This is the ICl2 Lewis structure. Iodine has 7 valence electrons, Chlorine has 7 as well, but there are two of those and then we need to add an extra electron right there. That generates us a total of 22 valence. Electrons Iodine is the least electronegative. We’ll articulate that in the center Put the Chlorines on either side. Then we’ll put two electrons between atoms to use chemical bonds, that’s 2 4 and then around the outside 6. 8. 10. 12. 14. 16. So we’ve ill-used 16. We have six left, so we’ll have to gave three duets on this Iodine now That’s. Ok, because Iodine is in group 4 and it can hold more than eight valence electrons. So we’ll place two pairs up now and one down here. So we’ve exploited all 22 valence electrons, The Chlorines they have octets and the Iodine it’s. Ok, It has more than eight but being in period 4 that’s fine. So this is the Lewis structure for ICl2. If you check the formal bills, you’ll note that there is a negative charge on the Iodine and the Chlorines both have a formal fee of zero. Since we do have a negative charge now, this negative charge represents impression. We should throw brackets around this molecule to show that it is an ion And we’ll articulated our negative price right there and we’re done That’s, the Lewis structure for ICl2. This is Dr B and thanks for watching.