Lewis Structure Of No2 1

Lewis Structure for NO₂ ^- (Nitrite ion)

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

lewis structure of NO2-

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

Steps of drawing NO_two ^- lewis structure

Post-obit steps are required to draw NO₂ ^- lewis structure and they are explained in particular in this tutorial.

Find total number of electrons of the valance shells of nitrogen and oxygen atoms and charge of the anion
Full electrons pairs
Eye atom option from nitrogen and oxygen atom
Put lonely pairs on atoms
Stability of lewis construction - Bank check the stability and minimize charges on atoms by converting lone pairs to bonds.

Drawing right lewis construction 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 ane nitrogen cantlet and two oxygen atoms in the nitrate ion. Also at that place is a -1 charge.

Nitrogen and oxygen are located at VA and VIA groups respectively in the periodic tabular array. So nitrogen has five electrons in its valence shell. In oxygen atom, in that location are six electrons in its valence trounce.

Total valence electrons given by nitrogen atom = 5

There are 2 oxygen atoms in NO_ii, Therefore

Full valence electrons given past oxygen atoms = half dozen *two = 12

Due to -ane charge, another electrons is added

Due to -1 charge, received electrons = 1

Total valence electrons = five + 12 + 1 = 18

Total valence electrons pairs

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

Total electron pairs are determined past dividing the number full valence electrons by two. For, NO₂ ^-, there are xviii valence electrons pairs, then full pairs of electrons are 9.

Heart atom of NO₂ ^-

To be the center atom, ability of having greater valance is important. Therefore nitrogen has the more chance to be the heart cantlet (Run across the effigy). So, at present nosotros can build a sketch of NO₂ ^- ion.

center atom of NO2

Lone pairs on atoms

In that location are already 2 N-O bonds in the sketch. Therefore merely seven valence electrons pairs are remaining.

Start to mark those seven valence electrons pairs on exterior atoms (oxygen atoms) as lonely pairs. One oxygen atom will take three lone pairs post-obit the octal rule (oxygen and nitrogen atoms cannot go on more than viii electrons in their valence shells).

Ii oxygen atoms will take 6 valence electrons pairs. Now one valence electrons pair is remaining. Mark that remaining one on nitrogen atom.

valence electrons of NO2- ion

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

The drawn structure for NO_ii ^- is not a stable i because both oxygen atoms and nitrogen atoms have charges.

Now, we should attempt to minimize charges by converting lone pair(s) which be on oxygen atoms to bonds. So we convert one solitary pair of i oxygen atom as a North-H bond.

At present there is a double bond between nitrogen and ane oxygen atom. In that location is a unmarried bond also with nitrogen atom and other oxygen cantlet.

minimize charges on NO2- ion in lewis structure

In new structure, charges of atoms reduced. Now at that place is no any charge on one oxygen atom and nitrogen cantlet. Now you understand this structure of NO_ii ^- is more than stable than previous structure due to less charges.

We cannot convert more lonely pairs of other oxygen atom to brand a bond with nitrogen atom because nitrogen cannot go along more than than eight electrons in its final valence trounce.