| Revision as of 10:45, 16 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 477076184 of page Dinitrogen_tetroxide for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 12:02, 21 December 2024 edit Trasheater Midir (talk | contribs)Extended confirmed users3,574 edits →Further readingTag: ProveIt edit |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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| verifiedrevid = 443694879 |
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| Watchedfields = changed |
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| Name = Dinitrogen tetroxide |
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| verifiedrevid = 477162897 |
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| ImageFileL1 = Dinitrogen tetroxide.svg |
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| Name = Dinitrogen tetroxide |
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| ImageSizeL1 = 111 |
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| ImageFile = |
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| ImageNameL1 = Full structural formula |
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| ImageFileR1 = Dinitrogen-tetroxide-3D-vdW.png |
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| ImageFileL1 = Dinitrogen tetroxide.svg |
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| ImageNameL1 = Full structural formula |
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| ImageSizeR1 = 131 |
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| ImageFileR1 = Dinitrogen-tetroxide-3D-vdW.png |
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| ImageNameR1 = Space-filling model |
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| ImageNameR1 = Space-filling model |
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| IUPACName = Dinitrogen tetraoxide |
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| ImageFile2 = Nitrogen dioxide at different temperatures.jpg |
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| OtherNames = Dinitrogen(II) oxide(-I) |
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| ImageSize2 = 240 |
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| Section1 = {{Chembox Identifiers |
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| ImageCaption2 = ] at −196 °C, 0 °C, 23 °C, 35 °C, and 50 °C. ({{chem|NO|2}}) converts to the colorless dinitrogen tetroxide ({{chem|N|2|O|4}}) at low temperatures, and reverts to {{chem|NO|2}} at higher temperatures. |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ImageFile2_Ref = {{chemboximage|correct|??}} |
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| ImageName2 = Nitrogen dioxide at different temperatures |
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| IUPACName = Dinitrogen tetroxide |
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| OtherNames = |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 10544-72-6 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 23681 |
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| ChemSpiderID = 23681 |
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| InChI = 1/N2O4/c3-1(4)2(5)6 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 29803 |
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| ChEBI = 29803 |
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| Gmelin = 2249 |
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| PubChem = 25352 |
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| EINECS = 234-126-4 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = M9APC3P75A |
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| UNNumber = 1067 |
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| RTECS = QW9800000 |
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| SMILES = (=O)()=O |
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| SMILES = (=O)()=O |
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| InChI = 1/N2O4/c3-1(4)2(5)6 |
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| InChIKey = WFPZPJSADLPSON-UHFFFAOYAS |
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| InChIKey = WFPZPJSADLPSON-UHFFFAOYAS |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = WFPZPJSADLPSON-UHFFFAOYSA-N |
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| StdInChIKey = WFPZPJSADLPSON-UHFFFAOYSA-N |
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| CASNo = 10544-72-6 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 25352 |
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| EINECS = 234-126-4 |
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| UNNumber = 1067 |
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| RTECS = QW9800000 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| N=2 | O=4 |
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| Formula = N<sub>2</sub>O<sub>4</sub> |
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| Appearance = White solid, colorless liquid, orange gas |
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| MolarMass = 92.011 g/mol |
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| Density = 1.44246{{nbsp}}g/cm<sup>3</sup> (liquid, 21 °C) |
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| Appearance = colourless gas / orange liquid |
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| Solubility = Reacts to form nitrous and nitric acids |
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| Density = 1.443 g/cm<sup>3</sup> (liquid, 21 °C) |
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| Solubility = reacts |
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| MeltingPtC = −11.2 |
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| MeltingPt_notes = and decomposes to NO<sub>2</sub> |
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| MeltingPt = −11.2 °C (261.9 K) |
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| BoilingPt = 21.1 °C (294.3 K) |
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| BoilingPtC = 21.69 |
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| VaporPressure = 96 kPa (20 °C)<ref></ref> |
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| VaporPressure = 96{{nbsp}}kPa (20{{nbsp}}°C)<ref> https://www.ilo.org/dyn/icsc/showcard.display?p_lang=en&p_card_id=0930&p_version=2</ref> |
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| RefractIndex = 1.00112 |
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| RefractIndex = 1.00112 |
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| MagSus = −23.0·10<sup>−6</sup>{{nbsp}}cm<sup>3</sup>/mol |
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}} |
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}} |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| MolShape = planar, ''D''<sub>2h</sub> |
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| MolShape = Planar, ''D''<sub>2h</sub> |
