2006-11-28 06:22:35 · 6 answers · asked by rmmeyyappan 1 in Science & Mathematics ➔ Chemistry
What everybody probably intends to say is that because Fluorine has a high electronegativity, there is a strong INDUCTIVE effect. This induction "pulls" electron density through the molecular orbitals towards fluorine and in essence ends up weakening the O-H bond at the business end of the acid. This weakening of the carboxylic acid bond results in a more acidic hydrogen. This inductive effect also assists in stabilization of the resulting carboxylate anion, which is delocalized throughout the carbonyl.
BTW, trifluoroacetic acid is much more acidic...
2006-11-28 06:35:39 · answer #1 · answered by Anonymous · 2⤊ 0⤋
Fluoroacetic Acid
2016-10-31 08:48:03 · answer #2 · answered by ? 4 · 0⤊ 0⤋
Because Fluorine has greater electronegativity than normal acetic acid... And thus pulls the elctron density towards it, allowing one of the hydrogen in the hydroxyl group to be given up more easily.
Regards,
Ryan
2006-11-28 06:31:04 · answer #3 · answered by Ryan Pediatrics 4 · 1⤊ 0⤋
Hey, we actually did this in class the other day. Fluorine is very electronegative and it pulls electron density towards it. That means that the electrons in the O-H bond are being pulled back toward the rest ofthe molecule, and that makes it easier to give up an H+.
2006-11-28 06:29:57 · answer #4 · answered by Amy F 5 · 2⤊ 0⤋
The fluorine is the most reactive element on the periodic table. It is highly electronegative and has high affinity for free electrons on other molecules. Hope this helps.
2006-11-28 06:29:21 · answer #5 · answered by Taylor S 1 · 1⤊ 0⤋
Because it gives up its H+ more readily?
2006-11-28 06:24:49 · answer #6 · answered by Silly me 4 · 0⤊ 0⤋