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 :

Similar Questions

Consider the following conversions:
$(i) \ O_{(g)} + e^- \to O^{-}_{(g)} ; \Delta H_1$
$(ii) \ F_{(g)} + e^- \to F^{-}_{(g)} ; \Delta H_2$
$(iii) \ Cl_{(g)} + e^- \to Cl^{-}_{(g)} ; \Delta H_3$
$(iv) \ Na_{(g)} \to Na^{+}_{(g)} + e^- ; \Delta H_4$
Which of the following statements is incorrect?

Which of the following represents the correct order of electron gain enthalpy (electron affinity) for halogens?

Select the process in which the least enthalpy change is associated:

Explain the trends in electron gain enthalpy across periods and down groups.

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