An electron has principal quantum number $n = 3$. The number of its $(i)$ sub-shells and $(ii)$ orbitals would be respectively:

For a magnetic quantum number $m = 0, \pm 1$,the value of the principal orbital (azimuthal quantum number $l$) corresponds to which subshell,and what is the minimum principal quantum number $n$ required for this set?

The wave function $(\Psi)$ of $2s$ is given by
$\Psi_{2s} = \frac{1}{2\sqrt{2\pi}} \left(\frac{1}{a_0}\right)^{3/2} \left(2 - \frac{r}{a_0}\right) e^{-r/2a_0}$
At $r = r_0$,a radial node is formed. Thus,$r_0$ in terms of $a_0$ is:

The number of angular and radial nodes in $3p$ orbital respectively are

The atomic number of an element is $35$. What is the total number of electrons present in all the $p-$ orbitals of the ground state atom of that element?

The graph showing the variation of probability density,$\psi^2(r)$ with the distance of the electron from the nucleus,$r$ is given below. This represents: