Question

The types of hybrid orbitals of nitrogen in $N{O}_2^{+},N{O}_3^{-}$ and $N{H}_4^{+}$ respectively are expected to be

• A. $s{p}^2,sp\text{and}s{p}^3$
• B. $s{p}^2,s{p}^3\text{and}sp$
• C. $sp,s{p}^2\text{and}s{p}^3$
• D. $sp,s{p}^3\text{and}s{p}^2$

Answer 1

The correct option is C $sp,s{p}^2\text{and}s{p}^3$

$1.$ Number of hybrid orbitals is the sum of the number of sigma bonds and the number of lone pair of electrons on central atom.

$2.$ Based on the number of hybrid orbitals hybridisation of molecules can be determined.

$\text{Molecule}$	$\text{No. of sigma bond}$	$\text{No. of lone pair of electrons}$	$\text{No. of hybrid orbitals}$	$\text{hybridisation}$
$N{O}_2^{+}$	2	0	2	$sp$
$N{O}_3^{-}$	3	0	3	$s{p}^2$
$N{H}_4^{+}$	4	0	4	$s{p}^3$

Hence, the correct choice is $\left(B\right).$