![]() Let us study the VSEPR theory to predict the shape of iodine trichloride.Īs per VSEPR theory, the number of bonded (bond pair) and non-bonded (lone pair) valence shell electrons determine the shape and molecular geometry of the molecule. It is well understood by the valence shell electron pair repulsion (VSEPR) theory. We cannot predict the shape and molecular geometry of iodine trichloride from the Lewis structure. So, the Lewis structure of the iodine trichloride can also be represented as: The one shared electron pair represents the single bond. Therefore, these elements can be surrounded by more than eight electrons. It is one of the exceptions of the octet rule, i.e., the elements of the third period or beyond the third period of the periodic table have 3d electrons for bonding. We can observe that every chlorine atom is surrounded by eight electrons but a central atom, iodine, is surrounded by ten electrons. Hence, the Lewis structure of iodine trichloride would be: In the skeletal structure of ICl3, Iodine will be the central atom and all three chlorine atoms will surround it. The total number of valence electron are = 28 electrons. Hence, both of the atoms have seven valence electrons. ![]() The electronic configuration of I and Cl is 4d105s25p5 and 3s23p5, respectively.
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