Lewis framework of NO3- ion is drawn step by step in this tutorial. Total valence electron of nitrogen and also oxygen atom and an adverse charge are taken into consideration to draw the NO3- lewis structure. You will certainly every truth of illustration lewis frameworks from this tutorial i m sorry will help you to draw much more lewis structures in the future.

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Lewis framework of nitrite ion


Now, we are going come learn, how to attract this lewis framework of NO3- ion.

Steps of illustration NO3- lewis structure

Following procedures are required to draw NO3- lewis structure and they are defined in detail in this tutorial.

find total number of electrons the the valance shells
the nitrogen and oxygen atoms and including fee of the anion complete electrons pairs in valence shells center atom choice from nitrogen and also oxygen atom placed lone bag on atoms stability of lewis structure - check the stability and minimize dues on atoms by converting lone bag to bonds.

Drawing exactly lewis framework is crucial to attract resonance structures. In one more tutorial, we learn exactly how to attract resonance frameworks of nitrate ion.

Total number of electrons of the valance shells the nitrogen and also oxygen atoms and charge that the anion

There are one nitrogen atom and three oxygen atom in the nitrate ion. Additionally there is a -1 fee on the nitrate ion.

Nitrogen and also oxygen are located at VA and also VIA groups respectively in the routine table. So nitrogen has five electrons in that valence shell. In oxygen atom, over there are six electrons in the valence shell.

complete valence electrons provided by nitrogen atom = 5

There room three oxygen atom in NO3-, Therefore

Total valence electrons offered by oxygen atoms = 6 *3 = 18

Due to -1 charge, another electrons is added

as result of -1 charge, obtained electrons to valence electrons= 1
full valence electron = 5 + 18 + 1 = 24

Total valence electron pairs

Total valance electrons pairs = σ bonds + π bond + lone bag at valence shells

Total electron bag are established by splitting the number total valence electron by two. For, NO2-, there space 24 valence electrons, so full pairs of electrons space 12.

Center atom that NO2-

To be the center atom, capability of having higher valance is important. Nitrogen can show valence,5. But, oxygen"s maximum valence is 2. Because of this nitrogen has the much more chance to be the center atom (See the figure). So, currently we can construct a sketch of NO3- ion.

map out of NO2- ion

Lone pairs on atoms

There are currently three N-O bond in the sketch. Thus only nine valence electrons pairs are staying to draw the rest of ion.

Start to mark those ripe valence electrons bag on exterior atoms (oxygen atoms) together lone pairs. One oxygen atom will certainly take three lone pairs adhering to the octal dominance (oxygen and nitrogen atom cannot keep an ext than eight electrons in their valence shells). Every nine valence electrons pairs (9) are spent when lone pairs are marked on oxygen atoms.

Therefore, there is no ine valence electrons bag to mark on nitrogen atom.


Check the security of attracted NO2- ion and minimize dues on atom by converting lone pairs to bonds

Check fees on atoms and also mark them together below. Charges are necessary to decide the lewis structure of the ion.


The drawn structure for NO3- is not a stable structure due to the fact that oxygen atoms and also nitrogen atoms have actually charges. As soon as a molecule or ion has actually so plenty of charges ~ above atoms, that structure is no stable.

Now, us should shot to minimization charges by convert lone pair or bag which exist ~ above oxygen atoms to bonds. So we transform one lone pair the one oxygen atom as a N-O bond.


Now there is a twin bond between nitrogen and one oxygen atom. Over there are likewise two single bonds (N-O) through nitrogen atom and also other oxygen atoms.


In brand-new structure, charges of atoms space reduced. Currently there is no any type of charge top top one oxygen atom. Also, fee of nitrogen atom is diminished from +2 come +1. Now you understand this structure of NO3- is much more stable 보다 previous structure as result of less fees on atoms.

But, we cannot convert much more lone pairs of other oxygen atom to do a bond through nitrogen atom since nitrogen can not keep an ext than eight electrons in its critical valence shell.

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Ask your chemistry questions and also find the answer How plenty of lone bag are around the nitrogen atom in nitrate ion?

No electrons pairs exist on nitrogen atom. But, top top nitrogen atom, over there is a +1 charge. Approximately the nitrogen atom, there are two solitary bonds and twin bond.

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