Fluor Chemische Eigenschaften,Einsatz,Produktion Methoden
ERSCHEINUNGSBILD
GELBES KOMPRIMIERTES GAS MIT STECHENDEM GERUCH.
PHYSIKALISCHE GEFAHREN
Das Gas ist schwerer als Luft.
CHEMISCHE GEFAHREN
Starkes Oxidationsmittel. Reagiert sehr heftig mit brennbaren und reduzierenden Stoffen. Reagiert sehr heftig mit Wasser unter Bildung giftiger und ?tzender D?mpfe: Ozon (s. ICSC 0068) und Fluorwasserstoff (s. ICSC 0283). Reagiert sehr heftig mit Ammoniak, Metallen, Oxidationsmitteln und vielen anderen Stoffen. Feuer- und Explosionsgefahr!
ARBEITSPLATZGRENZWERTE
TLV: 1 ppm (als TWA) 2 ppm (als STEL); (ACGIH 2005).
MAK: IIb (nicht festgelegt, aber Informationen vorhanden) (DFG 2006).
AUFNAHMEWEGE
Aufnahme in den K?rper durch Inhalation.
INHALATIONSGEFAHREN
Eine gesundheitssch?dliche Konzentration des Gases in der Luft wird beim Entweichen aus dem Beh?lter sehr schnell erreicht.
WIRKUNGEN BEI KURZZEITEXPOSITION
WIRKUNGEN BEI KURZZEITEXPOSITION: Das Gas wirkt stark ?tzend auf die Augen, die Haut und die Atmungsorgane. Inhalation des Gases kann zu Lungen?dem führen (s. Anm.). Die Flüssigkeit kann Erfrierungen hervorrufen. Die Auswirkungen treten u.U. verz?gert ein. ?rztliche Beobachtung notwendig.
LECKAGE
Gefahrenbereich verlassen! Fachmann zu Rate ziehen! Belüftung. Gasdichter Chemikalienschutzanzug mit umgebungsluftunabh?ngigem Atemschutzger?t.
R-S?tze Betriebsanweisung:
R7:Kann Brand verursachen.
R26:Sehr giftig beim Einatmen.
R35:Verursacht schwere Ver?tzungen.
S-S?tze Betriebsanweisung:
S9:Beh?lter an einem gut gelüfteten Ort aufbewahren.
S26:Bei Berührung mit den Augen sofort gründlich mit Wasser abspülen und Arzt konsultieren.
S36/37/39:Bei der Arbeit geeignete Schutzkleidung,Schutzhandschuhe und Schutzbrille/Gesichtsschutz tragen.
S45:Bei Unfall oder Unwohlsein sofort Arzt zuziehen (wenn m?glich, dieses Etikett vorzeigen).
Aussehen Eigenschaften
F2. Schwach grünlichgelbes, stark ätzendes Gas mit charakteristischem, durchdringendem Geruch.
Gefahren für Mensch und Umwelt
Fluor ist das stärkste Oxidationsmittel und reagiert mit vielen insbesondere brennbaren Stoffen äußerst heftig, zum Teil unter Flammenerscheinung. Kunststoffe und Kautschuk werden heftig angegriffen. PTFE ist beständig, bei erhöhter Temperatur und Strömung wirkt es auch darauf zerstörend. Metalle reagieren gegenüber Fluor unterschiedlich. Für Behälter sind bei Ausschluß von Feuchtigkeit Nickel, Gold und Monel sehr gut geeignet, während Chrom, Kupfer und Eisen nur gut geeignet sind; erhöhte Temperatur schränkt aber die Beständigkeit sehr stark ein. Stoffe wie Alkali- und Erdalkalimetalle, Zink,Zinn und Aluminium verbrennen lebhaft. Mit Wasser(-dampf) Bildung von Sauerstoff und Fluorwasserstoff.
Die Giftwirkung des Fluors ist in der Praxis von der Wirkung des Fluorids begleitet, da in Luft wie auch im Körper elementares Fluor unter Bildung von Fluorwasserstoff reduziert wird. Nach Einatmen schwere Reizungen an Augen und Atemwegen, Schwellung der Schleimhäute von Nase, Rachen und Luftröhre,Krämpfe der Atemmuskulatur. Nach Latenzzeit Erstickungsgefahr infolge Lungenödem. Nach Hautkontakt, auch mit konzentriertem Gas, schwere verbrennungsartige Verätzung möglich.
