F2 Lewis structure

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F₂ (fluorine) has two fluorine atoms.

In the F₂ Lewis structure, there is a single bond between the two fluorine atoms, and on each fluorine atom, there are three lone pairs.

Steps

To properly draw the F₂ Lewis structure, follow these steps:

#1 Draw a rough sketch of the structure
#2 Next, indicate lone pairs on the atoms
#3 Indicate formal charges on the atoms, if necessary

Let’s break down each step in more detail.

#1 Draw a rough sketch of the structure

• First, determine the total number of valence electrons

In the periodic table, fluorine lies in group 17. Hence, fluorine has seven valence electrons.

Since F₂ has two fluorine atoms, so…

Valence electrons of two fluorine atoms = 7 × 2 = 14

So the total valence electrons = 14

Learn how to find: 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

Here, there are only two atoms and both atoms are fluorine, so we can assume any one as the central atom.

Let’s assume that the central atom is right fluorine.

• And finally, draw the rough sketch

#2 Next, indicate lone pairs on the atoms

Here, we have a total of 5 electron pairs. And one F — 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 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 left fluorine.

So for each fluorine, there are three lone pairs.

Mark the lone pairs on the sketch as follows:

#3 Indicate formal charges on the atoms, if necessary

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

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

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

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

In the above structure, you can see that the central atom (right fluorine) forms an octet. And the outside atom (left fluorine) also forms an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of F₂.

Next: CH₂Cl₂ Lewis structure

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External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/F2-lewis-structure.html
• https://techiescientist.com/f2-lewis-structure/
• https://www.chemistryscl.com/general/F2-lewis-structure/
• https://lambdageeks.com/f2-lewis-structure/
• https://sciedutut.com/f2-lewis-structure/