What are the formal charges of both chlorines and iodine in icl2?

Formal charge of ICl₂⁻

Formal charge = group no - (no of non bonding electrons + no of bonds)

In I there are 7 electrons in outermost orbit. If we add one more electrons due to - ve charge on the ion, it becomes eight. This centrally placed iodine forms two single bond with two chlorine atoms on either side.

Each of chlorine atoms also contains 7 valance electrons like iodine.

So formal charge of chlorine

= group no - (no of non bonding electrons + no of bonds)

= 7 - (6 + 1)

= 0

So formal charge of iodine

= group no - (no of non bonding electrons + no of bonds)

= 7 - (5 + 2)

=0

Formal charge of ICl₂⁺

In this case, central iodine will have only 6 valence electrons due to absence one electron.

So formal charge of chlorine in ICl₂⁺

= group no - (no of non bonding electrons + no of bonds)

= 7 - (6 + 1)

= 0

formal charge of iodine in in ICl₂⁺

7 - (4 + 2)

= 1