Lewis structure of CF3Cl

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The Lewis structure of CF₃Cl contains four single bonds, with carbon in the center, and three fluorines and one chlorine on either side. There are three lone pairs on each fluorine atom and chlorine 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 CF₃Cl.

#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)

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 both fluorine and chlorine are the group 17 elements. Hence, carbon has four valence electrons, and both fluorine and chlorine have seven valence electrons.

Now CF₃Cl has one carbon atom, three fluorine atoms, and one chlorine atom.

So the total number of valence electrons = valence electrons of carbon atom + (valence electrons of fluorine atom × 3) + valence electrons of chlorine atom

Therefore, the total number of valence electrons = 4 + 21 + 7 = 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 carbon, fluorine, and chlorine as follows:

Electronegativity value of carbon = 2.55
Electronegativity value of fluorine = 3.98
Electronegativity value of chlorine = 3.16

Obviously, carbon is less electronegative than fluorine and chlorine. Hence, assume that carbon is the central atom.

So now, put carbon in the center and fluorines and chlorine on either side. And draw the rough skeleton structure for the Lewis structure of CF₃Cl something like this:

Also read: How to draw Lewis structure of XeCl₃^– (4 steps)

#2 Show chemical bond

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

Also read: How to draw Lewis structure of XeF₃^– (4 steps)

#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 (carbon and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell. And chlorine is a 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 fluorines and chlorine, so each fluorine and chlorine will get three lone pairs. And the central atom (carbon) will not get any lone pair, because all twelve lone pairs are used.

So the Lewis structure of CF₃Cl 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 XeF₃⁺ Lewis structure (4 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 carbon atom

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

Formal charge = 4 – 0 – ½ (8) = 0

• For each fluorine atom

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

Formal charge = 7 – 6 – ½ (2) = 0

• For 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 CF₃Cl 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 CF₃Cl.

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

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Related

• Lewis structure of XeCl₃^–
• Lewis structure of XeF₃^–
• XeF₃⁺ Lewis structure
• Lewis structure of CHF₃
• Lewis structure of XeF₅⁺

External links

• CF3Cl Lewis Structure in 6 Steps (With Images) – Pediabay
• Draw the Lewis structure for CF3Cl. Is it polar or nonpolar? – Homework.Study.com
• Chlorotrifluoromethane | CF3Cl | CID 6392 – National Institutes of Health (.gov)
• What is the molecular geometry of CF3Cl? – Answers
• CF3Cl (Chlorotrifluoromethane) Oxidation Number – ChemicalAid