N2F2 Lewis structure

N₂F₂ (dinitrogen difluoride) has two nitrogen atoms and two fluorine atoms.

In the N₂F₂ Lewis structure, there is a double bond between the two nitrogen atoms, and each nitrogen is attached with one fluorine atom. Each fluorine atom has three lone pairs, and each nitrogen atom has one lone pair.

Alternative method: Lewis structure of N₂F₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, nitrogen lies in group 15, and fluorine lies in group 17.

Hence, nitrogen has five valence electrons and fluorine has seven valence electrons.

Since N₂F₂ has two nitrogen atoms and two fluorine atoms, so…

Valence electrons of two nitrogen atoms = 5 × 2 = 10
Valence electrons of two fluorine atoms = 7 × 2 = 14

And the total valence electrons = 10 + 14 = 24

Learn how to find: Nitrogen valence electrons and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 24 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 24 ÷ 2 = 12

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since nitrogen is less electronegative than fluorine, assume that the central atom is nitrogen.

Here, there are two nitrogen atoms, so we can assume any one as the central atom.

Let’s assume that the central atom is left nitrogen.

Therefore, place nitrogens in the center and fluorines on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 12 electron pairs. And three bonds are already marked. So we have to only mark the remaining nine electron pairs as lone pairs on the sketch.

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

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are fluorines and right nitrogen.

So for each fluorine, there are three lone pairs, for right nitrogen, there are two lone pairs, and for left nitrogen, there is one lone pair.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

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

For left nitrogen atom, formal charge = 5 – 2 – ½ (4) = +1

For right nitrogen atom, formal charge = 5 – 4 – ½ (4) = +1

For each fluorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, both nitrogen atoms have charges, so mark them on the sketch as follows:

The above structure is not a stable Lewis structure because both nitrogen atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.

Convert a lone pair of the right nitrogen atom to make a new C — C bond with the left nitrogen atom as follows:

Final structure

The final structure of N₂F₂ comprises a central nitrogen-nitrogen double bond, with each nitrogen atom also sharing a single bond with a fluorine atom. In this arrangement, both nitrogen atoms satisfy the octet rule by maintaining one lone pair each, while the fluorine atoms complete their octets with three lone pairs. This configuration results in formal charges of zero for all four atoms, representing the most stable and energetically favorable distribution of electrons. Consequently, this specific bonding pattern represents the definitive and stable Lewis representation of dinitrogen difluoride.

Next: N₂O₅ Lewis structure

External video

• N2F2 Lewis Structure: How to Draw the Lewis Structure for N2F2 – YouTube • Wayne Breslyn

External links

• https://geometryofmolecules.com/n2f2-lewis-structure-molecular-geometry-hybridization-shape/
• https://techiescientist.com/n2f2-lewis-structure/
• https://lambdageeks.com/n2f2-lewis-structure/