The minimum number of quantum numbers required to specify an orbital in an atom is

An electron having the quantum numbers $n = 4, l = 3, m = 0, s = -\frac{1}{2}$ would be in the orbital

Which of the following sets of quantum numbers is not possible?

Which of the following ions does not have the same electronic configuration as $Ne$?

Which of the following electronic configurations has the least energy?

Which of the following combination of statements is true regarding the interpretation of the atomic orbitals?
$1$. An electron in an orbital of high angular momentum stays further away from the nucleus than an electron in an orbital of lower angular momentum.
$2$. For a given value of the principal quantum number,the size of the orbit is inversely proportional to the azimuthal quantum number.
$3$. According to wave mechanics,the ground state angular momentum is equal to $\frac{h}{2\pi}$.
$4$. The plot of $\Psi$ vs $r$ for various azimuthal quantum numbers shows peak shifting towards higher $r$ values.