Difference between revisions of "Nitronium perchlorate"
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Nitronium perchlorate is a colorless hygroscopic solid, which reacts with many solvents. | Nitronium perchlorate is a colorless hygroscopic solid, which reacts with many solvents. | ||
| − | ==Explosive== | + | ===Explosive=== |
Although the compound has been described as "safe", contact with flammable organic solvents such as [[acetone]] or [[diethyl ether]] has been described as explosive.<ref>Gordon, W. E.; Spinks, J. W. T.; Canadian Journal of Research, Section B: Chemical Sciences; vol. 18; (1940); p. 358 - 362</ref> | Although the compound has been described as "safe", contact with flammable organic solvents such as [[acetone]] or [[diethyl ether]] has been described as explosive.<ref>Gordon, W. E.; Spinks, J. W. T.; Canadian Journal of Research, Section B: Chemical Sciences; vol. 18; (1940); p. 358 - 362</ref> | ||
Latest revision as of 22:55, 28 August 2022
| Names | |
|---|---|
| IUPAC name
Nitronium perchlorate
| |
| Other names
Nitroxyl perchlorate
Nitryl perchlorate | |
| Properties | |
| NO6Cl NO2ClO4 | |
| Molar mass | 145.4561 g/mol |
| Appearance | White solid |
| Odor | Acrid |
| Density | 2.2 g/cm3[1] |
| Melting point | 135 °C (275 °F; 408 K) (decomposes) |
| Boiling point | (decomposes) |
| Reacts | |
| Solubility | Reacts with many solvents Soluble in fuming nitric acid, nitromethane, perchloric acid, phosphoryl chloride Almost insoluble in halocarbons |
| Solubility in carbon tetrachloride | 0.145456 g/100 ml (25 °C)[2] |
| Solubility in nitromethane | 11.6365 g/100 ml (25 °C)[3] |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
31.8 kJ/mol[4] |
| Hazards | |
| Safety data sheet | None |
| Flash point | None |
| Related compounds | |
| Related compounds
|
Nitronium tetrafluoroborate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Nitronium perchlorate, NO2ClO4, also known as nitryl perchlorate and nitroxyl perchlorate, is an inorganic chemical, the salt of the perchlorate anion and the nitronium cation.
Contents
Properties
Chemical
Of all perchlorates, nitronium perchlorate is the most powerful oxidizer.
It reacts extremely powerful with organic solvents, and can cause ignition.
Nitronium perchlorate reacts exothermically with water.
Physical
Nitronium perchlorate is a colorless hygroscopic solid, which reacts with many solvents.
Explosive
Although the compound has been described as "safe", contact with flammable organic solvents such as acetone or diethyl ether has been described as explosive.[5]
Availability
Nitronium perchlorate doesn't appear to be commercially available, so it must be prepared in situ.
Preparation
There are several routes to this compound.
A good route involves reacting dinitrogen pentoxide and anh. perchloric acid. Nitric acid may be formed as side product:[6]
- N2O5 + HClO4 → NO2ClO4 + H+ + NO3-
Nitric acid can be used, but the reaction produces water as side product, which must be removed to prevent hydrolysis:[7]
- HNO3 + HClO4 → NO2ClO4 + H2O
Both reactions take place in anhydrous nitromethane, at -40 °C.
Addition of dichlorine hexoxide to anh. nitric acid will produce nitronium perchlorate. The product is purified via sublimation under vacuum, with a reported yield of 53 %.[8]
Reacting dichlorine heptoxide with dinitrogen pentoxide in dry carbon tetrachloride will also yield nitronium perchlorate.[9]
A simpler reaction involves addition of nitryl chloride to silver perchlorate. Silver chloride precipitates out of the solution, while the product is purified.[10]
Some sources indicate that this compound can also be produced by reacting nitrogen dioxide and chlorine dioxide with an excess of ozone.
Projects
- Rocker propellant
- Source of nitronium ions
Handling
Safety
Nitronium perchlorate is a powerful oxidizer and highly corrosive. It will cause significant burns if it enters contact with skin.
Storage
Should not be kept for long periods of time.
Disposal
Should be carefully added in ice cold water, in small batches at a time, then the solution is neutralized with a base.
References
- ↑ Truter, M. R.; Cruickshank, D. W. J.; Jeffrey, G. A.; Acta Crystallographica; vol. 13; (1960); p. 855 - 862
- ↑ Goddard, D. R.; Hughes, E. D.; Ingold, C. K.; Journal of the Chemical Society; (1950); p. 2559 - 2575
- ↑ Goddard, D. R.; Hughes, E. D.; Ingold, C. K.; Journal of the Chemical Society; (1950); p. 2559 - 2575
- ↑ Gilliland, A. A.; Journal of Research of the National Bureau of Standards, Section A: Physics and Chemistry; vol. 66; (1962); p. 447 - 449
- ↑ Gordon, W. E.; Spinks, J. W. T.; Canadian Journal of Research, Section B: Chemical Sciences; vol. 18; (1940); p. 358 - 362
- ↑ Goddard, D. R.; Hughes, E. D.; Ingold, C. K.; Journal of the Chemical Society; (1950); p. 2559 - 2575
- ↑ Goddard, D. R.; Hughes, E. D.; Ingold, C. K.; Journal of the Chemical Society; (1950); p. 2559 - 2575
- ↑ Pascal, Jean-Louis; Hassan, Abduljabbar; Potier, Jacqueline; Comptes Rendus de l'Academie des Sciences, Serie II: Mecanique, Physique, Chimie, Sciences de la Terre et de l'Univers; vol. 302; (1986); p. 817 - 820
- ↑ Potier, A.; Potier, J.; Rousselet, D.; Comptes Rendus Hebdomadaires des Seances de l'Academie des Sciences; vol. 261; (1965); p. 4115 - 4118
- ↑ Schmeisser, M.; Angewandte Chemie; vol. 67; (1955); p. 493 - 501
