The total number of electrons that can be accommodated in all the orbitals having principal quantum number $n = 2$ and azimuthal quantum number $l = 1$ is

For principal quantum number $n = 4$,the total number of orbitals having $l = 3$ is:

If the $n^{th}$ specific period of the periodic table contains $\frac{(n+2)^2}{2}$ elements,then the maximum value of the azimuthal quantum number associated with that period is:

What is the difference between $2p_x, 2p_y,$ and $2p_z$ orbitals?

Identify the element if its expected electronic configuration is $[Ar] 3d^{10} 4s^{2}$.

If the magnetic quantum number of a given orbital is represented by $-3$,then what will be the minimum possible value of its principal quantum number $(n)$?