The correct order of ionisation energy of C,N | vedclass

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Question

(B) On moving from left to right in a period,ionisation energy generally increases due to an increase in effective nuclear charge.Thus,the expected or

Vedclass · Accepted Answer

$C < O < N < F$

Vedclass · Answer

(B) On moving from left to right in a period,ionisation energy generally increases due to an increase in effective nuclear charge.Thus,the expected order of ionisation energy for $C$,$N$,$O$,and $F$ is $C However,the ionisation energy of $N$ $(1s^2 2s^2 2p^3)$ is greater than that of $O$ $(1s^2 2s^2 2p^4)$.This is because $N$ has a stable half-filled $p$-orbital configuration,which requires more energy to remove an electron.Therefore,the correct order is $C < O < N < F$.

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$)	List-$II$ (Element)
$A$. $1510$	$1$. $H$
$B$. $495, 6500, 10200$	$2$. $Li$
$C$. $840, 1630, 13100$	$3$. $Be$
$D$. $600, 2050, 3100$	$4$. $B$

The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

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Match List-$I$ with List-$II$ with correct code:

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$) List-$II$ (Element)

$A$. $1510$ $1$. $H$

$B$. $495, 6500, 10200$ $2$. $Li$

$C$. $840, 1630, 13100$ $3$. $Be$

$D$. $600, 2050, 3100$ $4$. $B$

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