Element Fluorine - F
2020-11-21 by Nick Connor Atomic Mass of Fluorine Atomic mass of Fluorine is 18.9984 u. Element Fluorine (F), Group 17, Atomic Number 9, p-block, Mass 18.998. Sources, facts, uses, scarcity (SRI), podcasts, alchemical symbols, videos and images.
Comprehensive data on the chemical element Fluorine is provided on this page; including scores of properties, element names in many languages, most known nuclides of Fluorine. Common chemical compounds are also provided for many elements. In addition technical terms are linked to their definitions and the menu contains links to related articles that are a great aid in one's studies.
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Overview of Fluorine
- Atomic Number: 9
- Group: 17
- Period: 2
- Series: Halogens
Fluorine's Name in Other Languages
- Latin: Fluorum
- Czech: Fluor
- Croatian: Fluor
- French: Fluor
- German: Fluor - r
- Italian: Fluoro
- Norwegian: Fluor
- Portuguese: Flúor
- Russian: Фтор
- Spanish: Flúor
- Swedish: Fluor
Atomic Structure of Fluorine
- Atomic Radius: 0.57Å
- Atomic Volume: 17.1cm3/mol
- Covalent Radius: 0.72Å
- Cross Section (Thermal Neutron Capture)σa/barns: 0.0096
- Crystal Structure: Cubic
- Electron Configuration:
- 1s2 2s2p5
- Electrons per Energy Level: 2,7
- Shell Model
- Shell Model
- Ionic Radius: 1.33Å
- Filling Orbital: 2p5
- Number of Electrons (with no charge): 9
- Number of Neutrons (most common/stable nuclide): 10
- Number of Protons: 9
- Oxidation States: -1
- Valence Electrons: 2s2p5
- Electron Dot Model
- Electron Dot Model
Chemical Properties of Fluorine
- Electrochemical Equivalent: 0.70883g/amp-hr
- Electron Work Function:
- Electronegativity: 3.98 (Pauling); 4.1 (Allrod Rochow)
- Heat of Fusion: 0.2552kJ/mol
- Incompatibilities:
- Water, nitric acid, oxidizers, organic compounds
- Ionization Potential
- First: 17.422
- Second: 34.97
- Third: 62.707
- Valence Electron Potential (-eV): -10.1
Physical Properties of Fluorine
- Atomic Mass Average: 18.9984
- Boiling Point: 85.1K -188.05°C -306.49°F
- Coefficient of lineal thermal expansion/K-1: N/A
- Conductivity
- Electrical:
Thermal: 0.000279 W/cmK
- Electrical:
- Density: 1.696g/L @ 273K & 1atm
- Description:
- Greenish-yellow gas of the Halogen family
- Enthalpy of Atomization: 79.08 kJ/mole @ 25°C
- Enthalpy of Fusion: 0.26 kJ/mole
- Enthalpy of Vaporization: 3.31 kJ/mole
- Flammablity Class: Non-flammable gas (extreme oxidizer)
- Freezing Point:see melting point
- Heat of Vaporization: 3.2698kJ/mol
- Melting Point: 53.63K -219.52°C -363.14°F
- Molar Volume: 17.1 cm3/mole
- Optical Refractive Index: 1.000195
- Physical State (at 20°C & 1atm): Gas
- Realitive Gas Density (Air=1) = 1.31
- Specific Heat: 0.82J/gK
Regulatory / Health
- CAS Number
- 7782-41-4 cryogenic liquid
- UN/NA ID and ERG Guide Number
- 1045 / 124 compressed
- 9192 / 167 cryogenic liquid
- RTECS: LM6475000
- NFPA 704
- Health:
- Fire:
- Reactivity:
- Special Hazard: OxidizerOSHAPermissible Exposure Limit (PEL)
- 1 ppm = 1.55mg/m3 @ 25°C & 1 atm
- TWA: 0.1 ppm
- OSHA PEL Vacated 1989
- TWA: 0.1 ppm
- NIOSHRecommended Exposure Limit (REL)
- TWA: 0.1 ppm
- IDLH: 25 ppm
- Routes of Exposure: Inhalation; Skin and/or eye contact
- Target Organs: Eyes, skin, respiratory system, liver, kidneys
- Levels In Humans:
Note: this data represents naturally occuring levels of elements in the typical human, it DOES NOT represent recommended daily allowances.- Blood/mg dm-3: 0.5
- Bone/p.p.m: 2000-12,000
- Liver/p.p.m: 0.22-7
- Muscle/p.p.m: 0.05
- Daily Dietary Intake: 0.3-0.5 mg
- Total Mass In Avg. 70kg human: 2.6 g
Who / Where / When / How
- Discoverer: Henri Moissan
- Discovery Location: Paris France
- Discovery Year: 1886
- Name Origin:
- Latin: fluo (flow).
