Perchlorate (ClO4)-


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Yeo Bin Yook 1K
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Joined: Fri Apr 06, 2018 10:05 am

Perchlorate (ClO4)-

Postby Yeo Bin Yook 1K » Fri Jun 08, 2018 8:10 am

So this came up in my test and I'm still having a hard time understanding.
When I drew the Lewis Structure, I put the one negative formal charge on the chlorine, thinking that it would be better than putting it on oxygen that makes things less symmetric. However, I got it wrong and the answer said the extra electron should actually be on oxygen.

Why is this so?

jadam_1E
Posts: 30
Joined: Fri Apr 06, 2018 10:01 am

Re: Perchlorate (ClO4)-

Postby jadam_1E » Sat Jun 09, 2018 12:16 am

A good general rule when calculating formal charge: make the formal charge on the central atom as close as possible to 0. Also, oxygen is more electronegative than cl so it makes sense for cl to have the additional electron.

Megan Phan 1K
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Joined: Fri Apr 06, 2018 10:04 am

Re: Perchlorate (ClO4)-

Postby Megan Phan 1K » Wed Jun 13, 2018 3:09 am

Chlorine is the central atom, and for central atoms you want the formal charge to be 0. The negative charge should be on the others, especially in this instance O is more electronegative than Cl.

Riya Shah 4H
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Joined: Wed May 02, 2018 2:00 am

Re: Perchlorate (ClO4)-

Postby Riya Shah 4H » Tue Oct 30, 2018 1:57 pm

In ClO4- would all four oxygen atoms have a formal charge of -1?

Christine Chow 4G
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Joined: Thu Sep 27, 2018 11:28 pm

Re: Perchlorate (ClO4)-

Postby Christine Chow 4G » Tue Oct 30, 2018 2:58 pm

No, I believe 3 of the oxygens bonded to the chlorine are double bonded, so these would have a formal charge of 0. The one oxygen single bonded by chlorine will have a formal charge of -1.

janeane Kim4G
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Joined: Thu Sep 27, 2018 11:28 pm

Re: Perchlorate (ClO4)-

Postby janeane Kim4G » Tue Oct 30, 2018 3:07 pm

Can someone explain why 3 O would be double bonded with the Cl? Is there a way to determine if an element like Cl will/will not follow the octet guideline?

Christopher Tran 1J
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Joined: Thu Sep 27, 2018 11:15 pm

Re: Perchlorate (ClO4)-

Postby Christopher Tran 1J » Tue Oct 30, 2018 5:28 pm

Finding out the formal charge of the central atom should tell you whether or not the element will follow the octet guideline, given that the element is in Periods 3+.

For example, in ClO4-, three O are double bonded with the Cl so that the Cl has a formal charge of zero. If the three O were single bonded, then Cl would have had a formal charge of 3+, which is not a favorable structure.

Kristy 1F
Posts: 31
Joined: Thu Sep 27, 2018 11:19 pm

Re: Perchlorate (ClO4)-

Postby Kristy 1F » Fri Nov 02, 2018 12:12 am

Since the -1 charge should be on more electronegative atom. And the oxygen atom is more electronegative.


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