# In the Lewis structure of ICL_2^-, how many lone pairs of electrons are around the iodine atom?

Why $\text{three}$!
For $I C {l}_{2}^{-}$, there are $21 + 1$ valence electrons, i.e. $11$ electron pairs to distribute around the three halogens. The iodine atom is presumed to be central, with 2 bonding pairs, and 3 lone pairs. The geometry of electron pairs is presumed to be trigonal bipyramidal, but because we describe the structure based on atoms, not on electron pairs, $I C {l}_{2}^{-}$ assumes a linear geometry.
The ${I}_{3}^{-}$ ion is also very common. What would you predict as to its geometry? In this representation, where does the negative charge lie?