Compare two electrons with quantum number sets (4, 2, 1, +½) and (4, 1, 1, +½). be specific about each in terms of location and properties, based on their four quantum numbers.

1) The set of quantum numbers (4, 2, 1, +1/2) represent this:

a) first quantum number, 4: is the the main quantum number, it represents the main energy level, if it were the last electron of the atom, that means that the electron belonged to an element in the row number 4 of the periodic table, that is one element between the atomic numbers 19 and 36.

b:second quantum number, 2; is the sub-level of energy, it indicates the kinf (shepe) of orbital, the number 2 means that the orbital is type d.

c. third quantum number, 1: it represents the orientation of the orbital in the space.

d. fourth quantum number, +1/2: it is the spin quantum number, given that two electrons in an atom cannot have the same set of four quantum numbers  and two electrons can share the same orbital, when one electron has spin +1/2 the other electron in the same orbital has opposite spin (- 1/2).

2) Set of quantum numbers (4, 1, 1, +1/2).

This electron is in the same main energy level than the previous one (4), but it is in a p orbital (second quantum number = 1), instead of a d orbital, and the orientation is px (third quantum number = 1). The spin is +1/2 the same as the other electron.