[Torqz]

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

[AWK]

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

[clarkstill]

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...

[Torqz]

I don't think that would work at all.

Nitrogentrifluride looks like this:

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?