Lewis structure of SBR2 (with 6 simple steps to draw!) (2024)

Lewis structure of SBR2 contains two single bonds between sulfur (s) atom and each bromine (BR) atom.

Let us draw and understand this Lewis Dot structure step by step.

(Remark:Take a pen and paper with you and try to draw this Lewis structure with me.I am sure you will be sure how to draw Lewis structure of SBR2).

6 steps to sign the Lewis structure of SBR2

Step # 1: Calculate the total number of valence electrons

Here is the given Molecule SBR2 (sulfur vesicles).To draw the Lewis structure in SBR2, you must first find the totalValence electronsPresent in the SBR2 molecule.
(Valence electrons are the number of electrons present in the outer scale of an atom).

So let's calculate this first.

Calculation of Valence -Electrons in SBR2

• For sulfur:

Sulfuris a group 16 element on the periodic table.^[1]

That is why valence electrons are present in sulfur6(See photo below).

• For moped:

Bromis a group 17 element on the periodic table.^[2]

That is why valence electrons are present in moped7(See photo below).

Hence in an SBR2 molecule,

Valence -electrons given by sulfur (s) atom =6
Valence -electrons given by every bromine (br) atom =7
Then the total number of valence electrons in SBR2 -Molecule = 6 + 7 (2) =20

Step # 2: Select the middle atom

Always place the least electronegative atom in the middle while choosing the atom.

(Peel: Fluoris the most electronic item onThe periodic systemAnd the electronegativity drops when we go to the left of the periodic system, as well as at the top to the bottom of the periodic table).[3]

Here in the SBR2 molecule, if we compare sulfur atom (s) and bromatoma (BR), thenSulfur is less electronicgative than hum.

So sulfur must be placed in the middle and the remaining 2 bromatomas will surround it.

Step # 3: Place two electrons between the atoms to display a chemical bond

Now in the above sketch of the SBR2 molecule, place the two electrons (ie.Electron pair) between each sulfur atom and bromatoma to represent aChemicalbetween them.

These couples of electrons present between sulfur (s) and bromine (BR) atoms form a chemical bond, which is bound together in an SBR2 molecule with each other in an SBR2 molecule.

Step 4: Fill in the octet (or nod) in outside atoms.

Just calmly, I explain!

In the Lewis structure of SBR2, the outer atoms are mopeds.

So now you have to completeOctetOn these mopeds (because Broom 8 requires electrons to have a full outer scale).

Now you can look at the image above that all mopeds form an octet.

When16 Valence -ElectronsSBR2 -Molecule is used in the above structure.

But there is total20 Valence -ElectronsIn SBR2 -Molecule (as calculated in step # 1).

So the number of remaining electrons must be kept at the central atom =20 - 16 = 4.

So let's keep these four electrons (ie 2 electron pairs) on the central atom.

Now let's go to the next step.

Step 5: Check whether the central atom has ocet or not.

In this step we must check whether the central atom (ie sulfur) has an octet or not.

In simple words, we have to check whether the central sulfur (s) has atom 8 electrons or not.

As you can see from the image above, the central atom (ie sulfur) has 8 electrons.

Step 6: Last step - Check the stability in the Lewis structure by calculating the formal charge on each atom

Now you have come to the last step and here you have to check itFormal loadon sulfurllatoma (s) as well as any bromatoma (BR).

Consider the formula for formal load;

Formal load = Valens electrons - Non -binding electrons - (binding of electrons)/2

• For sulfur:
  Valence -Erctone = 6 (as in group 16)
  Non -binding electrons = 4
  Glue electrons = 4
• For moped:
  Valence -Electron = 7 (as in group 17)
  Non -binding electrons = 6
  Glue electrons = 2

So you can see above that the formal loads are on sulfur and bromine "tribute”.

That is why there will be no change in the above structure and the Lewis structure of SBR2 above is only the final stable structure.

Every electron pair (:) In the Lewis Dot structure of SBR2 stands for the individual binding (|).

Related Lewis structures to your practice:
Lewis structure of HOCL
Lewis structure of C6H6 (Benzen)
Lewis structure of NBR3
Lewis structure of SEF4
Lewis structure of H3PO4

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