CF2S Lewis structure

CF₂S has one carbon atom, two fluorine atoms, and one sulfur atom.

In CF₂S Lewis structure, there are two single bonds and one double bond around the sulfur atom, with two fluorine atoms and one sulfur atom attached to it. Each fluorine atom has three lone pairs, and the sulfur atom has two lone pairs.

Alternative method: Lewis structure of CF₂S

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, fluorine lies in group 17, and sulfur lies in group 16.

Hence, carbon has four valence electrons, fluorine has seven valence electrons, and sulfur has six valence electrons.

Since CF₂S has one carbon atom, two fluorine atoms, and one sulfur atom, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of two fluorine atoms = 7 × 2 = 14
Valence electrons of one sulfur atom = 6 × 1 = 6

And the total valence electrons = 4 + 14 + 6 = 24

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

• 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 carbon is less electronegative than fluorine and sulfur, assume that the central atom is carbon.

Therefore, place carbon in the center and fluorines and sulfur on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 12 electron pairs. And three bonds are already marked. So we have to only mark the remaining nine electron pairs as lone pairs on the sketch.

Also remember that both (carbon and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell. And sulfur is a period 3 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are fluorines and sulfur.

So for each fluorine and sulfur, there are three lone pairs, and for carbon, there is zero lone pair because all nine 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 carbon atom, formal charge = 4 – 0 – ½ (6) = +1

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

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

Here, both carbon and sulfur atoms have charges, so mark them on the sketch as follows:

The above structure is not a stable Lewis structure because both carbon and sulfur atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.

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

Final structure

The final structure of CF₂S comprises a central carbon atom linked to one sulfur atom and two fluorine atoms. In this arrangement, the carbon atom satisfies the octet rule by forming a double covalent bond with the sulfur atom and single covalent bonds with each fluorine atom, leaving no lone pairs on the carbon. Within this layout, the sulfur atom maintains two lone pairs alongside its double bond, and each fluorine atom successfully reaches a stable octet by retaining three lone pairs alongside its single shared bond. This configuration represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Thus, this specific electronic distribution serves as the definitive and most accurate Lewis representation of CF₂S.

Next: PI₅ Lewis structure

External video

• CF2S Lewis Structure: How to Draw the Lewis Structure for CF2S – YouTube • Wayne Breslyn

External links

• https://www.numerade.com/ask/question/draw-the-lewis-electronic-dot-structure-for-the-following-molecule-cf2s-83201/
• https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-electronic-dot-structure-following-molecule-cf2s-q42954697