Chlorine nitrate
From Wikipedia, the free encyclopedia
Chlorine nitrate
Ball and stick model of chlorine nitrate Ball and stick model of chlorine nitrate
Spacefill model of chlorine nitrate Spacefill model of chlorine nitrate
Stick model of chlorine nitrate Stick model of chlorine nitrate
Resonance stick models of chlorine nitrate Resonance stick models of chlorine nitrate
Names
Preferred IUPAC name
Systematic IUPAC name
Other names
Identifiers
ChemSpider
Properties
ClNO3
Molar mass
97.46 g/mol
Density
1.65 g/cm3
Melting point
−101 °C (−150 °F; 172 K)[1]
Hazards
GHS labelling:
GHS05: Corrosive GHS06: Toxic
Danger
NFPA 704 (fire diamond)
[画像:NFPA 704 four-colored diamond]
Chlorine nitrate
Chloro nitrate
Nitryl hypochlorite
3D model (JSmol)
PubChem CID
CompTox Dashboard (EPA)
- InChI=1S/ClNO3/c1-5-2(3)4Key: XYLGPCWDPLOBGP-UHFFFAOYSA-N
- ClON(=O)=O
- Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gas
- Flammability 0: Will not burn. E.g. water
- Instability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorus
- Special hazard OX: Oxidizer. E.g. potassium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Chemical compound
Chlorine nitrate, with chemical formula ClONO2 is an important atmospheric gas present in the stratosphere. It is an important sink of reactive chlorine and nitrogen, and thus its formation and destruction play an important role in the depletion of ozone.[2]
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:[3]
- Cl2O + N2O5 → 2 ClONO2
or by the reaction:[4]
- ClF + HNO3 → HF + ClONO2
It can also react with alkenes:
- (CH3)2C=CH2 + ClONO2 → O2NOC(CH3)2CH2Cl
Chlorine nitrate reacts with metal chlorides:[5]
- 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. Bibcode:1995JAChS.117.7887O. doi:10.1021/ja00135a006.
- ^ von Clarmann, Thomas; Johansson, Sören (2018). "Chlorine nitrate in the atmosphere". Atmos. Chem. Phys. 18 (20): 15363–15386. Bibcode:2018ACP....1815363V. doi:10.5194/acp-18-15363-2018 .
- ^ 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年10月01日). "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.