3.1.2 (a) Electron Configurations and Redox

Syllabus

(a) the outer shell s² electron configuration and the loss of these electrons in redox reactions to form 2+ ions

No one will require you to a full electron configuration for a Group 2 element larger than Calcium.

But even the larger atoms have an outer shell with only 2 electrons, both in that shell's s orbital.

As a result, electronic stability is gained by losing both these electrons to leave themselves with a full outer shell.

And a 2+ charge.

All reactions involving Group 2 as elements result in compounds with 2+ metal ions

OILRIG tells us that losing electrons is Oxidation.

So, Group 2 elements are quite good at getting themselves Oxidised.

Which must make them quite good at pushing electrons onto other elements and forcing them to gain and be reduced.

So Group 2 metals make rather good Reducing Agents.

That is all.

Really.