The first ionisation energy of oxygen is less | vedclass

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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the co

Vedclass · Accepted Answer

Greater inter-electron repulsion between two electrons in the same $p$-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen

Vedclass · Answer

(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the configuration $1s^2 2s^2 2p^4$.Although oxygen has a higher effective nuclear charge than nitrogen,the $2p^4$ configuration of oxygen experiences greater inter-electron repulsion between two electrons in the same $p$-orbital.This repulsion makes it easier to remove an electron from oxygen compared to the stable half-filled configuration of nitrogen,thus resulting in a lower first ionisation energy for oxygen.

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 first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?

Similar Questions

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

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

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

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

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

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

Identify the element having the highest ionization enthalpy.

In which of the following electronic configurations of an element is there a very large difference between the second and third ionization energy?

Which element having the following electronic configurations has the minimum ionization potential?

$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)

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