Question

The metals of $\mathrm{Group}2$ from top to bottom are $\mathrm{Be},\mathrm{Mg},\mathrm{Ca},\mathrm{Sr}\mathrm{and}\mathrm{Ba}.$

(1) Which one of these elements will form ions most readily and why?

(2) State the common feature in the electronic configuration of all these elements.

Answer 1

(1) Barium is one of these elements which will form ions most readily; Due to the lowest ionization energy.

(2) All these elements belong to $\mathrm{Group}2$ and all of the atoms in the group have $2$ valence electrons and valency is also $2$. Therefore, their general electronic configuration is [Noble gas] ns² where n = 2 to 7.