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

Explanation

(i) 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.
(ii) The chemical formula of the compounds are : `M(NO_(3))_(2)//Mg(NO_(3))_(2),MSO_(4)//MgSO_(4),M_(3)(PO_(4))_(2)//Mg_(3)(PO_(4))_(2)`.
(iii) .M. will form ionic compounds by losing two electrons.