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1 solution
Relevant wiki: Lewis Structure
Iodine 7e. Chlorine 7e. 1 iodine plus 2 chlorine gives 21e plus the negative charge on the ion gives us a total of 22e.. the are two bonds... ie: Cl-I-Cl ( Least Electronegative Atom Goes to The Centre In Most Cases)... 2 bonds contain 4e..so subtract 4e from 22e which gives us a total of 18e that don't participate in bonding(lone e)..if you want, you can divide by two to give you the no of lone pair's. Start adding the lone pairs to the most Electronegative atom (in most cases again), 3 pairs max for each atom and you are left with the central atone which is Iodine with 2 bonds and 3 non bonding pairs of e... 5 VSEPR pairs of electrons( Lone pairs+bond pairs) and 3 Lone pairs which gives the linear shape to the whole ion. For more info check : Lewis Structure theory and VSEPR theory. Any tips on how I could change or improve my solution KINDLY WELCOME!