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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.For the given e

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$N < P < F < Cl$

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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.For the given elements,the general trend is influenced by atomic size and electron-electron repulsion.$1.$ Among halogens,$Cl$ has a higher (more negative) electron gain enthalpy than $F$ because the small size of $F$ leads to significant inter-electronic repulsion.$2.$ Among group $15$ elements,$P$ has a higher electron gain enthalpy than $N$ due to the larger size and lower electron density of $P$ compared to $N$.$3.$ Comparing the groups,$N$ has the lowest value due to its very small size and high electron density,while $Cl$ has the highest value.Thus,the correct order is $N < P < F < Cl$.

Which of the following represents the correct order of increasing electron gain enthalpy (with negative sign) for the elements?
$a.$ Nitrogen
$b.$ Phosphorus
$c.$ Chlorine
$d.$ Fluorine

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Which of the following represents the correct order of increasing electron gain enthalpy (with negative sign) for the elements?$a.$ Nitrogen$b.$ Phosphorus$c.$ Chlorine$d.$ Fluorine