Textbook question

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Annabella_Amato_1I
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Textbook question

Postby Annabella_Amato_1I » Fri Dec 11, 2020 12:04 pm

In this case, is B(OH)3 acting as a Lewis base or Lewis acid? And why? Thanks!
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Kyle Walsh 2J
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Joined: Wed Sep 30, 2020 9:48 pm

Re: Textbook question

Postby Kyle Walsh 2J » Fri Dec 11, 2020 12:45 pm

Hi! So in this question, B(OH)3 is acting as the Lewis acid, as it is accepting the electron pair from the (OH)- to turn into B(OH)4-. You can double check this by confirming that H30+ is formed, meaning that the original compound was acidic and the conjugate is basic. Hope this helped!

Anh Trinh 1J
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Re: Textbook question

Postby Anh Trinh 1J » Fri Dec 11, 2020 6:57 pm

B(OH)3 is acting as a Lewis acid because in the product side, it accepts the OH- from the water molecule. Also, comparing the water molecule on the reaction and product side, you can see that it had 4 H atoms and 2 atoms before the reaction, and only 3 H atoms and 1 O atoms are left, so it has donated the OH- to B(OH)3.

Jiapeng Han 1C
Posts: 91
Joined: Wed Sep 30, 2020 9:50 pm

Re: Textbook question

Postby Jiapeng Han 1C » Sat Dec 12, 2020 4:04 am

Like AlCl3, B in B(OH)3 also has empty orbital which means that it could accept electron pair from the OH- group, meaning it is a Lewis acid.


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