$
C
$Br_2$
D
$I_2$
Detailed Solution
An oxidising agent accepts electrons; the higher its standard reduction potential, the stronger it is.
$E^\circ(X_2/X^-)$: $F_2$ = +2.87 V, $Cl_2$ = +1.36 V, $Br_2$ = +1.09 V, $I_2$ = +0.54 V
Fluorine has the highest value because of its low F–F bond dissociation enthalpy and the very high hydration enthalpy of the small $F^-$ ion, even though its electron gain enthalpy is less negative than that of chlorine.
Oxidising power: $F_2 > Cl_2 > Br_2 > I_2$
Hence the strongest oxidising agent is $F_2$.
$E^\circ(X_2/X^-)$: $F_2$ = +2.87 V, $Cl_2$ = +1.36 V, $Br_2$ = +1.09 V, $I_2$ = +0.54 V
Fluorine has the highest value because of its low F–F bond dissociation enthalpy and the very high hydration enthalpy of the small $F^-$ ion, even though its electron gain enthalpy is less negative than that of chlorine.
Oxidising power: $F_2 > Cl_2 > Br_2 > I_2$
Hence the strongest oxidising agent is $F_2$.