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According to the answer in the textbook, Iodine forms a single bond with oxygen. My question is why can't Iodine form double bonds with all three oxygen molecules? In the end, I still managed to have a VSEPR of Ax3E with a trigonal pyramid shape, less than 109.5
It has to do with the formal charge stability. In the photo the charge of I is 2 and the charge of O is -1 for a total charge of -1. In the case of double bonds I is a charge of -1 and O is 0 which is a total charge of -1. The reason why Iodine should not have a charge of -1 and is less stable is because Oxygen is more electronegative than Iodine so Oxygen is the preferred atom in this case to hold a negative charge, in this case -1. It's more stable if Iodine does not have a charge of -1.
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