What is the formal charge of Cl− in the perchlorate ion, ClO−4, assuming the Cl−O bonds are all single bonds?

Question

What is the formal charge of CI^- in the perchlorate ion, CIO^-₄ assuming the CI-O bonds are all single bonds?

Answer 1

To find the formal charge, you want to draw the Lewis structure and then determine formals charges.

I cannot easily draw on this Wyzant platform, but I'll do my best to at least describe the Lewis structure so hopefully you can draw it. I'll then explain the formal charge.

Put Cl in the center and attach the 4 O atoms with single bonds. Put 3 lone pairs of electrons around each O atom. Now all atoms should have the octet.

Without using any double bonds (as instructed in the problem), the Cl will have a formal charge of +3 and each O will have a formal charge of -1 (total of -4). The net charge adds to -1 on the ion.

So, the answer is that Cl has a formal charge of +3.