Quantum Numbers

Consider the following sets of quantum numbers :

which of the following sets of quantum number is not possible ?

The orientation of an atomic orbital is governed by

The number of orbitals possible for the following quantum numbers is/are

$\mathrm{n}=3,\hspace{0.17em}\hspace{0.17em}\mathrm{l}=2, \mathrm{m}=+2$

The orbital angular momentum of a $\mathrm{p}-$electron is given as:

The allowed set of quantum numbers for an electron in a hydrogen atom is

To which orbital among the following may an electron having zero angular momentum belong? 

What is the correct set of four quantum numbers for the valence electrons of rubidium atom $\left(\mathrm{Z} = 37\right)$?

The sub-shell that comes after the $\mathrm{f}$ sub-shell is called the $\mathrm{g}$ sub-shell. What is true for the $\mathrm{g}$ sub-shell?

On which orbital angular momentum of an electron is independent?

Maximum number of electrons that can be accommodated in the subshell with azimuthal quantum number $\mathrm{l}=4$, is:

For a one-electron atom, the set of allowed quantum numbers is:

What is the maximum number of orbitals having $\mathrm{n}=5$ and $\mathrm{l}=3$?

The correct set of four quantum numbers for the valence electron of rubidium ($\mathrm{Z}=37$) is

Which set of quantum numbers is not possible?

What is the maximum number of orbitals that can be identified with the following quantum numbers? $\mathrm{n}=3; \mathrm{l}=\mathrm{l}; {\mathrm{m}}_{\mathrm{l}}=0;$

For Principal quantum number $\mathrm{n}=4$, the total number of orbitals having $\mathrm{l}=3$ is

Maximum number of electrons in a subshell of an atom is determined by the following

Principal, Azimuthal and magnetic quantum numbers are respectively related to

The principle quantum number describes