Page 1 of 1
12.13
Posted: Thu Dec 07, 2017 7:15 pm
by Mike Matthews 1D
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?
Re: 12.13
Posted: Thu Dec 07, 2017 7:56 pm
by Mitch Walters
I would think you should ignore the d orbital. So just write Ag+.
Re: 12.13
Posted: Thu Dec 07, 2017 11:51 pm
by Essly Mendoza 1J
The solutions manual states that Ag+ is a lewis acid, but can anyone explain why? Thank you!
Re: 12.13
Posted: Thu Dec 07, 2017 11:55 pm
by Kaileigh Yang 2I
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+.
Re: 12.13
Posted: Sat Dec 09, 2017 12:57 pm
by Isaac Eyler 1E
Can someone explain why in part B of this problem, BF3 is a lewis acid?
Re: 12.13
Posted: Sat Dec 09, 2017 12:59 pm
by Isaac Eyler 1E
Can someone explain why in part B of this problem, BF3 is a lewis acid?