Hybrid orbitals are formed by the combination of atomic orbitals of similar energy of valence shell of the same atom.
The no. of hybridized orbitals of an atom is equal to the no. of orbitals of similar energy of valence shell undergoing hybridization.
For example: If one 4s orbital and three 4p orbitals are undergoing hybridization, then there will be a total of 1(one 4s)+3(three 4p) = 4 hybridized orbitals and it will be known as hybridization.
we can calculate the no. of hybridized orbitals within the molecule by knowing the hybridization of each atom present in it.
We can calculate the hybridization of each atom in a molecule by drawing the lewis structure of that molecule.
Hydrogen has only 1 2s orbital, hence it cannot undergo hybridization.
We can draw the structure of which is the hybrid of two resonance structures, which can be shown as follow:
From the given figure, the hybridization of a nitrogen atom () is , which represents that, three hybrid orbitals are present in nitrogen, as it has three sigma bonds connected to it.
Also, hybridization of the oxygen atom () atom which is bonded with the hydrogen atom () atom is , represents the oxygen atom has four hybrid orbitals are present as it has two sigma bonds and two lone pairs of electrons in it.
However the other two oxygen atoms are showing resonance in the Lewis dot structure hence, these two oxygen are equivalent to each other showing the same hybridization which is , which means they have three hybrid orbitals within them.
Hence, the total hybrid orbitals present in = Hybridized orbitals of nitrogen + Hybridized orbitals of oxygen = .
Hence, there are 13 hybrid orbitals present in the case of.