SBr4 Lewis Structure in 5 Steps (With Images) (2024)

SBr4 Lewis Structure in 5 Steps (With Images) (1)

So you have seen the above image by now, right?

Let me explain the above image in short.

SBr4 lewis structure has a Sulfur atom (S) at the center which is surrounded by four Bromine atoms (Br). There are 4 single bonds between the Sulfur atom (S) and each Bromine atom (Br). There is 1 lone pair on the Sulfur atom (S) and 3 lone pairs on all the four Bromine atoms (Br).

If you haven’t understood anything from the above image of SBr4 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of SBr4.

So let’s move to the steps of drawing the lewis structure of SBr4.

Steps of drawing SBr4 lewis structure

Step 1: Find the total valence electrons in SBr4 molecule

In order to find the total valence electrons in SBr4 molecule, first of all you should know the valence electrons present in sulfur atom as well as bromine atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of sulfur as well as bromine using a periodic table.

Total valence electrons in SBr4 molecule

→ Valence electrons given by sulfur atom:

SBr4 Lewis Structure in 5 Steps (With Images) (2)

Sulfur is a group 16 element on the periodic table. [1] Hence the valence electrons present in sulfur is 6.

SBr4 Lewis Structure in 5 Steps (With Images) (3)

You can see the 6 valence electrons present in the sulfur atom as shown in the above image.

→ Valence electrons given by bromine atom:

SBr4 Lewis Structure in 5 Steps (With Images) (4)

Bromine is a group 17 element on the periodic table. [2] Hence the valence electrons present in bromine is 7.

SBr4 Lewis Structure in 5 Steps (With Images) (5)

You can see the 7 valence electrons present in the bromine atom as shown in the above image.

Hence,

Total valence electrons in SBr4 molecule = valence electrons given by 1 sulfur atom + valence electrons given by 4 bromine atoms = 6 + 7(4) = 34.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

Now here the given molecule is SBr4 and it contains sulfur atom (S) and bromine atoms (Br).

SBr4 Lewis Structure in 5 Steps (With Images) (6)

You can see the electronegativity values of sulfur atom (S) and bromine atom (Br) in the above periodic table.

If we compare the electronegativity values of sulfur (S) and bromine (Br) then the sulfur atom is less electronegative.

So here the sulfur atom (S) is the center atom and the bromine atoms (Br) are the outside atoms.

SBr4 Lewis Structure in 5 Steps (With Images) (7)

Step 3: Connect each atoms by putting an electron pair between them

Now in the SBr4 molecule, you have to put the electron pairs between the sulfur atom (S) and bromine atoms (Br).

SBr4 Lewis Structure in 5 Steps (With Images) (8)

This indicates that the sulfur (S) and bromine (Br) are chemically bonded with each other in a SBr4 molecule.

Step 4: Make the outer atoms stable

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of SBr4 molecule, you can see that the outer atoms are bromine atoms.

These outer bromine atoms are forming an octet and hence they are stable.

SBr4 Lewis Structure in 5 Steps (With Images) (9)

Also, in step 1 we have calculated the total number of valence electrons present in the SBr4 molecule.

The SBr4 molecule has a total 34 valence electrons and out of these, only 32 valence electrons are used in the above sketch.

So the number of electrons which are left = 34 – 32 = 2.

You have to put these 2 electrons on the central sulfur atom in the above sketch of SBr4 molecule.

SBr4 Lewis Structure in 5 Steps (With Images) (10)

Now let’s proceed to the next step.

Step 5: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of SBr4.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on sulfur (S) atom as well as bromine (Br) atoms present in the SBr4 molecule.

For calculating the formal charge, you have to use the following formula;

Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons

You can see the number of bonding electrons and nonbonding electrons for each atom of SBr4 molecule in the image given below.

SBr4 Lewis Structure in 5 Steps (With Images) (11)

For Sulfur (S) atom:
Valence electrons = 6 (because sulfur is in group 16)
Bonding electrons = 8
Nonbonding electrons = 2

For Bromine (Br) atom:
Valence electron = 7 (because bromine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge=Valence electrons(Bonding electrons)/2Nonbonding electrons
S=68/22=0
Br=72/26=0

From the above calculations of formal charge, you can see that the sulfur (S) atom as well as bromine (Br) atom has a “zero” formal charge.

This indicates that the above lewis structure of SBr4 is stable and there is no further change in the above structure of SBr4.

