F_{2} (fluorine) has **two fluorine** atoms. In the lewis structure of F_{2}, there is a single bond between the two fluorine atoms, and on each fluorine atom, there are three lone pairs.

## Steps

Here’s how you can draw the F_{2} lewis structure step by step.

Step #1: draw sketch

Step #2: mark lone pairs

Step #3: mark charges (if there are)

Let’s break down each step in detail.

### #1 Draw Sketch

- First, determine the total number of valence electrons

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

Since F_{2} has two fluorine atoms, so…

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

So the **total valence electrons** = 14

- 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 Mark Lone Pairs

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 Mark Charges

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.

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

Therefore, this structure is the stable lewis structure of F_{2}.

**Next:** CH_{2}Cl_{2} Lewis Structure