Schutzma?nahmen und Verhaltensregeln
Nur im Abzug arbeiten. Abgase über Waschflaschen führen. Flaschen und Anlageteile vor offenen Flammen und Wärmequellen sowie besonders vor Feuchtigkeit schützen. Arbeiten an Anlagen und Leitungen nur nach sorgfältigem Freispülen durchführen.
Säurebeständige Schutzhandschuhe (nur als kurzzeitiger Schutz).
Verhalten im Gefahrfall
Labor räumen; Umgebung warnen.
Raum nur mit umluftunabhängigem Atemschutzgerät und Schutzanzug betreten.
Stoff brennt selbst nicht. Löschmaßnahmen auf die Umgebung abstimmen.
Erste Hilfe
Nach Hautkontakt: Sofort gründlich unter fließendem Wasser spülen. Mit Polyethylenglykol 400 abtupfen. Arzt!
Nach Augenkontakt: Mindestens 15 Minuten unter fließendem Wasser bei weit geöffnetem Lidspalt ausspülen. Augenarzt!
Nach Einatmen: Frischluft. Auxiloson-Spray einatmen lassen. Arzt!
Nach Kleidungskontakt: Kontaminierte Kleidung sofort ausziehen. Betroffene Haut sofort mit viel Wasser abspülen.
Nach jedem Kontakt mit Fluor Arzt konsultieren.
Ersthelfer: siehe gesonderten Anschlag
Sachgerechte Entsorgung
Defekte Druckgasflaschen müssen durch eine Spezialfirma entsorgt werden.
Beschreibung
Fluorine is a highly toxic, pale yellow gas about
1.3 times as heavy as air at atmospheric temperature
and pressure. When cooled below its
boiling point (-306.8°F or -188.2°C), it is a
liquid about 1.5 times as dense as water.
Chemische Eigenschaften
Fluorine (F) is a chemical element(group VIla, halogens).It is a pale yellow,highly toxic, corrosive, flammable gas. It is a stable, extremely strong oxidant, which may react violently with combustible materials, including plastics, reducing agents, and organic material. It reacts with water to form corrosive acids. Fluorine is very toxic and may be fatal if inhaled. Fluorine reacts violently with many oxidising agents (e.g. perchlorates, peroxides, permanganates, chlorates, nitrates, chlorine, bromine, and fluorine), strong acids (hydrochloric, sulphuric, and nitric), organic compounds, combustible materials like oil and paper, hydrogen, bromine, iodine, and chemically active metals like, potassium, sodium, magnesium, and zinc.
Fluorine is the most electro negative of all elements and the most chemically energetic of all nonmetallic elements. Fluorine is a high-tonnage chemical that is used in production of fluorides, in synthesis of fluorocarbons,and as an oxidizer for rocket fuels. Because of its severe oxidizing characteristics, special permits are required for shipping of fluorine,and all containers,piping,and processing equipment used for fluorine service must be passivated prior to use. Thereafter, they must be designated for exclusive fluorine service.
Physikalische Eigenschaften
Fluorine does not occur in a free state in nature, and because fluorine is one of the mostreactive elements, no chemical can free it from any of its many compounds. The reason forthis is that fluorine atoms are the smallest of the halogens, meaning the electron donated by ametal (or some nonmetals) are closer to fluorine’s nucleus and thus exert a great force betweenthe fluorine nuclei and the elements giving up one electron. The positive nuclei of fluorinehave a strong tendency to gain electrons to complete the outer shell, which makes it a strongoxidizer.
Because the fluorine atom has only nine electrons, which are close to the nucleus, thepositive nucleus has a strong tendency to gain electrons to complete its outer shell. As a gasits density (specific gravity) is 1.695, and as a liquid, its density is 1.108. Its freezing point is–219.61°C, and its boiling point is –188°C. Fluorine, as a diatomic gas molecule (F
2), is paleyellow in color. Fluorine is the most electronegative nonmetallic element known (wants togain electrons) and is, therefore, the strongest oxidizing agent known.
