12.13

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Mike Matthews 1D
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Joined: Fri Sep 29, 2017 7:04 am

12.13

Postby Mike Matthews 1D » Thu Dec 07, 2017 7:15 pm

12.13 Asks you to draw the Lewis structure for several different species and to identify each as a Lewis acid or Lewis base. I'm confused because part c asks for the Lewis structure of Ag+. How does one go about doing this since the electron configuration of Ag+ is [Kr]4d95s1?

Mitch Walters
Posts: 45
Joined: Fri Sep 29, 2017 7:07 am

Re: 12.13

Postby Mitch Walters » Thu Dec 07, 2017 7:56 pm

I would think you should ignore the d orbital. So just write Ag+.

Essly Mendoza 1J
Posts: 25
Joined: Fri Sep 29, 2017 7:04 am

Re: 12.13

Postby Essly Mendoza 1J » Thu Dec 07, 2017 11:51 pm

The solutions manual states that Ag+ is a lewis acid, but can anyone explain why? Thank you!

Kaileigh Yang 2I
Posts: 49
Joined: Sat Jul 22, 2017 3:00 am

Re: 12.13

Postby Kaileigh Yang 2I » Thu Dec 07, 2017 11:55 pm

Ag+ is a Lewis acid because if Ag+ accepts an electron it would become just Ag. In one example of 2NH3 + Ag+ --> [Ag(NH3)2]+, the lone pair of e- on NH3 would go to the Ag+.

Isaac Eyler 1E
Posts: 12
Joined: Fri Sep 29, 2017 7:04 am

Re: 12.13

Postby Isaac Eyler 1E » Sat Dec 09, 2017 12:57 pm

Can someone explain why in part B of this problem, BF3 is a lewis acid?

Isaac Eyler 1E
Posts: 12
Joined: Fri Sep 29, 2017 7:04 am

Re: 12.13

Postby Isaac Eyler 1E » Sat Dec 09, 2017 12:59 pm

Can someone explain why in part B of this problem, BF3 is a lewis acid?


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