Lewis structure of N2O

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The Lewis structure of N₂O contains one triple bond and one single bond, with one nitrogen in the center, and one other nitrogen and oxygen on either side. The left nitrogen atom has one lone pair, the oxygen atom has three lone pairs, and the center nitrogen atom does not have any lone pair.

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

Steps

By using the following steps, you can easily draw the Lewis structure of N₂O:

#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 N₂O has two nitrogen atoms and one oxygen atom.

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

Therefore, the total number of valence electrons = 10 + 6 = 16

• 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 center nitrogen is the central atom (as there are two nitrogens).

So now, put one nitrogen in the center and one other nitrogen and oxygen on either side. And draw the rough skeleton structure for the Lewis structure of N₂O something like this:

Also read: How to draw Lewis structure of I₃^– (4 steps)

#2 Show chemical bond

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

#3 Mark lone pairs

As calculated earlier, we have a total of 16 valence electrons. And in the above structure, we have already used four valence electrons. Hence, twelve valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs.

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 left nitrogen and oxygen, so left nitrogen and oxygen will get three lone pairs. And the central atom (center nitrogen) will not get any lone pair, because all six lone pairs are used.

So the Lewis structure of N₂O looks something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (center 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 BCl₃ (4 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 center nitrogen already has four valence electrons. Hence, nitrogen needs four more valence electrons to complete its octet.

So convert two lone pairs from the left nitrogen atom to make a new bond with the center nitrogen atom. And then, the Lewis structure of N₂O looks something like this:

Here, the lone pair of left nitrogen is converted (instead of oxygen). This is because nitrogen is less electronegative than oxygen, and so it can give more electrons to share them.

In the above structure, you can see that the octet is completed on the central atom (center nitrogen), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, 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 CN^– (5 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 left nitrogen atom

Valence electrons = 5
Nonbonding electrons = 2
Bonding electrons = 6

Formal charge = 5 – 2 – ½ (6) = 0

• For right nitrogen atom

Valence electrons = 5
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 5 – 0 – ½ (8) = +1

• For 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 N₂O 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 N₂O.

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

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Related

• Lewis structure of I₃^–
• Lewis structure of BCl₃
• Lewis structure of CN^–
• Lewis structure of CF₄
• Lewis structure of PF₃

External links

• N2O Lewis Structure in 6 Steps (With Images) – Pediabay
• N2O Lewis Structure| Nitrous oxide-Laughing Gas – What’s Insight
• N2O Lewis Structure, Resonance Structures, Oxidation Number – Chemistry School
• N2O lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
• N2O Lewis Structure, Geometry – Kemicalinfo
• Nitrous Oxide (N2O) Formal Charge – Chemistry Learner
• N2O Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram – Techiescientist
• The following three Lewis structures can be drawn for N2O – Pearson
• What is the Lewis electron dot formula (Lewis structure) of Nitrous Oxide (N2O)? – Socratic
• Chemical Bonding: N2O Lewis Structure – The Geoexchange
• N2O Lewis Structure; how can N form a double bond? – Laurence Lavelle
• Finding the central atom of N2O – Chemistry Stack Exchange
• Why does the Lewis Dot structure of N2O has N as central atom and not O as central atom? – Quora
• N2O Geometry and Hybridization – Chemistry Steps
• How does the bonding work in N2O? – Reddit