Chlorine nitrate

Chlorine nitrate
Ball and stick model of chlorine nitrate	Spacefill model of chlorine nitrate
Names
	Preferred IUPAC name Chlorine nitrate
	Systematic IUPAC name Chloro nitrate
	Other names Nitryl hypochlorite
Identifiers
CAS Number	14545-72-3;
3D model (JSmol)	Interactive image;
ChemSpider	102875;
PubChem CID	114934;
CompTox Dashboard (EPA)	DTXSID00163043 ;
	InChI InChI=1S/ClNO3/c1-5-2(3)4 Key: XYLGPCWDPLOBGP-UHFFFAOYSA-N;
	SMILES ClON(=O)=O;
Properties
Chemical formula	ClNO3
Molar mass	97.46 g/mol
Density	1.65 g/cm3
Melting point	−101 °C (−150 °F; 172 K)
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
NFPA 704 (fire diamond)	3 0 2 OX
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

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 NO_x.^{[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

^ 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. (1967-10-01). "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.

[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. Bibcode:1995JAChS.117.7887O. 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.

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