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I have no university degree in chemistry and I’m curious about some examples - explained with the applicable rules (or the exception from the existing rules) - for the following statements (from this answer):

  • If fluoride is oxidized, it loses an single electron.
  • If fluoride acts as a base and donates a pair of electrons, it shares a pair of electrons.

Now, what are some examples of

  • oxidation of fluoride?
  • fluoride acting as a base?
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As far as I think Fluorine ($\ce{F2}$) is the strongest oxidising agent, as the standard reduction potential for the conversion $\ce{F2 + 2e- -> 2F- }$ is very highly positive i.e. $E^0_{F_2/F^-} = + 2.87 V$. If you have any other species which have even more positive reduction potential than this, then only oxidation of $\ce{F-}$ is observed i.e. the reverse reaction occurs. But such species are very rare and thus generally oxidation of fluorides are not observed.
You can surely have examples of Fluorides acting as Lewis base. For example, if you react $\ce{KF}$( basically $\ce{K+F-} $ ) with Antimony pentafluoride ($\ce{SbF5}$), $\ce{F- } $ will donate i ts lone pair to $\ce{Sb}$ and then they will form the compound $\ce{K+ SbF6-}$. This is a classic example of fluoride acting as lewis base.

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