Lewis structure of NH2Cl

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The Lewis structure of NH₂Cl contains three single bonds, with nitrogen in the center, and two hydrogens and chlorine on either side. There are three lone pairs on the chlorine atom, one lone pair on the 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 NH₂Cl.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

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, hydrogen is a group 1 element, and chlorine is a group 17 element. Hence, nitrogen has five valence electrons, hydrogen has one valence electron, and chlorine has seven valence electrons.

Now NH₂Cl has one nitrogen atom, two hydrogen atoms, and one chlorine atom.

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

Therefore, the total number of valence electrons = 5 + 2 + 7 = 14

• 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 the central atom from nitrogen and chlorine.

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 chlorine as follows:

Electronegativity value of nitrogen = 3.04
Electronegativity value of chlorine = 3.16

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

So now, put nitrogen in the center and hydrogens and chlorine on either side. And draw the rough skeleton structure for the Lewis structure of NH₂Cl something like this:

Also read: How to draw Lewis structure of H₃PO₄ (5 steps)

#2 Show chemical bond

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

Also read: How to draw Lewis structure of CHO₂^– (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 14 valence electrons. And in the above structure, we have already used six valence electrons. Hence, eight valence electrons are remaining.

Two valence electrons represent one lone pair. So eight valence electrons = four lone pairs.

Note that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell. Hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 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 chlorine. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So chlorine will get three lone pairs. And the central atom (nitrogen) will get one lone pair.

Now draw the Lewis structure of NH₂Cl something like this:

In the above structure, you can see that the octet is completed on the central atom (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 BrO₂^– (5 steps)

#4 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 = 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

• For chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of NH₂Cl looks something like this:

In the above structure, you can see that the formal charges of all atoms are zero. Therefore, this is the stable Lewis structure of NH₂Cl.

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

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Related

• Lewis structure of H₃PO₄
• Lewis structure of CHO₂^–
• Lewis structure of BrO₂^–
• Lewis structure of IF₃
• Lewis structure of CNO^–

External links

• NH2Cl Lewis Structure – How to draw the Electron Dot Structure for NH2Cl – The Geoexchange
• NH2Cl lewis structure, Molecular geometry, and Polar or nonpolar – Topblogtenz
• NH2Cl Lewis Structure in 6 Steps (With Images) – Pediabay
• NH2Cl Lewis Structure, Geometry, Hybridization, and Polarity – Techiescientist
• Chloramine, NH2Cl Molecular Geometry & Polarity – Tutor-Homework.com
• Draw the Lewis structure for NH2Cl and determine whether it is polar or nonpolar – Homework.Study.com
• Lewis structure and molecular geometry for NH2Cl – Brainly
• Draw the Lewis structures of monochloramine (NH2Cl) and hydrazine (N2H4) (Assign lone pairs, radical electrons, and atomic charges where appropriate.) – Chegg