What happens when Group 2A elements form ions?

Hint: Modern periodic table consists of 18 vertical columns known as groups arranged as left to right and seven horizontal rows known as periods arranged from top to bottom. In this periodic table elements are arranged according to their increasing atomic number.

Complete answer:
Group 1,2,13-17 are known as main group elements in which the last electron will enter in s or p subshell, group 3-12 are known by the name transition elements and also called d-group elements and group 18 is of inert gases or noble gases i.e. those elements which have fully filled outermost atomic shell and have high stability. Rather than this there are two rows below the table known as inner transition elements in which the last electron will enter into the f-subshell.
Group 2 elements are alkaline earth metals in which beryllium, magnesium, calcium, strontium, barium and radium are present when group 2 elements form ions they will lose 2 electrons. As we know that neutral atoms become ions by losing or gaining electrons. The number of valence electrons an atom has will determine whether it will lose electrons to become a positively charged ion known by the name cation or gains electrons to become a negatively charged ion known by the name anion.
 In this case elements located in group 2 will always lose electrons to become cations. Basically they will lose 2 electrons to form cations with charge of +2.
Hence Group 2A elements form ions by losing two electrons.

Note:
Beryllium which is located in group 2 and period 1 lose 2 electrons which allows it to have a stable configuration and for the other elements it will also lose 2 electrons which also allows them to have a stable octet configuration.