Lewis acid vs. base

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Rebecca Chu 1C
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Joined: Fri Apr 06, 2018 11:02 am

Lewis acid vs. base

Postby Rebecca Chu 1C » Sun May 20, 2018 10:35 pm

How am I supposed to distinguish a Lewis acid from a Lewis base if I'm given a molecule?

Ziana Bhanji 1E
Posts: 30
Joined: Fri Apr 06, 2018 11:01 am

Re: Lewis acid vs. base

Postby Ziana Bhanji 1E » Sun May 20, 2018 10:49 pm

We know that bases donate pairs of electrons and acids accept pairs of electrons. A Lewis acid is therefore any substance, such as the H+ ion, that can accept a pair of nonbonding electrons. In other words, a Lewis acid is an electron-pair acceptor.

I found this video quite explanatory:

Maria Zamarripa 1L
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Joined: Fri Apr 06, 2018 11:05 am
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Re: Lewis acid vs. base

Postby Maria Zamarripa 1L » Thu May 24, 2018 11:04 am

So basically and acid would be an electron acceptor and a base is an electron donor.

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Joined: Tue Nov 21, 2017 3:00 am

Re: Lewis acid vs. base

Postby hannahtweedy » Thu May 24, 2018 8:18 pm

Also if you do a Lewis structure, and there are unbonded valence electrons on the central atom, it's a Lewis base

Hannah Lee 1B
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Joined: Fri Apr 06, 2018 11:03 am

Re: Lewis acid vs. base

Postby Hannah Lee 1B » Fri May 25, 2018 2:43 pm

Since lewis acids are electron acceptors and bases are electron donors, when you draw the molecule an acid would have space to accept electrons (for example, BF3 can accept a pair to form a full octet) and a base would have extra lone pairs (ex. NH3)

Alejandro Salazar 1D
Posts: 31
Joined: Fri Sep 29, 2017 7:05 am

Re: Lewis acid vs. base

Postby Alejandro Salazar 1D » Sat May 26, 2018 4:09 pm

Lewis Acids: molecule that accepts a pair of electrons from another atom
1. has an incomplete octet
2. has a double or triple bond
3. or, typically has a positive charge or neutral. H+

Lewis Bases: molecule that donates a pair of electron to another atom
1. has a lone pair
2. or typically has a negative or neutral charge. OH-

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