Which of the following sets of quantum numbers is impossible for an electron?

Which of the following orbitals has a dumbbell shape?

Select the correct statements for quantum numbers.
$(i)$ Magnetic quantum number $(m_l)$ gives information about the spatial orientation of orbitals with respect to the standard set of coordinate axes.
$(ii)$ Electron spin quantum number is represented by '$s$' and has values of $\pm \frac{1}{2}$.
$(iii)$ Principal quantum number $(n)$ determines the size of the orbitals and also,to a large extent,the energy of the orbitals.

The correct electronic configuration for the ground state of silicon (atomic number $= 14$) is

What is the number of orbitals in the $2p$ and $3p$ subshells? Where are they located?

According to which principle is the electronic configuration of nitrogen $1s^2 2s^2 2p_x^1 2p_y^1 2p_z^1$ and not $1s^2 2s^2 2p_x^2 2p_y^1 2p_z^0$?