Dichlorine monoxide
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| Names | |
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| Other names
Oxygen dichloride
Dichlorine oxide Chlorine(I) oxide Hypochlorous oxide Hypochlorous anhydride |
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| Identifiers | |
7791-21-1 
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| 3D model (Jmol) | Interactive image |
| ChEBI |
CHEBI:30198
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| ChemSpider |
23048
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| ECHA InfoCard | 100.029.312 |
| PubChem | 24646 |
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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 | |
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Std molar
entropy (S |
265.9 J K−1 mol−1 |
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Std enthalpy of
formation (ΔfH |
+80.3 kJ mol−1 |
| Hazards | |
| Safety data sheet | |
| NFPA 704 | |
| Related compounds | |
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Other cations
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Nitrous oxide, dibromine monoxide, water |
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Related compounds
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Oxygen difluoride, chlorine dioxide |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is  ?) |
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| Infobox references | |
Dichlorine monoxide, is an inorganic compound with the molecular formula Cl2O. It was first synthesised in 1834 by Antoine Jérôme Balard, who along with Gay-Lussac also determined its composition. In older literature it is often referred to as chlorine monoxide, which can be a source of confusion as that name now refers to the neutral species ClO.
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 chlorine oxide family of compounds, as well as being the anhydride of hypochlorous acid. It is a strong oxidiser and chlorinating agent.
The earliest method of synthesis was to treat mercury(II) oxide with chlorine gas. However this method is expensive, as well as highly dangerous due to the risk of mercury poisoning.
A safer and more convenient method of production is the reaction of chlorine gas with hydrated sodium carbonate, at 20-30°C.
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 it must therefore be continuously removed to prevent thermal decomposition.
The structure of dichlorine monoxide is similar to that of water and hypochlorous acid, with the molecule adopting a bent molecular geometry due to the lone pairs on the oxygen; resulting in C2Vmolecular symmetry. The bond angle is slightly larger than normal, likely due to steric repulsion between the bulky chlorine atoms.
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