Lewis structure of F2

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The Lewis structure of F₂ contains a single bond between the two fluorine atoms, and each fluorine atom has three lone pairs.

Steps

By using the following steps, you can easily draw the Lewis structure of F₂:

#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… fluorine is a group 17 element. Hence, fluorine has seven valence electrons.

Now F₂ has two fluorine atoms.

So the total number of valence electrons = valence electrons of fluorine atom × 2

Therefore, the total number of valence electrons = 7 × 2 = 14

• Now decide the central atom

There are two fluorine atoms in F₂. Hence, we can assume any one as the central atom. Let’s assume that right fluorine is the central atom.

So now, put two fluorines next to each other. And draw the rough skeleton structure for the Lewis structure of F₂ something like this:

Also read: How to draw Lewis structure of PO₄^3- (5 steps)

#2 Show Chemical Bond

Place two electrons between the atoms to show a chemical bond as follows:

Also read: How to draw Lewis structure of HCl (4 steps)

#3 Mark Lone Pairs

As calculated earlier, we have a total of 14 valence electrons. And in the above structure, we have already used two valence electrons. Hence, twelve valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs.

Note that fluorine is a period 2 element, so it can not 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 atom is left fluorine, so left fluorine will get three lone pairs. And the central atom (right fluorine) will also get three lone pairs.

So the Lewis structure of F₂ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (right fluorine), and also on the outside atom. 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 Lewis structure of ClO₂^– (5 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 each fluorine 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 F₂ looks something like this:

In the above structure, you can see that the formal charges of both fluorines are zero. Therefore, this is the stable Lewis structure of F₂.

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

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Related

• Lewis structure of PO₄^3-
• Lewis structure of HCl
• Lewis structure of ClO₂^–
• Lewis structure of H₂O₂
• Lewis structure of ClO₃^–

External links

• Chemical Bonding: F2 Lewis Structure – The Geoexchange
• F2 Lewis Structure in 6 Steps (With Images) – Pediabay
• Fluorine (F22) Molecule Lewis Structure – Chemistry School
• How to draw F2 Lewis Structure – Science Education and Tutorials
• F2 Lewis Structure, Molecular Geometry, Hybridization, Polarity, and MO Diagram – Techiescientist
• F2 Lewis Structure, Geometry – Kemicalinfo
• Lewis Dot of Difluoride F2 – Kent’s Chemistry
• F2 lewis structure – OneClass