An element M with electronic configuration (2,8, 2) combines separately with `(NO_3)^(-1),(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 element Mbelong? Does M form covalent or ionic compounds? Justify your answer.

Explanation

The element M has electronic configuration (2, 8, 2), it has two valence electrons and a valency of +2.
Hence, it forms compounds `M(NO_3)_(2)^(-), MSO_4`, and `M_3 (PO_4)_2`, with radicals `(NO_3), (SO_4)^(2-) and (PO_4)^(3-)` respectively.
Since M has two valence electrons, it belongs to the 2nd group, and since it has three shells, it belongs to the 3rd period of the periodic table.
M forms ionic compounds since it is a metal.