ClF3 Lewis structure

ClF₃ (chlorine trifluoride) has one chlorine atom and three fluorine atoms.

In the ClF₃ Lewis structure, there are three single bonds around the chlorine atom, with three fluorine atoms attached to it. Each fluorine atom has three lone pairs, and the chlorine atom has two lone pairs.

Alternative method: Lewis structure of ClF₃

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, both chlorine and fluorine lie in group 17.

Hence, both chlorine and fluorine have seven valence electrons.

Since ClF₃ has one chlorine atom and three fluorine atoms, so…

Valence electrons of one chlorine atom = 7 × 1 = 7
Valence electrons of three fluorine atoms = 7 × 3 = 21

And the total valence electrons = 7 + 21 = 28

Learn how to find: Chlorine valence electrons and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 28 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 28 ÷ 2 = 14

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since chlorine is less electronegative than fluorine, assume that the central atom is chlorine.

Therefore, place chlorine in the center and fluorines on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 14 electron pairs. And three Cl — F bonds are already marked. So we have to only mark the remaining eleven electron pairs as lone pairs on the sketch.

Also remember that chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell. And fluorine is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are fluorines.

So for each fluorine, there are three lone pairs, and for chlorine, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

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

For chlorine atom, formal charge = 7 – 4 – ½ (6) = 0

For each fluorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, both chlorine and fluorine atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of ClF₃ features a central chlorine atom connected to three fluorine atoms through single covalent bonds. In this configuration, the chlorine atom utilizes an expanded valence shell to accommodate ten electrons, which include three bonding pairs and two lone pairs. Within this layout, each of the three fluorine atoms satisfies the octet rule by maintaining three lone pairs alongside its single shared bond. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved, including the central chlorine and all three fluorine atoms. Therefore, this specific electronic distribution serves as the definitive and most accurate Lewis representation of chlorine trifluoride.

Next: Cl₂ Lewis structure

External video

• ClF3 Lewis Structure – How to Draw the Lewis Structure for ClF3 – YouTube • Wayne Breslyn

External links

• https://techiescientist.com/clf3-lewis-structure/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/ClF3-lewis-structure.html
• https://geometryofmolecules.com/clf3-lewis-structure-molecular-structure-hybridization-bond-angle-and-shape/
• https://topblogtenz.com/chlorine-trifluoride-clf3-lewis-dot-structure-and-molecular-geometry/
• https://lambdageeks.com/clf3-lewis-structure/