Which of the following has the highest first | vedclass

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(C) The electronic configurations of the given elements are: $B (Z=5): 1s^2 2s^2 2p^1$ $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1

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Nitrogen

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(C) The electronic configurations of the given elements are: $B (Z=5): 1s^2 2s^2 2p^1$ $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ Generally,ionization energy increases across a period from left to right. However,$N$ has a stable half-filled $p$-orbital $(2p^3)$,which requires more energy to remove an electron compared to $O$ $(2p^4)$. Therefore,$N$ has a higher first ionization energy than $O$,$C$,and $B$.

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

Which of the following has the highest first ionization energy?

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

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

$A$ $899, 1757, 14847$

$B$ $737, 1450, 7731$

Which of the following statements is correct?

Which of the following atoms has the highest first ionization energy?

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