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This article is about the chemical ion F . For the addition of fluoride ions to water supplies, see Water fluoridation.

Fluoride is the ionic form of fluorine. Fluorides are organic and inorganic compounds containing the element fluorine. As a halogen, fluorine forms a monovalent ion (−1 charge). Fluoride forms a binary compound with another element or radical. Examples of fluoride compounds include hydrofluoric acid (HF), sodium fluoride (NaF) and calcium fluoride (CaF2), and uranium hexafluoride (UF6).



Fluoride compounds, usually calcium fluoride, are naturally found in low concentration in drinking water and some foods, such as tea, seaweed, and fish bones (as in fish soup).

Water with underground sources are more likely to have higher levels of fluoride, while the total concentration in seawater has an average concentration of 1.3 parts per million (ppm).[1] Fresh water supplies generally contain between 0.01-0.3 ppm, while the ocean contains between 1.2 and 1.5 ppm.[2]


Hydrofluoric acid is used in the etching of glass and other industrial applications, including integrated circuit manufacturing.

Fluoride, as a concentrated gel, foam, or varnish, is used as a prescription drug.[3] Fluorine is also part of certain drug molecules to resist detoxification in the liver by the Cytochrome P450 oxidase because the strong C-F bonds are not easily broken. This is to ensure that orally administered medication are not inactivated before reaching the blood stream.[citation needed]

Fluoride ion has a very significant use in synthetic organic chemistry. The silicon-fluorine chemical bond is quite strong. Silyl ether protecting groups can be easily removed by the addition of fluoride ion. Sodium fluoride or tetra-n-butylammonium fluoride (TBAF) are the most common reagents used.

In biochemistry, fluoride salts are commonly used to inhibit the activity of serine/threonine phosphatases.

Sulfur hexafluoride is a nearly-inert, non-toxic propellant. Uranium hexafluoride is used in the separation of isotopes of uranium between the fissile isotope U-235 and the non-fissile isotope U-238 in preparation of nuclear reactor fuel and atomic bombs.

Water fluoridation

Main article: Water fluoridation

Fluoride containing compounds such as sodium fluoride, calcium fluoride, and sodium monofluorophosphate are commonly added to toothpaste, drinking water, prescribed treatments, and other commercially available oral hygiene products because fluoride increases the resistance of the enamel to decay[citation needed]. Originally, sodium fluoride was used to fluoridate water; however, hexafluorosilicic acid (H2SiF6) and its salt sodium hexafluorosilicate (Na2SiF6) are more commonly used, especially in the United States.

Some studies suggest that fluoridation is associated with a median decline in the number of children with cavities of 12.5%, and a median decline of 2.25 teeth with cavities. [4] The fluoridation of water is not without critics, however (see Water fluoridation controversy).

Salt fluoridation

In countries where large, centralized water systems are uncommon, salt fluoridation is sometimes used as an alternative to water fluoridation. In countries where salt fluoridation is common, such as Switzerland, France, and Jamaica, among many others, caries experience has also decreased in groups using fluoridated salt compared to groups using salt without fluoride. [5][6]



In high concentrations, fluoride compounds are toxic and can cause death. In mice, the LD50 is estimated to be 184 milligrams of stannous fluoride per kilogram of body mass.[7] An individual report involving fatality following the accidental administration of fluoride ion to a child at 5 mg/kg was cited by G. M. Whitford in 1987,[8] while after experimenting on himself in 1899, Herbert H Baldwin reported symptoms of acute toxicity (e.g. gastrointestinal upset) occurred at doses as low as 0.1-0.3 mg/kg.[9]

When ingested directly, fluoride compounds are readily absorbed by the intestines. Over time, the compound is excreted through the urine, and the half life for concentration of fluorine compounds is on an order of hours. It is thought that fluoride is taken out of circulation by the body and trace amounts become bound in bone. Urine tests are a good indication of high exposure to fluoride compounds in the recent past.

Skin or eye contact with many fluoride compounds in high concentrations is dangerous. In case of accidental swallowing, milk, calcium carbonate, or milk of magnesia is given to slow absorption. Eye or skin contact is treated by removing any contaminated clothing and flushing with water.


