Question

Write ground-state electron configurations for the ions Mg⁺, Na⁺, F^-and Zn²⁺. Which do you expect will be paramagnetic due to the presence of unpaired electrons?
(Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s² 2s¹ or in condensed form as [He]2s¹.)

ion	electron configuration	paramagnetic
Mg+		_____yes no
Na+		_____yes no
F-		_____yes no
Zn2+		_____yes no

Answer 1

The metal ions which have one or more unpaired electrons are paramagnetic. Except Mg+, all ions viz., Na+, F-, Zn2+ it is not paramagnetic has full sub shell and are nor paramagnetic.

Electronic configuration of Mg+ is 1s2 2s2 2p6 3s1, it is thus paramagnetic

Electronic configuration of Na+ is 1s2 2s2 2p6, it is not paramagnetic

Electronic configuration of F- is also 1s2 2s2 2p6 and it is not paramagnetic

Electronic configuration of Zn2+ is 1s2 2s2 2p6 3s2 3p6 3d10, it is not paramagnetic