Alkaline earth metals are found in Group 2 of the periodic table, and they include elements like beryllium, magnesium, calcium, strontium, barium, and radium. The ionization process for alkaline earth metals typically involves the loss of two electrons from their outermost energy level.
As a result, alkaline earth metal ions carry a charge of +2. This is because when these elements lose two electrons to achieve a stable electronic configuration, they are left with two more protons than electrons, resulting in a net positive charge.
For example:
- Magnesium (Mg) loses two electrons to form Mg2+.
- Calcium (Ca) loses two electrons to form Ca2+.
This +2 charge helps explain why alkaline earth metals tend to form ionic compounds, as they readily bond with nonmetals that can accept those two electrons, forming stable ionic configurations.