Lewis Structure of NH2F (With 6 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of NH2F in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of NH2F molecule.

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

Lewis structure of NH2F contains a single bond between the Nitrogen (N) & Fluorine (F) atom as well as between Nitrogen (N) & Hydrogen (H) atoms. The Nitrogen atom (N) is at the center and it is surrounded by two Hydrogen (H) and one Fluorine atom (F). The Nitrogen atom has 1 lone pair and the fluorine atom has 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 NH2F).

6 Steps to Draw the Lewis Structure of NH2F

Step #1: Calculate the total number of valence electrons

Here, the given molecule is NH2F. In order to draw the lewis structure of NH2F, first of all you have to find the total number of valence electrons present in the NH2F 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 NH2F

• For Nitrogen:

Nitrogen is a group 15 element on the periodic table.

Hence, the valence electrons present in nitrogen is 5 (see below image).

• For Hydrogen: 

Hydrogen is a group 1 element on the periodic table.

Hence, the valence electron present in hydrogen is 1 (see below image).

• For Fluorine: 

Fluorine is a group 17 element on the periodic table.

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

Hence in a NH2F molecule, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by Fluorine (F) atom = 7
So, total number of Valence electrons in NH2F molecule = 5 + 1(2) + 7 = 14

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). ^[1]

Here in the NH2F molecule, if we compare the nitrogen atom (N) and fluorine atom (F), then the nitrogen is less electronegative than fluorine.

So, nitrogen should be placed in the center and the fluorine atom will surround it.

Also as per the rule, we have to keep hydrogen outside.

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

Now in the above sketch of NH2F molecule, put the two electrons (i.e electron pair) between the nitrogen-fluorine atoms and nitrogen-hydrogen atoms to represent a chemical bond between them.

These pairs of electrons present between the Nitrogen & Fluorine atoms as well as between the Nitrogen & Hydrogen atoms form a chemical bond, which bonds these atoms with each other in a NH2F 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 NH2F, the outer atoms are hydrogen atoms and fluorine atom.

So now, you have to check whether these hydrogen atoms are forming a duplet or not! (because hydrogen requires only 2 electrons to have a complete outer shell).

You also have to see whether the fluorine atom is forming an octet or not! (because fluorine requires 8 electrons to have a complete outer shell).

You can see in the above image that both the hydrogen atoms form a duplet. And the fluorine atom also forms an octet.

Also, only 12 valence electrons of NH2F molecule are used in the above structure.

But there are total 14 valence electrons in NH2F molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 14 – 12 = 2.

So let’s keep these 2 electrons (i.e 1 electron pairs) on the central atom.

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 has 8 electrons or not.

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), fluorine (F) atom as well as hydrogen atoms (H).

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 electron = 7 (as it is in group 17)
  Nonbonding electrons = 6
  Bonding electrons = 2
• For Hydrogen:
  Valence electron = 1 (as it is in group 1)
  Nonbonding electrons = 0
  Bonding electrons = 2

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

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

Hence, there will not be any change in the above structure and the above lewis structure of NH2F is the final stable structure only.

Each electron pair (:) in the lewis dot structure of NH2F represents the single bond ( | ). So the above lewis dot structure of NH2F can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of SeI2
Lewis Structure of H2Te
Lewis Structure of TeCl2
Lewis Structure of CH2I2
Lewis Structure of GaI3 

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