Sodium monofluorophosphate

SMFP is best known as an ingredient in some toothpastes. It functions as a source of fluoride via the following hydrolysis reaction: ==Tooth decay==

Tooth decay is caused by bacteria naturally present in one's mouth. These bacteria form a sticky, colorless soft film on the teeth called plaque. When foods containing carbohydrates (starches and sugars) are eaten, the bacteria that form plaque use the sugar as a form of energy. They also turn it into a glue-like substance that helps them stick to the surface of the tooth. The plaque produces acid, which attacks the enamel. Chemistry of decay Tooth enamel consists mostly of calcium hydroxyphosphate, Ca5(PO4)3OH, also known as the mineral hydroxyapatite. Apatite is a hard, insoluble compound. Acid (H+), produced especially after a high-sugar meal, attacks the apatite: :Ca5(PO4)3OH(s) + H+(aq) → Ca5(PO4)3+(aq) + H2O(ℓ) Chemistry of enamel fluoridation The degradation of apatite by loss of OH− causes the enamel to dissolve. The process is reversible as saliva supplies back OH− to reform apatite. If fluoride, F−, ions are present in saliva, fluorapatite, Ca5(PO4)3F, also forms. :Ca5(PO4)3+(aq) + F−(aq) → Ca5(PO4)3F(s) Fluorapatite resists attacks by acids better than apatite itself, so the tooth enamel resists decay better than enamel containing no fluoride. ==Preparation and structure==

Sodium monofluorophosphate is produced industrially by the reaction of sodium fluoride with sodium metaphosphate: :NaPO3 + NaF → Na2PO3F The process involves scission of a pyrophosphate bond, analogous to hydrolysis. SMFP can also be prepared by treating tetrasodium pyrophosphate or disodium phosphate with hydrogen fluoride. In the laboratory, SMFP can be prepared by hydrolysis of difluorophosphate ions with dilute sodium hydroxide: :PO2F2− + 2 NaOH → Na2PO3F + H2O + F− Structure The structure of the fluorophosphate anion consists of phosphorus at the center of a tetrahedron defined by three oxygen atoms and one fluorine. Formal representations depict a double bond between one oxygen atom and phosphorus, with single bonds for the other two oxygen atoms and the fluorine. In this very formal depiction, negative charge is localized on the O atoms of the single P-O bonds. SMFP is isoelectronic with sodium sulfate. The anion has C3v symmetry. ==Discovery and development==

Sodium monofluorophosphate was first described in 1929 by the German chemist Willy Lange, who was then with the University of Berlin. His fruitless attempts to prepare free monofluorophosphoric acid led him to look at the acid's esters. Together with Gerda von Krüger, one of his students, Lange thus synthesized diethyl fluorophosphate which proved to be quite toxic, being the first ever nerve agent. In the 1930s, Gerhard Schrader, working for the German company IG Farben, tried to develop synthetic insecticide. His work focused on esters of phosphoric acids and resulted in the discovery of Isoflurophate, Tabun, Soman, and Sarin. In the meantime, Lange, who was married to a Jewish woman, emigrated from Germany to the United States and started work for Procter and Gamble Company. In 1947, he and Ralph Livingston of Monsanto Company published the preparation of the free fluorophosphoric acids and mentioned the use of isoflurophate in the treatment of glaucoma and myasthenia gravis. The well known toxicity of these esters led to fears that the simple salts might also be toxic, and such fears precluded any large scale commercial use of the salts. In 1950, under sponsorship of the manufacturer of the compounds, Ozark Chemical Company, the toxicity of sodium monofluorophosphate was studied by Harold Hodge at the University of Rochester who included anti-cavity testing. In 1967 Colgate-Palmolive filed several patents on the use of sodium monofluorophosphate in toothpaste. ==Safety==

The usual content of SMFP in toothpaste is 0.76%. The compound is used in place of sodium fluoride, particularly in children's toothpastes, because it is less acutely toxic, although both have modest toxicities. The in rats is 0.9 g/kg. ==References==