Question
The types of hybrid orbitals of nitrogen in $$NO_2^ + ,NO_3^ - $$ and $$NH_4^ + $$ respectively are expected to be
A.
$$sp,s{p^3}\,{\text{and}}\,s{p^2}$$
B.
$$sp,s{p^2}\,{\text{and}}\,s{p^3}$$
C.
$$s{p^2},sp\,{\text{and}}\,s{p^3}$$
D.
$$s{p^2},s{p^3}\,{\text{and}}\,sp$$
Answer :
$$sp,s{p^2}\,{\text{and}}\,s{p^3}$$
Solution :
$$X = \frac{1}{2}\left( {VE + MA - c + a} \right)$$
where, $$VE =$$ No. of valence electrons on the central atom.
$$MA =$$ No. of monovalent atoms surrounding the central atom.
$$c =$$ Charge on the cation; $$a =$$ Charge on the anion
$${\text{For}}\,NO_2^ + ,X = \frac{1}{2}\left( {5 + 0 - 1} \right) = 2$$ $$\left( {sp\,{\text{hybrid orbitals}}} \right)$$
$${\text{For}}\,NO_3^ - ,X = \frac{1}{2}\left( {5 + 0 + 1} \right) = 3$$ $$\left( {s{p^2}{\text{hybrid orbitals}}} \right)$$
$${\text{For}}\,NH_4^ + ,X = \frac{1}{2}\left( {5 + 4 - 1} \right) = 4$$ $$\left( {s{p^3}\,{\text{hybrid orbitals}}} \right)$$