XeF2 (xenon difluoride) has one xenon atom and two fluorine atoms. In the lewis structure of XeF2, there are two single bonds around the xenon atom, with two fluorine atoms attached to it, and each atom has three lone pairs.
Here’s how you can draw the XeF2 lewis structure step by step.
Step #1: draw sketch
Step #2: mark lone pairs
Step #3: mark charges (if there are)
Let’s break down each step in detail.
#1 Draw Sketch
- First, determine the total number of valence electrons
Hence, xenon has eight valence electrons and fluorine has seven valence electrons.
Since XeF2 has one xenon atom and two fluorine atoms, so…
Valence electrons of one xenon atom = 8 × 1 = 8
Valence electrons of two fluorine atoms = 7 × 2 = 14
And the total valence electrons = 8 + 14 = 22
- Second, find the total electron pairs
We have a total of 22 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 = 22 ÷ 2 = 11
- Third, determine the central atom
We have to place the least electronegative atom at the center.
Since xenon is less electronegative than fluorine, assume that the central atom is xenon.
Therefore, place xenon in the center and fluorines on either side.
- And finally, draw the rough sketch
#2 Mark Lone Pairs
Here, we have a total of 11 electron pairs. And two Xe — F bonds are already marked. So we have to only mark the remaining nine electron pairs as lone pairs on the sketch.
Always start to mark the lone pairs from outside atoms. Here, the outside atoms are fluorines.
So for each atom, there are three lone pairs.
Mark the lone pairs on the sketch as follows:
#3 Mark Charges
Use the following formula to calculate the formal charges on atoms:
Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons
For xenon atom, formal charge = 8 – 6 – ½ (4) = 0
For each fluorine atom, formal charge = 7 – 6 – ½ (2) = 0
Here, both xenon and fluorine atoms do not have charges, so no need to mark the charges.
And in the above structure, you can see that the central atom (xenon) forms an octet. Hence, the octet rule is satisfied.
Therefore, this structure is the stable lewis structure of XeF2.
Next: XeF4 Lewis Structure