The chemical formula NO3– to represent the Nitrate ion. That is acquired from Nitric acid, HNO3. Salts containing the Nitrate ion are referred to as ‘Nitrates‘. These salts exist abundantly in nature and also find themselves used in a variety of applications. 


 A diet rich in Nitrate elevates endurance and also increases plasma levels. This boost helps regulation of blood flow in the muscles. Nitrates naturally happen in the soil. They find use in fertilizers and also explosives amongst other things.

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We say the the Nitrate ion is non-polar. Let’s watch why the is the case.

To determine the polarity the the NO3– ion, us must first account for its properties. These include its electronegativity, its molecule geometry, and its resulting dipole moment if any.

Electronegativity and also Bond Nature

To determine if the bonds current in the NO3– ion room polar or non-polar, we look come the routine table. The difference in charges in between the Nitrogen and also Oxygen atom is .40

Now, in accordance v the Pauling scale, this tells us that the Nitrogen-Oxygen shortcut in the NO3– ion is non-polar.

Molecular Shape and also Symmetry

The NO3– ion has three Oxygen atom bonded to the main Nitrogen atom as displayed in the figure. 

It has three resonance structures as the dual bond between the Nitrogen atom and also Oxygen atom deserve to be placed between any type of of the various other Oxygen atoms together well.


According to the VSEPR theory, the Oxygen atoms repel every other and also spread much away in an also manner. This results in identical bond angles of 120°, making the structure symmetrical. This results in no overall net charge as result of its structure making the a non-polar ion.

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Net Dipole Moment and also 1- Charge

The 1- fee over the whole molecule is spread evenly. The interacts through polar solvents such together water due to this charge. This is even though the is structurally non-polar. 


In the averaged out resonance structure, the negative charge is dispersed evenly as shown in the figure.

In three dimensions, it deserve to be viewed that the dipoles ~ above the bonds all allude in opposite directions. This leads to a zero net dipole moment. 

Using the above, we deserve to safely say the the Nitrate ion is non-polar. 


As shown above, the NO3– ion has actually an as whole 1- charge. However, this negative charge is distributed evenly because of its symmetric shape. This outcomes in a zero network dipole moment. Further, the Nitrogen- Oxygen bonds room non-polar follow to the Pauling scale.