chapter 3 hw #57 question

[Nabeeha Khan 1D]

For part C of question number 57 you have to write the lewis structure for a perchlorate ion. My question is why can't the chlorine atom form four double bonds with all of the oxygens so that the oxygens all have a zero formal charge?

[Chem_Mod]

The negative charge would rather be on the oxygen rather than the chlorine atom because O is more electronegative than Cl.

[Alicia Yu 1A]

You may want to reference this website, it explains it pretty well.
https://chemistry.stackexchange.com/questions/6447/why-does-clo%E2%82%84%E2%81%BB-only-have-3-double-bonds

[Anna De Schutter - 1A]

Would we be given a chart that tells us the electronegativity of each element in order to solve this question? Or is there another way to know that O is more electronegative than Cl?
Thank you! :)

[Miya Lopez 1I]

Could someone please explain to me how we know that we are supposed to use oxygen for this problem? Am I missing something in the question where it says to use oxygen, or is it because it's a certain type of ion?

Thank you:)

[Joanna Pham - 2D]

I believe the formula for perchlorate for given to us in a chart/diagram in Fundamentals Section D