Dichlorine monoxide
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Other names
Oxygen dichloride
Oxygen chloride Dichlorine oxide Chlorine (I) oxide Hypochlorous oxide Hypochlorous anhydride | |
Identifiers | |
3D model (
JSmol ) |
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ChEBI | |
ChemSpider | |
ECHA InfoCard
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100.029.312 |
PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
Cl2O | |
Molar mass | 86.9054 g/mol |
Appearance | brownish-yellow gas |
Melting point | −120.6 °C (−185.1 °F; 152.6 K) |
Boiling point | 2.0 °C (35.6 °F; 275.1 K) |
very soluble, hydrolyses 143 g Cl2O per 100 g water | |
Solubility in other solvents | soluble in CCl4 |
Structure | |
0.78 ± 0.08 D | |
Thermochemistry | |
Std molar
entropy (S⦵298) |
265.9 J K−1 mol−1 |
Std enthalpy of (ΔfH⦵298)formation |
+80.3 kJ mol−1 |
Hazards | |
GHS labelling: | |
Danger | |
H290, H314, H400, H411 | |
P234, P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P311, P321, P363, P390, P391, P405, P406, P501 | |
NFPA 704 (fire diamond) | |
Safety data sheet (SDS) | [1] |
Related compounds | |
Other cations
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Related compounds
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Oxygen difluoride, nitrous oxide, chlorine dioxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Dichlorine monoxide is an
At room temperature it exists as a brownish-yellow gas which is soluble in both water and organic solvents. Chemically, it is a member of the
Preparation
The earliest method of synthesis was to treat mercury(II) oxide with chlorine gas.[3] However, this method is expensive, as well as highly dangerous due to the risk of mercury poisoning.
- 2 Cl2 + HgO → HgCl2+ Cl2O
A safer and more convenient method of production is the reaction of chlorine gas with hydrated sodium carbonate at 20–30 °C.[3]
- 2 Cl2 + 2 Na2CO3 + H2O → Cl2O + 2 NaHCO3+ 2 NaCl
- 2 Cl2 + 2 NaHCO3→ Cl2O + 2 CO2 + 2 NaCl + H2O
This reaction can be performed in the absence of water but requires heating to 150–250 °C; as dichlorine monoxide is unstable at these temperatures[4] it must therefore be continuously removed to prevent thermal decomposition.
- 2 Cl2 + Na2CO3 → Cl2O + CO2 + 2 NaCl
Structure
The structure of dichlorine monoxide is similar to that of water and
In the solid state, it crystallises in the tetrahedral space group I41/amd, making it isostructural to the high pressure form of water, ice VIII.[5]
Reactions
Dichlorine monoxide is highly soluble in water,
- 2 HOCl ⇌ Cl2O + H2O K (0 °C) = 3.55x10−3 dm3/mol
Despite this, it has been suggested that dichlorine monoxide may be the active species in the reactions of
With inorganic compounds
Dichlorine monoxide reacts with
- VOCl3+ Cl2O → VO2Cl + 2 Cl2
- TiCl4+ Cl2O → TiOCl2 + 2 Cl2
- SbCl5+ 2 Cl2O → SbO2Cl + 4 Cl2
Similar reactions have also been observed with certain inorganic halides.[13][14]
- AsCl3+ 2 Cl2O → AsO2Cl + 3 Cl2
- NO2Cl+ Cl2
With organic compounds
Dichlorine monoxide is an effective chlorinating agent. It can be used for either the side-chain or ring chlorination of deactivated
Photochemistry
Dichlorine monoxide undergoes photodissociation, eventually forming O2 and Cl2. The process is primarily radical based, with flash photolysis showing radical hypochlorite (ClO·) to be a key intermediate.[17]
- 2 Cl2O → 2 Cl2 + O2
Explosive properties
Dichlorine monoxide is explosive, although there is a lack of modern research into this behaviour.
References
- ^ "CHLORINE MONOXIDE". CAMEO Chemicals. National Oceanic and Atmospheric Administration. Retrieved 12 May 2015.
- ^ Balard, A.J. (1834). "Recherches sur la nature des combinaisons décolorantes du chlore" [Investigations into the nature of bleaching compounds of chlorine]. Annales de Chimie et de Physique. 2nd series (in French). 57: 225–304.
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- ISBN 9780123526519.)
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- S2CID 98084403.
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- ISSN 0020-1669.