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| Names | |
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| IUPAC name
N-Oxonitramide[1] | |
Other names
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| Identifiers | |
3D model (JSmol) |
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| ChEBI | |
| ChemSpider |
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| ECHA InfoCard | 100.031.013 
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| EC Number |
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PubChem CID |
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| UNII | |
| UN number | 2421 |
CompTox Dashboard (EPA) |
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| Properties | |
| N2O3 | |
| Molar mass | 76.011 g·mol−1 |
| Appearance | Deep blue liquid |
| Density |
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| Melting point | −100.7[2] °C (−149.3 °F; 172.5 K) |
| Boiling point | 3.5 °C (38.3 °F; 276.6 K) (dissociates[2]) |
| reacts to form nitrous acid | |
| Solubility | soluble in ether |
| −16.0·10−6cm3/mol | |
| Structure | |
| planar, Cs | |
| 2.122 D | |
| Thermochemistry | |
Heat capacity (C) |
65.3 J/(mol·K) |
Std molar |
314.63 J/(mol·K) |
Std enthalpy of |
91.20 kJ/mol |
| Hazards | |
| GHS labelling:[3] | |
   
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| Danger | |
| H270, H280, H310, H310+H330, H314, H330 | |
| P220, P244, P260, P262, P264, P270, P271, P280, P284, P301+P330+P331, P302+P350, P303+P361+P353, P304+P340, P305+P351+P338, P310, P320, P321, P322, P361, P363, P370+P376, P403, P403+P233, P405, P410+P403, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Related compounds |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Dinitrogen trioxide (also known as nitrous anhydride) is the inorganic compound with the formula N2O3. It is a nitrogen oxide. It forms upon mixing equal parts of nitric oxide and nitrogen dioxide and cooling the mixture below −21 °C (−6 °F):[4]
Dinitrogen trioxide is only isolable at low temperatures, i.e. in the liquid and solid phases. In liquid and solid states, it has a deep blue color.[2] At higher temperatures the equilibrium favors the constituent gases, with KD = 193 kPa (25 °C).[5][clarification needed]
This compound is sometimes called "nitrogen trioxide", but this name properly refers to another compound, the (uncharged) nitrate radical •NO3.
Dinitrogen trioxide molecule contains an N–N bond. One of the numerous resonant structures of the molecule of dinitrogen trioxide is O=N−NO2, which can be described as a nitroso group −N=O attached to a nitro group −NO2 by a single bond between the two nitrogen atoms. This isomer is considered as the "anhydride" of the unstable nitrous acid (HNO2), and produces it when mixed with water, although an alternative structure might be anticipated for the true anhydride of nitrous acid, i.e. O=N−O−N=O. This isomer can be produced from the reaction of tetrabutylammonium nitrite and triflic anhydrideindichloromethane solution at -30°C.[6]
If the nitrous acid is not then used up quickly, it decomposes into nitric oxide and nitric acid. Nitrite salts are sometimes produced by adding N2O3 to water solutions of bases:
Typically, N–N bonds are similar in length to that in hydrazine (145 pm). Dinitrogen trioxide, however, has an unusually long N–N bond at 186 pm. Some other nitrogen oxides also possess long N–N bonds, including dinitrogen tetroxide (175 pm). The N2O3 molecule is planar and exhibits Cs symmetry. The dimensions displayed on the picture below come from microwave spectroscopyoflow-temperature, gaseous N2O3:[4]
Similar to nitronium nitrate, this molecule can also co-exist in equilibrium with an ionic gas called nitrosonium nitrite ([NO]+[NO2]–) [7]
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Nitrogen species
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| Hydrides |
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| Organic |
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| Oxides |
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| Halides |
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| Oxidation states | |
