Arrange N, S, O and F in order of decreasing electron gain enthalpy.
Arrange N, S, O and F in order of decreasing electron gain enthalpy.
$\mathrm{F}>\mathrm{S}>\mathrm{O}>\mathrm{N}$
$\mathrm{N}>\mathrm{O}>\mathrm{S}>\mathrm{F}$
$\mathrm{O}>\mathrm{S}>\mathrm{F}>\mathrm{N}$
$\mathrm{S}>\mathrm{O}>\mathrm{N}>\mathrm{F}$
Solution
Electron gain enthalpy increases with decrease in atomic size. On moving from left to right in the periodic table, the atomic size decreases and electron gain enthalpy increase for fluorine.
In case of oxygen, due to its small size and compact nature, the incoming electron is not accomodated with ease resulting into low electron gain enthalpy than sulphur. So the correct order of electron gain enthalpy is $\mathrm{F}>\mathrm{S}>\mathrm{O}>\mathrm{N}$.