Despite lower value of its electron gain enthalpy with negative sign, fluorine `(F_(2))` is a stronger oxidising agent than chlorine `(Cl_(2))`. Explain.

(a)Draw the molecule structure of the following compounds : (i) N_(2)O_(5) (ii) XeOF_(4) (b)Despite lower value of its electron gain enthalpy with negative sign, fluorine (F_(2)) is a stronger oxidising agent than Cl_(2) .

(a)Draw the molecule structure of the following compounds : (i) N_(2)O_(5) (ii) XeOF_(4) (b)Despite lower value of its electron gain enthalpy with negative sign, fluorine (F_(2)) is a stronger oxidising agent than Cl_(2) .

(a) Draw the molecular structures of the following compounds : (i) N_(2)O_(5) " " (ii) XeOF_(4) (b) Explain the following observations : (i) Sulphur has a greater tendency for catenation than oxygen. (ii) ICI is more reactive than I_(2) . (iii) Despite lower value of its electron gain enthalpy with negative sign, fluorine (F_(2)) is a stronger oxidizing agent than Cl_(2) .

Explain the following observations : Despite lower value of its electron gain enthalpy with negative sign, fluorine (F_2) is a stronger oxidising agent than Cl_2 .

F_(2) is a stronger oxidising agent than Cl_(2)

F_(2) is a stronger oxidising agent than Cl_(2)

Why is F_2 stronger oxidising agent than Cl_2 ?