Ammonium bifluoride
| Ammonium bifluoride | |
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Ammonium hydrogen fluoride |
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Other names
Ammonium acid fluoride Ammonium hydrofluoride |
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| Identifiers | |
| CAS number | 1341-49-7  |
| ChemSpider | 21241205  |
| Jmol-3D images | Image 1 Image 2 |
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| Properties | |
| Molecular formula | H5F2N |
| Molar mass | 57.04 g mol−1 |
| Exact mass | 57.039005575 g mol-1 |
| Appearance | White crystals |
| Density | 1.50 g cm-3 |
| Melting point |
126 °C, 399 K, 259 °F (decomposes) |
| Boiling point |
240 °C, 513 K, 464 °F |
| Solubility in water | 63g/100ml 20°C |
| Solubility in alcohol | slightly soluble |
| Refractive index (nD) | 1.390 |
| Structure | |
| Crystal structure | Cubic, related to the CsCl structure |
| Coordination geometry |
[NH4]+ cation: tetrahedral [HF2]− anion: linear |
| Hazards | |
| GHS pictograms |   [1] |
| GHS hazard statements | H301, H314[1] |
| GHS precautionary statements | P280, P301+310, P305+351+338, P310[1] |
| NFPA 704 |
 0
3
0
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| Related compounds | |
| Other cations | potassium bifluoride |
| Related compounds | ammonium fluoride |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Ammonium hydrogen fluoride is the inorganic compound with the formula NH4HF2 or NH4F·HF. It is produced from ammonia and hydrogen fluoride. This colourless salt is a glass-etchant and an intermediate in a once-contemplated route to hydrofluoric acid.
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[edit] Structure
Ammonium bifluoride, as its name indicates, contains a bifluoride, or hydrogen(difluoride) anion: HF2−. This centrosymmetric triatomic anion features the strongest known hydrogen bond, with a F−H length of 114 pm.[2] and a bond energy greater than 155 kJ mol−1.[3]
In solid [NH4][HF2], each ammonium cation is surrounded by four fluoride centers in a tetrahedron, with hydrogen - fluorine hydrogen bonds present between the hydrogen atoms of the ammonium ion and the fluorine atoms. Solutions contain tetrahedral [NH4]+ cations and linear [HF2]− anions.
[edit] Production and applications
Ammonium bifluoride is a component of some etchants. It attacks silica component of glass:
Potassium bifluoride is a related more commonly used etchant.
Ammonium bifluoride has been considered as an intermediate in the production of hydrofluoric acid from hexafluorosilicic acid. Thus, hexafluorosilicic acid is hydrolyzed to give ammonium fluoride, which thermally decomposes to give the bifluoride:
- H2SiF6 + 6 NH3 + 2 H2O → SiO2 + 6 NH4F
- 2 NH4F → NH3 + [NH4]HF2
The resulting ammonium bifluoride is converted to the sodium bifluoride, which thermally decomposes to release HF.[4]
[edit] See also
[edit] References
- ^ a b c Online Sigma Catalogue , accessdate: June 16, 2011.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419.
- ^ Emsley, J. (1980) Very strong hydrogen bonds, Chemical Society Reviews, 9, 91-124. doi:10.1039/CS9800900091
- ^ Jean Aigueperse, Paul Mollard, Didier Devilliers, Marius Chemla, Robert Faron, Renée Romano, Jean Pierre Cuer (2005), “Fluorine Compounds, Inorganic” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a11 307
- A. F. Wells (1984) Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK.
