Is ICl5 Polar or Nonpolar? (And Why?)

ICl5 is a POLAR molecule.

But why? 

And how can you say that ICl5 is a polar molecule?

Want to know the reason?
Let’s dive into it!

ICl5 is a POLAR molecule because the I-Cl bonds present in the molecule are polar and it has asymmetric geometry which causes the partial positive (ẟ+) and partial negative (ẟ-) charge to appear on the molecule. These ẟ+ and ẟ- charges are responsible to make the entire ICl5 molecule polar.

Let me explain this in detail with the help of ICl5 lewis structure and its 3D geometry.

Why is ICl5 a Polar molecule? (Explained in 3 Steps)

ICl5 is a polar molecule because it has poles of partial positive charge (ẟ+) and partial negative charge (ẟ-) on it.

Let me explain this to you in 3 steps!

Step #1: Draw the lewis structure

Here is a skeleton of ICl5 lewis structure and it contains five I-Cl bonds.

(Note: If you want to know the steps of drawing the ICl5 lewis dot structure, then visit this article: ICl5 lewis structure, Or you can also watch this short 2 minute video).

So from the above diagram we have come to know that the ICl5 molecule has five I-Cl bonds.

Now in the next step we have to check whether these I-Cl bonds are polar or nonpolar.

And we also have to check the molecular geometry of ICl5.

Step #2: Check whether individual bonds are polar or nonpolar

The chemical bonds can be either nonpolar, polar or ionic depending on the difference of the electronegativity values (ΔEN) between the two atoms.

Have a look at the above image.

• If the electronegativity difference (ΔEN) is less than 0.4, then the bond is nonpolar covalent bond.
• If the electronegativity difference (ΔEN) is between 0.4 to 1.7, then the bond is polar covalent bond. 
• If the electronegativity difference (ΔEN) is greater than 1.7, then the bond is an ionic bond. ^{[1] [2] [3] [4]}

Now let’s come to the example of ICl5 molecule. It has five I-Cl bonds.

You can see the electronegativity values of Iodine (I) and Chlorine (Cl) atoms from the periodic table given below.

From the above image;

• Electronegativity of Iodine (I) = 2.66 ^[5]
• Electronegativity of Chlorine (Cl) = 3.16 ^[6]

Now let’s see the polarity of each bond.

For I-Cl bond;
The electronegativity difference (ΔEN) = 3.16 – 2.66 = 0.5
This value lies between 0.4 to 1.7, which indicates that the bond between Iodine (I) and Chlorine (Cl) is polar.
Hence, the I-Cl bonds are polar covalent bond.

You can see in the above image that because of higher electronegativity of Iodine atom, the partial positive charge (ẟ+) appears on the Iodine atom (I) and partial negative charge (ẟ-) appears on the Chlorine atoms (Cl).

But wait, we also have to look at the molecular geometry of ICl5 to know whether it has a symmetric shape or not.

Step #3: Check whether the molecule is symmetric or not

Have a look at this 3D structure of ICl5. The Iodine atom (I) is at the center and it is surrounded by 5 Chlorine atoms (Cl).

It also has one lone pair on the Iodine atom (I).

Due to the lone pair on the iodine atom (I), its molecular geometry becomes asymmetric.

Because of this, there are positive and negative poles of charges on the overall molecule of ICl5.

Hence, the ICl5 molecule is a polar molecule.

I hope you have understood the reason behind the polar nature of ICl5 molecule.

See the polarity of other molecules to make your concepts clear:
Is CO3 2- Polar or Nonpolar?
Is COF2 Polar or Nonpolar?
Is SeO3 Polar or Nonpolar?
Is Acetic acid (CH3COOH) Polar or Nonpolar?
Is H3O+ Polar or Nonpolar?