An element 'M' with electronic configuration (2, 8, 2) combines separately with NO3^-, SO4^2- and PO4^3- radicals.
An element 'M' with electronic configuration (2, 8, 2) combines separately with NO3-, SO42- and PO43- 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.
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(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(NO3)2 / Mg(NO3)2;MSO4/MgSO4;M3(PO4)2/Mg3(PO4)2.
(iii) 'M' will form ionic compounds by losing two electrons.
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