SO2F2 Lewis structure

SO₂F₂ (sulfuryl fluoride) has one sulfur atom, two oxygen atoms, and two fluorine atoms.

In SO₂F₂ Lewis structure, there are two double bonds and two single bonds around the sulfur atom, with two oxygen atoms and two fluorine atoms attached to it. Each oxygen atom has two lone pairs, and each fluorine atom has three lone pairs.

Alternative method: Lewis structure of SO₂F₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, both sulfur and oxygen lie in group 16, and fluorine lies in group 17.

Hence, both sulfur and oxygen have six valence electrons, and fluorine has seven valence electrons.

Since SO₂F₂ has one sulfur atom, two oxygen atoms, and two fluorine atoms, so…

Valence electrons of one sulfur atom = 6 × 1 = 6
Valence electrons of two oxygen atoms = 6 × 2 = 12
Valence electrons of two fluorine atoms = 7 × 2 = 14

And the total valence electrons = 6 + 12 + 14 = 32

Learn how to find: Sulfur valence electrons, Oxygen valence electrons, and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 32 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 = 32 ÷ 2 = 16

• Third, determine the central atom

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

Since sulfur is less electronegative than oxygen and fluorine, assume that the central atom is sulfur.

Therefore, place sulfur in the center and oxygen and fluorine on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 16 electron pairs. And four bonds are already marked. So we have to only mark the remaining twelve electron pairs as lone pairs on the sketch.

Also remember that sulfur is a period 3 element, so it can keep more than 8 electrons in its last shell. And both (oxygen 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 oxygens and fluorines.

So for each oxygen and each fluorine, there are three lone pairs, and for sulfur, there is zero lone pair because all twelve electron pairs are over.

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 sulfur atom, formal charge = 6 – 0 – ½ (8) = +2

For each oxygen atom, formal charge = 6 – 6 – ½ (2) = -1

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

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.

Convert a lone pair of the oxygen atom to make a new S — O bond with the sulfur atom as follows:

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:

Final structure

The final structure of SO₂F₂ involves a central sulfur atom connected to two oxygen atoms and two fluorine atoms. In this setup, the sulfur atom serves as an exception to the octet rule, utilizing an expanded valence shell to accommodate twelve electrons by forming double bonds with both oxygen atoms and single bonds with both fluorine atoms. Each oxygen atom fulfills its octet by retaining two lone pairs, while each fluorine atom maintains three lone pairs alongside its single bond. This arrangement is the most stable because it results in formal charges of zero for all atoms, representing the most energetically favorable state for the molecule. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of sulfuryl fluoride.

Next: POBr₃ Lewis structure

External links

• https://homework.study.com/explanation/draw-the-lewis-structure-for-so2f2-s-is-the-central-atom-give-the-number-of-electrons-in-each-species.html
• https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-diagram-so2f2-atoms-formal-charge-zero–b-draw-lewis-structure-so2f2-octet-rule-q16457477
• https://www.numerade.com/ask/question/a-draw-a-lewis-diagram-for-so2f2-in-which-all-atoms-have-a-formal-charge-of-zero-b-draw-a-lewis-structure-for-so2f2-in-which-the-octet-rule-is-satisfied-on-all-atoms-and-show-all-nonzero-for-16268/
• https://oneclass.com/homework-help/chemistry/7061153-lewis-structure-for-so2f2.en.html
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