Lewis structure of NO2F

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The Lewis structure of NO₂F contains one double bond and two single bonds, with nitrogen in the center, and two oxygens and fluorine on either side. The left oxygen atom has two lone pairs, the right oxygen atom has three lone pairs, and the fluorine atom also has three lone pairs.

Plus, there is a positive (+1) charge on the nitrogen atom, and a negative (-1) charge on the right oxygen atom.

Steps

By using the following steps, you can easily draw the Lewis structure of NO₂F.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Complete octet on central atom
#5 Calculate formal charge and check stability

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… nitrogen is a group 15 element, oxygen is a group 16 element, and fluorine is a group 17 element. Hence, nitrogen has five valence electrons, oxygen has six valence electrons, and fluorine has seven valence electrons.

Now NO₂F has one nitrogen atom, two oxygen atoms, and one fluorine atom.

So the total number of valence electrons = valence electrons of nitrogen atom + (valence electrons of oxygen atom × 2) + valence electrons of fluorine atom

Therefore, the total number of valence electrons = 5 + 12 + 7 = 24

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for nitrogen, oxygen, and fluorine as follows:

Electronegativity value of nitrogen = 3.04
Electronegativity value of oxygen = 3.44
Electronegativity value of fluorine = 3.98

Obviously, nitrogen is less electronegative than oxygen and fluorine. Hence, assume that nitrogen is the central atom.

So now, put nitrogen in the center and two oxygens and fluorine on either side. And draw the rough skeleton structure for the Lewis structure of NO₂F something like this:

Also read: How to draw Lewis structure of SiBr₄ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since nitrogen is surrounded by two oxygens and fluorine, use six electrons to show three chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 24 valence electrons. And in the above structure, we have already used six valence electrons. Hence, eighteen valence electrons are remaining.

Two valence electrons represent one lone pair. So eighteen valence electrons = nine lone pairs.

Note that all (nitrogen, oxygen, and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are two oxygens and fluorine, so two oxygens and fluorine will get three lone pairs. And the central atom (nitrogen) will not get any lone pair, because all nine lone pairs are used.

So the Lewis structure of NO₂F looks something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (nitrogen) doesn’t form an octet.

So in the next step, we have to complete the octet on the central atom.

Also read: How to draw Lewis structure of CH₃NO₂ (5 steps)

#4 Complete octet on central atom

Remember that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Now nitrogen already has six valence electrons. Hence, nitrogen needs two more valence electrons to complete its octet.

So convert one lone pair from one oxygen atom to make a new bond with the nitrogen atom. And then, the Lewis structure of NO₂F looks something like this:

Here, the lone pair of oxygen is converted (instead of fluorine). This is because oxygen is less electronegative than fluorine, and so it can give more electrons to share them.

In the above structure, you can see that the octet is completed on the central atom (nitrogen), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of AsF₃ (4 steps)

#5 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

• For nitrogen atom

Valence electrons = 5
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 5 – 0 – ½ (8) = +1

• For left oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

• For right oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

• For fluorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of NO₂F looks something like this:

In the above structure, you can see that the formal charges of atoms are closer to zero. Therefore, this is the most stable Lewis structure of NO₂F.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

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Related

• Lewis structure of SiBr₄
• Lewis structure of CH₃NO₂
• Lewis structure of AsF₃
• Lewis structure of NO₂Cl
• Lewis structure of BeCl₂

External links

• Chemical Bonding: NO2F Lewis Structure – The Geoexchange
• NO2F Lewis Structure in 6 Steps (With Images) – Pediabay
• NO2F Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Techiescientist
• Draw the Lewis structures of all the important resonance forms of NO₂F – Homework.Study.com
• Nitryl Fluoride, NO2F Molecular Geometry & Polarity – Tutor-Homework.com
• NO2F Lewis dot structure | Science, Chemistry – ShowMe
• Draw all resonance structures for the nitryl fluoride molecule, NO2F – Brainly
• Draw the Lewis dot structure of nitryl fluoride: NO2F – Chegg
• Draw the Lewis structure for NO2F. Is this molecule polar? or nonpolar? – OneClass