SBR2 Lewis structure in 6 steps (with images) (2024)

So you've seen the photo above, right?

Let me explain the photo above briefly.

SBR2 Lewis structure has a sulfur atom (s) in the middle that is surrounded by two bromatomas (BR).

If you have not understood anything from the above image of SBR2 (sulfur pants) Lewis structure, hold me stuck and you will receive the detailed step -by -step explanation of the signing of a Lewis structure ofSBR2.

So let's go to the steps to drawLewis -Trut structuredoor SBR2.

Steps to draw SBR2 Lewis structure

Step 1: Find the total false electrons in SBR2 -Molecule

To find the totalValence electronsIn SBR2 (zwavel dibromid)Molecule, First and foremost you must know the valence electrons that are present in sulfuratomAs well as bromatoma.
(Valence electrons are the electrons that are present in the outerbaanof every atom.)

Here I will tell you how you can easily find valence electrons of sulfur and bromine using a periodic system.

Total false electrons in SBR2 -Molecule

→ Valence -Electrons given by sulfur atom:

Sulfur is a group 16 element on the periodic system.^[1]That is why valence electrons are present in sulfur6.

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

→ Valence electrons given by bromatoma:

Broma is a group 17 element on the periodic table.^[2]That is why valence electrons are present in moped7.

You can see the 7 valence electrons in the bromatoma as shown in the image above.

Therefore

Total false electrons in SBR2 -Molecule= Valence electrons given by 1 sulfur atom + valence electrons given by 2 mopeds =6 + 7 (2) = 20.

Step 2: Select the central atom

Remember to select the centratomaElectroegativeRemains in the middle.

Now it is the Given Molecule SBR2 (sulfur fibromide) and contains the sulfur atom (s) and bromatomas (BR).

You can see the electronegativity values for sulfur atom (s) and bromatoma (BR) in the periodic table above.

If we compare the electroegativity values for sulfur (s) and moped (BR), thenSulfurllatoma is less electronicgative.

So here is the sulfur atom (IS) the middle atom, and the mopeds (BR) are the outside atoms.

Step 3: Connect each atoms by placing an electron pair in between

Now you have to place in SBR2 -MoleculeElectron pairBetween sulfur atom (s) and bromatomas (BR).

This indicates that sulfur (s) and moped (BR) arechemicalTogether in an SBR2 molecule.

Step 4: Make the outer atoms stable.

Now check the stability of the outer atoms in this step.

Here in the sketch of SBR2 -Molecule you can see that the outer atoms are mopeds.

These outer mopeds form oneOctetAnd that is why they are stable.

In step 1 we also calculated the total number of valence electrons in the SBR2 molecule.

SBR2 -Molecule has in total20 Valence -ElectronsAnd only from this16 Valence -ElectronsUsed in the sketch above.

So the number of remaining electrons =20 - 16 = 4.

You have to place these4Electrons on the central sulfur atom in the above sketch of SBR2 molecule.

Now let's continue to the next step.

Step 5: Check the octet on the central atom

In this step, check whether the (s) central sulfur atom (s) is stable or not.

To arrange the stability of the central bromine (BR) atom, we must check whether it is an octet or not.

You can see from the image above that the sulfur atom forms an octet.

And so the central sulfur atom is stable.

Now let's continue to the last step to check whether the Lewis structure in SBR2 is stable or not.

Step 6: Check the stability of the Lewis structure

Now you have come to the last step where you have to check the stability of the Lewis structure of SBR2.

The stability of the Lewis structure can be checked using a concept ofFormal load.

In short, now you must find the formal charge of the atom of sulfur (s) and bromine (BR) atoms present in the SBR2 molecule.

Use the following formula to calculate formal charging;

Formal load = false electrons - (binding of electrons)/2 - non -binding electrons

You can see the numberElectronsInNon -binding electronsFor every atom of SBR2 molecule in the image below.

To sulfur (s) atom:
Valence -electrons = 6 (because sulfur is in group 16)
Glue electrons = 4
Non -binding electrons = 4

For Brom (BR) atom:
Valence -Electron = 7 (because Broom is in group 17)
Glue electrons = 2
Non -binding electrons = 6

From the above calculations of formal load you can see that sulfur (s) atom and bromine (br) atom one"NUL"Formal load.

This indicates that the Lewis structure of SBR2 above is stable and that there is no further change in the above structure of SBR2.

In the Lewis Dot structure of SBR2 above you can also display every binding electron pair (:) as a single binding (|).You get the next Lewis structure from SBR2.

I hope you have understood all the above steps.

For more practice and better understanding, try other Lewis structures listed below.

Try (or see at least) these Lewis structures for a better understanding: