Lewis structure of NO2

The information on this page is ✔ fact-checked.

The Lewis structure of NO₂ contains one double bond and one single bond, with nitrogen in the center, and two oxygens on either side. The left oxygen atom has two lone pairs, the right oxygen atom has three lone pairs, and the nitrogen atom has one unpaired electron.

Plus, there is a positive (+1) charge on the nitrogen atom, and a negative (-1) charge on the right oxygen atom.

Steps

By using the following steps, you can easily draw the Lewis structure of NO₂:

#1 Draw skeleton
#2 Show chemical bond
#3 mark lone pairs
#4 Complete octet on central atom
#5 Calculate formal charge and check stability

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… nitrogen is a group 15 element and oxygen is a group 16 element. Hence, nitrogen has five valence electrons and oxygen has six valence electrons.

Now NO₂ has one nitrogen atom and two oxygen atoms.

So the total number of valence electrons = valence electrons of nitrogen atom + (valence electrons of oxygen atom × 2)

Therefore, the total number of valence electrons = 5 + 12 = 17

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for nitrogen and oxygen as follows:

Electronegativity value of nitrogen = 3.04
Electronegativity value of oxygen = 3.44

Obviously, nitrogen is less electronegative than oxygen. Hence, assume that nitrogen is the central atom.

So now, put nitrogen in the center and oxygens on either side. And draw the rough skeleton structure for the Lewis structure of NO₂ something like this:

Also read: How to draw Lewis structure of NH₃ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since nitrogen is surrounded by two oxygens, use four electrons to show two chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 17 valence electrons. And in the above structure, we have already used four valence electrons. Hence, thirteen valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs. Also, we have one unpaired electron.

Note that both (nitrogen and oxygen) are the period 2 elements, so they can not keep more than 8 electrons in their last shell.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are oxygens, so each oxygen will get three lone pairs. And the central atom (nitrogen) will get one unpaired electron.

So the Lewis structure of NO₂ looks something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (nitrogen) doesn’t form an octet.

So in the next step, we have to complete the octet on the central atom.

Also read: How to draw Lewis structure of HCN (5 steps)

#4 Complete octet on central atom

Remember that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Now nitrogen already has five valence electrons. Hence, nitrogen needs three more valence electrons to complete its octet.

So convert one lone pair from one oxygen atom to make a new bond with the nitrogen atom. And then, the Lewis structure of NO₂ looks something like this:

In the above structure, you can see that the octet is completed only on the outside atoms, and not on the central atom (nitrogen).

But as mentioned above… nitrogen is a period 2 element, so it can not keep more than 8 valence electrons in its last shell.

Therefore, we can not convert a lone pair of the oxygen atom to make a new bond with the nitrogen atom.

Now one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of SO₂ (6 steps)

#5 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

• For nitrogen atom

Valence electrons = 5
Nonbonding electrons = 1
Bonding electrons = 6

Formal charge = 5 – 1 – ½ (6) = +1

• For left oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

• For right oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

Mention the formal charges of atoms on the structure. So the Lewis structure of NO₂ looks something like this:

In the above structure, you can see that the formal charges of atoms are closer to zero. Therefore, this is the most stable Lewis structure of NO₂.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

📝 Your feedback matters. Visit our contact page.

Related

• Lewis structure of NH₃
• Lewis structure of HCN
• Lewis structure of SO₂
• Lewis structure of N₂
• Lewis structure of NO₃^–

External video

• NO2 Lewis Structure: How to Draw the Lewis Structure for NO2 – Wayne Breslyn

External links

• Lewis Structure for NO2 (Dinitrogen or Nitrogen Gas) – The University of Maryland
• NO2 Lewis Structure, Molecular Geometry, Hybridization, Polarity, and MO Diagram – Techiescientist
• How do you draw the lewis structure for NO2? – Socratic
• NO2 Lewis Structure, Geometry – Kemicalinfo
• NO2 Lewis Structure – Laurence Lavelle
• What is the Lewis dot structure of NO2? – Quora
• Why is the lewis dot structure of NO2 containing two double bonds incorrect? – Reddit