NHF2 Lewis Structure in 6 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

NHF2 lewis structure has a Nitrogen atom (N) at the center which is surrounded by one Hydrogen atom (H) and two Fluorine atoms (F). There is a single bond between the Nitrogen (N) & Hydrogen (H) atom as well as between the Nitrogen (N) & Fluorine (Fl) atom. There is 1 lone pair on the Nitrogen atom (N) and 3 lone pairs on Fluorine atoms (F).

If you haven’t understood anything from the above image of NHF2 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of NHF2.

So let’s move to the steps of drawing the lewis structure of NHF2.

Steps of drawing NHF2 lewis structure

Step 1: Find the total valence electrons in NHF2 molecule

In order to find the total valence electrons in NHF2 molecule, first of all you should know the valence electrons present in nitrogen atom, hydrogen atom as well as fluorine atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of nitrogen, hydrogen as well as fluorine using a periodic table.

Total valence electrons in NHF2 molecule

→ Valence electrons given by nitrogen atom:

Nitrogen is a group 15 element on the periodic table. ^[1] Hence the valence electrons present in nitrogen is 5.

You can see the 5 valence electrons present in the nitrogen atom as shown in the above image.

→ Valence electrons given by hydrogen atom:

Hydrogen is group 1 element on the periodic table. ^[2] Hence the valence electron present in hydrogen is 1.

You can see that only 1 valence electron is present in the hydrogen atom as shown in the above image.

→ Valence electrons given by fluorine atom:

Fluorine is group 17 element on the periodic table. ^[3] Hence the valence electron present in fluorine is 7.

You can see the 7 valence electrons present in the fluorine atom as shown in the above image.

Hence, 

Total valence electrons in NHF2 molecule = valence electrons given by 1 nitrogen atom + valence electrons given by 1 hydrogen atom + valence electrons given by 2 fluorine atoms = 5 + 1 + 7(2) = 20.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

(Remember: If hydrogen is present in the given molecule, then always put hydrogen outside.)

Now here the given molecule is NHF2 and it contains nitrogen atom (N), hydrogen atom (H) and fluorine atoms (F).

So as per the rule we have to keep hydrogen outside.

Now, you can see the electronegativity values of nitrogen atom (N) and fluorine atom (F) in the above periodic table.

If we compare the electronegativity values of nitrogen (N) and fluorine (F) then the nitrogen atom is less electronegative.

So here the nitrogen atom (N) is the center atom and the fluorine atom (F) is the outside atom.

Step 3: Connect each atoms by putting an electron pair between them

Now in the NHF2 molecule, you have to put the electron pairs between the nitrogen (N) & hydrogen (H) atom and between the nitrogen (N) & fluorine (F) atoms.

This indicates that these atoms are chemically bonded with each other in a NHF2 molecule.

Step 4: Make the outer atoms stable. Place the remaining valence electrons pair on the central atom.

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of NHF2 molecule, you can see that the outer atoms are hydrogen atom and fluorine atoms.

These hydrogen atom and fluorine atom are forming a duplet and octet respectively and hence they are stable.

Also, in step 1 we have calculated the total number of valence electrons present in the NHF2 molecule.

The NHF2 molecule has a total 20 valence electrons and out of these, only 18 valence electrons are used in the above sketch.

So the number of electrons which are left = 20 – 18 = 2.

You have to put these 2 electrons on the central nitrogen atom in the above sketch of NHF2 molecule.

Now let’s proceed to the next step.

Step 5: Check the octet on the central atom

In this step, you have to check whether the central nitrogen atom (N) is stable or not.

In order to check the stability of the central nitrogen (N) atom, we have to check whether it is forming an octet or not.

You can see from the above picture that the nitrogen atom is forming an octet. That means it has 8 electrons.

And hence the central nitrogen atom is stable.

Now let’s proceed to the final step to check whether the lewis structure of NHF2 is stable or not.

Step 6: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of NHF2.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on nitrogen (N) atom, hydrogen (H) atom as well as fluorine (F) atoms present in the NHF2 molecule.

For calculating the formal charge, you have to use the following formula;

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

You can see the number of bonding electrons and nonbonding electrons for each atom of NHF2 molecule in the image given below.

For Nitrogen (N) atom:
Valence electrons = 5 (because nitrogen is in group 15)
Bonding electrons = 6
Nonbonding electrons = 2

For Hydrogen (H) atom:
Valence electron = 1 (because hydrogen is in group 1)
Bonding electrons = 2
Nonbonding electrons = 0

For Fluorine (F) atom:
Valence electrons = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
N	=	5	–	6/2	–	2	=	0
H	=	1	–	2/2	–	0	=	0
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the nitrogen (N) atom, hydrogen (H) atom as well as fluorine (F) atom has a “zero” formal charge.

This indicates that the above lewis structure of NHF2 is stable and there is no further change in the above structure of NHF2.

In the above lewis dot structure of NHF2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of NHF2.

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

BeI2 Lewis Structure	CHBr3 Lewis Structure
SiCl2Br2 Lewis Structure	SbF5 Lewis Structure
ClBr3 Lewis Structure	GeH4 Lewis Structure