Fluorine

F l u o r i n e =)

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Fluorine salts, known as fluorides, were used for centuries in welding metals and for frosting glass before the element itself was isolated. Fluorine gas is the most reactive of all the elements and quickly attacks all metals - steel wool bursts into flames when exposed to it! Fluorine is used to make uranium hexafluoride, needed by the nuclear power industry, and sulfur hexafluoride insulating gas for high-power electricity transformers, and to treat polythene to make it impermeable to solvents. Fluoride is added to drinking water in some areas and to toothpaste to help prevent tooth decay. The average human body contains about 3 milligrams; too much fluo

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 * Name:** Fluorine
 * Symbol:** F
 * Atomic Number:** 9
 * Atomic Mass:** 18.998404 amu
 * Melting Point:** -219.62 °C (53.530006 K, -363.31598 °F)
 * Boiling Point:** -188.14 °C (85.01 K, -306.652 °F)
 * Number of Protons/Electrons:** 9
 * Number of Neutrons:** 10
 * Classification:** Halogen
 * Crystal Structure:** Cubic
 * Density @ 293 K:** 1.696 g/cm3
 * Color:** Greenish ride is toxic.

Protons:9 Neutrons:10

Henri Moissan was born on September 8, 1852, in Paris, France. He worked in the laboratory at the Museum of Natural History and the School of Pharmacy in Paris. Afterward, Moissan became a professor of toxicology in 1886 and inorganic chemistry in 1889 at the School of Pharmacy. It was during this time that Moissan began researching fluorine compounds. In 1886, he isolated the reactive gas fluorine and studied its behaviors with other elements. In 1900, he published his studies in, Le Fluor et ses composés (“Fluorine and Its Compounds). Moissan died at the age of 54.

[|http://www.jewishvirtuallibrary.org/jsource/biography/moissan.]