SO3 (sulfur trioxide) has one sulfur atom and three oxygen atoms. In the lewis structure of SO3, there are three double bonds around the sulfur atom, with three oxygen atoms attached to it, and on each oxygen atom, there are two lone pairs.
Here’s how you can draw the SO3 lewis structure step by step.
Step #1: draw sketch
Step #2: mark lone pairs
Step #3: mark charges
Step #4: minimize charges
Step #5: minimize charges again (if there are)
Let’s break down each step in detail.
#1 Draw Sketch
- First, determine the total number of valence electrons
Hence, both sulfur and oxygen have six valence electrons.
Since SO3 has one sulfur atom and three oxygen atoms, so…
Valence electrons of one sulfur atom = 6 × 1 = 6
Valence electrons of three oxygen atoms = 6 × 3 = 18
And the total valence electrons = 6 + 18 = 24
- 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 sulfur is less electronegative than oxygen, assume that the central atom is sulfur.
Therefore, place sulfur in the center and oxygens on either side.
- And finally, draw the rough sketch
#2 Mark Lone Pairs
Here, we have a total of 12 electron pairs. And three S — O 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 oxygens.
So for each oxygen, there are three lone pairs, and for sulfur, there is zero lone pair because all nine electron pairs are over.
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 sulfur atom, formal charge = 6 – 0 – ½ (6) = +3
For each oxygen atom, formal charge = 6 – 6 – ½ (2) = -1
Here, both sulfur and oxygen atoms have charges, so mark them on the sketch as follows:
The above structure is not a stable lewis structure because both sulfur and oxygen atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.
#4 Minimize Charges
Convert a lone pair of the oxygen atom to make a new S — O bond with the sulfur atom as follows:
#5 Minimize Charges Again
Since there are charges on sulfur and oxygen atoms, again convert a lone pair of the oxygen atom to make a new S — O bond with the sulfur atom as follows:
#6 Minimize Charges Again
There are still charges on sulfur and oxygen atoms, so again convert a lone pair of the oxygen atom to make a new S — O bond with the sulfur atom as follows:
In the above structure, you can see that the central atom (sulfur) forms an octet. Hence, the octet rule is satisfied.
Also, the above structure is more stable than the previous structures. Therefore, this structure is the stable lewis structure of SO3.
Next: C2H4 Lewis Structure