Chemical Bonding: ICl₃Lewis Structure

Drawing the Lewis Structure for ICl₃

Viewing Notes:

• In the ICl₃ Lewis structure Iodine (I) is the least electronegative atom and goes in the center of the Lewis structure.
• The ICl₃ Lewis structure you'll need to put more than eight valence electrons on the Iodine atom.
• In the Lewis structure for ICl₃ there are a total of 28 valence electrons.

Transcript: This is the ICl3 Lewis structure. For ICl3, we have 7 valence electrons for Iodine; 7 for Chlorine, but we have three Chlorines; a total of 28 valence electrons. I is the least electronegative, put that in the center, and then Chlorines will go around it. Put two electrons between the atoms to form chemical bonds. We used 6. Then around the outside, 8, 24, and then we'll put the remaining ones on the Iodine, 26, and 28. Iodine's in period 4, so it's OK for it to violate the octet rule and have more than eight valence electrons. So we've used all 28 valence electrons. The Chlorines have octets. The Iodine has an octet, plus some.

And we're done. That is the ICl3 Lewis structure. This is Dr. B., and thanks for watching.