The **Lewis structure of I _{2}** contains a single bond between the two iodine atoms, and each iodine atom has three lone pairs.

## Steps

By using the following steps, you can easily draw the Lewis structure of I_{2}.

#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)

Letâ€™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.

- Letâ€™s calculate the total number of valence electrons

We know thatâ€¦ iodine is a group 17 element. Hence, iodine has **seven** valence electrons.

Now I_{2} has two iodine atoms.

So the total number of valence electrons = valence electrons of iodine atom Ã— 2

Therefore, the **total number of valence electrons** = 7 Ã— 2 = 14

- Now decide the central atom

There are two iodine atoms in I_{2}. Hence, we can assume any one as the central atom. Letâ€™s assume that **right iodine is the central atom**.

So now, put two iodines next to each other. And draw the rough skeleton structure for the Lewis structure of I_{2} something like this:

**Also read:** How to draw Lewis structure of C_{3}H_{8} (3 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 IF_{4}^{–} (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 iodine is a period 5 element, so it can 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 iodine, so left iodine will get three lone pairs. And the central atom (right iodine) will also get three lone pairs.

So the Lewis structure of I_{2} looks something like this:

In the above structure, you can see that the octet is completed on the central atom (right iodine), 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 ICl_{3} (4 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 – Â½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

- For
**each iodine**atom

Valence electrons = 7

Nonbonding electrons = 6

Bonding electrons = 2

Formal charge = 7 – 6 – Â½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of I_{2} looks something like this:

In the above structure, you can see that the formal charges of both iodines are zero. Therefore, this is the **stable Lewis structure of I**** _{2}**.

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

## Related

- Lewis structure of C
_{3}H_{8} - Lewis structure of IF
_{4}^{–} - Lewis structure of ICl
_{3} - Lewis structure of ClF
_{5} - Lewis structure of SF
_{3}^{–}

## External links

- Iodine (I2) Molecule Lewis Structure – Chemistry School
- I2 Lewis Structure in 6 Steps (With Images) – Pediabay
- Chemical Bonding: I2 Lewis Structure – The Geoexchange
- I2 Lewis Structure (Iodine Gas) – Pinterest
- Write Lewis formulas for the following: H2, N2, I2, HCl, HI – Homework.Study.com
- Draw the Lewis dot structure of Iodine (I2) – Chegg
- How to draw I2 Lewis structure – Science Education and Tutorials
- How many electrons are shown in the electron dot structures of iodine? – Answers

Deep

Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.