Step 1: Find valence e- for all atoms. Add them together.

N-5

O-6x2=12

Total=17 ( getting odd number for total valence electrons is uncommon)

Step2: Find octet e- for each atom and add them together.

N-8

O-8x2=16

Total=24

Step3: Subtract step 1 total from step 2. This step gives you bonding e-.

24-17=7e-

Step 4: Find number of bonds by diving the number in step 3 by 2(because each bond is made of 2 e-)

7e-/2= 3 bond pairs and 1 extra unbonded electron

Step 5: Find the number of nonbonding (lone pairs) e-. Subtract step 3 number from step 1.

17-7= 10e-=5 lone pairs

Use information from step 4 and 5 to draw the lewis structure.

According to electronegativity rule, Nitrogen has the least Electronegativity .So put nitrogen in the centre.Fill in the bond pairs and lone pairs as follows.

Lewis dot structure of NO2

Alternatively a dot method can be used to draw the lewis structure of NO₂.
Calculate the total valence electrons in NO₂ molecule.
N=5,O=6x2=12
Total=17
Put Nitrogen in center.
Put a pair of electrons connecting the side atom with central atom.Put remaining electrons on the side atoms.Move electrons from side atoms until all elemts get 8 electrons.Nitrogen in NO2 is an exception to octet rule and does not follow octet rule.

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