Question
The correct order of increasing bond angles in the following triatomic species is
Solution
B.
As the number of lone pair of electrons increases, bond angle decreases. NO2+ ion is isoelectronic with the CO2 molecule. It is a linear ion and its central atom (N+) undergoes sp-hybridisation, hence bond angle is 180o.
In NO2- ion, N -atom undergoes sp2 hybridisation. The angle between hybrid orbital should be 120o but one lone pair of electrons is lying on N- atom, hence bond angle decreases to 115o.
In NO2 molecule, N -atom has one unpaired electron in a sp2-hybrid orbital. The bond angle should be 120o but actually, it is 132o. It may be due to one unpaired electron in a sp2-hybrid orbital.
Therefore, the increasing order of bond angles.
