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7 Interesting Facts Of Fluorine

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Fluorine is a chemical element, with symbol F and has an atomic number 9. It is the lightest halogen and exists as an exceedingly hazardous light yellow diatomic gas at normal conditions.

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7 Interesting Facts Of Fluorine

  1. 1. www.worldofchemicals.com 7 Interesting Facts Of Fluorine www.worldofchemicals.comhttps://goo.gl/Esz8vi
  2. 2. What is Fluorine? • Fluorine is a chemical element, with symbol F and has an atomic  number 9.  • It is the lightest halogen and exists as an exceedingly hazardous  light yellow diatomic gas at normal conditions.  • As the most electronegative component, it is reactive in nature.  • Every other component, including some noble gasses forms  compounds with fluorine. •  Fluorine reacts to all other elements and no chemical substance  can liberate fluorine from any of its compounds. Hence, fluorine  does not exist free in nature and was difficult for scientists to  discover.  • It exits in volcanic gasses and warm waters. Its main source is  fluorite; however, it also occurs in cryolite, seawater, bones and  teeth. Fluorine is produced by electrolysis under unique conditions. www.worldofchemicals.comhttps://goo.gl/Esz8vi
  3. 3. How did fluorine get its name? • Fluorine is derived from the Latin word "Fluere" which  signifies "Stream" or "Flux".  • Fluorine as calcium fluoride, or fluorite, was utilized as a  flux in mineral refining.  • Natural fluorine is a light yellow gas that is dangerous,  destructive and reactive.  • It is the most electronegative of all the elements and  responds with about all natural and inorganic  substances, including metal, glass, pottery and water.  • Generally fluorine forms compounds with the non- responsive noble gasses, including xenon, radon and  krypton. www.worldofchemicals.comhttps://goo.gl/Esz8vi
  4. 4. What are some Characteristics of fluorine (F) that distinguish from other elements? • Electron Configuration: Fluorine molecules have nine electrons, one less than neon, and electron configuration of 1s22s22p5: two electrons in a filled inward shell and seven in outer shell requiring one more to be filled. The external electrons are incapable at atomic protecting, and experience a high effective atomic charge of 9-2 = 7; this influences the atom’s physical property. • Reactivity: Reactions of basic fluorine with metals require different conditions. Alkali metals cause blasts and alkaline metals are dynamic; to keep passivation from the formation of metal fluoride layers, other metals such as aluminium and iron must be powdered. • Isotopes: Only one isotope of fluorine occurs normally in large quantity, the steady isotope 19 F. It has a high magnetogyric proportion and is sensible to magnetic fields; since it is likewise the main stable isotope, it is utilized as magnetic resonance imaging. www.worldofchemicals.comhttps://goo.gl/Esz8vi
  5. 5. What are some uses of fluorine (F)? • Fluorine is a gas under normal temperatures and pressures. • It is normally shipped as a compressed gas in cylinders or generated by electrolysis of hydrogen fluoride or by recycling chemical products containing fluoride. • Hydrofluoric corrosive (HF) is utilized to cut glass, including the greater part of the glass used in manufacturing bulbs. • Fluorine joins with carbon to shape a class of compounds known as fluorocarbons. • Few of these compounds, for example: dichlorodifluoromethane (CF2Cl2) were broadly utilized as a part of aerating and AC’s and refrigerating system and in vaporized spray cans. Today, fluorine is still produced through the electrolysis of potassium fluoride and hydrofluoric acid and through the electrolysis of liquid potassium acid fluoride (KHF2). www.worldofchemicals.comhttps://goo.gl/Esz8vi
  6. 6. Medical implication of fluorine (F) • Studies from the mid-twentieth century onwards indicate topical fluoride lessens dental caries. • This was first ascribed to the transformation of tooth enamel hydroxyapatite into the stronger fluorapatite, yet thinks about on pre- fluoridated teeth discredited this hypothesis. • Reviews of the scholarly literature in 2000 and 2007 related water fluoridation with a critical decrease of tooth decay in youngsters. • 20 per cent of present day pharmaceuticals contain fluorine. • The major part of inhaled sedatives is intensely fluorinated; the model halothane is considerably more idle and powerful than its contemporaries. www.worldofchemicals.comhttps://goo.gl/Esz8vi
  7. 7. Where is fluorine found in the Environment? • Presence of fluorine in natural water is controlled by weathering of rocks. • Weathering is a complete process involving adsorption-desorption and dissolution precipitation reaction. • During weathering the circulation of water in rocks and soils, fluorine also be dissolve in ground water. • Fluorine in apatite is very stable while the fluorine from mica is drained out quickly. • The occurrence of fluorine in ground water varies depending upon the type of the rocks from which it originate www.worldofchemicals.comhttps://goo.gl/Esz8vi
  8. 8. Interesting facts about fluorine (F) • Fluorine is the most receptive and most electronegative of all the chemical elements. The elements with which it doesn't respond are oxygen, helium, neon, and argon. Fluorine is the only element which will shape compounds with noble gasses xenon, krypton, and radon. • Fluorine is the thirteenth most abundant component in the Earth's crust. It is reactive to the point that it is not discovered normally in natural form, but rather just in mixes. Fluorine is found in minerals, including fluorite, topaz, and feldspar. • It is reactive in nature, storing fluorine is tough. Hydrofluoric acid (HF), for instance, is so destructive it will break up glass. All things being equal, HF is more secure and is easier to transport and handle than pure fluorine. • There is just a single stable isotope of fluorine, F-19. www.worldofchemicals.comhttps://goo.gl/Esz8vi
  9. 9. Thank You https://goo.gl/Esz8vi To read this article follow the link: www.worldofchemicals.comhttps://goo.gl/Esz8vi
  10. 10. Thank You https://goo.gl/Esz8vi To read this article follow the link: www.worldofchemicals.comhttps://goo.gl/Esz8vi

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