Hydrogen fluoride
From Wikinfo
- For criticism see Criticism of Hydrogen_fluoride
| Hydrogen fluoride | |
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| Other names | Hydrogen fluoride Fluoric acid Hydrofluoride Hydrofluoric acid Fluorine monohydride |
| Molecular formula | HF |
| Molecular mass | 20.01 g/mol |
| Physical state | Liquid/Gas |
| CAS number | 7664-39-3 |
| Density | 0.922 kg m-3 |
| Solubility (water) | miscible |
| Melting point | -84 °C (190 K, -118 °F) |
| Boiling point | 19.54 °C (293 K, 67.2 °F) |
| NFPA 704 |
 0
4
2
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| Disclaimer and references | |
Hydrogen fluoride is a chemical compound with the formula HF. It is the principal industrial source of fluorine, often in the aqueous form as hydrofluoric acid, and thus is the precursor to many important compounds including pharmaceuticals and polymers (e.g. Teflon). HF is widely used in the petrochemical industry and a component of many superacids. HF boils just below room temperature whereas the other hydrogen halides condense at much lower temperatures. Unlike the other hydrogen halides, HF is lighter than air and its odour is particularly penetrating. Aqueous solutions of HF, called hydrofluoric acid, are strongly corrosive.
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Structure
HF forms orthorhombic crystals, consisting of zig-zag chains of HF molecules. The HF molecules, with a short H-F bond of 0.95 Å, are linked to neighboring molecules by intermolecular H--F distances of 1.55 Å.[1]
Liquid HF also consists of chains of HF molecules, but the chains are shorter, consisting on average of only five or six molecules.[2] The higher boiling point of HF relative to analogous species, such as HCl, is attributed to hydrogen bonding between HF molecules, as indicated by the existence of chains even in the liquid state.
Acidity
Dilute aqueous HF solutions are weakly acidic in contrast to corresponding solutions of the other hydrogen halides. A qualitative explanation for this behavior is related to the tendency of HF to hydrogen-bond and form ion-pair clusters such as F−·H3O+.[3][4]
In concentrated hydrogen fluoride solution, F− ions forms a [HF2]−(aq) complex with HF molecules. HF molecules remaining ionize to compensate the loss of F− ions. More H+ ions are thus formed, making concentrated HF an effectively strong acid.
Anhydrous hydrogen fluoride is an extremely strong acid (H0 ~ −11), comparable in strength to anhydrous sulfuric acid (H0 ~ −12).
Production and uses
Hydrogen fluoride is produced as a side product of the extraction of the fertilizer precursor phosphoric acid from various minerals. This theme is developed in the article on hydrofluoric acid.
The anhydrous compound hydrogen fluoride is more commonly used than its aqueous solution, hydrofluoric acid. HF serves a catalyst in alkylation processes in oil refineries. A component of high-octane gasoline called "alkylate" is generated in FCC units that combine C3 and C4 olefins and isobutane to generate gasoline.[5]
HF is a reactive solvent in the electrochemical fluorination of organic compounds. In this approach, HF is oxidized in the presence of a hydrocarbon and the fluorine replaces C-H bonds with C-F bonds. Perfluorinated carboxylic acids and sulfonic acids are produced in this way.[5]
Elemental fluorine, F2, is prepared by electrolysis of a solution of HF and potassium bifluoride. Several million kilograms of F2 are produced annually.[6]
Health effects
Upon contact with moisture, including tissue, hydrogen fluoride immediately converts to hydrofluoric acid, which is highly corrosive and toxic, and requires immediate medical attention.
References
- ^ Johnson, M. W.; Sándor, E.; Arzi, E. (1975). "The Crystal Structure of Deuterium Fluoride". Acta Crystallographica B31: pages 1998–2003. DOI:10.1107/S0567740875006711.
- ^ Mclain, Sylvia E. (2004). "On the Structure of Liquid Hydrogen Fluoride". Angewandte Chemie, International Edition 43: 1952–55. DOI:10.1002/anie.200353289.
- ^ Giguere, Paul A. (1980). "The nature of hydrofluoric acid. A spectroscopic study of the proton-transfer complex H3O+...F−". J. Am. Chem. Soc. 102: 5473. DOI:10.1021/ja00537a008.
- ^ Radu Iftimie, Vibin Thomas, Sylvain Plessis, Patrick Marchand, and Patrick Ayotte (2008). "Spectral Signatures and Molecular Origin of Acid Dissociation Intermediates". J. Am. Chem. Soc. 130: 5901. DOI:10.1021/ja077846o.
- ^ a b J. Aigueperse, P. Mollard, D. Devilliers, M. Chemla, R. Faron, R. Romano, J. P. Cuer, “Fluorine Compounds, Inorganic” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005
- ^ M. Jaccaud, R. Faron, D. Devilliers, R. Romano “Fluorine” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.
- "ATSDR - MMG: Hydrogen Fluoride". Retrieved May 14, 2006
- Barbalace, Kenneth. "Chemical Database - Hydrogen Fluoride. EnvironmentalChemistry.com". 1995 - 2006. Retrieved May 14, 2006
- Honeywell, Industrial Fluorines G525-521, "Recommended Medical Treatment for Hydrofluoric Acid Exposure"
- Cotton, F. A. and Wilkinson, G., Advanced Inorganic Chemistry, John Wiley and Sons: New York, 1988. ISBN 0471849979
| This page uses content from Wikipedia. The original article was at Hydrogen fluoride. The list of authors can be seen in the page history. The text of this Wikinfo article is available under the GNU Free Documentation License and the Creative Commons Attribution-Share Alike 3.0 license. |
