Talk:Nitrogen pentafluoride

3d shell?[edit]

It seems the structure above (replace P with N) will be stabler. --Makecat _Talk 06:44, 25 July 2012 (UTC)[reply]

Maybe the MO diagram on p.57 of ref1 can describe it better. --Makecat _Talk 06:50, 25 July 2012 (UTC)[reply]

Also, I thought d-orbital hybridization doesn't actually contribute anything significant to bonding in hypervalent molecules? Double sharp (talk) 04:43, 7 December 2012 (UTC)[reply]

On this topic 122.162.2.215 also asked: " nitrogen does not have a 3D orbital. So how does it expands its orbitals to from a 4th n a 5th bond?"

This "lack" of orbital could explain why this molecule does exist. However Nitrogen does have a 3D orbital, it is empty and of higher energy, so likely cannot be used in a low energy molecule. Graeme Bartlett (talk) 20:19, 3 December 2013 (UTC)[reply]