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(C) Electron gain enthalpy is the energy released when an electron is added to an isolated gaseous atom. Its value is negative,and the more easily an

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Electron gain enthalpy decreases from fluorine to iodine in the group

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(C) Electron gain enthalpy is the energy released when an electron is added to an isolated gaseous atom. Its value is negative,and the more easily an atom accepts an electron,the more negative its electron gain enthalpy becomes (i.e.,its magnitude increases).With an increase in nuclear charge,the electron gain enthalpy generally increases.Due to the extra stability of nitrogen (it has a half-filled valence shell $[He] \, 2s^2 \, 2p^3$),it is very difficult to add an electron to it,resulting in an almost zero electron gain enthalpy.In general,on moving down a group,electron gain enthalpy decreases due to an increase in atomic size. However,from $F$ to $Cl$,the electron gain enthalpy increases.Due to the very small size of the $F$ atom and the absence of a $3^{rd}$ shell,the incoming electron experiences inter-electronic repulsion,making the electron gain enthalpy of $F$ less negative than that of $Cl$. Thus,$Cl$ has the highest electron gain enthalpy in the periodic table. Therefore,the statement that electron gain enthalpy decreases from fluorine to iodine is incorrect,as it increases from $F$ to $Cl$ and then decreases.

Which one of the following statements is incorrect?

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