Write about the magnetic quantum number $(m_{l})$.

(N/A) The magnetic orbital quantum number,denoted as $m_{l}$,provides information about the spatial orientation of an orbital with respect to a standard set of coordinate axes.
Value of $m_{l}$: For any subshell defined by the azimuthal quantum number '$l$',there are $2l+1$ possible values of $m_{l}$,ranging from $-l$ to $+l$ including zero:
$m_{l} = -l, -(l-1), \ldots, 0, \ldots, +(l-1), +l$
Relation between $l$ and the number of orbitals:
$1$. For $l = 0$ ($s$-orbital): $m_{l} = 0$. Total values = $2(0)+1 = 1$. This indicates a single $s$-orbital.
$2$. For $l = 1$ ($p$-orbital): $m_{l} = -1, 0, +1$. Total values = $2(1)+1 = 3$. These correspond to $p_{x}, p_{y},$ and $p_{z}$ orbitals.
$3$. For $l = 2$ ($d$-orbital): $m_{l} = -2, -1, 0, +1, +2$. Total values = $2(2)+1 = 5$. These correspond to five $d$-orbitals.
$4$. For $l = 3$ ($f$-orbital): $m_{l} = -3, -2, -1, 0, +1, +2, +3$. Total values = $2(3)+1 = 7$. These correspond to seven $f$-orbitals.
Each orbital is defined by a set of values for $n, l,$ and $m_{l}$. The following table summarizes the relationship between the subshell and the number of orbitals:

Value for $l$	$0, 1, 2, 3, 4, 5$
Notation for subshell	$s, p, d, f, g, h$
Number of orbitals	$1, 3, 5, 7, 9, 11$