Fluorine perchlorate, also called perchloryl hypofluorite is the rarely encountered chemical compound of fluorine, chlorine, and oxygen with the chemical formula or . It is an extremely unstable gas that explodes spontaneously and has a penetrating odor.
Synthesis
One synthesis uses fluorine and perchloric acid, though the action of ClF5 on water is another method.
F2 + HClO4 -> FClO4 + HF
Another method of synthesis involves the thermal decomposition of tetrafluoroammonium perchlorate, , which yields very pure that may be manipulated and frozen without explosions.
NF4ClO4 ->[\ \Delta\ ] NF3{ } + FClO4
Structure
Fluorine perchlorate is not analogous to perchloric acid because the fluorine atom is more electronegative than oxygen. It contains an oxygen atom in a rare oxidation state of 0 due to the electronegativity of oxygen, which is higher than that of chlorine but lower than that of fluorine.
Safety
FClO4 has a very dangerous and unpredictable series of reactions associated with it, as a covalent perchlorate (chlorine in the +7 oxidation state) and a compound featuring a very sensitive O-F single bond. Small amounts of reducing agent, such as organic compounds, can trigger explosive detonation. Products of these decomposition reactions could include oxygen halides, interhalogen compounds, and other hazardous substances.
Accidental synthesis is possible if precursors are carelessly mixed. Like similar covalent fluorides and perchlorates, it needs to be handled with extreme caution.
Reaction
FClO4 is a strong oxidant and it reacts with iodide ion:
FOClO3 + 2I^- -> ClO4^- + F^- + I2
FClO4 can also react with tetrafluoroethylene:
CF2=CF2 + FOClO3 -> CF3CF2OClO3
It may be a radical addition reaction.