Lewis structure of SO2Cl2

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The Lewis structure of SO₂Cl₂ contains two double bonds and two single bonds, with sulfur in the center, and two oxygens and two chlorines on either side. There are two lone pairs on each oxygen atom, three lone pairs on each chlorine atom, and the sulfur atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of SO₂Cl₂.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)
#5 Convert lone pair and calculate formal charge again (if formal charges are not closer to zero)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… both sulfur and oxygen are the group 16 elements, and chlorine is a group 17 element. Hence, both sulfur and oxygen have six valence electrons, and chlorine has seven valence electrons.

Now SO₂Cl₂ has one sulfur atom, two oxygen atoms, and two chlorine atoms.

So the total number of valence electrons = valence electrons of sulfur atom + (valence electrons of oxygen atom × 2) + (valence electrons of chlorine atom × 2)

Therefore, the total number of valence electrons = 6 + 12 + 14 = 32

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for sulfur, oxygen, and chlorine as follows:

Electronegativity value of sulfur = 2.58
Electronegativity value of oxygen = 3.44
Electronegativity value of chlorine = 3.16

Obviously, sulfur is less electronegative than oxygen and chlorine. Hence, assume that sulfur is the central atom.

So now, put sulfur in the center and two oxygens and two chlorines on either side. And draw the rough skeleton structure for the Lewis structure of SO₂Cl₂ something like this:

Also read: How to draw Lewis structure of C₄H₁₀ (3 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since sulfur is surrounded by two oxygens and two chlorines, use eight electrons to show four chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 32 valence electrons. And in the above structure, we have already used eight valence electrons. Hence, twenty-four valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-four valence electrons = twelve lone pairs.

Note that both (sulfur and chlorine) are the period 3 elements, so they can keep more than 8 electrons in their last shell. And oxygen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are two oxygens and two chlorines, so two oxygens and two chlorines will get three lone pairs. And the central atom (sulfur) will not get any lone pair, because all twelve lone pairs are used.

So the Lewis structure of SO₂Cl₂ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (sulfur), and also on the outside atoms. Therefore, the octet rule is satisfied.

Now calculate the formal charge and check the stability of the above structure.

Also read: How to draw ClO₂ Lewis structure (6 steps)

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

• For sulfur atom

Valence electrons = 6
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 6 – 0 – ½ (8) = +2

• For each oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

• For each chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of SO₂Cl₂ looks something like this:

In the above structure, you can see that the formal charges of atoms are not closer to zero. Therefore, convert lone pair and calculate formal charge again.

Also read: How to draw Lewis structure of SCl₄ (4 steps)

#5 Convert lone pair and calculate formal charge again

As mentioned earlier, sulfur is a period 3 element, so it can keep more than 8 electrons in its last shell.

So convert one lone pair from each oxygen atom to make a new bond with the sulfur atom. And then, the Lewis structure of SO₂Cl₂ looks something like this:

Now one last thing we need to do is, calculate the formal charge again and check the stability of the above structure.

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

• For sulfur atom

Valence electrons = 6
Nonbonding electrons = 0
Bonding electrons = 12

Formal charge = 6 – 0 – ½ (12) = 0

• For each oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

• For each chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of SO₂Cl₂ looks something like this:

In the above structure, you can see that the formal charges of all atoms are zero. Therefore, this is the stable Lewis structure of SO₂Cl₂.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

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Related

• Lewis structure of C₄H₁₀
• ClO₂ Lewis structure
• Lewis structure of SCl₄
• Lewis structure of SeO₃
• Lewis structure of H₂SO₃

External links

• SO2Cl2 Lewis Structure in 5 Steps (With Images) – Pediabay
• SO2Cl2 Lewis structure, Molecular geometry, and Polar or nonpolar – Topblogtenz
• SO2Cl2 (Sulfuryl chloride) Lewis Structure – Chemistry School
• What is the Lewis structure of SO2Cl2? – Quora
• Sulfuryl Chloride, SO2Cl Molecular Geometry & Polarity – Tutor-Homework.com
• What is the Lewis structure of SO2Cl2? – Homework.Study.com
• SO2Cl2 Lewis Structure (Sulfuryl Chloride) – Pinterest
• Lewis structure of SO2Cl2 – Laurence Lavelle
• Lewis structure of SO2Cl2 – Reddit
• Draw the Lewis Structure for SO2Cl2 – Chegg
• Draw a Lewis structure for SO2Cl2 in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms – Bartleby
• For this molecule, SO2Cl2, what is the formal charge of the central atom based on the Lewis resonance structure that obeyed the octet rule? – Brainly
• Draw the Lewis structure for SO2Cl2 – Numerade