# Lewis Structure of N2F2 (With 6 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of N2F2 in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of N2F2 molecule.

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of N2F2 contains one double bond between the two Nitrogen (N) atoms and a single bond between Nitrogen (N) & Fluorine (F) atoms. The two Nitrogen atoms (N) are at the center and they are surrounded by 2 Fluorine atoms (F). The Nitrogen atoms have 1 lone pair and the Fluorine atoms have 3 lone pairs.

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 N2F2).

## 6 Steps to Draw the Lewis Structure of N2F2

### Step #1: Calculate the total number of valence electrons

Here, the given molecule is N2F2. In order to draw the lewis structure of N2F2, first of all you have to find the total number of valence electrons present in the N2F2 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 N2F2

• 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 Fluorine:

Fluorine is a group 17 element on the periodic table. [2]

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

Hence in a N2F2 molecule,

Valence electrons given by each Nitrogen (N) atom = 5
Valence electron given by each Fluorine (F) atom = 7
So, total number of Valence electrons in N2F2 molecule = 5(2) + 7(2) = 24

### Step #2: Select the center atom (H is always outside)

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). [3]

Here in the N2F2 molecule, if we compare the nitrogen atom (N) and fluorine atom (F), then nitrogen is less electronegative than fluorine.

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

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

Now in the above sketch of N2F2 molecule, put the two electrons (i.e electron pair) between the nitrogen-nitrogen atoms and nitrogen-fluorine atoms to represent a chemical bond between them.

These pairs of electrons present between the Nitrogen atoms as well as between the Nitrogen and Fluorine atoms form a chemical bond, which bonds these atoms with each other in a N2F2 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 N2F2, the outer atoms are fluorine atoms.

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

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

Also, only 18 valence electrons of N2F2 molecule are used in the above structure.

But there are total 24 valence electrons in N2F2 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 24 – 18 = 6.

So let’s keep these six electrons (i.e 3 electron pairs) on the central atoms.

Now, 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 convert the lone pair into double bond or triple bond

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

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

As you can see from the above image, one of the nitrogen atoms has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of this nitrogen atom, we have to convert the lone pair into a double bond.

Now you can see from the above image that both the central nitrogen atoms are having 8 electrons. So they fulfill the octet rule and both the nitrogen atoms are stable.

(Note: Here we have shifted the electron pair from the nitrogen atom and not from the fluorine atom, because nitrogen atom is less electronegative than fluorine. And the less electronegative atom has more tendency to donate the electron pair.)

### Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom

Now, you have come to the final step and here you have to check the formal charge on nitrogen atoms (N) as well as fluorine atoms (F).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

• For Nitrogen:
Valence electrons = 5 (as it is in group 15)
Nonbonding electrons = 2
Bonding electrons = 6
• For Fluorine:
Valence electrons = 7 (as it is in group 17)
Nonbonding electrons = 6
Bonding electrons = 2

So you can see above that the formal charges on nitrogen as well as fluorine are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of N2F2 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of N2F2 represents the single bond ( | ). So the above lewis dot structure of N2F2 can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of CH2
Lewis Structure of HO2-
Lewis Structure of C2HCl
Lewis Structure of S2O
Lewis Structure of BrCl3

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Author
##### Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online chemistry learning platform that provides students with easily understandable explanations.