What is the common oxidation state of Group 2 metals in compounds?

What is the common oxidation state of Group 2 metals in compounds?

• A. +1
• B. 0
• C. +2
• D. -2

Answer: (C)

Group 2 metals tend to form ions by losing both of their outer electrons, giving a 2+ charge. Their outer electron configuration is ns2, and shedding those two electrons leads to a stable noble-gas configuration. That’s why, in compounds, the common oxidation state is +2. For example, Mg2+ in MgCl2 and Ca2+ in CaCO3 illustrate this pattern. Losing just one electron would give a less stable 1+ state, staying neutral would be elemental metal, and gaining electrons to become -2 is not typical for these metals, which are inclined to form cations instead.

Group 2 metals tend to form ions by losing both of their outer electrons, giving a 2+ charge. Their outer electron configuration is ns2, and shedding those two electrons leads to a stable noble-gas configuration. That’s why, in compounds, the common oxidation state is +2. For example, Mg2+ in MgCl2 and Ca2+ in CaCO3 illustrate this pattern. Losing just one electron would give a less stable 1+ state, staying neutral would be elemental metal, and gaining electrons to become -2 is not typical for these metals, which are inclined to form cations instead.