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Emily Glaser 1F
Posts: 156
Joined: Thu Jul 27, 2017 3:01 am


Postby Emily Glaser 1F » Fri Dec 08, 2017 12:38 am

Why is HF considered a weak acid considering its electronegativity

Ethan Vuong 3G
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

Re: HF

Postby Ethan Vuong 3G » Fri Dec 08, 2017 3:19 am

It is considered a weak acid because it has a short bond length between the fluorine and the hydrogen ion. This means there is more energy holding them together and less acidic.

Golbarg Rahimi 3k
Posts: 26
Joined: Sat Jul 22, 2017 3:01 am

Re: HF

Postby Golbarg Rahimi 3k » Fri Dec 08, 2017 7:40 am

In our book it states that in these molecules as we go across a period we have to consider electronegativity but as we go down a group we have to consider bond length and the radius. So we compare HCL and HF based on their radius since they are in the same group. Cl has a larger radius and more acidic

Naama 1A
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: HF

Postby Naama 1A » Fri Dec 08, 2017 8:25 am

I think that since the bond between H and F is so strong, it would be harder to separate them and give up the hydrogen ion (which would make it a Bronsted acid). Because of the strength of the bond, it is considered a weak acid.

Phillip Winters 2F
Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

Re: HF

Postby Phillip Winters 2F » Fri Dec 08, 2017 9:24 am

Fluorine has a very small atomic radius so in turn it also has a very short bond length, resulting in a very strong bond, and the fluorine is less likely to give up a hydrogen

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