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(A) The electronic configuration of $N$ $(Z=7)$ is $1s^2 2s^2 2p^3$,which has a stable half-filled $p$-orbital.The electronic configuration of $O$ $(Z

Vedclass · Accepted Answer

Both $A$ and $R$ are correct and $R$ is the correct explanation of $A$.

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(A) The electronic configuration of $N$ $(Z=7)$ is $1s^2 2s^2 2p^3$,which has a stable half-filled $p$-orbital.The electronic configuration of $O$ $(Z=8)$ is $1s^2 2s^2 2p^4$.Due to the half-filled stability of the $2p$ subshell in nitrogen,it requires more energy to remove an electron compared to oxygen.In oxygen,the $2p^4$ configuration means that two electrons must occupy the same $2p$ orbital,leading to increased inter-electronic repulsion,which makes it easier to remove an electron.Thus,both Assertion $A$ and Reason $R$ are correct,and $R$ is the correct explanation for $A$.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

Similar Questions

Which of the following has maximum first ionisation energy?

Which of the following orders for ionization energy is correct?

Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

Of the following isoelectronic ions,the one which has the lowest ionisation potential is

Amongst the following elements with their electronic configurations given below,which one has the highest ionization energy?

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