įluorine's first ionization energy is third-highest among all elements, behind helium and neon, which complicates the removal of electrons from neutral fluorine atoms. The outer electrons are ineffective at nuclear shielding, and experience a high effective nuclear charge of 9 − 2 = 7 this affects the atom's physical properties. Ĭharacteristics Electron configuration įluorine atoms have nine electrons, one fewer than neon, and electron configuration 1s 22s 22p 5: two electrons in a filled inner shell and seven in an outer shell requiring one more to be filled. Fluorine has no known metabolic role in mammals a few plants and sea sponges synthesize organofluorine poisons (most often monofluoroacetates) that help deter predation. Organofluorine compounds often persist in the environment due to the strength of the carbon–fluorine bond. Global fluorochemical sales amount to more than US$69 billion a year.įluorocarbon gases are generally greenhouse gases with global-warming potentials 100 to 23,500 times that of carbon dioxide, and SF 6 has the highest global warming potential of any known substance. The fluoride ion from dissolved fluoride salts inhibits dental cavities, and so finds use in toothpaste and water fluoridation. Pharmaceuticals such as atorvastatin and fluoxetine contain C−F bonds. Molecules containing a carbon–fluorine bond often have very high chemical and thermal stability their major uses are as refrigerants, electrical insulation and cookware, and PTFE (Teflon). The rest of the fluorite is converted into corrosive hydrogen fluoride en route to various organic fluorides, or into cryolite, which plays a key role in aluminium refining.

Owing to the expense of refining pure fluorine, most commercial applications use fluorine compounds, with about half of mined fluorite used in steelmaking. Industrial production of fluorine gas for uranium enrichment, its largest application, began during the Manhattan Project in World War II. Only in 1886 did French chemist Henri Moissan isolate elemental fluorine using low-temperature electrolysis, a process still employed for modern production.

Proposed as an element in 1810, fluorine proved difficult and dangerous to separate from its compounds, and several early experimenters died or sustained injuries from their attempts. Fluorite, the primary mineral source of fluorine which gave the element its name, was first described in 1529 as it was added to metal ores to lower their melting points for smelting, the Latin verb fluo meaning 'flow' gave the mineral its name. As the most electronegative element, it is extremely reactive, as it reacts with all other elements except for argon, neon, and helium.Īmong the elements, fluorine ranks 24th in universal abundance and 13th in terrestrial abundance. It is the lightest halogen and exists at standard conditions as a highly toxic, pale yellow diatomic gas.

F molar mass