In the 16th century, when Nostradamus demonstrated his prophetic capabilities and Paracelsus expressed his view that the dose alone makes a thing a poison, another contemporary and professional colleague was interested in metallurgical affairs: the German physician Georg Bauer, of Chemnitz. Under his latinized name "Georgius Agricola" he is known in the history of medicine as the man who very aptly described the diseases of the miners of his time (1), diseases which he still ascribed to evil ghosts doing mischief in the mines. This was but a very small aspect in his "De re metallica", the first written detailed description -fully in Latin- of how to prepare metals from ores and which soon became translated into many languages (2). It even was published in Chinese (3). In his work Bauer explains how admixture of fluxes ("lapides igni liquescentes (fluores)" = lat.: "stones which become liquid in fire (flows)") facilitates the smelting of ores. Fluxes work as a solvent for ores that would otherwise need much more heat (and thus energy) to become liquid for further processing. The aid, called "Flußspat" (fluorspar) by the German miners, had for the first time been mentioned by Basilius Valentinus towards the end of the 15th century (4), and was more extensively described in one of Bauer´s early works in 1530 (5). Fluorspar occurs in nature in several beautifully colored varieties. The violet variety ("fluores colore violaceo") looks like amethyst, the green one resembles emerald and so these varieties were occasionally sold instead of the gems (hence the name "false amethyst" or "false emerald" for fluorspar). 

Attack on glass

If to a sample of fluorspar some acid, e. g. sulfuric acid, is added and the mixture is gently heated, toxic fumes develop which attack glass. There are rumors that already in 1670 a Nuremberg glassworker, Heinrich Schwanhard, made use of this reaction for artistic etchings on glass (6-8), but this could not be verified; Schwanhard rather used nitric acid on a softer variety of glass, as a review by Partington (9) revealed. The first account of the fluorspar process was published by John George Weygand in 1725, the recipe being given him by Matthäus Pauli, of Dresden, who in turn had become aware of this secret knowledge of an unknown English glassworker around 1720 (9). The first, though superficial, examination of the chemical reaction was published by Andreas Marggraf in 1768 (4). 

Identification of fluorspar

Inspired by Marggraf´s work, the Swedish apothecary Carl Wilhelm Scheele started , in 1771, a systematic investigation to find out the chemical nature of fluorspar and the details of its reaction with acids. He too observed the attack of glass by fumes which he obtained by slowly heating, in a glass retort, a mixture of fluorspar and sulfuric acid. The solid residue in the retort, extracted with water, revealed the presence of lime upon addition of ammonia. The fumes, if led into water, released a white mass identified as silica. The resulting solution showed an acid reaction. Scheele called it "Flußspatsäure" (acid of fluorspar, fluoric acid). On adding it to lime water a white precipitate was formed which showed the same behavior as fluorspar, i.e. fluoric acid could again be released upon treatment of the filtered and dried precipitate with sulfuric acid (10). 

It is thus Scheele´s work which showed means to identify fluorspar (a "fluate" of lime): 

 The chemical nature of the acid of fluorspar

Even  though the name "fluoric acid" (fr.: "acide fluorique", ital: "acido fluorico") applied to the new acid discovered by Scheele clearly reminds us today of the element "fluorine" bound in it, nothing was known by the time about the chemical nature of this acid, the name being merely derived from the latin term "fluores" for fluorspar. After Scheele´s first experiments, some researchers raised doubts whether it really is a new acid, but claimed it might be simple muriatic acid or an acid derived from the sulfuric acid used in the experiments. Years after Scheele had shown that the acid can also be made by treatment of fluorspar with phosphoric acid or nitric acid (10-12) it was still supposed by some researchers that it might be formed by a modification of phosphoric acid which often accompanies it in natural products (rock phosphate, fossil bone samples) (13, 14).

A new element - fluorine

When muriatic acid was identified as a compound of the newly discovered element chlorine with hydrogen (which fact also showed that oxygen [greek: "acid forming"] is not an essential component of acids, as was believed until then) fluoric acid was suddenly considered to be a hydrogen compound of another new element with properties similar to chlorine. The name "fluorine" at first was proposed for the new prospective element, later the term "Phtor" (greek for "destructive") seemed to be more appropriate because of the destructive properties of its compounds. But "Phtor" was accepted only in the eastern hemisphere (15).

