Fluorine is found in nature in the form of calcium fluoride, CaF₂, called fluorite, which forms regular crystals.

Fluorine Atomic Number 9 Meaning

Fluorine

Atomic Number:	9	Atomic Radius:	135 pm[8] pm (Van der Waals)
Atomic Symbol:	F	Melting Point:	-219.67 °C
Atomic Weight:	19.00	Boiling Point:	-188.11 °C
Electron Configuration:	[He]2s²2p⁵	Oxidation States:	−1 (oxidizes oxygen)

History

Name: Fluorine: Symbol: F: Atomic Number: 9: Atomic Mass: 18.998 atomic mass units: Number of Protons: 9: Number of Neutrons: 10: Number of Electrons: 9: Melting. Fluorine (F) Atomic Data for Fluorine (F) Atomic Number = 9 Atomic Weight = Reference E95: Isotope: Mass: Abundance: Spin: Mag Moment: 19 F. Atomic Structure of Fluorine; Chemical Properties of Fluorine; Physical Properties of Fluorine; Regulatory / Health; Who/When/Where/How. Fluorine Page Two. Nuclides / Isotopes; Potential Parent Nuclides. Fluorine Page Three. Common Chemical Compounds of Fluorine. Overview of Fluorine. Atomic Number: 9; Group: 17; Period: 2; Series: Halogens.

From the Latin and French fluere: flow or flux. In 1529, Georigius Agricola described the use of fluorspar as a flux, and as early as 1670 Schwandhard found that glass was etched when exposed to fluorspar treated with acid. Scheele and many later investigators, including Davy, Gay-Lussac, Lavoisier, and Thenard, experimented with hydrofluoric acid, some experiments ending tragically.

The element was finally isolated in 1866 by Moissan after nearly 74 years of continuous effort.

Properties

Fluorine is the most electronegative and reactive of all elements. It is a pale yellow, corrosive gas, which reacts with most organic and inorganic substances. Finely divided metals, glass, ceramics, carbon, and even water burn in fluorine with a bright flame.

Until World War II, there was no commercial production of elemental fluorine. The nuclear bomb project and nuclear energy applications, however, made it necessary to produce large quantities.

Uses

Fluorine and its compounds are used in producing uranium (from the hexafluoride) and more than 100 commercial fluorochemicals, including many high-temperature plastics. Hydrofluoric acid etches glass of light bulbs. Fluorochlorohydrocarbons are extensively used in air conditioning and refrigeration.

The presence of fluorine as a soluble fluoride in drinking water to the extent of 2 ppm may cause mottled enamel in teeth when used by children acquiring permanent teeth; in smaller amounts, however, fluoride helps prevent dental cavities.

Elemental fluorine has been studied as a rocket propellant as it has an exceptionally high specific impulse value.

Compounds

One hypothesis says that fluorine can be substituted for hydrogen wherever it occurs in organic compounds, which could lead to an astronomical number of new fluorine compounds. Compounds of fluorine with rare gases have now been confirmed in fluorides of xenon, radon, and krypton.

Handling

Elemental fluorine and the fluoride ion are highly toxic. The free element has a characteristic pungent odor, detectable in concentrations as low as 20 ppb, which is below the safe working level. The recommended maximum allowable concentration for a daily 8-hour time-weighted exposure is 1 ppm.

Safe handling techniques enable the transport liquid fluorine by the ton.

Chemical properties of fluorine - Health effects of fluorine - Environmental effects of fluorine

9
Atomic mass	18.998403 g.mol^-1
Electronegativity according to Pauling	4
Density	1.8*10^-3 g.cm^-3 at 20°C
Melting point	-219.6 °C Jeep transmission.
Boiling point	-188 °C
Vanderwaals radius	0.135 nm
Ionic radius	0.136 nm (-1) ; 0.007 (+7)
Isotopes	2
Electronic shell	[ He ] 2s²2p⁵
Energy of first ionisation	1680.6 kJ.mol^-1
Energy of second ionisation	3134 kJ.mol^-1
Energy of third ionisation	6050 kJ mol^-1
Standard potential	Half life 2 for mac os. - 2.87 V
Discovered by	Moissan in 1886

Fluorine

Fluorine is an univalent poisonous gaseous halogen, it is pale yellow-green and it is the most chemically reactive and electronegative of all the elements. Fluorine readily forms compounds with most other elements, even with the noble gases krypton, xenon and radon. It is so reactive that glass, metals, and even water, as well as other substances, burn with a bright flame in a jet of fluorine gas.
In aqueous solution, fluorine commonly occurs as the fluoride ion F^-. Fluorides are compounds that combine fluoride with some positively charged counterpart.

Applications

Atomic fluorine and molecular fluorine are used for plasma etching in semiconductor manufacturing, flat panel display production and MEMs fabrication.
Fluorine is indirectly used in the production of low friction plastics such as teflon and in halons such as freon, in the production of uranium. Fluorochlorohydrocarbons are used extensively in air conditioning and in refrigeration.
Fluorides are often added to toothpaste and, somewhat controversially, to municipal water supplies to prevent dental cavities. Fore more information visit our page on mineral water.

Fluorine in the environment

Annual world production of the mineral fluorite in around 4 million tonnes, and there are around 120 million tonnes of mineral reserves. The main mining areas for fluorite are China, Mexico and Western Europe.
Fluorine occurs naturally in the earth's crust where it can be found in rocks, coal and clay. Fluorides are released into the air in wind-blown soil. Fluorine is the 13th most aboundant element in the Earth's crust: 950 ppm are contanined in it. Soils contain approximatively 330 ppm of fluorine, ranging from 150 to 400 ppm. Some solis can have as much as 1000 ppm and contaminated solis have been found with 3500 ppm. Hydrogen fluorides can be released into air through combustion processes in the industry. Fluorides that are found in air will eventually drop onto land or into water. When fluorine is attached to very small particles it can remain in the air for a long period of time.
In the atmosphere 0.6 ppb of fluorine are present as salt spray and organicochloride compounds. Up to 50 ppb has been recorded in city environments.

Health effects of fluorine

Small amounts of fluorine are naturally present in water, air, plants and animals. As a result

Fluorine Atomic Number