CH2F2 Lewis structure

CH₂F₂ (difluoromethane) has one carbon atom, two hydrogen atoms, and two fluorine atoms.

In the CH₂F₂ Lewis structure, there are four single bonds around the carbon atom, with two hydrogen atoms and two fluorine atoms attached to it, and on each fluorine atom, there are three lone pairs.

Alternative method: Lewis structure of CH₂F₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, hydrogen lies in group 1, and fluorine lies in group 17.

Hence, carbon has four valence electrons, hydrogen has one valence electron, and fluorine has seven valence electrons.

Since CH₂F₂ has one carbon atom, two hydrogen atoms, and two fluorine atoms, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of two hydrogen atoms = 1 × 2 = 2
Valence electrons of two fluorine atoms = 7 × 2 = 14

And the total valence electrons = 4 + 2 + 14 = 20

Learn how to find: Carbon valence electrons, Hydrogen valence electrons, and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 20 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 = 20 ÷ 2 = 10

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from carbon and fluorine. Place the least electronegative atom at the center.

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

Therefore, place carbon in the center and hydrogen and fluorine on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 10 electron pairs. And four bonds are already marked. So we have to only mark the remaining six electron pairs as lone pairs on the sketch.

Also remember that both (carbon and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell. And hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogens and fluorines. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for each fluorine, there are three lone pairs, and for carbon, there is zero lone pair because all six electron pairs are over.

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 carbon atom, formal charge = 4 – 0 – ½ (8) = 0

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

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

Here, the atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of CH₂F₂ consists of a central carbon atom linked to two hydrogen atoms and two fluorine atoms through single covalent bonds. In this configuration, the carbon atom satisfies the octet rule by forming four total bonds, while each fluorine atom fulfills its octet by maintaining three lone pairs alongside its single shared bond. Within this layout, both hydrogen atoms achieve their stable duet state through their respective single bonds. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of difluoromethane.

Next: CH₃^– Lewis structure

External video

• CH2F2 Lewis Structure – How to Draw the Lewis Structure for CH2F2 – YouTube • Wayne Breslyn

External links

• https://techiescientist.com/ch2f2-lewis-structure/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/CH2F2-lewis-structure.html
• https://geometryofmolecules.com/ch2f2-lewis-structure-hybridization-molecular-structure-bond-angles/
• https://topblogtenz.com/ch2f2-lewis-structure-molecular-geometry-hybridization-bond-angle/
• https://lambdageeks.com/ch2f2-lewis-structure/
• https://sciedutut.com/ch2f2-lewis-structure/