Chemical Bonding: ICl₅ Lewis Structure

Drawing the Lewis Structure for ICl₅

Viewing Notes:

• In ICl₅ Lewis structure Iodine (I) is the least electronegative atom and goes in the center of the Lewis structure.
• The ICl₅ Lewis structure you'll need to put more than eight valence electrons on the Iodine atom.
• In the Lewis structure for ICl₅ there are a total of 42 valence electrons.

Transcript: This is the ICl5 Lewis structure. For ICl5, we have a total of 42 valence electrons. We'll put the Iodine in the center, it's the least electronegative, and then we'll put the Chlorines on the outside. Next, we'll draw single bonds between the Iodine and the Chlorines to form chemical bonds. Each of these lines is two valence electrons, so we've used a total of 10 valence electrons at this point. Next, we'll complete the octet for the Chlorine atoms. So we have 10, 12, 14, and 40.

So we've used 40 valence electrons and we've filled the octets on all of the Chlorines, but we have 42 so we have two extra valence electrons. Since Iodine is in period 5 on the periodic table, it can hold more than 8 valence electrons. So let's take the remaining two and just put them right here on the Iodine. If you check the formal charges, you'll find that for each atom in ICl5, the formal charge is zero.

So this is the Lewis structure for ICl5. This is Dr. B., thanks for watching.