The isolation of the new element, to demonstrate its existence, occupied many researchers for a long time. A first step was the preparation of pure water-free hydrofluoric acid by Thénard and Gay-Lussac (15,16). Their product fumed strongly in air, rapidly dissolved glass, and caused extraordinary burns on contact with the skin - a phenomenon the authors described in some detail. Other researchers experienced even more toxic effects, some had to pay a high price (severe disease or even loss of life) for their -finally unsuccessful- attempts to isolate the element, as they were not careful enough in handling the hydrogen fluoride (HF). Thénard and Gay-Lussac also described fluoboric acid, a new complex acid similar to fluosilicic acid. When the famous chemist Berzelius summarized, in 1824,  his experiments with a series of new fluorine compounds, many more fluoride-bearing natural minerals had alreday been discovered (e. g. apatites, cryolite, hornblendes) by chemists of the time, and sodium and potassium fluorides had already been prepared. Berzelius then showed that the fluorides of ammonium, magnesium, beryllium, aluminum, cadmium, copper, lead, tin, antimony, uranium, and many other metals differ from their salts of any other acids known at the time, and thus confirmed that fluoric acid bears in fact a new radical (16a). But its isolation still posed a challenge.

Until the French chemist Henri Moissan prepared elemental fluorine in 1886 (16), quite a number of researchers got an example of resistance by the way how vigorously it resisted any attempts to get it in the free state. Moissan prepared elemental fluorine by electrolysis (in a specially tightened apparatus) of liquefied, water-free hydrogen fluoride to which some potassium bifluoride had been added to increase electric conductance. Beginning shortly afterwards (17), a number of patents were filed on methods for the electrolytic production of elemental fluorine. However, its high reactivity and rather uncontrollable behaviour in certain reactions prevented any widespread uses in the chemical indusrtry for a long time. Most of its compounds were prepared, therefore,  by tricky indirect reactions involving fluorides. 

Properties of fluorine

Fluorine, a yellow gas (18), is the most electronegative and the most reactive chemical element. It reacts with nearly all organic and inorganic materials, even with gold and platinum. Hydrogen and fluorine react with explosive violence. With water, fluorine forms hydrofluoric acid and ozone. A jet of fluorine from a pressure container reacts with human flesh and can cause extremely severe burns that are very difficult to heal. Mechanisms of tissue destruction include destructive oxidation by fluorine, thermal damage from the heat of reaction, and tissue poisoning by HF formed. "HF is formed by the reaction of fluorine with moisture on the skin. HF is a protoplamic poison with great penetrating power and causes deep-seated burns that heal very slowly." Even the salts of fluorine ("fluorides") which collect on the inside of pipes, valves and other equipment are extremely dangerous when inhaled or ingested, therefore "every precaution should be taken to avoid breathing or swallowing them" (19).  

Military uses of elemental fluorine

During World War II fluorine was used for very special purposes: the Fiat Final Report No. 838 on "Elemental Fluorine" states that since 1940 Germany´s IG Farbenindustrie operated several fluorine electrolysis cells. One of them.was built at Gaitow during the war for a secret project of the Oberkommando des Heeres (German Army High Command). It "represented the largest production of elemental fluorine in Germany. The fluorine was reported to have been produced solely for the manufacture of a new incendiary agent, chlorine tri-fluoride" (20). An important finding in the research at Leverkusen "was the explosive property possessed by liquefied or compressed fluorine which had not been properly purified. In their initial work on storing elemental fluorine under high pressures a few explosions of the steel cylinders occurred. The explosive property of the fluorine was attributed to traces of such impurities as O₃, F₂O₂, OF₂ and ClOF, which were present in amounts too small to be determined."

In the United States, fluorine was used during World War II for the production of uranium hexafluoride, which, at elevated temperature, is a gas that may be used for the separation of uranium isotopes. The enriched radioactive uranium was used for the construction of the first atomic bombs which went down on Hiroshima and Nagasaki in 1945 (21,22). Uranium refining for nuclear energy is still one of the major uses for elemental fluorine. 

Too reactive to stay free

Given the high reactivity even in the presence of traces of impurities, it is obviously impossible to keep elemental fluorine in a free elemental state -except for a fraction of a second- under natural conditions.

