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

An electronic transition from $1s$ orbital of an atom causes

Describe the orbitals with the following quantum numbers using $s, p, d, f$ notation:
$(a) n = 1, l = 0$
$(b) n = 3, l = 1$
$(c) n = 4, l = 2$
$(d) n = 4, l = 3$

The magnetic quantum number for the valence electron of sodium is

Identify the element from the following having six unpaired electrons in its observed electronic configuration.

Although no currently known element contains electrons in $g$ orbitals in the ground state,it is possible that such an element will be found or that electrons in excited states of known elements could be in $g$ orbitals. For $g$ orbitals,$l = 4$. What is the lowest value of $n$ for which $g$ orbitals could exist? What are the possible values of $m_l$? How many electrons could a set of $g$ orbitals hold?