Fluoride ions replace hydroxide ions in calcium hydroxyapatite, Ca5[(PO4)3OH], in teeth, forming calcium fluoroapatite, Ca5[(PO4)3F], which is more chemically stable and dissolves at a pH of 4.5, compared to 5.5 pH for calcium hydroxyapatite. This is generally believed to lead to fewer cavities, since stronger acids are needed to attack the tooth enamel. In 1951, Joseph C. Muhler and Harry G. Day of Indiana University reported their research results on stannous fluoride as a tooth decay preventive and the university first sold the technology to Procter & Gamble to use in Crest toothpaste. Groups that have evaluated available studies and support water fluoridation include The American Dental Association (ADA), World Health Organization (WHO), and some other health organizations which recommend raising the fluoride level of municipal water supplies to a level between 0.7 and 1.2 ppm.

The most widely accepted adverse effect of low concentration fluoridation at this time is fluorosis [4]. It is a condition caused by 'excessive' intake of fluorine compounds over an extended period of time, and can cause yellowing of teeth. The definition of 'excessive' in the context of fluorosis falls on the order of parts per million and is generally accepted to mean significantly higher than the 0.7 to 1.2 ppm amounts recommended for fluoridated water. However, dosage is crucial to adverse effects, and therefore, what concentration is problematic will depend on the amount of fluoride ingested, how much is absorbed, and the weight of the person ingesting it. For this reason, many doctors have advised against using fluoridated water to make up formula for infants.

Contested claims

Main article: Water fluoridation controversy

Some opponents of fluoridation have expressed concern that fluoride damages body function. One of the key concerns is that fluoride can weaken bone strength, leading to an increase in hip and wrist fracture [10]. Additional concerns of fluoridation opponents include the potential for fluoride to damage the brain[11], reduce thyroid function[12], and cause bone cancer in adolescent boys[13]. While a recent review from the US National Research Council supports concerns that fluoride may cause some of these effects, at least at high doses[14], however, more than 100 national and international health service agencies and professional organizations continue to accept that there are benefits of community water fluoridation in preventing dental decay.[15]

See also


  1. ^ Fluoride in Drinking-water: Background document for development of WHO Guidelines for Drinking-water Quality. World Health Organization, 2004, page 2. Page accessed on February 22, 2007.
  2. ^ Environmental Health Criteria 227: Fluorides. World Health Organization, 2002, page 38. Page accessed on February 22, 2007.
  3. ^ Centers for Disease Control and Prevention. Fluoridation - Other fluoride products. Page accessed on March 22, 2007.
  4. ^ a b McDonagh M S, Whiting P F, Wilson P M, Sutton A J, Chestnutt I, Cooper J, Misso K, Bradley M, Treasure E, & Kleijnen J. (2000). "Systematic review of water fluoridation". British Medical Journal 321 (7265): 855-859. doi:10.1136/bmj.321.7265.855.
  5. ^ Estupiñán-Day, S R; Horowitz H, Warpeha R, Sutherland B, Thamer M (2001). "Salt fluoridation and dental caries in Jamaica". Journal of Community Dentistry and Oral Epidemiology 29: 247-252.
  6. ^ Fabien, V; Obry-Musset A M, Hedelin G, Cahen P M (1996). "Caries prevalence and salt fluoridation among 9-year-old schoolchildren in Strasbourg, France". Journal of Community Dentistry and Oral Epidemiology 24: 408-411.
  7. ^ Tin(II) Fluoride MSDS
  8. ^ Whitford, G. M.. "Fluoride in Dental Products". Journal of Dental Research 66 (5): 1056.
  9. ^ Baldwin, H. B. (1899). "The Toxic Action of Sodium Fluoride". Journal of the American Chemical Society 21 (6): 517-521. doi:10.1021/ja02056a008.
  10. ^ Colquhoun, John. Why I Changed My Mind about Fluoridation', Perspectives in Biology & Medicine 1997;41,27-44. Page accessed 23 February, 2007.
  11. ^ National Research Council. Neurotoxicity and Neurobehavioral effects' Fluoride in Drinking Water: A Scientific Review of EPA's Standards (2006). Page accessed 23 February, 2007.
  12. ^ National Research Council. Effects of the Endocrine System' Fluoride in Drinking Water: A Scientific Review of EPA's Standards (2006). Page accessed 23 February, 2007.
  13. ^ Environmental Working Group. Harvard Study: Strong Link Between Fluoridated Water and Bone Cancer in Boys' April 5, 2006. Page accessed 23 February, 2007.
  14. ^ National Research Council. Fluoride in Drinking Water: A Scientific Review of EPA's Standards Page accessed 23 February, 2007.
  15. ^ National and International Organizations that Support Fluoride, from the Massachusetts Coalition for Oral Health website, page accessed March 19, 2006.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Fluoride". A list of authors is available in Wikipedia.
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