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chapter 3 hw #57 question

Posted: Sun May 20, 2018 8:44 pm
by 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?

Re: chapter 3 hw #57 question

Posted: Sun May 20, 2018 9:29 pm
by Chem_Mod
The negative charge would rather be on the oxygen rather than the chlorine atom because O is more electronegative than Cl.

Re: chapter 3 hw #57 question

Posted: Sun May 20, 2018 9:30 pm
by Alicia Yu 1A

Re: chapter 3 hw #57 question

Posted: Sun May 20, 2018 9:36 pm
by 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! :)

Re: chapter 3 hw #57 question

Posted: Thu May 24, 2018 10:18 pm
by 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:)

Re: chapter 3 hw #57 question

Posted: Fri May 25, 2018 6:54 am
by Joanna Pham - 2D
I believe the formula for perchlorate for given to us in a chart/diagram in Fundamentals Section D