Focus 6 #13

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Focus 6 #13

Postby JamieVu_2C » Sun Dec 01, 2019 4:52 pm

Draw the Lewis structure of boric acid, B(OH)3.
(a) Is resonance important for its description? (b) The proton transfer equilibrium for boric acid is given in a footnote to Table 6C.1. In that
reaction does boric acid act as a Lewis acid, a Lewis base, or neither? Justify your answer by using Lewis structures of boric acid and its conjugate base.

How do conjugate systems delocalize electrons, and how does resonance play a part? If there are resonance structures, then the electrons are delocalized, so the bonds are weak, but how would that make B(OH)3 a weak acid if its bonds are strong?

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Re: Focus 6 #13

Postby Chem_Mod » Mon Dec 02, 2019 3:21 pm

Resonance shouldn't be taken account when analyzing the acidity of boric acid. There are no pi bonds in boric acid. The boron in boric acid can act as the Lewis acid to accept an OH group from water, which generates H+ and that is a property of an acid.

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