The last electron in a bivalent negatively charge ion is described by the following quantum numbers: n=3, l=0, m=0, s=+½

Question

1 Write the orbital configuration of the ionic species

2 write the shell configuration of the natural atom

3 Give the name and symbol of the atom

4 what group of the periodic table does it belong to?

Answer 1

There are a couple of things wrong with this problem. 1) A normal negatively charged ion will not end with a configuration that is 3s² or 3s¹.( l = 0 means s, m is forced to be 0, and 3 is the principal quantum number) 2) The spin is arbitrary, so, unless your class has the convention that the electrons fill from - to + spins, the question is ambiguous.

The answer will be F^2- or Ne^2- depending on the convention.

To get a bivalent positive ion that ends in s², you'd have to go to Ti. Anyway, I hope this wasn't quite the question...