Lewis structure of N2H2

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The Lewis structure of N₂H₂ contains one double bond and two single bonds, with two nitrogens in the center, and each nitrogen is attached with one hydrogen. There is one lone pair on each nitrogen atom, and the hydrogen atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of N₂H₂:

#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 hydrogen is a group 1 element. Hence, nitrogen has five valence electrons and hydrogen has one valence electron.

Now N₂H₂ has two nitrogen atoms and two hydrogen atoms.

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

Therefore, the total number of valence electrons = 10 + 2 = 12

• Now decide the central atom

We can not assume hydrogen as the central atom, because the central atom is bonded with at least two other atoms. And hydrogen has only one electron in its last shell, so it can not make more than one bond.

Therefore, choose nitrogen as the central atom.

But there are two nitrogen atoms in N₂H₂. Hence, we can assume any one as the central atom. Let’s assume that right nitrogen is the central atom.

So now, put two nitrogens in the center and two hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of N₂H₂ something like this:

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

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since two nitrogens are surrounded by two hydrogens, use six electrons to show three chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 12 valence electrons. And in the above structure, we have already used six valence electrons. Hence, six valence electrons are remaining.

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

Note that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell. And hydrogen is a period 1 element, so it can not keep more than 2 electrons in its 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 hydrogens and left nitrogen. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So left nitrogen will get two lone pairs. And the central atom (right nitrogen) will get one lone pair.

Now draw the Lewis structure of N₂H₂ something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (right 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 CH₃COOH (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 right nitrogen already has six valence electrons. Hence, right nitrogen needs two more valence electrons to complete its octet.

So convert one lone pair from the left nitrogen atom to make a new bond with the right nitrogen atom. And then, the Lewis structure of N₂H₂ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (right 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 ClO^– (4 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 each nitrogen atom

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

Formal charge = 5 – 2 – ½ (6) = 0

• For each hydrogen atom

Valence electrons = 1
Nonbonding electrons = 0
Bonding electrons = 2

Formal charge = 1 – 0 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of N₂H₂ looks something like this:

In the above structure, you can see that the formal charges of both (nitrogen and hydrogen) are zero. Therefore, this is the stable Lewis structure of N₂H₂.

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

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Related

• Lewis structure of NOCl
• Lewis structure of CH₃COOH
• Lewis structure of ClO^–
• Lewis structure of Cl₂O
• Lewis structure of ClO₄^–

External video

• N2H2 Lewis Structure: How to Draw the Lewis Structure for Dinitrogen dihydride – YouTube • Wayne Breslyn

External links

• N2H2 Lewis Structure in 6 Steps (With Images) – Pediabay
• N2H2 Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram – Techiescientist
• Chemical Bonding: N2H2 Lewis Structure – The Geoexchange
• N2H2 Lewis structure, molecular geometry, hybridization, polarity – Topblogtenz
• N2H2 Lewis structure, Molecular Geometry, Hybridization, Bond Angle and Shape – Geometry of Molecules
• N2H2 Lewis Structure, Geometry – Kemicalinfo
• N2H2 Lewis Structure (Dinitrogen Dihydride) – Pinterest
• The Lewis structure of N2H2 – Homework.Study.com
• Draw the Lewis structure for N2H2 – Chegg
• Determine the Lewis Dot Structure for the diazene molecule, N2H2 – Pearson
• How many bonding pairs and lone pairs are there for N2H2? – Quora
• The lewis structure of n2h2 shows __________ – Brainly
• Write the most stable Lewis structure for the following molecule: N2H2 – Numerade