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  4. Which of the following arrangements represents the correct order of electron gain enthalpy?

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Q. Which of the following arrangements represents the correct order of electron gain enthalpy?

Classification of Elements and Periodicity in Properties

Solution:

In chlorine and fluorine. $Cl$ has high electron gain enthalpy because the small size of $F$ and there is very high electronic repulsion among the electrons of fluorine. This makes incoming of another electron not very favourable. In sulphur and oxygen, sulphur has high electron gain enthalpy than oxygen because of larger size and lower electron density.
So, $O < S < F < Cl$
The $Cl$ has a most negative electron gain enthalpy and $O$ has a least negative electron gain enthalpy.
By considering the negative sign, the more negative value will be small and less negative value will be large.
Thus, the correct order will be $Cl < F < S < O$