# What would be the structure of ICl_2^(-) ion?

There are $3 \times {7}_{\text{valence electrons"+1_"negative charge"=22*"electrons}}$ to arrange over three centres. And, typically, we put the LEAST electronegative atom centrally...
And so....$C l - I - C l$, from left to right, chlorine has 1 bonding pair and bears 3 lone pairs, iodine has 2 bonding pairs, and bears 3 lone pairs, and the terminal chlorine has bonding pair and bears 3 lone pairs, as before.