For electron gain enthalpies of the elements | vedclass

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Question

(B) The electron gain enthalpy $(\Delta_{eg} H)$ becomes less negative as we move down a group due to an increase in atomic size.$1$. For $Cl$ and $F$

Vedclass · Accepted Answer

$\Delta_{eg} H (Se) < \Delta_{eg} H (S)$

Vedclass · Answer

(B) The electron gain enthalpy $(\Delta_{eg} H)$ becomes less negative as we move down a group due to an increase in atomic size.$1$. For $Cl$ and $F$: $\Delta_{eg} H (Cl) = -349 \ kJ/mol$ and $\Delta_{eg} H (F) = -328 \ kJ/mol$. Since $-349 $2$. For $Se$ and $S$: $\Delta_{eg} H (Se) = -195 \ kJ/mol$ and $\Delta_{eg} H (S) = -200 \ kJ/mol$. Since $-195 > -200$,the statement $\Delta_{eg} H (Se) $3$. For $I$ and $At$: $\Delta_{eg} H (I) = -295 \ kJ/mol$ and $\Delta_{eg} H (At) = -270 \ kJ/mol$. Since $-295 $4$. For $Te$ and $Po$: $\Delta_{eg} H (Te) = -190 \ kJ/mol$ and $\Delta_{eg} H (Po) = -183 \ kJ/mol$. Since $-190 < -183$,the statement $\Delta_{eg} H (Te) < \Delta_{eg} H (Po)$ is correct.

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

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