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In Lewis Structure for ICl2-, why does I (Iodine) get the extra electron and not Chlorine....

In Lewis Structure for ICl2-, why does I (Iodine) get the extra electron and not Chlorine. Iodine is less electronegative, it has a larger ion size, both Cl and I are one electron away from an octet, and they can both hold more electrons than 8 because Iodine is in Period 5 while Cl is in Period 3. I understand how the Lewis structure looks, but I am wondering why Iodine gets that extra electron. What is the rule in this case with regards to that extra electron that results from a charge of (-) that I can apply to other compounds?

This is my first question I posted and if someone could really break it down for me that would be awesome. Thank you very much.

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