g Write the set of four quantum numbers (n, l, ml, and ms) for each of the electrons in a nitrogen (N) atom in the ground state. (Select all that apply.) 1s orbital: (0, 1, 1, +1/2) (1, 0, 0, −1/2) (1, 0, 1, +1/2) (1, 0, −1, −1/2) (1, 1, 0, −1/2) (1, 0, 0, +1/2) (0, 1, 0, −1/2) 2s orbital: (2, 0, 0, −1/2) (2, 0, −1, −1/2) (0, 2, 2, +1/2) (2, 0, 1, +1/2) (2, 1, 0, −1/2) (2, 0, 0, +1/2) (1, 2, 0, −1/2) 2px, 2py, 2pz orbitals: (1, 0, 2, +1/2) (2, −1, 0, −1/2) (2, 1, −1, +1/2) (2, 1, 0, +1/2) (2, 1, 1, +1/2) (2, 1, 2, −1/2) (2, 2, 1, −1/2) How are these sets of quantum numbers in accordance with the Pauli exclusion principle and Hund's rule? If one electron in a particular orbital has ms = +1/2, a second electron in the same orbital will have ms = −1/2 since ---Select--- in an atom can have exactly the same set of four quantum numbers according to the Pauli exclusion principle. In accordance with Hund's rule, the 2px, 2py, and 2pz orbitals need to receive one electron each, so that there will be the ---Select--- number of unpaired electrons. These three electrons should have the same value of ms in order to have parallel spins. If there are more electrons available, the orbitals can then receive the additional electrons.