In the above lewis dot structure of SBr4, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of SBr4.

SBr4 Lewis Structure in 5 Steps (With Images) (12)

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

CFCl3 Lewis StructureNCl2- Lewis Structure
AsCl5 Lewis StructureCOBr2 Lewis Structure
GeF4 Lewis StructureCl2O2 Lewis Structure

About author

Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.

Read more about our Editorial process.

SBr4 Lewis Structure in 5 Steps (With Images) (2024)

FAQs

What is the geometric shape of SBr4? ›

Electron geometry: In sulfur tetrabromide, there are 4 Br atoms and 1 lone pair that means 5 electron groups around the central atom sulfur. Therefore, the electron geometry of S B r 4 is trigonal bipyramidal.

What is the shape of SiBr4? ›

Si⁴⁺ is bonded in a tetrahedral geometry to four equivalent Br¹⁻ atoms. There is one shorter (2.19 Å) and three longer (2.20 Å) Si-Br bond lengths.

What are the 4 steps of Lewis structure? ›

Step 1: Determine the total number of valence electrons. Step 2: Write the skeleton structure of the molecule. Step 3: Use two valence electrons to form each bond in the skeleton structure. Step 4: Try to satisfy the octets of the atoms by distributing the remaining valence electrons as nonbonding electrons.

What is the Lewis structure short answer? ›

A Lewis Structure is a very simplified representation of the valence shell electrons in a molecule. It is used to show how the electrons are arranged around individual atoms in a molecule. Electrons are shown as "dots" or for bonding electrons as a line between the two atoms.

Is SBr4 polar or nonpolar? ›

Re: Intermolecular forces. SBr4 is a nonpolar molecule because the central atom (S) is surrounded by 4 identical (Br) molecules that are equivalent in their electronegativity, so the dipoles cancel each other out, and as a result, there is no dipole-dipole interaction.

Does SBr4 exist? ›

The compound SbR4 does not exist as a stable chemical entity. However, the question likely refers to SbBr4, which would be antimony(III) bromide if the formula were correct and a halide existed in that stoichiometry. Antimony is a metalloid, and when combined with bromine, a halogen, it forms a chemical compound.

How many bonds will be formed in the compound SiBr4? ›

Refer to the given Lewis structure of S i B r 4 . Based on this structure, the central Si atom has four bonds and zero lone pairs while each Br atom has one bond and three lone pairs.

What is the name for SBr4? ›

SBr4 Lewis Structure | How to Draw the Lewis Structure for SBr4 (Sulphur Tetrabromide) SBr4 is a chemical formula for Sulphur Tetrabromide.

How many valence electrons does SBr4 have? ›

Explanation: And so we got SBr4 , i.e. 6sulfur+4×7bromine=34⋅valence electrons ... 17 electrons pairs to distribute by VESPER... Electronic geometry around sulfur is thus trigonal bipyramidal to a first approx.

What is the octet rule of SBr4? ›

Explanation: The compound SBr4 has a molecular formula of SBr4. The Lewis structure of SBr4 shows that there are 32 valence electrons (4 from sulfur, 7 each from the 4 bromine atoms and an additional electron to account for the violation of the octet rule by sulfur).

What is the total number of valence electrons in a SBr4 molecule? ›

Explanation: And so we got SBr4 , i.e. 6sulfur+4×7bromine=34⋅valence electrons ...

What is the correct name for SBr4? ›

SBr4 is a chemical formula for Sulphur Tetrabromide molecule.

What is the molecular shape of SBr42+? ›

SBr42+ is a cation with a central sulfur atom bonded to four bromine atoms. It does not have any lone pairs of electrons, making it a tetrahedral shape.

References

Top Articles
Latest Posts
Recommended Articles
Article information

Author: Nicola Considine CPA

Last Updated:

Views: 6043

Rating: 4.9 / 5 (49 voted)

Reviews: 88% of readers found this page helpful

Author information

Name: Nicola Considine CPA

Birthday: 1993-02-26

Address: 3809 Clinton Inlet, East Aleisha, UT 46318-2392

Phone: +2681424145499

Job: Government Technician

Hobby: Calligraphy, Lego building, Worldbuilding, Shooting, Bird watching, Shopping, Cooking

Introduction: My name is Nicola Considine CPA, I am a determined, witty, powerful, brainy, open, smiling, proud person who loves writing and wants to share my knowledge and understanding with you.