SeS3 Lewis structure

SeS₃ has one selenium atom and three sulfur atoms.

In SeS₃ Lewis structure, there are three double bonds around the selenium atom, with three sulfur atoms attached to it, and on each sulfur atom, there are two lone pairs.

Alternative method: Lewis structure of SeS₃

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, both selenium and sulfur lie in group 16.

Hence, both selenium and sulfur have six valence electrons.

Since SeS₃ has one selenium atom and three sulfur atoms, so…

Valence electrons of one selenium atom = 6 × 1 = 6
Valence electrons of three sulfur atoms = 6 × 3 = 18

And the total valence electrons = 6 + 18 = 24

Learn how to find: Selenium 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 selenium is less electronegative than sulfur, assume that the central atom is selenium.

Therefore, place selenium in the center and sulfurs on either side.

• And finally, draw the rough sketch

Lone pair

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

Also remember that selenium is a period 4 element, so it can keep more than 8 electrons in its last shell. And sulfur is a period 3 element, so it can also keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are sulfurs.

So for each sulfur, there are three lone pairs, and for selenium, 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 selenium atom, formal charge = 6 – 0 – ½ (6) = +3

For each sulfur atom, formal charge = 6 – 0 – ½ (6) = -1

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

The above structure is not a stable Lewis structure because both selenium 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 Se — S bond with the selenium atom as follows:

Since there are charges on selenium and sulfur atoms, again convert a lone pair of the sulfur atom to make a new Se — S bond with the selenium atom as follows:

There are still charges on selenium and sulfur atoms, so again convert a lone pair of the sulfur atom to make a new Se — S bond with the selenium atom as follows:

Final structure

The final structure of SeS₃ involves a central selenium atom connected to three sulfur atoms. In this setup, the selenium atom utilizes an expanded valence shell to accommodate twelve electrons, forming double bonds with all three sulfur atoms. Each sulfur atom fulfills its octet by retaining two lone pairs alongside the double bond. This arrangement is the most stable because it results in formal charges of zero for every atom in the molecule, as both selenium and sulfur contribute six valence electrons and “own” six in this configuration. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of SeS₃.

Next: IBr₅ Lewis structure

External links

• https://homework.study.com/explanation/draw-the-lewis-structure-for-ses3-what-is-the-hybridization-of-the-central-atom.html
• https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-structure-ses3-answer-following-questions-many-valence-electrons-present-compou-q1488686
• https://brainly.com/question/29594393
• https://oneclass.com/homework-help/chemistry/7040271-ses3-lewis-structure.en.html