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An element X (2, 8, 2) combines separately with $$NO_3$$ and $$(SO_4)_2$$, $$(PO_4)_3$$ radicals. Write the formulae of the three compounds so formed. To which group of the periodic tables does the element 'X' belong? Will it form covalent or ionic compound? Why?


Solution

X(2,8,2) - This element is Magnesium. It belongs to group 2 of the periodic table.
$$Mg^{2+}+NO_{3}^{-} \rightarrow Mg(NO_{3})_{2}$$[Magnesium Nitrate]
$$Mg^{2+}+(SO_{4})^{2-} \rightarrow Mg(SO_{4})$$[Magnesium Sulphate]
$$Mg^{2+}+(PO_{4})^{3-} \rightarrow Mg_{3}(PO_{4})_{2}$$[Magnesium Sulphate]
Element X which is Magnesium will form ionic compounds by losing 2 electrons from its valence shell.

Chemistry

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