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Postby VahagnAldzhyan » Wed Dec 06, 2017 11:36 pm

Why is it that having more bonded oxygens creates stability around the molecule?

Hazem Nasef 1I
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Joined: Tue Oct 10, 2017 7:13 am

Re: Oxoacids

Postby Hazem Nasef 1I » Wed Dec 06, 2017 11:48 pm

It's not necessarily having more oxygens, but rather having more atoms that stabilize the anion by withdrawing delocalizing the negative charge. For example, as Dr. Lavelle discussed in class, trichloroacetic acid (an acetic acid molecule in which the three hydrogen atoms are replaced with chlorine atoms) is a stronger acid than acetic acid because the three chlorine atoms delocalize the negative charge of the oxygen.

Hope this helps!

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Re: Oxoacids

Postby 605011646 » Thu Dec 07, 2017 1:22 pm

Can anions be more stable due to the delocalizing being done by more electronegative atoms?

Justin Chang 2K
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Re: Oxoacids

Postby Justin Chang 2K » Thu Dec 07, 2017 4:48 pm

Yeah, more electronegative elements can help stabilize and delocalize the charge.

Clarisse Wikstrom 1H
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Re: Oxoacids

Postby Clarisse Wikstrom 1H » Thu Dec 07, 2017 6:42 pm

This explains why oxoacids are strong acids. They are more willing to lose their H+ because after losing the H+, they have more options for resonance, which makes the compound more stable.

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