E represent the lone pair on the central atom, as per ICl2- lewis structure, iodine has three lone pairs.X represent the bonded atoms to the central atom, as we know, iodine is bonded with two chlorine atoms.A denotes the central atom, so, iodine is the central atom, A = Iodine.Check the stability with the help of a formal charge concept Now we will check the stability of the above structure with the help of a formal charge concept.Д¦. So, both atoms (iodine and chlorine) completed their octet and we use all the total valence electrons that are available for drawing the ICl2- lewis structure. But this is not the issue, some elements can violate the octet to gains stability. So, put these 6 remaining valence electrons around the iodine central atom.ДЄs we see in the above figure, the iodine central atom gets 10 electrons(6 represented as dot + 2 single bonds) in its outer shell and violates the octet rule. having more than 8 valence electrons in the outer shell, this is because iodine is below period two on the periodic table and have an extra d-orbital available hence, it has the ability to expand the octet. But the iodine atom already has 4 electrons in its octet because of two single bonds connected to it.Д«ut iodine atom can expand the octet i.e. We have 6 remaining valence electrons and iodine is the central atom that needs 8 electrons in its octet to attains stability. Complete central atom octet and make covalent bond if necessary So, we are left with only 6 valence electrons.ДҐ. In the above structure, (12 valence electrons represented as dots + 2 single bond that contains 4 electrons) are uses, hence, (12 + 4) = 16 valence electrons are used from total of 22 valence electron available for ICl2. Now count the remaining valence electrons. Hence, (one single bond + 6 valence electron as dots) means a total of 8 valence electrons are present around each chlorine atom, hence, both of them completed their octet comfortably.

This is because each chlorine atom already sharing two valence electrons with the help of a single bond.

providing 8 valence electrons in the outer shell of each chlorine atom.ДЄs you see in the above figure, we have place 6 valence electrons represented as dots around both sides chlorine atoms. Now start placing the remaining valence electrons on the outer atom(chlorine) to complete their octet i.e. Place remaining valence electrons starting from outer atom first

Sp3d bond angle