Monofluorophosphate is an anion with the formula PO₃F²⁻, which is a phosphate group with one oxygen atom substituted with a fluoride atom. The charge of the ion is −2. The ion resembles sulfate in size, shape and charge, and can thus form compounds with the same structure as sulfates. These include Tutton's salts and langbeinites. The most well-known compound of monofluorophosphate is sodium monofluorophosphate, commonly used in toothpaste. Related ions include difluorophosphate () and hexafluorophosphate (). The related neutral molecule is phosphenic fluoride PO₂F. Organic derivatives can be highly toxic and include diisopropyl fluorophosphate. Some of the Novichok agents are monofluorophosphate esters. Names are given to these by naming the groups attached as esters and then adding "fluorophosphonate" to the end of the name. Two organic groups can be attached. Other related nerve gas substances may not be esters, and instead have carbon-phosphorus or nitrogen-phosphorus bonds. The organic fluorophosphonates react with serine esterases and

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as found in most animals. Some of the organic esters are detoxified in mammals by an enzyme in the blood and liver called paraoxonase PON1. Willy Lange from Berlin discovered sodium monofluorophosphate in 1929. He fruitlessly tried to make monofluorophosphoric acid. However, he did discover the highly toxic organic esters. Following this discovery various nerve gases like

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and PbF₂ can lower the melting temperature, and increase water resistance. These glasses can also be coloured by various other elements, and organic dyes. Some mixed anion compounds are known with other anions like

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, chloride, difluorophosphate or tetrafluoroborate.

Production

Hydrolysis of difluorophosphate with an alkali produces monofluorophosphate. : + 2 MOH → M₂PO₃F + H₂O + F⁻ Industrial production is by reaction of a

with a metaphosphate. :MF + MPO₃ → M₂PO₃F Disodium hydrogen phosphate or tetrasodium pyrophosphate can react with hydrogen fluoride to form the sodium salt. :Na₂HPO₄ or Na₄P₂O₇ Phosphoric acid reacts with metal fluorides dissolved in molten urea to yield monofluorphosphates.

Properties

Monofluorophosphates are stable at room temperature, but will decompose when heated. For example, at , silver monofluorophosphate gives off phosphoryl fluoride (POF₃) as a gas leaving behind silver phosphate (Ag₃PO₄) and silver pyrophosphate (Ag₄P₂O₇). In inorganic compounds the monofluorophosphate ion has an average P–O bond length of 1.51 Å. The P–F bond is longer, on average 1.58 Å. The O P F angle is 104.8°, smaller than the tetrahedral 109.47°. To compensate the O P O bond angle is 113.7° on average. Most commonly the monofluorophosphtae ion takes on point group 1, but a significant number have point group ''m''. Only two are known with 3''m'' and one with 3. When compared to sulfates, some are isotypical with the monofluorophosphates. Yet others have sulfates that take on a different form. But most know monofluorophosphates have no known equivalent sulfate.

Compounds

Organic

Uses

Zinc monofluorophosphate can be used as a corrosion inhibitor for steel when salt is present. Glutamine monofluorophosphate has been used as a fluoride-bearing medicine.

Production

Properties

Compounds

Organic

Uses

References

Other reading