Fluorine

By Shale Briskin

FluorineFluorine

• General Information• The Discovery of Fluorine• Characteristics• Sources• Uses• Bohr-Rutherford Diagram• Bibliography/References

General Information

• Atomic Number: 9• Atomic Mass Number: 18.998 atomic mass

units (amu)• Located in Halogen Group 17 and Period 2• Valence Electron Number: 7• Electron Configuration: 1s22s22p5

• Ionic Bond: -1• Yellowish-brown appearance

The Discovery of Fluorine• Fluorine was described in fluorite form in 1530 by

Georgius Agricola for its use in flux.• In 1886, fluorine was finally isolated by Henri

Moissan via the electrolysis of potassium fluoride and hydrofluoric acid.

• Moissan also thoroughly isolated the fluorine gas from the hydrogen gas.

• Other chemists had spent the previous 74 years trying to do what Moissan did.

• The first big-scale production of fluorine was needed for the atomic bomb Manhattan project in World War II.

Characteristics• See General Info Section• Gas phase• 3.98 electronegativity (Pauling scale)• Toxic• 1st Ionization Energy: 1681 kJ/mol• Density: 0°C; 101.325 kPa; 1.7 g/L• Melting Point: 53.53 °K; -219.62 °C• Atomic Radius: 50 pm• Covalent Radius: 71 pm• Nonmagnetic• Multiple Isotopes, including Fluorine-18

Sources• Fluorine-18 (a 9-neutron isotope) is an important

source of positrons, which are the antiparticle/antimatter counterparts of electrons

• Fluorine appears in fluorspar (CaF) and cryolite (Na2AF6)

• By electrolyzing a solution of potassium hydrogen fluoride with anhydrous hydrogen fluoride in a container of transparent fluorspar or metal, fluorine can be collected

• Fluorine can also be obtained from mineral fluorite• Major mining areas include the U.S., Canada,

England, Russia, Mexico, and Italy

Uses• Fluorine and its compounds are used in producing

isotopically fractionated/pure uranium• Hydrofluoric acid is used to etch the glass of light

bulbs• Small amounts of fluorides in water prevent tooth

decay• Fluorine is indirectly used in the production of low

friction plastics such as Teflon, and in halons such as Freon.

• Sodium hexafluoroaluminate (cryolite), is used in the electrolysis of aluminum

• Sodium fluoride has been used as an insecticide, and particularly against cockroaches

• Fluorochlorohydrocarbons are used in both air conditioning and refrigeration

Bohr-Rutherford Diagram

199F

Bibliography/References• Barbalace, Kenneth. Periodic Table of Elements - Fluorine –F. 15 Jan. 2007.

<http://EnvironmentalChemistry.com//yogi/periodic/F.html> (15 Jan. 2007).

• Bentor, Yinon. Chemical Element.com - Fluorine. 15 Jan. 2007. <http://www.chemicalelements.com/elements/f.html> (15 Jan. 2007).

• Bohr-Rutherford Diagrams. 15 Jan. 2007. <http://www.tvdsb.on.ca/saunders/courses/online/SNC1D/McIntosh/chemistry/bohr-rutherford_diagrams.htm> (15 Jan. 2007).

• "Fluorine." Wikipedia, The Free Encyclopedia. 14 Jan 2007, 18:03 UTC. <http://en.wikipedia.org/w/index.php?title=Fluorine&oldid=100692146>. (15 Jan 2007).

• Helmenstine, Anne Marie. Fluorine. 15 Jan 2007. <http://chemistry.about.com/library/blf.htm> (15 Jan. 2007).

• "Positron." Wikipedia, The Free Encyclopedia. 13 Jan 2007, 18:04 UTC. <http://en.wikipedia.org/w/index.php?title=Positron&oldid=100475302>. (15 Jan 2007).

• Thomas Jefferson National Accelerator Facility - Office of Science Education. “It’s Elemental: The Element Fluorine.” 15 Jan. 2007. <http://education.jlab.org/itselemental/ele009.html> (15 Jan. 2007).

• Winter, Mark. Periodic Table: Scholar Edition: Fluorine: Uses. 15 Jan. 2007. <http://www.webelements.com/webelements/scholar/elements/fluorine/uses.html> (15 Jan. 2007).