References:

(1) Ackerknecht E.H.: "Geschichte der Medizin", Ferdinand Enke Verlag, Stuttgart, 1979, p.95; (2)  "Georgii Agricolae de re metallica libri XII", Basel 1556, German translation by G. Fraustedt, H. Prescher: "Bergbau und Hüttenkunde, 12 Bücher", Berlin 1974; (3) Vogel H.: "Agricola´s ´De re metallica´ im China der Ming-Zeit - früher Versuch west-östlichen Technologietransfers", Spektrum d. Wiss. No. 10 (Oct. 1992) p. 30; (4) Gmelins Handbuch der anorganischen Chemie, 8. Auflage, System-Nr. 5, "Fluor", Verlag Chemie, Leipzig/Berlin 1926, p.1; (5) "Georgii Agricolae Bermannus sive de re metallica", Basel 1530, German translation by H. Wilsdorf, H. Prescher and H. Techel: "Bermannus oder Über den Bergbau. Ein Dialog", Berlin 1955; (6) Berzelius J. J.: "De l´acide hydrofluorique" in "Traité de chimie", Vol. 2, Brüssel, 1833, p. 179; (7) Rabuteau A. P. A.: "Eléments de toxicologie", Paris 1887; (8) Roholm K.: "Fluorine Intoxication", Kopenhagen/London 1937; (9) Partington J. R.: "The early history of hydrofluoric acid", Mem. Proc. Manchester Lit. Phil. Soc. 67 (1923) 73; (10) "Carl Wilhelm Scheele: Sämmtliche physische und chemische Werke. Nach dem Tode des Verfassers gesammelt und in deutscher Sprache herausgegeben von Sigismund Friedrich Hermbstädt", 2 Vols., Unchanged reprint of the 1793 edition, Niederwalluf, 1971, Vol. 2, pp. 3-31 (first publ. 1771); (11) Ref. 10, pp. 235-246 (first publ. 1780); (12) Ref. 10, pp. 407-422 (first publ. 1786); (13) Pelletier B., Donadei L.: "Mémoirs sur le phosphate calcaire", Ann. Chim. 7 (1790) 79; (14) Morichini D.: "Analisi dello smalto di un dente fossile di elefante e dei denti umani. Memoria di Domenico Morichini presentata da Giachino Pessuti", Mem. Mat. Fis. Soc. ital. Sci. (Modena) 12:2 (1805) 73-88 and 268-269; (15) Banks R.E.: "Isolation of fluorine by Moissan: Setting the scene", J. Fluorine Chem. 33 (1986) 3-26; (16) Moissan H.: "Das Fluor und seine Verbindungen", transl. by Dr. Theodor Zettel, author. German Edition, Verlag von M. Krayn, Berlin 1900; (16a) Berzelius J. J.: "Untersuchungen über die Flussspathsäure und deren merkwürdigsten Verbindungen", Poggendorffs Annalen der Physik 1 (1824) 1-48 and pp. 189-230; (17) Société Poulenc frères and Maurice Meslans, Paris: "Apparat zur elektrolytischen Darstellung von Fluor", German Patent (DE) 129,825; filed June 27, 1900; granted April 14, 1902; (18) Burdon J., Emson B., Edwards A.J.: "Is fluorine gas really yellow?", J. Fluorine Chem. 34 (1987) 471; (19) United States Atomic Energy Commission, Oak Ridge, Tennessee: "Precautions to be observed in handling, shipping and storage of fluorine", declassified manuscript, June 14, 1946; (20) Karr, Errol H.: "Elemental Fluorine. IG Farbenindustrie Leverkusen", Technical Industrial Intelligence Agency, June 15, 1946, Fiat Final Report No. 838, Declassified; (21) Henry DeWolf: Smyth: "Atomic energy for military purposes. The official report on the development of the atomic bomb under the auspices of the United States Government, 1940 - 1945", written at the request of Maj. Gen. L. R. Groves, Princeton University Press, 1946; (22) Voegtlin C., Hodge H.C.: "Pharmacology and Toxicology of uranium compounds. With a section on the pharmacology and toxicology of fluorine and hydrogen fluoride", McGraw Hill Book Company, New York, Toronto, London, 1949

Source: http://www.fluoride-history.de