Lewis Structure of NO2F (With 5 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of NO2F in just 5 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of NO2F molecule.

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

Lewis structure of NO2F 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 Fluorine atom (F).

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 NO2F).

5 Steps to Draw the Lewis Structure of NO2F

Step #1: Calculate the total number of valence electrons

Here, the given molecule is NO2F. In order to draw the lewis structure of NO2F, first of all you have to find the total number of valence electrons present in the NO2F 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 NO2F 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 Fluorine: 

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

Hence, the valence electrons present in fluorine is 7 (see below image).

Hence in a NO2F molecule, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electrons given by each Oxygen (O) atom = 6
Valence electrons given by Fluorine (F) atom = 7
So, total number of Valence electrons in NO2F 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 NO2F molecule, if we compare the nitrogen atom (N), oxygen atom (O) and fluorine atom (F), then nitrogen is less electronegative.

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

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

Now in the above sketch of NO2F, 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 NO2F 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 NO2F molecule, the outer atoms are oxygen atoms and fluorine atom.

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

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

Also, all the 24 valence electrons of NO2F 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 NO2F 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 NO2F.

Each electron pair (:) in the lewis dot structure of NO2F represents the single bond ( | ). So the above lewis dot structure of NO2F can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of XeOF4
Lewis Structure of ICl
Lewis Structure of H2SO3
Lewis Structure of HSO4-
Lewis Structure of CCl2F2 

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