Fluorine Uses

The history of fluorine dates back to 1771 AD, when it was first identified by Scheele. In 1529, it was described in the use of fluorspar, as a flux, by Georgius Agricola. After nearly 100 years, in 1670 it was found that fluorspar treated acid could help in glass etching. Then over 200 years later, in 1866 with nearly 74 years of continuous effort, fluorine was isolated by Henry Moissan of France.

Flourine (F) is a member of Group VII A in the periodic table. It is the lightest non-metallic halogen of the group, that includes Chlorine (Cl), Bromine (Br), Iodine (I) and Astatine (At). The name fluorine is derived from a Latin word fluore for flow or flux. This is because fluorspar, calcium and fluoride were used in smelting metals to make them flow.

Properties of Fluorine
Some of the properties of fluorine can be listed as under:

• Fluorine is one of the most electronegative and reactive chemical elements.
• It is pale yellow in color and a corrosive gas. It can react with all organic and inorganic compounds.
• Glass, ceramics, carbon, finely divided metals and even water burn in fluorine with a yellow flame.
• Fluorine has a pungent odor and can be easily detected in concentrations as low as 20 parts per billion
• This is a highly reactive element and is never found in 'free form'. The most common fluorine minerals are fluorspar (CaF²), apatite [Ca₅(F,Cl,OH)(PO₄)3] and cryolite (Na₃AlF₆).

Reactions of Fluorine
Florine can react with hydrogen explosively even in dark and at low temperatures. It reacts violently with water to form hydrogen fluoride and releases oxygen that is highly charged with ozone.
2 F₂ + 2 H₂O ==> 4 HF + O₂

Fluorine also reacts with potassium chlorate as it is an powerful oxidizing agent. It oxidizes the potassium chlorate solution into potassium perchlorate.
F₂ + 2 KClO₃ + H₂O ==> 2 HF + KClO₄

Fluorine also reacts with sulfur, selenium, and tellurium to form halides. It cannot react with oxygen or nitrogen directly. It can combine with chlorine only when heated by forming a gaseous product of chlorine fluoride and chlorine trifluoride. Fluorine can readily combine with bromine and iodine and form colorless liquids like BrF³ and IF⁵. This was a short description of the chemical characteristics of this very reactive element, fluorine. Let us now see, what are the uses of fluorine.

What is Fluorine Used for?
There are some commercial uses of fluorine that will help you understand all the areas where fluorine uses are involved:

• The most common use of fluorine in its elemental form is in rocket fuels. It has a working similar to oxygen and also helps the other matters in rocket fuel to burn.
• The other uses of elemental fluorine is in manufacturing and the chemical laboratories. Isotopically fractionated uranium is created with the help of fluorinated compounds, that is an important step in uranium purification in power plants.
• Fluorinated compounds help in production of polymers and plastics, some of which are specially designed to withstand high temperatures and large amount of stress.
• Fluorinated compounds are used to make polytetrafluoroethylene (teflon) that is used in manufacturing teflon ^TM and Tefzel _TM.
• Fluorine that is combined with oxygen has replaced chloroflurocarbons or CFC's used in refrigerator coolers. It was found that CFC's were very dangerous for Earth's ozone layer and thus, were replaced by fluorinated compounds.
• Fluorinated compounds are used for glass etching and other industries involving hydrofluoric acid.
• Hydrofluoric acid is used to mark light bulbs and highly sensitive glass pieces that are too thin for other etching methods.
• The most common use of fluorine, that is a part of everyone's life, is as a common ingredient in toothpastes. Fluoride is used to prevent tooth decay and thus added to toothpastes and mouth washes.
• Young children with developing teeth can be made to grow stronger, healthier and resistant to tooth decay by using fluorinated toothpastes.
• The other common use of fluorinated compounds is in purification of public water supplies. This has shown to reduce the incidence of dental carries and other dental problems greatly.

Facts About Fluorine
Some of the facts about fluorine, which you may like to know, have been listed as under.

• Florine is a highly explosive, corrosive and poisonous halogen.
• Fluorine is found in gaseous state at room temperature.
• Fluorine is obtained from its mineral fluorite forms, from nature.
• The atomic number of Fluorine is 9 and the atomic mass is 18.998404 amu.
• The melting point of fluorine is -219.62°C and boiling point is -188.14 °C .
• Fluorine is a diatomic element and can react with all elements including noble gases.
• It has a higher oxidation potential than ozone.
• Fluorine can damage the soft tissues of the respiratory tract.

These are some of the fluorine uses and facts about fluorine. Fluorine is abundantly found in the Earth's crust. Fluorine is being imported to United States since 1995, after the last remaining mines closed down. This highly reactive element is surely one of the most commercially used elements of the periodic table.