Flourine

Fluorine

Element Type: Halogen

Atomic Number: 9

Symbol: F

By: Cassandra Alozie

Element Properties:

Bohr Model of Fluorine

Electron Configuration:[He] 2s2 2p5

Periodic Table

• Fluorine is found in nature in the form of Calcium Fluoride (Fluorite) which at standard state, forms crystal structures.
• Fluorine is the most electronegative and reactive element.
• At standard conditions, Fluorine can also be found as a pale yellow, corrosive gas that reacts with most inorganice and organic compounds.

Atomic Mass: 18.998403 amu

Melting Point: 53.48 K

Boiling Point: 85.03 K

Density: 1.697 g/L

Electronegativity: 3.98

Discovery:

Ferdinand Frederick Henri Moissan

Group 17:

HALOGENS

• Althought many scietiest before were thought to have experimented with other derivatives of fluorine as early as 1810, French Scientist, Ferdinand Frederick Henry Moissan, is credited for the isolation--and thus discovery-- of flourine in 1866.
• earned Nobel Peace Price in 1906 for successfully isolation Fluorine.

Period 2

FUN FACT!

"Fluorine ranks 24th in universal abundace and 13th in terrestrial abundance."

Sources:

Uses:

References:

• Fluorine occurs in fluorspar (CaF) and cryolite and is largely distributed in other minerals.

Elemental fluorine is used as a rocket propellant for its high specific impulse value.

Other Uses:

• http://www.rsc.org/periodic-table/element/9/fluorine
• http://www.livescience.com/28779-fluorine.html
• http://chemistry.about.com/od/10elementfacts/fl/10-Interesting-Fluorine-Facts.htm
• http://www.chemicalelements.com/elements/f.html

Interesting Facts:

Biological Uses:

• Biologically, Fluoride is an essentiol ion used by many animals for teeth and bone streghthening.
• In some cases, fluoride is also added to water in miniscule amounts, as it is thought to prevent dental cavities.

• was no commercial production of fluorine until World War II.
• The development of the Atomic Bomb and other nuclear weapons made the production of Fluorine necessary.
• In the nuclear power industry, fluorine is used to seperate uranium isotopes and also used to make insulatin gas for high-power electricity transformers.
• Before then, fluorine salts, flourides, were primarily used for welding and frosting glass.
• Fluorine is also notably used in many solvents and high-temperature plastics such as TEFLON (polytetrafluoroethylene).

• Fluorine is one of the few elements that can attack diamond.
• There is only one stable isotope of fluorine, F19.
• Although fluorine is relatively common on Earth, it is rare in the universe.

Environmental Effects:

• Plant exposure to fluorine, even in low concentrations, will damage leaves and stunt growth.
• Animals that are exposed to fluorine by fluorine-containing plants, may accumulate large amounts of fluorine in body, which in effect causes dental decay and bone degradation.

• When fluorine from the air ends up in water it will settle into the sediment. When it ends up in soils, fluorine will become strongly attached to soil particles. In the environment fluorine cannot be destroyed; it can only change form.