Q.1. An element X (2,8,2) combines separately with NO3 and (SO4)2 -, (PO4)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?
Q.2. Two elements X and Y have atomic numbers 12 and 16 respectively. Write the
electronic configuration for these elements. To which period of the modern periodic
table do these two elements belong? What type of bond will be formed between
them and why?

a) On adding the number of electron of X, it is 12 which indicate Magnesium. It combine with NO3¯ and SO42¯to form Mg(NO3)2 and Mg(SO4). Magnesium belongs to 2nd group which forms ionic compound due to its metallic character.

b)  12X = 2 8 2   ;  16Y = 2 8 6

  X = Magnesium = 2nd group and 3 period

   Y = Sulphur = 6th-A group and 3 period

  The bond formed will be ionic in nature because magnesium is metallic and sulphur is non-metallic.

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Ans 1 - Magnesium is the compound. It belongs to the 2nd group of the periodic table. The compond it forms with the radicals are - MgSO4 and Mg3(PO4)2.With NO3 , it shall form Mg(NO3)2.All the bonds formed are ionic bonds because MgSO4,Mg3(PO4 )  and Mg(NO3)2 is an ionic compound since magnesium is a metal, and SO4 is considered a non-metal. Covalent compounds occur between two non-metals.


Ans 2 - Compound A is Magnesium and compound B is Sulphur.Magnesium is present in group 2 whereas Sulphur is present in group 16 in the modern periodic table.

Electronic Config. of Mg - 2,8,2  and that of Sulphur is 2,8,6. They shall form an ionic bond.

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Thanks Ansh !

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