NHF2 Lewis structure

NHF₂ (fluorimide) has one nitrogen atom, one hydrogen atom, and two fluorine atoms.

In the NHF₂ Lewis structure, there are three single bonds around the nitrogen atom, with one hydrogen atom and two fluorine atoms attached to it. Each fluorine atom has three lone pairs, and the nitrogen atom has one lone pair.

Alternative method: Lewis structure of NHF₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, nitrogen lies in group 15, hydrogen lies in group 1, and fluorine lies in group 17.

Hence, nitrogen has five valence electrons, hydrogen has one valence electron, and fluorine has seven valence electrons.

Since NHF₂ has one nitrogen atom, one hydrogen atom, and two fluorine atoms, so…

Valence electrons of one nitrogen atom = 5 × 1 = 5
Valence electrons of one hydrogen atom = 1 × 1 = 1
Valence electrons of two fluorine atoms = 7 × 2 = 14

And the total valence electrons = 5 + 1 + 14 = 20

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

• Second, find the total electron pairs

We have a total of 20 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 = 20 ÷ 2 = 10

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from nitrogen and fluorine. Place the least electronegative atom at the center.

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

Therefore, place nitrogen in the center and hydrogen and fluorine on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 10 electron pairs. And three bonds are already marked. So we have to only mark the remaining seven 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. And hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogen and fluorines. But no need to mark on hydrogen, because hydrogen already has two electrons.

So for each fluorine, there are three lone pairs, and for 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 nitrogen atom, formal charge = 5 – 2 – ½ (6) = 0

For hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

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

Here, the atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of NHF₂ comprises a central nitrogen atom linked to one hydrogen atom and two fluorine atoms through single covalent bonds. In this arrangement, the nitrogen atom satisfies the octet rule by forming three bonds and retaining one lone pair. Within this layout, each fluorine atom fulfills its octet by maintaining three lone pairs alongside its single shared bond, while the hydrogen atom achieves a stable duet. This configuration represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of difluoramine.

Next: CH₃CH₂Cl Lewis structure

External video

• NHF2 Lewis Structure: How to Draw the Lewis Structure for NHF2 – YouTube • Wayne Breslyn

External links

• https://lambdageeks.com/nhf2-lewis-structure/
• https://oneclass.com/homework-help/chemistry/7028094-nhf2-lewis-structure.en.html