(a) How would the tendency to lose electrons change as you go (i) from left to right across a period? (ii) down a group?
(b) An element X (2,8, 2) combines separately with `(NO_3)^- , (SO_4)^(2-)` and `(PO_4)^(3-)` radicals. Write the formulae of the three compounds so formed. To which group of the periodic table does the element ‘X' belong? Will it form covalent or ionic compound? Why?

Explanation

(a) (i) Tendency to lose electrons decreases. (ii) Increases.
(b) The three compounds are `X(NO_3)_2, XSO_4` and `X_3(PO_4)_2`
Valence electrons of element X is 2. Therefore, element X belongs to group 2. It will form ionic compounds because X loses 2 electrons to achieve the electronic configuration of inert gas and forms a positively charged ion.