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Chlorine nitrate

Topic: Chemistry

 From HandWiki - Reading time: 4 min
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
Properties
ClNO3
Molar mass 97.46 g/mol
Density 1.65 g/cm3
Melting point −101 °C (−150 °F; 172 K)[1]
Hazards
GHS pictograms GHS05: CorrosiveGHS06: Toxic
GHS Signal word Danger
NFPA 704 (fire diamond)
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

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. Bibcode: 1995JAChS.117.7887O. 
  2. ↑ von Clarmann, Thomas; Johansson, Sören (2018). "Chlorine nitrate in the atmosphere". Atmos. Chem. Phys. 18 (20): 15363–15386. doi:10.5194/acp-18-15363-2018. Bibcode: 2018ACP....1815363V. 
  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. 
Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)−4 C NO−3,
NH4NO3 		O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3,
Fe(NO3)2 		Co(NO3)2,
Co(NO3)3 		Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb(NO3)3 Te I Xe(NO3)2
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2 		Tl(NO3)3,
TlNO3 		Pb(NO3)2 Bi(NO3)3
BiO(NO3) 		Po At Rn
FrNO3 Ra(NO3)2   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La(NO3)3 Ce(NO3)3,
Ce(NO3)4 		Pr Nd(NO3)3 Pm Sm Eu(NO3)3 Gd(NO3)3 Tb(NO3)3 Dy Ho Er Tm Yb Lu
Ac(NO3)3 Th(NO3)4 Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr

Template:Hypochlorites



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