Relative Acidity Concept Question

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Grace Lee 3G
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Relative Acidity Concept Question

Postby Grace Lee 3G » Wed Dec 06, 2017 9:31 pm

If an atom has a higher electronegativity, is it a stronger acid?

skalvakota2H
Posts: 52
Joined: Sat Jul 22, 2017 3:01 am

Re: Relative Acidity Concept Question

Postby skalvakota2H » Thu Dec 07, 2017 12:00 am

Atoms with higher electronegativity will be less inclined to share its electrons with a proton. Thus, increasing electronegativity of an atom will decrease basicity, and weaker bases have stronger conjugate acids.

Another way to think about this is that with increasing electronegativity, the H-A bond in the acid becomes more polar and demonstrate more ionic character; this implies that the proton in HA will be lost and the proton is more readily lost only when the acid is strong.

Clara Hu 1G
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Re: Relative Acidity Concept Question

Postby Clara Hu 1G » Thu Dec 07, 2017 12:54 pm

In the example given in class, hypochlorous acid was the most acidic out of HClO, HBrO, and HIO because CL has the highest electronegativity which stabilizes the negatively charged O by withdrawing electron density.

Kyle Alves 3K
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Re: Relative Acidity Concept Question

Postby Kyle Alves 3K » Fri Dec 08, 2017 4:56 pm

electronegativity can also be seen as in making the conjugate base more stable and therefore showing it is a stronger acid. For example:
between HIO and HIO3, HIO3 is a stronger acid with a more stable conjugate base as the e- charge is more equally dispersed between 3 Os than one O. The more dispersed, the more stable the atom, the more stable the conjugate base= the stronger an acid.

Kyle Alves 3K
Posts: 46
Joined: Thu Jul 27, 2017 3:01 am

Re: Relative Acidity Concept Question

Postby Kyle Alves 3K » Fri Dec 08, 2017 5:05 pm

Probably a simpler example because the last one is confusing:
between HCl and HBr, Cl is more electronegative so pulls in e- greater, making the bond stronger
therefore, HBr would e a stronger acid as it is less stable with its longer bond length


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