Week 6: Halogen of the Week- Fluorine

Name: Fluorine
Symbol: F
Atomic number: 9
Atomic weight: 18.998.4032
Group in periodic table: 17
Group name: Transition non-metal
Period in periodic table: 2
Block in periodic table: p
Color: pale yellow or brown gas
Classification: Halogen

F2 is a supremely reactive, poisonous, pale, yellowish brown gas. Elemental fluorine is the most chemically reactive and electronegative of all the elements and it will readily "burn" hydrocarbons at room temperature, making molecular fluorine is highly dangerous, more so than other halogens such as the poisonous chlorine gas.

Fluorine's highest electro-negativity, so it readily forms compounds with most other elements, and its small atomic radius gives unique properties to many of its compounds. For example, the carbon–fluorine bond is one of the strongest bonds in organic chemistry. Drugs are often fluorinated, to prevent their metabolism and prolong their half-lives.

F2 is a corrosive pale yellow or brown gas that is a powerful oxidizing agent. Fluorine combines with the noble gases argon, krypton, xenon, and radon. Even in dark, cool conditions, fluorine reacts explosively with hydrogen. Fluorides are compounds that combine fluorine with some positively charged counterpart. They often consist of crystalline ionic salts. Fluorine compounds with metals are among the most stable of salts.

The mineral fluorspar (also called fluorite), consisting mainly of calcium fluoride, was described in 1530 by Georgius Agricola for its use as a flux which is used to promote the fusion of metals or minerals. The name Fluorine comes from the Latin: fluere, meaning "to flow".

Fluorine is incorporated into compounds with biological activity. And while Fluorine is not an essential nutrient, it had been thought that it had an important role to play in preventing tooth decay. However, according to Paul Pitchford (Healing With Whole Foods), that is a total misinformation. In fact, according to Paul, Flourine is a by-product of the alluminum industry which used to be very costly to dispose of. Then, someone had the bright idea of using it in drinking water and toothpaste supposedly as a preventative of tooth decay. While the exterior of the teeth may be protected, frequently, the inner core of the teeth are rotten. Also, because Fluorine and the other halogens have lighter molecular weights than iodine, they can offset and displace it in the body, causing a host of problems with the endocrine system and related glands that rely on iodine for their proper functioning.