question_answer

An element 'M' with electronic configuration (2, 8, 2) combines separately with \[{{(N{{O}_{3}})}^{-}},\,{{(S{{O}_{4}})}^{2-}}\] and \[{{(P{{O}_{4}})}^{3-}}\] 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.

Answer:

(i) (a) \[M{{(N{{O}_{3}})}_{2}},\] (b) \[MS{{O}_{4}},\] (c) \[{{M}_{3}}{{(P{{O}_{4}})}_{2}}\].

(ii) M belongs to second group.

(iii) M will form ionic bond as it losses electrons.