For electron gain enthalpies of the elements denoted as ${\mathrm{\Delta }}_{\mathrm{eg}}\mathrm{H}$, the incorrect option is: 

In 16^th group elements, when an electron is added to an isolated gaseous sulphur atom more heat is liberated. So sulphur has lowest electron gain enthalpy than remaining elements in the group.
$\begin{array}{l}{\mathrm{\Delta H}}_{\mathrm{eg}}\left(\mathrm{S}\right)=-200{\mathrm{kJ}.\mathrm{mol}}^{-1}\\ {\mathrm{\Delta H}}_{\mathrm{eg}}\left(\mathrm{Se}\right)=-195{\mathrm{kJ}.\mathrm{mol}}^{-1}\end{array}$