NH2F 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.

NH2F lewis structure has a Nitrogen atom (N) at the center which is surrounded by two Hydrogen atoms (H) and one Fluorine atom (F). There is a single bond between the Nitrogen (N) & Fluorine (F) atom as well as between the Nitrogen (N) and Hydrogen (H) atoms.

If you haven’t understood anything from the above image of NH2F lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of NH2F.

So let’s move to the steps of drawing the lewis structure of NH2F.

Steps of drawing NH2F lewis structure

Step 1: Find the total valence electrons in NH2F molecule

In order to find the total valence electrons in NH2F 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 NH2F 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 NH2F molecule = valence electrons given by 1 nitrogen atom + valence electrons given by 2 hydrogen atoms + valence electrons given by 1 fluorine atom = 5 + 1(2) + 7 = 14.

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 NH2F and it contains nitrogen atom (N), hydrogen atoms (H) and fluorine atom (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 NH2F molecule, you have to put the electron pairs between the nitrogen (N) & fluorine (F) atom and between the nitrogen (N) & hydrogen (H) atoms.

This indicates that these atoms are chemically bonded with each other in a NH2F 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 NH2F molecule, you can see that the outer atoms are hydrogen atoms and fluorine atom.

These hydrogen atoms 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 NH2F molecule.

The NH2F molecule has a total of 14 valence electrons and out of these, only 12 valence electrons are used in the above sketch.

So the number of electrons which are left = 14 – 12 = 2.

You have to put these 2 electrons on the central nitrogen atom in the above sketch of NH2F 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 NH2F 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 NH2F.

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) atoms as well as fluorine (F) atom present in the NH2F 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 NH2F 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

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

This indicates that the above lewis structure of NH2F is stable and there is no further change in the above structure of NH2F.

In the above lewis dot structure of NH2F, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of NH2F.

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:

About 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. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.

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