Which of the following statements is correct?

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(B) The second electron affinity is always endothermic (positive) because an electron is added to a negatively charged ion,leading to inter-electronic

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The magnitude of the second electron affinity of sulphur is less than that of oxygen

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(B) The second electron affinity is always endothermic (positive) because an electron is added to a negatively charged ion,leading to inter-electronic repulsion. For oxygen $(O^-)$,the electron is added to a smaller $2p$ orbital,resulting in higher repulsion compared to sulphur $(S^-)$ where the electron is added to a larger $3p$ orbital. Therefore,the magnitude of the second electron affinity of sulphur is less than that of oxygen. Additionally,the first electron affinity of chlorine is greater than that of fluorine due to the small size and high inter-electronic repulsion in the $2p$ subshell of fluorine. The correct order is $Cl > F > Br > I$.

Column-$I$ Electronic Configuration	Column-$II$ Electron Gain Enthalpy / $kJ \ mol^{-1}$
$(A) \ 1s^2 2s^2 2p^6$	$(1) -53$
$(B) \ 1s^2 2s^2 2p^6 3s^1$	$(2) -328$
$(C) \ 1s^2 2s^2 2p^5$	$(3) -141$
$(D) \ 1s^2 2s^2 2p^4$	$(4) +53$

Similar Questions

Which one of the elements has the maximum electron affinity?

The formation of the $O^{2-}$ ion is first exothermic and then endothermic,as shown by the following reaction steps:
$O_{(g)} + e^- \to O^-_{(g)}; \Delta H^o = -142 \ kJ \ mol^{-1}$
$O^-_{(g)} + e^- \to O^{2-}_{(g)}; \Delta H^o = 844 \ kJ \ mol^{-1}$
This is due to:

Identify the set of elements in which they are arranged in the increasing order of electron gain enthalpies.

Explain the periodicity of electron gain enthalpy of elements in the periodic table.

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