12.13

[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?

[Mitch Walters]

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

[Essly Mendoza 1J]

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

[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+.

[Isaac Eyler 1E]

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

[Isaac Eyler 1E]

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