Bifluoride
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| Names | |||
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| Other names
Hydrogen(difluoride) Bifluoride anion Hydrogen difluoride anion | |||
| Identifiers | |||
18130-74-0  | |||
| ChemSpider | 35308425 | ||
| Jmol interactive 3D | Image | ||
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| Properties | |||
| F2H | |||
| Molar mass | 39.00 g·mol−1 | ||
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
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| Infobox references | |||
Bifluoride is an inorganic anion with the chemical formula HF−
2 (also written [HF2]−). It contributes no color to bifluoride salts. Salts of bifluoride are used to etch glass.
Acid-base properties and production
Bifluoride undergoes the typical chemical reactions of a weak acid. Upon treatment with a standard acid, it converts to hydrofluoric acid and a metal salt. Oxidation of bifluoride gives fluorine. When heated, bifluoride salts decompose to produce fluoride salts and hydrogen fluoride:
- [HF2]−
HF + F−
Bifluoride protonates to give hydrogen fluoride:
- HF−
2 + H+ 2 HF
Because of this capture of a proton (H+), bifluoride has basic character. Its conjugate acid is the reactive intermediate, μ-fluoro-fluorodihydrogen (H2F2), which subsequently dissociates to become hydrogen fluoride. In solution, most bifluoride ions are dissociated.
- HF−
2 + H
2O 2 HF + HO−
Bifluoride salts arise by treatment of hydrogen fluoride with base:
- HF + F− → [HF2]−
Structure
This centrosymmetric triatomic anion features a symmetric hydrogen bond, the strongest known hydrogen bond, with an F−H length of 114 pm[1] and a bond strength of >155 kJ mol−1.[2] A molecular orbital diagram reveals the atoms to be held together by a 3-center 4-electron bond.[3] It is isoelectronic with the fluoroheliate anion, FHeO−, whose existence is suspected[4] but not confirmed. "Hydrogen(difluoride)" is written as one word because it is an anion; "hydrogen difluoride" would instead imply the electrically neutral compound HF2 (CAS number 12528-21-1). It is classified as a weak base.
Salts
Some HF2− salts are common, examples include potassium bifluoride (KHF2, also called potassium hydrogen fluoride) and ammonium bifluoride ([NH4][HF2]). Many salts claimed to be anhydrous sources of simple fluoride (F−) ions, for example, tetra-n-butylammonium fluoride, can decompose to yield bifluoride instead.
Autodissociation of pure HF
The bifluoride ion also contributes to the unusually high auto-protolysis constant of liquid anhydrous hydrogen fluoride, which autodissociates in a manner similar to the self-ionization of water. This equilibrium can be denoted as
- HF
H+ + F−
However, both the H+ and F− ions are solvated by HF, so a better descriptive equation is
- 3HF H2F+(HF) + HF2−(HF)
References
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Wikimedia Commons has media related to bifluoride ion. |
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
- ↑ Emsley, J., "Very Strong Hydrogen Bonds", Chemical Society Reviews, 1980, 9, 91-124.
- ↑ Pimentel, G. C. The Bonding of Trihalide and Bifluoride Ions by the Molecular Orbital Method. J. Chem. Phys. 1951, 19, 446-448. doi:10.1063/1.1748245
- ↑ "Collapse of helium’s chemical nobility predicted by Polish chemist" (PDF). Retrieved 2009-05-15.