Which of the following compound is planar and non-polar?

A compound anion having a central iodine atom is called an iodine tetrachloride anion. As the primary element of group 7A (group 17), iodine $\left(\mathrm{I}\right)$ has 7 valence electrons on its own. It will share 4 valence electrons with the 4 nearby chlorine $\left(\mathrm{Cl}\right)$ atoms through 4 single covalent connections. This leaves the core iodine atom with 3 non-bonding valence electrons, which when combined with the -1 charge applied to this compound anion, resulting in 2 non-bonding valence electron pairs on this atom.

A square planar molecular geometry is produced by a core atom, four covalently bonded peripheral atoms, and two nonbonding pairs, according to VSEPR theory:

Due to chlorine's greater electronegative nature than iodine, each $\mathrm{I}-\mathrm{Cl}$bond is polar. This complex anion, however, is not polar by itself .