Textbook 6A.13

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Daria Obukhova 2B
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Joined: Wed Sep 30, 2020 9:50 pm

Textbook 6A.13

Postby Daria Obukhova 2B » Wed Dec 09, 2020 4:35 pm

This question asks to: Draw the Lewis structure or symbol for each of the following species and identify each one as a Lewis acid or Lewis base:
(a) NH3; (b) BF3; (c) Ag+ ; (d) F- ; (e) H-

I'm having trouble with the single elements...how do we determine if (c) through (e) are acids or bases?

Marc Lubman 3B
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Re: Textbook 6A.13

Postby Marc Lubman 3B » Wed Dec 09, 2020 4:56 pm

Hi Daria, for each element you simply have to consider whether it prefers to accept or donate a pair of electrons. In the case of silver, as a metal (and especially a metal cation), it's most likely to accept electrons and thus act as a Lewis acid. This is, in fact, how coordination complexes form, since metals will accept electrons from ligands to form a coordinate covalent bond. F- is very unlikely to accept more electrons and even has one extra, so it's pretty likely to give a pair up and thus act as a Lewis base. The same goes for H-, which is extremely unlikely to hold any more electrons. H+ is relatively stable though, so H- is not too against giving up both of its electrons and thus acting as a Lewis base.

Pranav Daggubati 3C
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Joined: Wed Sep 30, 2020 9:35 pm

Re: Textbook 6A.13

Postby Pranav Daggubati 3C » Wed Dec 09, 2020 5:27 pm

Remember that lewis acids and bases involve electron pairs. Bases are those with electron pairs that can be donated, while acids are the acceptors.

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