The two nitrogen oxygen bonds in nitro group are same in length justify
Answers
Answered by
0
At first sight, NO2 seems similar to CO2, carbon dioxide. But an NO2 molecule contains one more electron than CO2. If an electron is removed from NO2, you get the NO2+ (nitronium or nitryl) ion. It is isoelectronic with CO2, having two N=O double bonds and no unpaired electrons, so repulsion between the two regions of electron density is minimised by the 180° bond angle, and it is linear, as with CO2.
NO2+ ion
Neutral NO2 has one more 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.
Shape of ONO
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°.
Nitrite ion
Nitrite ion with an O-N-O bond angle of 115.4° (according to Gillespie and Hargittai).
NO2+ ion
Neutral NO2 has one more 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.
Shape of ONO
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°.
Nitrite ion
Nitrite ion with an O-N-O bond angle of 115.4° (according to Gillespie and Hargittai).
Similar questions