is the rarely-encountered chemical compound FClO4
. One synthesis uses fluorine and perchloric acid
, though the action of ClF5
on water is another method.
It is extremely unstable and has a penetrating odor.
Fluorine perchlorate should be analogous to perchloric acid, but with the replacement of the lone hydrogen
atom with an atom of fluorine. 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.
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, e.g. 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, handle with extreme caution especially if safety data/MSDS is not fully available.
(one chemist's experiences with perchlorates)