The **Lewis structure of ICl _{5}** contains five single bonds, with iodine in the center, and five chlorines on either side. There are three lone pairs on each chlorine atom, and one lone pair on the iodine atom.

## Steps

By using the following steps, you can easily draw the Lewis structure of ICl_{5}.

#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… both iodine and chlorine are the group 17 elements. Hence, both iodine and chlorine have **seven** valence electrons.

Now ICl_{5} has one iodine atom and five chlorine atoms.

So the total number of valence electrons = valence electrons of iodine atom + (valence electrons of chlorine atom × 5)

Therefore, the **total number of valence electrons** = 7 + 35 = 42

- Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for iodine and chlorine as follows:

Electronegativity value of iodine = 2.66

Electronegativity value of chlorine = 3.16

Obviously, iodine is less electronegative than chlorine. Hence, assume that **iodine is the central atom**.

So now, put iodine in the center and chlorines on either side. And draw the rough skeleton structure for the Lewis structure of ICl_{5} something like this:

**Also read:** How to draw Lewis structure of C_{6}H_{6} (5 steps)

### #2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since iodine is surrounded by five chlorines, use ten electrons to show **five chemical bonds** as follows:

**Also read:** How to draw Lewis structure of SBr_{2} (4 steps)

### #3 Mark lone pairs

As calculated earlier, we have a total of 42 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, thirty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty-two valence electrons = **sixteen lone pairs**.

Note that iodine is a period 5 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 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 atoms are chlorines, so each chlorine will get three lone pairs. And the central atom (iodine) will get one lone pair.

So the Lewis structure of ICl_{5} looks something like this:

In the above structure, you can see that the octet is completed on the central atom (iodine), and also on the outside atoms. 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 NBr_{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 – ½ bonding electrons

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

- For
**iodine**atom

Valence electrons = 7

Nonbonding electrons = 2

Bonding electrons = 10

Formal charge = 7 – 2 – ½ (10) = 0

- For
**each chlorine**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 ICl_{5} looks something like this:

In the above structure, you can see that the formal charges of both (iodine and chlorine) are zero. Therefore, this is the **stable Lewis structure of ICl**** _{5}**.

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

## Related

- Lewis structure of C
_{6}H_{6} - Lewis structure of SBr
_{2} - Lewis structure of NBr
_{3} - Lewis structure of HOCl
- Lewis structure of SeF
_{4}

## External links

- ICl5 Lewis Structure, Geometry, Hybridization, and Polarity – Techiescientist
- Drawing the Lewis Structure for ICl5 – The Geoexchange
- ICl5 Lewis Structure in 5 Steps (With Images) – Pediabay
- ICL5 lewis structure: Drawings, Hybridization, Shape, Charges, Pairs – Lambda Geeks
- ICl5 Lewis Structure (Iodine Pentachloride) – Pinterest
- Draw the best Lewis structure for ICl5 – Chegg
- Iodine Pentachloride, ICl5 Molecular Geometry & Polarity – Tutor-Homework.com
- Draw and explain the Lewis structure for ICl5 – Homework.Study.com
- Draw the best Lewis structure for ICl5 – Brainly

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.