An element 'M' with electronic configuration (2,8,2) combines separately with `(NO_(3))^(-),(SO_(4))^(2-) and (PO_(4))^(3-)` radicals. Write the formula of the three compounds so formed . To which group and period of the Modern Periodic Table does the elements 'M' belong ? Will 'M' form covalent or ionic compounds ? Give reason to justify your answer.

Explanation

`*` The electronic configuration (2,8,2) of the element 'M' suggests that it belongs to group 2 and period 3 of the Modern Periodic Table and its valency is 2 .
`*` The chemical formulae of the compounds formed are :
(i) `M(NO_(3))_(2)" "(ii) MSO_(4) " "(iii) M_(3)(PO_(4))_(2)`
`*` 'M' will form ionic compounds by losing two valence electrons to achieve a noble gas configuration , that is , a stable octet in the valence shell.