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Is NO2 Polar or Nonpolar?
Nitrogen dioxide has a bent shape with a 134° bond angle, caused by an unpaired electron on the central nitrogen. Oxygen (3.44) is more electronegative than nitrogen (3.04), and the asymmetric geometry means the two N=O dipoles do not cancel, giving NO2 a net dipole of 0.32 D.
Why is NO2 Polar?
Nitrogen dioxide has a bent shape with a 134° bond angle, caused by an unpaired electron on the central nitrogen. Oxygen (3.44) is more electronegative than nitrogen (3.04), and the asymmetric geometry means the two N=O dipoles do not cancel, giving NO2 a net dipole of 0.32 D.
- Electronegativity difference: O (3.44) is significantly more electronegative than N (3.04), creating partial charges on each atom and making the individual bonds polar.
- Bent shape (134°): The asymmetric molecular geometry means the bond dipoles point in directions that do not cancel — they add up to produce a net dipole moment of 0.32 D.
- Net dipole moment (0.32 D): Any molecule with a nonzero net dipole moment is classified as polar. The 0.32 D dipole moment of NO2 confirms its polar character.
Molecular Geometry of NO2
NO2 has a bent molecular geometry with a bond angle of 134°. Here is why this shape determines polarity:
- The central atom's electron pairs arrange themselves to minimize repulsion, resulting in the bent shape.
- The 134° bond angle creates an asymmetric arrangement — the bond dipoles point in directions that do not perfectly oppose each other.
- Asymmetry is the key: if NO2 had a perfectly symmetric geometry, its bond dipoles would cancel and the molecule would be nonpolar. The bent shape prevents this cancellation.
Electronegativity and Polarity
Electronegativity measures how strongly an atom attracts bonding electrons. A difference greater than ~0.5 on the Pauling scale generally means the bond is polar.
In NO2:
- N (central atom) electronegativity: 3.04
- O (outer atom) electronegativity: 3.44
- Difference: 0.40 — below the ~0.5 threshold, so the N–O bonds are only weakly polar
The combination of polar bonds and an asymmetric bent geometry means the partial charges do not cancel — making NO2 a polar molecule with a net dipole of 0.32 D.
Is NO2 Polar or Nonpolar? (Quick Answer)
NO2 (Nitrogen Dioxide) is polar. NO2 is a polar molecule because its bent geometry and the slight electronegativity difference between nitrogen and oxygen produce a small but nonzero dipole moment of 0.32 D.
Frequently Asked Questions
Is NO2 polar or nonpolar?
NO2 is a polar molecule because its bent geometry and the slight electronegativity difference between nitrogen and oxygen produce a small but nonzero dipole moment of 0.32 D.
Why is Nitrogen Dioxide polar?
Nitrogen dioxide has a bent shape with a 134° bond angle, caused by an unpaired electron on the central nitrogen. Oxygen (3.44) is more electronegative than nitrogen (3.04), and the asymmetric geometry means the two N=O dipoles do not cancel, giving NO2 a net dipole of 0.32 D.
What is the shape of NO2?
NO2 has a bent molecular geometry with a bond angle of 134°. This shape results in an asymmetric charge distribution and a net dipole moment of 0.32 D, making the molecule polar.
Does NO2 have a dipole moment?
Yes. NO2 has a dipole moment of 0.32 D. Its bent geometry and polar bonds combine to produce a net dipole, confirming its polar character.