In which of the following pairs does the mole | vedclass

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(D) The first ionization energy $(IE_1)$ of a molecule is generally higher than that of its constituent atom because the electrons in a molecule are h

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(D) The first ionization energy $(IE_1)$ of a molecule is generally higher than that of its constituent atom because the electrons in a molecule are held more strongly due to the formation of stable covalent bonds and the increased effective nuclear charge experienced by the bonding electrons.For $F_2$,$O_2$,and $N_2$,the bond dissociation energy and the stability of the molecular orbitals result in a higher energy requirement to remove an electron compared to the isolated atoms ($F$,$O$,and $N$ respectively).Therefore,for all the given pairs,the molecule has a higher $IE_1$ value than its corresponding atom.

Element	Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$
$A$	$899, 1757, 14847$
$B$	$737, 1450, 7731$

In which of the following pairs does the molecule have a higher $IE_1$ value compared to its corresponding atom?

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Consider the following ionization enthalpies of two elements $A$ and $B$.

Element Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$

$A$ $899, 1757, 14847$

$B$ $737, 1450, 7731$

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