I was wondering about $\ce{HClO4}$ which is a very strong acid . I thought it can be made stronger by replacing $\ce O$ with $\ce F$ to make $\ce{HClF6}$ but didn't find its existence . I thought that it might be unstable due to repulsions between $\ce F$ . So than i switched to $\ce{HIF6}$ and there was no existence of this also as well as $\ce{HBrF6}$ . Is there a reason that the halogens cannot form $\ce{HXF6}$ acids similar to $\ce{HSbF6}$?

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    $\begingroup$ Related (involving sfur as the centrasl atom): chemistry.stackexchange.com/questions/102290/…. You tend to lose hydrogen halide molecules from your proposed complexes. $\endgroup$ – Oscar Lanzi Oct 3 '18 at 14:50
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    $\begingroup$ ClF6- , BrF6- and IF6- all exist, as does IF8- . However I doubt the parent acids will be stable, but my good chemistry books are a long way away at the moment. $\endgroup$ – Ian Bush Oct 3 '18 at 16:43
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    $\begingroup$ There are a whole bunch of these ions. But the reference does not document any case where anions can be protonated to acids. $\endgroup$ – Oscar Lanzi Oct 4 '18 at 1:24
  • $\begingroup$ Why can't they protonated to acids. is there any known reason $\endgroup$ – Harsh jain Oct 4 '18 at 5:05
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    $\begingroup$ Nothing wrong with protonation as such. The issue could be they decompose when protonated; compare with a nitrite or a bicarbonate.. $\endgroup$ – Oscar Lanzi Oct 4 '18 at 10:00

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