SBr4 Lewis structure

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SBr₄ has one sulfur atom and four bromine atoms.

In SBr₄ Lewis structure, there are four single bonds around the sulfur atom, with four bromine atoms attached to it. Each bromine atom has three lone pairs, and the sulfur atom has one lone pair.

Steps

To properly draw the SBr₄ Lewis structure, follow these steps:

#1 Draw a rough sketch of the structure
#2 Next, indicate lone pairs on the atoms
#3 Indicate formal charges on the atoms, if necessary

Let’s break down each step in more detail.

#1 Draw a rough sketch of the structure

• First, determine the total number of valence electrons

In the periodic table, sulfur lies in group 16, and bromine lies in group 17.

Hence, sulfur has six valence electrons and bromine has seven valence electrons.

Since SBr₄ has one sulfur atom and four bromine atoms, so…

Valence electrons of one sulfur atom = 6 × 1 = 6
Valence electrons of four bromine atoms = 7 × 4 = 28

And the total valence electrons = 6 + 28 = 34

Learn how to find: Sulfur valence electrons and Bromine valence electrons

• Second, find the total electron pairs

We have a total of 34 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 = 34 ÷ 2 = 17

• Third, determine the central atom

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

Since sulfur is less electronegative than bromine, assume that the central atom is sulfur.

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

• And finally, draw the rough sketch

#2 Next, indicate lone pairs on the atoms

Here, we have a total of 17 electron pairs. And four S — Br bonds are already marked. So we have to only mark the remaining thirteen 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 bromine is a period 4 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 bromines.

So for each bromine, there are three lone pairs, and for sulfur, there is one lone pair.

Mark the lone pairs on the sketch as follows:

#3 Indicate formal charges on the atoms, if necessary

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 – 2 – ½ (8) = 0

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

Here, both sulfur and bromine atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (sulfur) forms an octet. And the outside atoms (bromines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of SBr₄.

Next: PF₃Cl₂ Lewis structure

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External links

• https://lambdageeks.com/sbr4-lewis-structure/
• https://homework.study.com/explanation/draw-the-lewis-structure-for-sbr4-and-provide-the-following-information-a-electron-geometry-b-molecular-geometry-c-hybridization-d-polarity.html
• https://sciedutut.com/sbr4-lewis-structure/
• https://www.chegg.com/homework-help/questions-and-answers/write-lewis-structure-sbr4-provide-answer-electron-pair-geometry-molecular-geometry-hybrid-q4694006