ORDER OF BOND ANGLE IN O3 NO2- NOF
Answers
Explanation:
NO2- is the smallest from these three. O3 has the smallest when compared to NO2
Neutral NO2 has one extra electron, which is accommodated in an orbital on the nitrogen atom. This introduces extra repulsions. The single-electron region is not as electron-rich as the N-O multiple bonds, so it does not have their repulsive power. Thus the bond angle is 134°, rather than the 120° expected if the repulsions between the electron-rich areas were identical.
O3 (ozone) shows trigonal planar for the electron pair geometry and and bent the molecular geometry. The one lone electron pair exerts a little extra repulsion on the two bonding oxygen atoms to create a slight compression to a 116 degree bond angle from the ideal of 120 degree.
If you meant NO2-
NO2- has one more electron than NO2, so it has a non-bonding pair ("lone pair") of electrons on nitrogen. This exerts a greater repulsion than the single electron in NO2, so the O-N-O angle is reduced further, to 115.4°.
Explanation:
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