The probability of finding an electron in the $d_{xy}$ orbital is maximum along:

For an electron with quantum numbers $s = +1/2$ and $m_l = -1$,which of the following orbitals is not possible?

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?

Identify the correct statements among the following:
$i. E_{2s}(H) > E_{2s}(Li) < E_{2s}(Na) > E_{2s}(K)$
$ii.$ The maximum number of electrons in the shell with principal quantum number $n$ is equal to $2n^2$.
$iii.$ Extra stability of half-filled subshell is due to smaller exchange energy.
$iv.$ Only two electrons,irrespective of their spin,may exist in the same orbital.

What is the number of radial and angular nodes in a $5f$ orbital?

Which of the following sets of quantum numbers is correctly matched?