Chlorine nitrate, with chemical formula ClONO2 is an important atmospheric gas present in the stratosphere. It is an important sink of chlorine that contributes to the depletion of ozone.
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Names | |||
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Preferred IUPAC name
Chlorine nitrate | |||
Systematic IUPAC name
Chloro nitrate | |||
Other names
Nitryl hypochlorite
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Identifiers | |||
3D model (JSmol)
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PubChem CID
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CompTox Dashboard (EPA)
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Properties | |||
ClNO3 | |||
Molar mass | 97.46 | ||
Density | 1.65 g/cm3 | ||
Melting point | −101 °C (−150 °F; 172 K)[1] | ||
Hazards | |||
GHS labelling: | |||
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NFPA 704 (fire diamond) | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Chemical properties edit
It explosively reacts with metals, metal chlorides, alcohols, ethers, and most organic materials. When it is heated to decomposition, it emits toxic fumes of Cl2 and NOx.[citation needed]
Synthesis and reactions edit
It can be produced by the reaction of dichlorine monoxide and dinitrogen pentoxide at 0 °C:[2]
- Cl2O + N2O5 → 2 ClONO2
or by the reaction:[3]
- ClF + HNO3 → HF + ClONO2
It can also react with alkenes:
- (CH3)2C=CH2 + ClONO2 → O2NOC(CH3)2CH2Cl
Chlorine nitrate reacts with metal chlorides:[4]
- 4 ClONO2 + TiCl4 → Ti(NO3)4 + 4 Cl2
References edit
- ^ Obermeyer, Axel; Borrmann, Horst; Simon, Arndt (August 1995). "Crystal Structures and Bonding in NOCl, NO2Cl, and NO3Cl". Journal of the American Chemical Society. 117 (30): 7887–7890. doi:10.1021/ja00135a006.
- ^ Schmeisser, M.; Ruff, J. K. & Lustig, M. Chlorine(1) Nitrate Inorganic Syntheses, Wiley-Blackwell, https://doi.org/10.1002/9780470132401.ch34, 1967, 127-130
- ^ Schack, Carl J. (1967-10-01). "New synthesis of chlorine nitrate". Inorganic Chemistry. 6 (10): 1938–1939. doi:10.1021/ic50056a047. ISSN 0020-1669.
- ^ 张青莲 (1991). 《无机化学丛书》第六卷:卤素、铜分族、锌分族. 北京: 科学出版社. pp. P338-341. ISBN 7-03-002238-6.