Chemistry:Dinitrogen trioxide
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| Names | |
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| IUPAC name
N-Oxonitramide[1]
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 2421 |
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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 |
| −16.0·10−6 cm3/mol | |
| Structure | |
| planar, Cs | |
| 2.122 D | |
| Thermochemistry | |
Heat capacity (C)
|
65.3 J/(mol·K) |
Std molar
entropy (S |
314.63 J/(mol·K) |
Std enthalpy of
formation (ΔfH⦵298) |
91.20 kJ/mol |
| Hazards | |
| GHS pictograms |    
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| GHS Signal word | Danger |
| HH270Script error: No such module "Preview warning".Category:GHS errors, HH280Script error: No such module "Preview warning".Category:GHS errors, HH310+H330Script error: No such module "Preview warning".Category:GHS errors, HH310Script error: No such module "Preview warning".Category:GHS errors, HH314Script error: No such module "Preview warning".Category:GHS errors, HH330Script error: No such module "Preview warning".Category:GHS errors | |
| P220, P244, P260, P262, P264, P270, P271, P280, P284, P301+330+331, P302+350, P303+361+353, P304+340, P305+351+338, P310, P320, P321, P322, P361, P363, P370+376, P403, P403+233, P405, P410+403 | |
| 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). | |
 verify (what is   ?)
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| Infobox references | |
Dinitrogen trioxide (also known as nitrous anhydride) is the inorganic compound with the formula N
2O
3. 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]
- NO + NO
2 ⇌ N
2O
3
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 •NO
3.
Structure and bonding
Dinitrogen trioxide molecule contains an N–N bond. One of the numerous resonant structures of the molecule of dinitrogen trioxide is O=N–NO
2, which can be described as a nitroso group –N=O attached to a nitro group –NO
2 by a single bond between the two nitrogen atoms. This isomer is considered as the "anhydride" of the unstable nitrous acid (HNO
2), 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 anhydride in dichloromethane 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 N
2O
3 to water solutions of bases:
- N
2O
3 + 2 NaOH → 2 NaNO
2 + H
2O
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 N
2O
3 molecule is planar and exhibits Cs symmetry. The dimensions displayed on the picture below come from microwave spectroscopy of low-temperature, gaseous N
2O
3:[4]
References
- ↑ "Dinitrogen trioxide". https://pubchem.ncbi.nlm.nih.gov/compound/nitrogen%20trioxide#section=IUPAC-Name&fullscreen=true.
- ↑ 2.0 2.1 2.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 444. ISBN 978-0-08-037941-8.
- ↑ "Dinitrogen trioxide" (in en). https://pubchem.ncbi.nlm.nih.gov/compound/61526#section=Safety-and-Hazards.
- ↑ 4.0 4.1 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 521–22. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
- ↑ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
- ↑ Reddy, G. Sudhakar; Suh, Elijah J.; Corey, E. J. (2022-06-17). "Nitrosyl Triflate and Nitrous Anhydride, Same Mode of Generation, but Very Different Reaction Pathways. Direct Synthesis of 1,2-Oxazetes, Nitroso or Bisoxazo Compounds from Olefins". Organic Letters 24 (23): 4202–4206. doi:10.1021/acs.orglett.2c01466. ISSN 1523-7052. PMID 35653176.
External links
- National Pollutant Inventory – Oxides of nitrogen fact sheet
- Webelements: Compound data – dinitrogen trioxide
- Oxides of nitrogen – synthesis and uses
- Ivtantermo – dinitrogen trioxide table of values
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