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(B) The electron gain enthalpy (with negative sign) represents the energy released when an electron is added to a neutral gaseous atom.Generally,elect

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$O < S < F < Cl$

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(B) The electron gain enthalpy (with negative sign) represents the energy released when an electron is added to a neutral gaseous atom.Generally,electron gain enthalpy becomes more negative across a period.However,for halogens,the electron gain enthalpy of $F$ is less negative than that of $Cl$ due to the small size of the $F$ atom,which leads to strong inter-electronic repulsions.Similarly,for oxygen and sulfur,the electron gain enthalpy of $O$ is less negative than that of $S$ due to the small size of the $O$ atom.The values are: $Cl$ $(349 \ kJ/mol)$,$F$ $(333 \ kJ/mol)$,$S$ $(200 \ kJ/mol)$,and $O$ $(142 \ kJ/mol)$.Thus,the correct order of increasing electron gain enthalpy (magnitude) is $O < S < F < Cl$.

Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species?

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