Lewis Structure of NO2Cl (With 5 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of NO2Cl in just 5 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of NO2Cl molecule.

So, if you are ready to go with these 5 simple steps, then let’s dive right into it!

Lewis structure of NO2Cl contains one double bond between the Nitrogen atom (N) & one Oxygen atom (O) and the rest other atoms are single bonded with each other. The Nitrogen atom (N) is at the center and it is surrounded by 2 Oxygen atoms (O) and 1 Chlorine atom (Cl).

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of NO2Cl).

5 Steps to Draw the Lewis Structure of NO2Cl

Step #1: Calculate the total number of valence electrons

Here, the given molecule is NO2Cl. In order to draw the lewis structure of NO2Cl, first of all you have to find the total number of valence electrons present in the NO2Cl molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in NO2Cl molecule

• For Nitrogen:

Nitrogen is a group 15 element on the periodic table. ^[1]

Hence, the valence electrons present in nitrogen is 5 (see below image).

• For Oxygen:

Oxygen is a group 16 element on the periodic table. ^[2]

Hence, the valence electron present in oxygen is 6 (see below image).

• For Chlorine:

Chlorine is a group 17 element on the periodic table. ^[3]

Hence, the valence electron present in chlorine is 7 (see below image).

Hence in a NO2Cl molecule, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electrons given by each Oxygen (O) atom = 6
Valence electrons given by Chlorine (Cl) atom = 7
So, total number of Valence electrons in NO2Cl molecule = 5 + 6(2) + 7 = 24

Step #2: Select the center atom

While selecting the center atom, always put the least electronegative atom at the center.

(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table). ^[4]

Here in the NO2Cl molecule, if we compare the nitrogen atom (N), oxygen atom (O) and chlorine atom (Cl), then nitrogen is less electronegative.

So, nitrogen should be placed in the center and the remaining 2 oxygen atoms and 1 chlorine atom will surround it.

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of NO2Cl, put the two electrons (i.e electron pair) between each atom to represent a chemical bond between them.

These pairs of electrons present between these atoms form a chemical bond, which bonds these atoms with each other in a NO2Cl molecule.

Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom

Don’t worry, I’ll explain!

In the Lewis structure of NO2Cl molecule, the outer atoms are oxygen atoms and chlorine atom.

So now, you have to complete the octet on these oxygen atoms and chlorine atom (because oxygen and chlorine requires 8 electrons to have a complete outer shell).

Now, you can see in the above image that the oxygen atoms and chlorine form an octet.

Also, all the 24 valence electrons of NO2Cl molecule (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.

Hence there is no change in the above sketch of NO2Cl molecule.

Let’s move to the next step.

Step #5: Check whether the central atom has octet or not. If it does not have an octet, then move the electron pair from the outer atom to form a double bond or triple bond

In this step, we have to check whether the central atom (i.e nitrogen) has an octet or not. 

In simple words, we have to check whether the central Nitrogen (N) atom is having 8 electrons or not.

As you can see from the above image, the central atom (i.e nitrogen) has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of nitrogen atom, we have to move the electron pair from the outer atom (i.e oxygen atom) to form a double bond.

(Note: We have to move the electron pair from the oxygen atom because it is less electronegative, and the less electronegative atom has more tendency to donate the electron pair.)

Now you can see from the above image that the central atom (i.e nitrogen), is having 8 electrons. So it fulfills the octet rule.

This indicates that this is the stable lewis structure of NO2Cl.

Each electron pair (:) in the lewis dot structure of NO2Cl represents the single bond ( | ). So the above lewis dot structure of NO2Cl can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of TeF4
Lewis Structure of ClF
Lewis Structure of SO
Lewis Structure of XeCl2
Lewis Structure of SeF2 

---

Article by;