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(C) The $1s$ orbital can accommodate a maximum of $2$ electrons according to Pauli's exclusion principle,which states that no two electrons in an atom

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Pauli's exclusion principle

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(C) The $1s$ orbital can accommodate a maximum of $2$ electrons according to Pauli's exclusion principle,which states that no two electrons in an atom can have the same set of all four quantum numbers. Since an orbital is defined by $n$,$l$,and $m_l$,the only way to distinguish two electrons in the same orbital is by their spin quantum number ($m_s = +1/2$ or $-1/2$). Therefore,a configuration like $1s^7$ is impossible as it attempts to place $7$ electrons in a single orbital.

List-$I$ (Orbital)	List-$II$ (Radial nodes and nodal plane)
$A$. $2s$	$I$. $1$ Radial node + two nodal planes
$B$. $3s$	$II$. $1$ Radial node + one nodal plane
$C$. $3p$	$III$. $2$ Radial nodes + No nodal plane
$D$. $4d$	$IV$. $1$ Radial node + No nodal plane

If the electronic configuration of a nitrogen atom were $1s^7$,its energy would be lower than that of the ground state configuration $1s^2\,2s^2\,2p^3$ due to being closer to the nucleus. However,the $1s^7$ configuration is not observed because it violates which of the following rules?

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