Step 1: Find valence e^{-} in all atoms. Add them together.

N=5

O=6

Total=11

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

N=8

F-8

Total=16

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

16-11=5e^{-}

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

5e^{-}/2= 2 bond pairs and an extra unbonded electron

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

11-5= 6e^{-}=3 lone pairs

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

Put atom with lowest electro negativity in the center. Arrange the remaining atoms around it. Finally put the bond pairs and lone pairs of electrons on the atoms.

## Lewis dot structure of NO_{}

Alternatively a dot method can be used to draw the lewis structure of NO_{}.

Calculate the total valence electrons in NO_{} molecule.

N=5

O=6

Put nitrogen and oxygen side by side.

Put a pair of electrons connecting the side atom with central atom.Pur remaining electrons on the sides.Make sure each side atom get 8 electrons to get octet state.

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