Isotopes
There are a total of 16 isotopes of fluorine. Only one, F-19, is stable. It makesup 100% of the fluorine found on Earth. All the others are radioactive with half-livesranging from 2.5 milliseconds to 4.57100×10
-22 years.
Origin of Name
From the Latin and French words for “flow,” fluere.
Occurrence
Fluorine is the 13th most abundant element on the Earth. It makes up about 0.06% of theEarth’s crust. Fluorine is widely distributed in many types of rocks and minerals, but neverfound in its pure form. Fluorine is as plentiful as nitrogen, chlorine, and copper, but lessplentiful than aluminum or iron.
The most abundant fluorine mineral is fluorite—calcium fluoride (CaF
2)—which is oftenfound with other minerals, such as quartz, barite, calcite, sphalerite, and galena. It is mined in Cumberland, England, and in Illinois in the United States. Other minerals from which fluorineis recovered are fluorapatite, cryolite, and fluorspar, which are found in many countriesbut mainly in Mexico and Africa.
Today fluorine is produced by the electrolysis of potassium fluoride (KF), hydrofluoric acid(HF), and molten potassium acid fluoride (KHF
2).
Charakteristisch
Fluorine reacts violently with hydrogen compounds, including water and ammonia. It alsoreacts with metals, such as aluminum, zinc, and magnesium, sometimes bursting into flames,and with all organic compounds, in some cases resulting in such complex fluoride compoundsas fluorocarbon molecules. It is an extremely active, gaseous element that combines spontaneouslyand explosively with hydrogen, producing hydrogen fluoride acid (HF), which is usedto etch glass. It reacts with most metals except helium, neon, and argon. It forms many differenttypes of “salts” when combining with a variety of metals. Fluorine, as a diatomic gas,is extremely poisonous and irritating to the skin and lungs, as are many fluoride compounds.Fluorine and its compounds are also corrosive.
Verwenden
Fluorine is used in the manufacture of vari ous fluorocarbons and fluorides, as a rocketpropellant, and in many inorganic and or ganic syntheses.
Definition
Nonmetallic halogen element in group 17 of the periodic table. An 9, aw 18.99840, valence of 1, no other
stable isotopes, the most electronegative element
and most powerful oxidizing agent known.
Allgemeine Beschreibung
Fluorine is a pale yellow gas with a pungent odor. Fluorine is commonly shipped as a cryogenic liquid. Fluorine is toxic by inhalation and skin absorption. Contact with skin in lower than lethal concentrations causes chemical burns. Fluorine reacts with water to form hydrofluoric acid and oxygen. Fluorine is corrosive to most common materials. Fluorine reacts with most combustible materials to the point that ignition occurs. Under prolonged exposure to fire or intense heat the containers may violently rupture and rocket.
Air & Water Reaktionen
Water vapor will react combustibly with Fluorine; an explosive reaction occurs between liquid Fluorine and ice, after an intermediate induction period, [NASA SP-3037: 52(1967)]: If liquid air, which has stood for some time is treated with Fluorine, a precipitate is formed which is likely to explode. Explosive material is thought to be Fluorine Hydrate, [Mellor 2:11(1946-1947)].
Hazard
Many of the fluorine compounds, such as CFCs, are inert and nontoxic to humans. Butmany other types of compounds, particularly the salts and acids of fluorine, are very toxicwhen either inhaled or ingested. They are also strong irritants to the skin.
There is also danger of fire and explosion when fluorine combines with several elementsand organic compounds.
Poisonous fluoride salts are not toxic to the human body at the very low concentrationlevels used in drinking water and toothpaste to prevent dental decay.
Health Hazard
reactions; highly irritating and corrosive to the eyes, skin, and mucous membranes.
Toxicity The acute toxicity of fluorine is high. Even very low concentrations irritate the
respiratory tract, and brief exposure to 50 ppm can be intolerable. High
concentrations can cause severe damage to the respiratory system and can result in
the delayed onset of pulmonary edema, which may be fatal. Fluorine is highly
irritating to the eyes, and high concentrations cause severe injury and can lead to
permanent damage and blindness. Fluorine is extremely corrosive to the skin,
causing damage similar to second-degree thermal bums. Fluorine is not considered
to have adequate warning properties.
