# Can fluorine ever have a positive oxidation state?

I know fluorine is the most electronegative element but can we humans ever synthesize fluorine in a positive oxidation state like +1?

• What element would have a negative oxidation state to balance that +1? May 5 at 0:18
• There has been a previous discussion: chemistry.stackexchange.com/questions/62397/… May 5 at 4:03
• There is possible to have a ion $\ce{F+}$ in gaseous or plasmatic state, so yes, it is possible to have fluorine in oxidation state +I. May 5 at 6:24

As noted in the referenced question, fluorine is not in the +1 oxidation state in hypofluorous acid (which, incidentally, is the only hypohalous acid that has been isolated) nor in any other compound where its bonds give it a complete octet. Even where the fluorine has a positive formal charge, attaching it to less electronegative atoms will lead to an oxidation state of -1.

However, it is possible for fluorine to show a zero oxidation state and for a fluorine atom to apparently show a positive charge. As one might expect, this occurs in one of the most unusual compounds in all of chemistry.

Striking gold -- and a lucky 7

That compound is "gold heptafluoride", $$\ce{AuF7}$$, whose unusual structure is reflected in the IUPAC name: instead of gold(VII) fluoride, it is officially called difluorinegold(V) fluoride. It is more accurately formulated $$\ce{AuF5\cdot F2}$$. It has been isolated at liquid nitrogen temperatures [1].

Himmel and Riedel [2] give calculations showing that unlike other heptafluorides, not all seven fluorine atoms are bonded to the central (gold) atom. Rather, the gold is bonded octahedrally to five individual fluorine atoms and a difluorine ($$\ce{F2}$$) ligand, the latter attached end on and rotated so that in the most stable conformation (according to most of the several optimization schemes used), the remote fluorine atom is eclipsed with one of the other ligands as if attracted to it (a, below, picture from [2]). The staggered arrangement one might expect (b) is instead a transition state in this fluxional molecule. If we assume that the individual fluorine ligands are negatively charged as usual, this interaction indicates that at least the remote fluorine atom, labeled $$\text{F}_b$$, is positively charged.

And indeed, Table 2 of the paper shows the following charge distribution:

Thus the relatively electronegative gold atom, its effective electronegativity further enhanced by the other fluorine ligands, actually imparts positive charge to both fluorine atoms in the molecular fluorine ligand, as if there were a more electronegative moiety even than atomic fluorine. Note the significantly greater portion of positive charge on the remote fluorine, the one which wheels around to attract one of the fluoride ligands in the eclipsed conformation.

To sum up, difluorine gold (V) fluoride has:

• A difluorine ligand, apparently the first known case of thus

• A gold-fluorine moiety, either $$\ce{AuF5}$$ or $$\ce{AuF6}$$ depending on how one views the structure, that is effectively more electronegative than fluorine itself

• A resulting positive charge on some fluorine atoms.

References

1. Timakov, A. A.; Prusakov, V. N.; Drobyshevskii, Y. V. (1986). "Gold heptafluoride". Dokl. Akad. Nauk SSSR (in Russian). 291: 125–128.

2. Daniel Himmel and Sebastian Riedel, "After 20 Years, Theoretical Evidence That 'AuF7' Is Actually AuF5‚F2", Inorganic Chemistry 46 (13), 5338-5342 (2007).

• Cool, but 0 isn't positive, and I'm pretty sure positive values are possible for fluorine. May 5 at 13:37
• Right. I mention (partial) positive charge as distinct from oxidation state. If we are looking at species where the fluorine has its full octet, we can get +1 oxidation state (with the usual convention) only by having it bound by pairwise bonds to two fluorine atoms. Gold heptafluoride has fluorine in one such bond, not two. Ergo oxidation state 0 even though there is a positive partial charge. May 5 at 13:48
• But after a bit of searching I found only theoretical study of $\ce{F4^+}$ researchgate.net/publication/… May 5 at 14:02
• I think it's just if isolated cation can hold together, though. Not all that different from F+ in plasma - there's probably no counterion for such cation. May 5 at 14:14
• The reference does mention the possibility of matrix isolation of its identified thermochemically stable species including $\ce{F4^+}$. Such a matrix would presumably have to include some counterion. May 5 at 14:21