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

Lewis Structure of NOF

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

Awesome!

Here, I have explained 6 simple steps to draw the lewis dot structure of NOF (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 NOF contains a double bond between the Nitrogen (N) & Oxygen (O) atom and a single bond between the Nitrogen (N) and Fluorine (F) atom. The Nitrogen atom (N) is at the center and it is surrounded by Oxygen and Fluorine atoms. The Nitrogen has 1 lone pair, Oxygen has 2 lone pairs and the Fluorine 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 NOF).

6 Steps to Draw the Lewis Structure of NOF

Step #1: Calculate the total number of valence electrons

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

  • 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 Oxygen:

Oxygen is a group 16 element on the periodic table.

Hence, the valence electron present in oxygen is 6 (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 NOF molecule, 

Valence electrons given by Nitrogen (N) atom = 5
Valence electrons given by Oxygen (O) atom = 6
Valence electrons given by Fluorine (F) atom = 7
So, total number of Valence electrons in NOF molecule = 5 + 6 + 7 = 18

Step #2: Select the center atom

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).

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

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

step 1

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

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

step 2

These pairs of electrons present between the Nitrogen (N), Fluorine (F) and Oxygen (O) atoms form a chemical bond, which bonds these atoms with each other in a NOF 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 NOF, the outer atoms are oxygen atom and fluorine atom.

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

step 3

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

Also, only 16 valence electrons of NOF molecule are used in the above structure.

But there are total 18 valence electrons in NOF molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 18 – 16 = 2.

So let’s keep these two electrons (i.e 1 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 has 8 electrons or not.

step 5

As you can see from the above image, the central atom (i.e nitrogen) has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of nitrogen atom, we have to move the electron pair from the outer atom (i.e oxygen atom) to form a double bond.

step 6

Now you can see from the above image that the central atom (i.e nitrogen), is having 8 electrons. 

So it fulfills the octet rule.

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), oxygen atom (O) as well as fluorine atom (F).

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

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

step 7
  • For Nitrogen:
    Valence electrons = 5 (as it is in group 15)
    Nonbonding electrons = 2
    Bonding electrons = 6
  • For Oxygen:
    Valence electron = 6 (as it is in group 16)
    Nonbonding electrons = 4
    Bonding electrons = 4
  • 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
N=526/2=0
O=644/2=0
F=762/2=0

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

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

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

NOF Lewis Structure

Related lewis structures for your practice:
Lewis Structure of ClF5
Lewis Structure of IF4-
Lewis Structure of PBr3
Lewis Structure of NO2-
Lewis Structure of CO3 2- 

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