Chronic toxicity is unlikely to occur due to the corrosive effects of fluorine
exposure. Fluorine has not been found to be carcinogenic or to show reproductive or
developmental toxicity in humans.
Brandgefahr
Fluorine is not flammable, but is a very strong oxidizer, reacting vigorously with
most oxidizable materials at room temperature, frequently with ignition. Water
should not be used to fight fires involving fluorine
Flammability and Explosibility
Fluorine is not flammable, but is a very strong oxidizer, reacting vigorously with most oxidizable materials at room temperature, frequently with ignition. Water should not be used to fight fires involving fluorine.
Landwirtschaftliche Anwendung
Fluorine is the lightest of the halogens, occurring naturally in fluorapatite, fluorite and cryolite. A pale yellow toxic gas, fluorine is made by electrolysis of potassium fluoride in liquid hydrogen fluoride. It is the most reactive, electronegative and oxidizing of all elements, and reacts with almost all elements, giving fluorides. It is used in rocket propulsion and in the production of uranium and fluorocarbons.
Materials Uses
Nickel, iron, aluminum, magnesium, copper,
and certain of their alloys are quite satisfactory
for handling fluorine at room temperature, for
these are among the metals with which formation
of a surface fluoride film retards further
reaction.
m?gliche Exposition
Elemental fluorine is used in the con version of uranium tetrafluoride to uranium hexafluoride;
in the synthesis of organic and inorganic fluorine com pounds; and as an oxidizer in rocket fuel.
Environmental Fate
Fluorine remains persistent in the environment. In water,
fluorides attach to aluminum in freshwater and calcium and
magnesium in seawater and settle into the sediment. Fluorides
may be taken up from soil and accumulate in plants or
they may be deposited on the upper parts of the plants. The
amount of fluoride taken up by plants depends on the type of
plant, the nature of the soil, and the amount and form of
fluoride in the soil. Levels of fluorides in surface water
average about 0.2 ppm, while well water levels range from
0.02 to 1.5 ppm. The 15 000 water systems serving about 162
million people in the USA are fluoridated in the range of
0.7–1.2 ppm.
Lager
Work with fluorine requires special precautions and protective equipment and should be carried out only by specially trained personnel. Fluorine will react with many materials normally recommended for handling compressed gases.
Versand/Shipping
UN1045 Fluorine, compressed, Hazard Class:
2.3; Labels: 2.3-Poisonous gas, 5.1-Oxidizer, 8-Corrosive
material, Inhalation Hazard Zone A. Cylinders must be
transported in a secure upright position, in a well-ventilated
truck. Protect cylinder and labels from physical damage.
The owner of the compressed gas cylinder is the only entity
allowed by federal law (49CFR) to transport and refill
them. It is a violation of transportation regulations to refill
compressed gas cylinders without the express written per mission of the owner.
l?uterung methode
Pass the gas through a bed of NaF at 100o to remove HF and SiF4. [For description of stills used in fractional distillation, see Greenberg et al. J Phys Chem 65 1168 1961; Stein et al. Purification of Fluorine by Distillation, Argonne National Laboratory, ANL-6364 1961 (from Office of Technical Services, US Dept of Commerce, Washington 25).] HIGHLY TOXIC.
Inkompatibilit?ten
Fluorine is an extremely powerful oxi dizing gas. Keep away from heat, water, nitric acid, oxidi zers, organic compounds. Containers may explode if
heated. Reacts violently with reducing agents; ammonia, all
combustible materials, metals (except the metal containers
in which it is shipped). Reacts violently with H2O to form
hydrofluoric acid, oxygen and ozone. The most potent
oxidizer.
Waste disposal
Return refillable compressed
gas cylinders to supplier. Fluorine may be combusted by
means of a fluorine-hydrocarbon air burner followed by a
caustic scrubber and stack. Consult with environmental
regulatory agencies for guidance on acceptable disposal
practices. Generators of waste containing this contaminant
(≥100 kg/mo) must conform with EPA regulations gov erning storage, transportation, treatment, and waste
disposal.
Fluor Upstream-Materialien And Downstream Produkte
Upstream-Materialien
Downstream Produkte
