Chemical Bonding: IF₅ Lewis Structure

Drawing the Lewis Structure for IF₅

Viewing Notes:

• In the IF₅ Lewis structure Iodine (I) is the least electronegative atom and goes in the center of the Lewis structure.
• The IF₅ Lewis structure you'll need to put more than eight valence electrons on the Iodine atom.
• In the Lewis structure for IF₅ there are a total of 42 valence electrons.

Transcript: This is the IF5 Lewis structure. For IF5, we have a total of 42 valence electrons. Iodine is the least electronegative. We'll put that at the center, and then we'll put Fluorines around the outside. Next, we'll draw a single bond between the Iodine and each of the Fluorines to form chemical bonds. So we've used a total of 2, 4, 6, 8, 10 valence electrons. Let's complete the octets for the Fluorines. So we have 10, 12, 14, and 40.

So we've used 40 valence electrons. We had 42 to start out with. All the Fluorines have octets. Iodine's in period 5 on the periodic table, so it can have more than eight valence electrons. So let's just put that last pair on the Iodine here. Now Iodine has 2, 4, 6, 8, 10, 12, but that's fine. If you check the formal charges for each of the atoms in this molecule, you'll find that they're zero.

So this is the Lewis structure for IF5. This is Dr. B., and thanks for watching.