- Abundance of Fluorine:
- Earth's Crust/p.p.m.: 950
- Seawater/p.p.m.:
- Atlantic Suface: 0.0001
- Atlantic Deep: 0.000096
- Pacific Surface: 0.0001
- Pacific Deep: 0.00004
- Atmosphere/p.p.m.: N/A
- Sun (Relative to H=1E12): 0.000363
- Sources of Fluorine:
- Found in the minerals fluorite (CaF2) and cryolite (Na2AlF6). Around 2,400 tons of fluorine gas and 4,700,000 tons of fluorite are produced each year. Primary mining areas are Canada, USA, UK, Russia, Mexico and Italy.
- Uses of Fluorine:
- Combines more readily than any other element. Used in refrigerants and other chloro fluorocarbons. Also in toothpaste as sodium fluoride (NaF) and stannous fluoride (SnF2); also in Teflon.
- Additional Notes:
- Fluorine gas is highly toxic and corrosive. Even exposure to low concentrations causes lung and eye irritation. Metal fluorides are also very toxic while organic fluorides are often quite harmless.
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References
A list of reference sources used to compile the data provided on our periodic table of elements can be found on the main periodic table page.Related Resources
- Anatomy of the Atom
Answers many questions regarding the structure of atoms. - Molarity, Molality and Normality
Introduces stoichiometry and explains the differences between molarity, molality and normality. - Molar Mass Calculations and Javascript Calculator
Molar mass calculations are explained and there is a JavaScript calculator to aid calculations. - Chemical Database
This database focuses on the most common chemical compounds used in the home and industry.
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Fluorine Atomic Number And Mass Number
Alternative Title: F
Fluorine (F), most reactive chemical element and the lightest member of the halogen elements, or Group 17 (Group VIIa) of the periodic table. Its chemical activity can be attributed to its extreme ability to attract electrons (it is the most electronegative element) and to the small size of its atoms.
118 Names and Symbols of the Periodic Table Quiz
The periodic table is made up of 118 elements. How well do you know their symbols? In this quiz you’ll be shown all 118 chemical symbols, and you’ll need to choose the name of the chemical element that each one represents.
atomic number | 9 |
---|---|
atomic weight | 18.998403163 |
melting point | −219.62 °C (−363.32 °F) |
boiling point | −188 °C (−306 °F) |
density (1 atm, 0 °C or 32 °F) | 1.696 g/litre (0.226 ounce/gallon) |
oxidation states | −1 |
electron config. | 1s22s22p5 |
History
The fluorine-containing mineral fluorspar (or fluorite) was described in 1529 by the German physician and mineralogist Georgius Agricola. It appears likely that crude hydrofluoric acid was first prepared by an unknown English glassworker in 1720. In 1771 the Swedish chemist Carl Wilhelm Scheele obtained hydrofluoric acid in an impure state by heating fluorspar with concentrated sulfuric acid in a glass retort, which was greatly corroded by the product; as a result, vessels made of metal were used in subsequent experiments with the substance. The nearly anhydrous acid was prepared in 1809, and two years later the French physicist André-Marie Ampère suggested that it was a compound of hydrogen with an unknown element, analogous to chlorine, for which he suggested the name fluorine. Fluorspar was then recognized to be calcium fluoride.
The isolation of fluorine was for a long time one of the chief unsolved problems in inorganic chemistry, and it was not until 1886 that the French chemist Henri Moissan prepared the element by electrolyzing a solution of potassium hydrogen fluoride in hydrogen fluoride. He received the 1906 Nobel Prize for Chemistry for isolating fluorine. The difficulty in handling the element and its toxic properties contributed to the slow progress in fluorine chemistry. Indeed, up to the time of World War II the element appeared to be a laboratory curiosity. Then, however, the use of uranium hexafluoride in the separation of uranium isotopes, along with the development of organic fluorine compounds of industrial importance, made fluorine an industrial chemical of considerable use.
