N2F4 Lewis structure

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N2F4 Lewis Structure
N2F4 Lewis structure

N2F4 (tetrafluorohydrazine) has two nitrogen atoms and four fluorine atoms.

In N2F4 Lewis structure, there is a single bond between the two nitrogen atoms, and each nitrogen is attached with two fluorine atoms. Each fluorine atom has three lone pairs, and each nitrogen atom has one lone pair.


Use these steps to correctly draw the N2F4 Lewis structure:

#1 First draw a rough sketch
#2 Mark lone pairs on the atoms
#3 Calculate and mark formal charges on the atoms, if required

Let’s discuss each step in more detail.

#1 First draw a rough sketch

  • First, determine the total number of valence electrons
Periodic table

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 N2F4 has two nitrogen atoms and four fluorine atoms, so…

Valence electrons of two nitrogen atoms = 5 × 2 = 10
Valence electrons of four fluorine atoms = 7 × 4 = 28

And the total valence electrons = 10 + 28 = 38

  • Second, find the total electron pairs

We have a total of 38 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 = 38 ÷ 2 = 19

  • 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
N2F4 Lewis Structure (Step 1)
Rough sketch of N2F4 Lewis structure

#2 Mark lone pairs on the atoms

Here, we have a total of 19 electron pairs. And five bonds are already marked. So we have to only mark the remaining fourteen 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, and for each nitrogen, there is one lone pair.

Mark the lone pairs on the sketch as follows:

N2F4 Lewis Structure (Step 2)
Lone pairs marked, and got the stable Lewis structure of N2F4

#3 Calculate and mark formal charges on the atoms, if required

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

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

For each nitrogen atom, formal charge = 5 – 2 – ½ (6) = 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.

In the above structure, you can see that the central atom (left nitrogen) forms an octet. And the outside atoms (right nitrogen and fluorines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of N2F4.

Next: Cl2O2 Lewis structure

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