Match the $LIST$-$I$ with $LIST$-$II$:

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

Identify the incorrect statement from the following.

The principal quantum number represents:

Given below are two statements:
Statement $I$ : For a given shell,the total number of allowed orbitals is given by $n^2$.
Statement $II$ : For any subshell,the spatial orientation of the orbitals is given by $-l$ to $+l$ values including zero.
In the light of the above statements,choose the correct answer from the options given below:

Consider the following statements:
$(A)$ The principal quantum number $'n'$ is a positive integer with values of $'n'=1, 2, 3, \dots$.
$(B)$ The azimuthal quantum number $'l'$ for a given $'n'$ (principal quantum number) can have values as $'l'=0, 1, 2, \dots, (n-1)$.
$(C)$ Magnetic orbital quantum number $'m_l'$ for a particular $'l'$ (azimuthal quantum number) has $(2l+1)$ values.
$(D)$ $\pm 1/2$ are the two possible orientations of electron spin.
$(E)$ For $l=5$,there will be a total of $11$ orbitals.
Which of the above statements are correct?

The two electrons $X$ and $Y$ have the following sets of quantum numbers:

$X: n=3, l=2, m=-2, s=+1/2$

$Y: n=3, l=0, m=0, s=+1/2$

Which of the following is the correct statement?