Delocalization of charge and stability

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Ethan McCarthy 1F
Posts: 31
Joined: Wed Feb 27, 2019 12:17 am

Delocalization of charge and stability

Postby Ethan McCarthy 1F » Tue Jul 30, 2019 9:07 pm

When we say the conjugate base is more stable because it better delocalizes the charge (when comparing two acids and their conjugate bases), what does this mean?

Bella Martin
Posts: 47
Joined: Wed Sep 21, 2016 2:57 pm

Re: Delocalization of charge and stability

Postby Bella Martin » Tue Jul 30, 2019 11:21 pm

I'm actually not familiar with this every being specifically asked in a homework or sample test question. I'm not sure we got into too much depth on it? Any insight, anyone?

Chris Charton 1B
Posts: 69
Joined: Mon Jun 17, 2019 7:23 am

Re: Delocalization of charge and stability

Postby Chris Charton 1B » Tue Jul 30, 2019 11:37 pm

One thing it can refer to is the electronegativity of the central atom of the conjugate base. For example; ClO4- vs H2PO4- Cl is more electronegative than P, so it handles the negative charge more effectively. HClO4 is thus a stronger acid than H3PO4.

Emma Popescu 1L
Posts: 105
Joined: Wed Sep 11, 2019 12:16 am

Re: Delocalization of charge and stability

Postby Emma Popescu 1L » Fri Nov 29, 2019 9:30 pm

Does it say this in the textbook or did Dr. Lavelle mention it in lecture? If it is in the textbook, what page?

KaitlynBali_4B
Posts: 51
Joined: Fri Aug 02, 2019 12:16 am

Re: Delocalization of charge and stability

Postby KaitlynBali_4B » Sun Dec 01, 2019 12:39 am

The book explains that more electronegative atoms in the conjugate bases of acids is what allows for electron delocalization, essentially the spread of the negative charge of the base, in the anion. This electron delocalization is what allows for the anions to be stable. The book discusses this on page 468.


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