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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Torqz on June 19, 2015, 04:06:43 AM

Title: Problems with Nitrogen Trifluride anion.
Post by: Torqz on June 19, 2015, 04:06:43 AM

Hello there,

I am wondering if anyone can help me with a lewis structure for NF₃^- please?

(Aslo a dot and cross diagram if thats even possible?)

Its was in an exam I sat yesterday - I think NF₃ would be all single covalents with a lone pair on the nitrogen right? But I am not sure what will happen to the lone pair if another electron is added to the mix...

Thank you,

Pete A

Title: Re: Problems with Nitrogen Trifluride anion.
Post by: AWK on June 19, 2015, 05:22:47 AM

It does not exist as anion, but neutral molecule does.

Title: Re: Problems with Nitrogen Trifluride anion.
Post by: clarkstill on June 19, 2015, 09:39:52 AM

I suppose you could make the radical anion? It'd be pretty hard to do, as you'd need to put an electron into one of the N-F sigma* orbitals, so the product would have one N-F bond with a bond order of 1/2. I imagine you'd need the mother of all single electron reducing agents to do it though...

Title: Re: Problems with Nitrogen Trifluride anion.
Post by: Torqz on July 04, 2015, 07:00:37 PM

I don't think that would work at all.

Nitrogentrifluride looks like this:

https://en.wikipedia.org/wiki/Nitrogen_trifluoride (https://en.wikipedia.org/wiki/Nitrogen_trifluoride)

How could there be another electron in one of the bonds, which are allready full bonds when there is a lone pair?