The incorrect set of quantum numbers $(n, l, m, s)$ for an electron in $3p$ orbital is

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?

The set of quantum numbers for the outermost electron for copper $(Cu)$ in its ground state is:

If the nitrogen atom had electronic configuration $1s^7$,it would have energy lower than that of the normal ground state configuration $1s^2, 2s^2, 2p^3$ because the electrons would be closer to the nucleus. Yet,$1s^7$ is not observed because it violates:

The maximum number of sub-levels,orbitals and electrons in $N$ shell of an atom are respectively

Which of the following sets of quantum numbers is possible?