[budullewraagh]

i know that C(NO2)4 exists and is a rocket propellant.  i checked my merck index for a chemical that is the same but with added H on every O which would reduce each N to +3.  i could not find this.  does it exist?

[hmx9123]

Such as species doesn't exist, except in calculations and possibly in some really screwy gas phase unstable state.

[budullewraagh]

that's a shame.  how about FH7?  fluorine can do the whole +7 thing but i don't understand how.

[hmx9123]

I'd have to give that one the big 'no', too.

[budullewraagh]

yeah well i tried.  what oxidizes a fluorine atom??  nitrates do but i still dont get how that could happen.  odd.

[hmx9123]

Nitrates oxidize a fluorine atom?  This is news to me.  I don't know of much that can oxidize fluorine the atom, or the diatomic molecule.

[Corvettaholic]

From webelements, I think there are nitrogen-fluorine combo's:

http://www.webelements.com/webelements/compounds/text/N/F3N1-7783542.html

If you look under nitrogen, it lists fluorides, but if you look under fluorine by itself, you don't get jack. Maybe the table is incomplete?

[budullewraagh]

Nitrates oxidize a fluorine atom?  This is news to me.  I don't know of much that can oxidize fluorine the atom, or the diatomic molecule.

FNO3 exists; it's used as an oxidizing agent in rockets.  F can get to +7, which makes me scratch my head.  

[hmx9123]

FNO₃ may exist, but it doesn't mean that you used a nitrate to oxidize fluorine.

[budullewraagh]

so what do you think oxidized the fluorine?  a permanganate?

[hmx9123]

Depends.  What was the reaction that produced it?  Did you start with NO₂F?  Did you start with F₂ and NO, NO₂ or something along those lines?  Perhaps it was done with ridiculous temperatures?  Try looking up that compound to find the references for it.  That will give you a lot better idea about it.