Trends on the Periodic Table with Acids

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Nathan Barger 3B
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Joined: Fri Sep 25, 2015 3:00 am

Trends on the Periodic Table with Acids

Postby Nathan Barger 3B » Wed Dec 02, 2015 4:36 pm

My questions deals with elements, their positions on the periodic table and how strong or weak acids are. Is there a trend between the position of elements on the periodic table and how acidic they are when bonded with Hydrogen. For example, when discussing acids, H-F is considered a weak acid but H-I is a very strong acid with H-Br and H-Cl being in between the two. So does this mean that acids become stronger the lower the element involved in the bond is on the periodic table?

704628249
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Joined: Fri Sep 25, 2015 3:00 am

Re: Trends on the Periodic Table with Acids

Postby 704628249 » Wed Dec 02, 2015 6:19 pm

Basically, the weaker the A-H bond, the easier it is for H20 to remove the H+. So weaker bonds are more acidic.

Prina Patel 1H
Posts: 62
Joined: Fri Sep 25, 2015 3:00 am

Re: Trends on the Periodic Table with Acids

Postby Prina Patel 1H » Thu Dec 03, 2015 8:51 pm

Fluorine is very electronegative so it won't easily give up its electrons which is what a strong acid would do easily. The disassociation energy trend is that that it decreases going to the left and up which can tell you if a certain acid is stronger than another. The lower the disassociation energy the weaker the acid. If you notice Hydrogen and Fluorine both have small radii so the disassociation is small and the radii of Hydrogen and Iodine together is bigger than those of HF so the disassociation energy if higher.


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