Lewis structure of CS2

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The Lewis structure of CS₂ contains two double bonds, with carbon in the center, and two sulfurs on either side. There are two lone pairs on each sulfur atom, and the carbon atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of CS₂:

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Complete octet on central atom
#5 Calculate formal charge and check stability

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… carbon is a group 14 element and sulfur is a group 16 element. Hence, carbon has four valence electrons and sulfur has six valence electrons.

Now CS₂ has one carbon atom and two sulfur atoms.

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

Therefore, the total number of valence electrons = 4 + 12 = 16

• 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 carbon and sulfur as follows:

Electronegativity value of carbon = 2.55
Electronegativity value of sulfur = 2.58

Obviously, carbon is less electronegative than sulfur. Hence, assume that carbon is the central atom.

So now, put carbon in the center and sulfurs on either side. And draw the rough skeleton structure for the Lewis structure of CS₂ something like this:

Also read: How to draw Lewis structure of NO (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since carbon is surrounded by two sulfurs, use four electrons to show two chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 16 valence electrons. And in the above structure, we have already used four valence electrons. Hence, twelve valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs.

Note that carbon is a period 2 element, so it can not keep more than 8 electrons in its last shell. And sulfur is period 3 element, so it can 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 sulfurs, so each sulfur will get three lone pairs. And the central atom (carbon) will not get any lone pair, because all six lone pairs are used.

So the Lewis structure of CS₂ looks something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (carbon) doesn’t form an octet.

So in the next step, we have to complete the octet on the central atom.

Also read: How to draw Lewis structure of NF₃ (4 steps)

#4 Complete octet on central atom

Remember that carbon is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Now carbon already has four valence electrons. Hence, carbon needs four more valence electrons to complete its octet.

So convert one lone pair from each sulfur atom to make a new bond with the carbon atom. And then, the Lewis structure of CS₂ looks something like this:

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

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

Also read: How to draw Lewis structure of PCl₃ (4 steps)

#5 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 carbon atom

Valence electrons = 4
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 4 – 0 – ½ (8) = 0

• For each sulfur atom

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

Formal charge = 6 – 4 – ½ (4) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of CS₂ looks something like this:

In the above structure, you can see that the formal charges of both (carbon and sulfur) are zero. Therefore, this is the stable Lewis structure of CS₂.

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

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Related

• Lewis structure of NO
• Lewis structure of NF₃
• Lewis structure of PCl₃
• Lewis structure of SF₆
• Lewis structure of CH₃OH

External video

• CS2 Lewis Structure: How to Draw the Lewis Structure for CS2 – YouTube • Wayne Breslyn

External links

• Chemical Bonding: CS2 Lewis Structure – The Geoexchange
• CS2 lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
• CS2 Lewis Structure in 6 Steps (With Images) – Pediabay
• CS2 Lewis Structure, Hybridization, Molecular Shape, and Polarity – Techiescientist
• CS2 Lewis Structure, Hybridization, Polarity and Molecular Shape – Geometry of Molecules
• CS2 Lewis Structure, Geometry – Kemicalinfo
• Lewis Structure for CS2 (Carbon Disulfide) – The University of Maryland
• Draw the Lewis structure for CS2 – Homework.Study.com
• How to draw CS2 Lewis Structure? – Science Education and Tutorials
• Carbon Disulfide Formula, Lewis Structure, Polar, Uses, MSDS – Chemistry Learner
• the lewis structure for CS2 is? – Chegg
• What is the molecular geometry of the CS2 molecule? – Socratic
• The Lewis Dot Structure for CS2 – MakeTheBrainHappy
• Carbon Disulfide, CS2 Molecular Geometry & Polarity – Tutor-Homework.com
• Write the Lewis structure for carbon disulfide (CS2) – OneClass
• Draw the Lewis structure of carbon disulfide CS2 – Quizlet
• What is the hybridization of CS2? – Quora
• Determine the number of bonding electrons and the number of nonbonding electrons in the structure of cs2 – Brainly