Occurrence and distribution
The fluorine-containing mineral fluorspar (fluorite, CaF2) has been used for centuries as a flux (cleansing agent) in various metallurgical processes. The name fluorspar is derived from the Latin fluere, “to flow.” The mineral subsequently proved to be a source of the element, which was accordingly named fluorine. The colourless, transparent crystals of fluorspar exhibit a bluish tinge when illuminated, and this property is accordingly known as fluorescence.
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Fluorine Atomic Number 9
Fluorine is found in nature only in the form of its chemical compounds, except for trace amounts of the free element in fluorspar that has been subjected to radiation from radium. Not a rare element, it makes up about 0.065 percent of Earth’s crust. The principal fluorine-containing minerals are (1) fluorspar, deposits of which occur in Illinois, Kentucky, Derbyshire, southern Germany, the south of France, and Russia and the chief source of fluorine, (2) cryolite (Na3AlF6), chiefly from Greenland, (3) fluoroapatite (Ca5[PO4]3[F,Cl]), widely distributed and containing variable amounts of fluorine and chlorine, (4) topaz (Al2SiO4[F,OH]2), the gemstone, and (5) lepidolite, a mica as well as a component of animal bones and teeth.
Physical and chemical properties
At room temperature fluorine is a faintly yellow gas with an irritating odour. Inhalation of the gas is dangerous. Upon cooling fluorine becomes a yellow liquid. There is only one stable isotope of the element, fluorine-19.
Because fluorine is the most electronegative of the elements, atomic groupings rich in fluorine are often negatively charged. Methyl iodide (CH3I) and trifluoroiodomethane (CF3I) have different charge distributions as shown in the following formulas, in which the Greek symbol δ indicates a partial charge:
The first ionization energy of fluorine is very high (402 kilocalories per mole), giving a standard heat formation for the F+ cation of 420 kilocalories per mole.
The small size of the fluorine atom makes it possible to pack a relatively large number of fluorine atoms or ions around a given coordination centre (central atom) where it forms many stable complexes—for example, hexafluorosilicate (SiF6)2− and hexafluoroaluminate (AlF6)3−. Fluorine is the most powerfully oxidizing element. No other substance, therefore, is able to oxidize the fluoride anion to the free element, and for this reason the element is not found in the free state in nature. Bitnami redmine. For more than 150 years, all chemical methods had failed to produce the element, success having been achieved only by the use of electrolytic methods. However, in 1986 American chemist Karl O. Christe reported the first chemical preparation of fluorine, where “chemical preparation” means a method that does not use techniques such as electrolysis, photolysis, and discharge or use fluorine itself in the synthesis of any of the starting materials. He used K2MnF6 and antimony pentafluoride (SbF5), both of which can be easily prepared from HF solutions.
The high oxidizing power of fluorine allows the element to produce the highest oxidation numbers possible in other elements, and many high oxidation state fluorides of elements are known for which there are no other corresponding halides—e.g., silver difluoride (AgF2), cobalt trifluoride (CoF3), rhenium heptafluoride (ReF7), bromine pentafluoride (BrF5), and iodine heptafluoride (IF7).
Fluorine (F2), composed of two fluorine atoms, combines with all other elements except helium and neon to form ionic or covalent fluorides. Some metals, such as nickel, are quickly covered by a fluoride layer, which prevents further attack of the metal by the element. Certain dry metals, such as mild steel, copper, aluminum, or Monel (a 66 percent nickel, 31.5 percent copper alloy), are not attacked by fluorine at ordinary temperatures. For work with fluorine at temperatures up to 600 °C (1,100 °F), Monel is suitable; sintered alumina is resistant up to 700 °C (1,300 °F). When lubricants are required, fluorocarbon oils are most suitable. Fluorine reacts violently with organic matter (such as rubber, wood, and cloth), and controlled fluorination of organic compounds by the action of elemental fluorine is only possible if special precautions are taken.
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