ClF Lewis structure

ClF (chlorine monofluoride) has one chlorine atom and one fluorine atom.

In the ClF Lewis structure, there is a single bond between the chlorine and fluorine atom, and on both chlorine and fluorine atoms, there are three lone pairs.

Alternative method: Lewis structure of ClF

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 ClF has one chlorine atom and one fluorine atom, so…

Valence electrons of one chlorine atom = 7 × 1 = 7
Valence electrons of one fluorine atom = 7 × 1 = 7

And the total valence electrons = 7 + 7 = 14

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

• Second, find the total electron pairs

We have a total of 14 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 = 14 ÷ 2 = 7

• 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.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 7 electron pairs. And one Cl — F bond is already marked. So we have to only mark the remaining six 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 atom is fluorine.

So for each atom, there are three 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 – 6 – ½ (2) = 0

For 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 ClF contains one chlorine atom and one fluorine atom connected by a single covalent bond. In this layout, both the chlorine and the fluorine atoms satisfy the octet rule by sharing one pair of electrons and maintaining three lone pairs each. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for both atoms, reflecting the most energetically favorable electronic distribution. Thus, this specific electronic distribution serves as the definitive and most accurate Lewis representation of chlorine monofluoride.

Next: SO Lewis structure

External video

• ClF Lewis Structure: How to Draw the Lewis Structure for ClF (Chlorine Monofluoride) – YouTube • Wayne Breslyn

External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/ClF-Lewis-structure.html
• https://lambdageeks.com/clf-lewis-structure/