Lewis Structure of NHF2 (With 6 Simple Steps to Draw!)

Lewis Structure of NHF2

Ready to learn how to draw the lewis structure of NHF2?


Here, I have explained 6 simple steps to draw the lewis dot structure of NHF2 (along with images).

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

Lewis structure of NHF2 contains a single bond between the Nitrogen-Fluorine atom and Nitrogen-Hydrogen atom. The Nitrogen atom (N) is at the center and it is surrounded by 2 Fluorine atoms (F) and 1 Hydrogen atom (H). The Nitrogen atom has 1 lone pair while 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 NHF2).

6 Steps to Draw the Lewis Structure of NHF2

Step #1: Calculate the total number of valence electrons

Here, the given molecule is NHF2 (Fluorimide). In order to draw the lewis structure of NHF2, first of all you have to find the total number of valence electrons present in the NHF2 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 NHF2

  • 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 Hydrogen: 

Hydrogen is a group 1 element on the periodic table. [2]

Hence, the valence electron present in hydrogen is 1 (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 NHF2 molecule, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electron given by Hydrogen (H) atom = 1
Valence electrons given by each Fluorine (F) atom = 7
So, total number of Valence electrons in NHF2 molecule = 5 + 1 +  7(2) = 20

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

While selecting the 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 NHF2 molecule, if we compare the hydrogen (H) atom, nitrogen atom (N) and fluorine atom (F), then hydrogen is less electronegative than nitrogen and fluorine. But as per the rule, we have to keep hydrogen outside.

So, nitrogen (which is less electronegative than fluorine) should be placed in the center and the fluorine atom as well as hydrogen will surround it.

step 1

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

Now in the above sketch of NHF2 molecule, put the two electrons (i.e electron pair) between the atoms to represent a chemical bond between them.

step 2

These pairs of electrons present between the atoms form a chemical bond, which bonds these atoms with each other in a NHF2 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 NHF2, the outer atoms are hydrogen atom as well as fluorine atom.

Hydrogen already has a duplet (see below image).

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

step 3

Now, you can see in the above image that the fluorine atom forms an octet.

Also, only 18 valence electrons of NHF2 molecule are used in the above structure.

But there are total 20 valence electrons in NHF2 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 20 – 18 = 2.

So let’s keep these two electrons (i.e electron pair) on the central atom.

step 4

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 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.

step 5

As you can see from the above image, the central atom (i.e nitrogen), has 8 electrons. So it fulfills the octet rule and the nitrogen atom is stable.

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 atom (N), hydrogen atom (H) as well as each fluorine atom (F).

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

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

step 6
  • For Nitrogen:
    Valence electron = 5 (as it is in group 15)
    Nonbonding electrons = 2
    Bonding electrons = 6
  • For Hydrogen:
    Valence electron = 1 (as it is in group 1)
    Nonbonding electrons = 0
    Bonding electrons = 2
  • For Fluorine:
    Valence electron = 7 (as it is in group 17)
    Nonbonding electrons = 6
    Bonding electrons = 2
Formal charge=Valence electronsNonbonding electrons(Bonding electrons)/2

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

Hence, there will not be any change in the above structure and the above lewis structure of NHF2 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of NHF2 represents the single bond ( | ). So the above lewis dot structure of NHF2 can also be represented as shown below.

nhf2 lewis structure

Related lewis structures for your practice:
Lewis Structure of BrCN
Lewis Structure of BeI2
Lewis Structure of CHBr3
Lewis Structure of SiCl2Br2
Lewis Structure of SbF5 

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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 learning platform that provides students with easily understandable explanations.

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