Can fluorine ever have a positive oxidation state?
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 &quot;gold heptafluoride&quot;, $\ce{AuF7}$, 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 $\ce{AuF5\cdot F2}$.
Himmel and Riedel [1] 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 [1]).  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, it's effective elecyltronegativity 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.


Reference
1.
Daniel Himmel and Sebastian Riedel, &quot;After 20 Years, Theoretical Evidence That 'AuF7' Is Actually AuF5‚F2&quot;, Inorganic Chemistry 46 (13), 5338-5342 (2007).