Which of the following $p, d, f$ orbitals are not possible? Why?

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

An element has an outermost orbital configuration of $4s^2$. What is its atomic number?

Which of the following orbitals has a dumbbell shape?

How many maximum electrons can be accommodated in a $p$-orbital with $n = 6$ and $m = 0$?

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?