For electron gain enthalpies of the elements denoted as ΔegH, the incorrect option is:

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For electron gain enthalpies of the elements denoted as $Δ_{eg} H$ , the incorrect option is:

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$Δ_{eg} H (I) < Δ_{eg} H (At)$

$Δ_{eg} H (Cl) < Δ_{eg} H (F)$

$Δ_{eg} H (Se) < Δ_{eg} H (S)$

$Δ_{eg} H (Te) < Δ_{eg} H (Po)$

answer is A.

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Detailed Solution

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.
$\begin{array}{l} {ΔH}_{eg} (S) = - 200 {kJ . mol}^{- 1} \\ {ΔH}_{eg} (Se) = - 195 {kJ . mol}^{- 1} \end{array}$