[help9989]

A chlorine difluoride molecule can exist in two ionic forms, ClF2+ and ClF2-.

(a) Draw the Lewis structures for both these ions.


(b) Compare the approximate F-Cl-F angles in both ions using the VSEPR criteria; 180 degrees

(c) Which ion has the greater bond angle: explain your reasoning.

I know that the VSEPR theory is that because electron pairs repel each other, molecules adjust their shapes so that valence electron pairs are as far apart as possible. But i do not know about the VSEPR critera.

[rabolisk]

(a) You drew the same two structures. One of them has to be wrong. You can't just assign a charge at the end. A charged molecule or polyatomic ion means that the number of electrons =/= number of protons. You have to count the valence electrons.

(b) Even if the structures were correct for both, 180 degrees is not correct. I suggest you read over the VSEPR theory and how it relates to molecular structures.

(c) This will follow from b.