NH2Cl Lewis structure

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NH₂Cl (monochloramine) has one nitrogen atom, two hydrogen atoms, and one chlorine atom.

In the NH₂Cl Lewis structure, there are three single bonds around the nitrogen atom, with two hydrogen atoms and one chlorine atom attached to it. The nitrogen atom has one lone pair, and the chlorine atom has three lone pairs.

Steps

Here’s how you can easily draw the NH₂Cl Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

#1 Draw a rough skeleton structure

• First, determine the total number of valence electrons

In the periodic table, nitrogen lies in group 15, hydrogen lies in group 1, and chlorine lies in group 17.

Hence, nitrogen has five valence electrons, hydrogen has one valence electron, and chlorine has seven valence electrons.

Since NH₂Cl has one nitrogen atom, two hydrogen atoms, and one chlorine atom, so…

Valence electrons of one nitrogen atom = 5 × 1 = 5
Valence electrons of two hydrogen atoms = 1 × 2 = 2
Valence electrons of one chlorine atom = 7 × 1 = 7

And the total valence electrons = 5 + 2 + 7 = 14

Learn how to find: Nitrogen valence electrons, Hydrogen valence electrons, and Chlorine valence electrons

• Second, find the total electron pairs

We have a total of 14 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 14 ÷ 2 = 7

• Third, determine the central atom

Here hydrogen can not be 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.

Now we have to choose the central atom from nitrogen and chlorine. Place the least electronegative atom at the center.

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

Therefore, place nitrogen in the center and hydrogen and chlorine on either side.

• And finally, draw the rough sketch

#2 Mention lone pairs on the atoms

Here, we have a total of 7 electron pairs. And three bonds are already marked. So we have to only mark the remaining four electron pairs as lone pairs on the sketch.

Also remember 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.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogens and chlorine. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for chlorine, there are three lone pairs, and for nitrogen, there is one lone pair.

Mark the lone pairs on the sketch as follows:

#3 If needed, mention formal charges on the atoms

Use the following formula to calculate the formal charges on atoms:

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

For nitrogen atom, formal charge = 5 – 2 – ½ (6) = 0

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, the atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (nitrogen) forms an octet. The outside atom (chlorine) also forms an octet, and both hydrogens form a duet. Hence, the octet rule and duet rule are satisfied.

Therefore, this structure is the stable Lewis structure of NH₂Cl.

Next: C₆H₆ Lewis structure

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External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/NH2Cl-lewis-structure.html
• https://topblogtenz.com/nh2cl-lewis-structure-molecular-geometry-polar-or-nonpolar/
• https://lambdageeks.com/nh2cl-lewis-structure/
• https://techiescientist.com/nh2cl-lewis-structure/
• https://oneclass.com/homework-help/chemistry/6925559-indicate-the-positions-of-the-m.en.html