The orbital angular momentum for a $d$-electron is

If the nitrogen atom had electronic configuration $1s^7$,it would have energy lower than that of the normal ground state configuration $1s^2, 2s^2, 2p^3$ because the electrons would be closer to the nucleus. Yet,$1s^7$ is not observed because it violates:

What is the maximum number of electrons that can be accommodated in a shell with principal quantum number $n = 4$?

$2p$ orbitals have

Match the column:

Column-$I$	Column-$II$
$A$. The orbital which has two angular nodes	$P$. $4d_{x^2-y^2}$
$B$. The $d$ orbital with zero nodal plane	$Q$. $3d_{z^2}$
$C$. The orbital with two radial nodes	$R$. $4f$
$D$. The orbital with three angular nodes	$S$. $3s$

Correct match will be $:-$

If the value of azimuthal quantum number is $3$,the possible values of magnetic quantum number would be