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Lewis Structure of NO2- (Nitrite ion)

source : chemistryscl.com

Lewis Structure of NO2- (Nitrite ion)

Lewis structure of NO2- ion is drawn in this tutorial. Total valence
electrons of nitrogen and oxygen atoms and negative charge also should be considered in the drawing
of NO2- lewis structure.

Now, we are going to learn, how to draw this lewis structure.

Steps of drawing NO2- lewis structure

Following steps are required to draw NO2- lewis structure and they are explained
in detail in this tutorial.

Find total number of electrons of the valance shells of nitrogen and
oxygen atoms and charge of the anion
Total electrons pairs
Center atom selection from nitrogen and oxygen atom
Put lone pairs on atoms
Stability of lewis structure – Check the stability and minimize charges on atoms by converting lone pairs to bonds.

Drawing correct lewis structure is important to
draw resonance
structures.

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

There are one nitrogen atom and two oxygen atoms in the nitrate ion. Also there is a -1 charge.

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

Total valence electrons given by nitrogen atom = 5

There are two oxygen atoms in NO2, Therefore

Total valence electrons given by oxygen atoms = 6 *2 = 12

Due to -1 charge, another electrons is added

Due to -1 charge, received electrons = 1
Total valence electrons = 5 + 12 + 1 = 18Total valence electrons pairs

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

Total electron pairs are determined by dividing the number total valence electrons by two. For,
NO2-, there are 18 valence electrons pairs, so total pairs of electrons are 9.

Center atom of NO2-

To be the center atom, ability of having greater valance is important. Therefore nitrogen has the more
chance to be the center atom (See the figure). So, now we can build a sketch of NO2-
ion.

Lone pairs on atoms

There are already two N-O bonds in the sketch. Therefore only seven valence electrons pairs are
remaining.

Start to mark those seven valence electrons pairs on outside atoms (oxygen atoms) as lone pairs. One oxygen atom
will take three lone pairs following the octal rule (oxygen and nitrogen atoms cannot keep more than
eight electrons in their valence shells).

Two oxygen atoms will take six valence electrons pairs. Now one valence electrons pair is
remaining. Mark that remaining one on nitrogen atom.

Check the stability of drawn NO2- ion and minimize charges on atoms by converting lone pairs to bonds

The drawn structure for NO2- is not a stable one because both oxygen atoms and nitrogen
atoms have charges.

Now, we should try to minimize charges by converting lone pair(s) which exist on oxygen atoms to bonds.
So we convert one lone pair of one oxygen atom as a N-H bond.

Now there is a double bond between nitrogen and one oxygen atom. There is a single bond also with nitrogen
atom and other oxygen atom.

In new structure, charges of atoms reduced. Now there is no any charge on one oxygen atom and nitrogen atom.
Now you understand this structure of NO2- is
more stable than previous structure due to less charges.

We cannot convert more lone pairs of other oxygen atom to make a bond with nitrogen atom because nitrogen
cannot keep more than eight electrons in its last valence shell.

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MakeTheBrainHappy: The Lewis Dot Structure for NO2+ – Answer to: Draw the Lewis structure for NO2-. By signing up, you'll get thousands of step-by-step solutions to your homework questions. You can…Lewis Structure of NO2 A molecule of nitrogen dioxide consists of one nitrogen atom and two atoms of oxygen. Let us look at the periodic table. Nitrogen belongs to group 15 (or group 5) and has an atomic number of 7, therefore has a valency of 5.Nitrogen dioxide does not have a single Lewis structure on account of its relatively strange electron configuration. The location of the double bond changes over time, meaning that at any point, either of the oxygen atoms could have a double bond with the nitrogen atom. As such, nitrogen dioxide is represented by the resonance Lewis structure:

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