After filling the $4d$ orbitals,an electron will enter in:

The total number of magnetic quantum numbers for a $d$-orbital is given by

Five valence electrons of $P^{15}$ are labelled as $\boxed{AB}_{3s} \,\boxed{X|Y|Z}_{3p}$. If the spin quantum numbers of $B$ and $Z$ are $+\frac{1}{2}$,the group of electrons with three of the quantum numbers $(n, l, m)$ the same are:

Which of the following does not have valence electrons in the $3d-$subshell?

The number of electrons with $(n+\ell)$ values equal to $3, 4$ and $5$ in an element with atomic number $(Z) = 24$ are respectively $(n =$ principal quantum number and $\ell =$ azimuthal quantum number).

Calculate the total number of angular nodes and radial nodes present in $3p$ orbital.