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
Resonance stick models of chlorine nitrate
Names
Preferred IUPAC name
Chlorine nitrate
Systematic IUPAC name
Chloro nitrate
Other names
Nitryl hypochlorite
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/ClNO3/c1-5-2(3)4
    Key: XYLGPCWDPLOBGP-UHFFFAOYSA-N
  • ClON(=O)=O
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: CorrosiveGHS06: Toxic
Danger
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
2
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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

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

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

  1. ^ 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.
  2. ^ 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.
  3. ^ Schmeisser, M.; Ruff, J. K. & Lustig, M. Chlorine(1) Nitrate Inorganic Syntheses, Wiley-Blackwell, https://doi.org/10.1002/9780470132401.ch34, 1967, 127-130
  4. ^ Schack, Carl J. (1967-10-01). "New synthesis of chlorine nitrate". Inorganic Chemistry. 6 (10): 1938–1939. doi:10.1021/ic50056a047. ISSN 0020-1669.
  5. ^ 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.
source: http://en.wikipedia.org/wiki/Chlorine_nitrate