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| Dipole = zero |
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| Dipole = small, non-zero |
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}} |
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}} |
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| Section4 = {{Chembox Thermochemistry |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = +9.16{{nbsp}}kJ/mol<ref name=Atkins>P.W. Atkins and J. de Paula, ''Physical Chemistry'' (8th ed., W.H. Freeman, 2006) p.999</ref> |
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| DeltaHf = -19.5 kJ/mol |
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| Entropy = 304.29{{nbsp}}J/K⋅mol<ref name=Atkins/> |
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| Entropy = 150.38 J K<sup>−1</sup> mol<sup>−1</sup> |
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}} |
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| Section5 = |
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| Section7 = {{Chembox Hazards |
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| Section6 = |
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| ExternalMSDS = |
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| Section7 = {{Chembox Hazards |
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| EUIndex = 007-002-00-0 |
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| ExternalSDS = |
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| EUClass = Very toxic ('''T+''')<br/>Corrosive ('''C''') |
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| RPhrases = {{R26}}, {{R34}} |
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| GHSPictograms = {{GHS03}}{{GHS05}}{{GHS06}}{{GHS07}} |
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| GHSSignalWord = Danger |
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| SPhrases = {{S1/2}}, {{S9}}, {{S26}}, {{S28}}, {{S36/37/39}}, {{S45}} |
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| HPhrases = {{H-phrases|270|314|330|335|336}} |
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| NFPA-H = 3 |
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| PPhrases = {{P-phrases|220|244|260|261|264|271|280|284|301+330+331|303+361+353|304+340|305+351+338|310|312|320|321|363|370+376|403|403+233|405|410+403|501}} |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-H = 3 |
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| NFPA-O = OX |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| FlashPt = Non-flammable |
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| LD50 = |
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| NFPA-S = OX |
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| NFPA_ref = <ref>{{cite web |url= https://cameochemicals.noaa.gov/chemical/4075 |title= Chemical Datasheet: Nitrogen tetroxide |work= ] ] |access-date= 8 September 2020}}</ref><ref>{{cite web |url= https://pubchem.ncbi.nlm.nih.gov/compound/Dinitrogen-tetroxide#section=NFPA-Hazard-Classification |title= Compound Summary: Dinitrogen tetroxide |work= ] |access-date= 8 September 2020}}</ref> |
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| PEL = |
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| FlashPt = Non-flammable |
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| LD50 = |
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| PEL = |
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| Section8 = {{Chembox Related |
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| Section8 = {{Chembox Related |
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| OtherFunction = {{ubl |
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| OtherFunctn = ]<br/>]<br/>]<br/>]<br/>] |
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| Function = ] ]s |
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| OtherFunction_label = ] ]s |
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| OtherCompounds = {{ubl |
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| ] |
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'''Dinitrogen tetroxide''', commonly referred to as '''nitrogen tetroxide''' ('''NTO'''), and occasionally (usually among ex-USSR/Russian rocket engineers) as '''amyl''', is the ] N<sub>2</sub>O<sub>4</sub>. It is a useful ] in chemical synthesis. It forms an ] with ]. Its molar mass is 92.011 g/mol. |
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Dinitrogen tetroxide is a powerful ] that is ] (spontaneously reacts) upon contact with various forms of ], which has made the pair a common ] for rockets. |
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==Structure and properties== |
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Dinitrogen tetroxide could be regarded as two ]s (-NO<sub>2</sub>) bonded together. It forms an ] with ].<ref>{{Cite journal |doi = 10.1021/ic50008a020|title = Dimers of Nitrogen Dioxide. II. Structure and Bonding|journal = Inorganic Chemistry|volume = 2|issue = 4|pages = 747–752|year = 1963|last1 = Bent|first1 = Henry A.}}</ref> The molecule is planar with an N-N bond distance of 1.78{{nbsp}}Å and N-O distances of 1.19{{nbsp}}Å. The N-N distance corresponds to a weak bond, since it is significantly longer than the average N-N single bond length of 1.45{{nbsp}}Å.<ref>{{cite book |last1 = Petrucci |first1 = Ralph H. |last2 = Harwood |first2 = William S. |last3 = Herring |first3 = F. Geoffrey |date=2002 |title = General chemistry: principles and modern applications |url = https://archive.org/details/generalchemistry00hill |url-access = registration |edition=8th |location=Upper Saddle River, N.J |publisher=Prentice Hall |isbn = 978-0-13-014329-7 |lccn=2001032331 |oclc=46872308 |page= }}</ref> This exceptionally weak σ bond (amounting to overlapping of the ''sp''<sup>2</sup> hybrid orbitals of the two NO<sub>2</sub> units<ref>{{Cite book|last=Rayner-canham|first=Geoff|url=https://www.worldcat.org/oclc/1026755795|title=Descriptive inorganic chemistry.|date=2013|isbn=978-1-319-15411-0|edition=6th|pages=400|oclc=1026755795}}</ref>) results from the simultaneous delocalization of the bonding electron pair across the whole N<sub>2</sub>O<sub>4</sub> molecule, and the considerable electrostatic repulsion of the doubly occupied molecular orbitals of each NO<sub>2</sub> unit.<ref>{{Cite journal|last1=Ahlrichs|first1=Reinhart|last2=Keil|first2=Frerich|date=1974-12-01|title=Structure and bonding in dinitrogen tetroxide (N2O4)|url=https://doi.org/10.1021/ja00832a002|journal=Journal of the American Chemical Society|volume=96|issue=25|pages=7615–7620|doi=10.1021/ja00832a002|issn=0002-7863}}</ref> |
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Unlike NO<sub>2</sub>, N<sub>2</sub>O<sub>4</sub> is ] since it has no unpaired electrons.<ref name=HW>Holleman, A. F.; Wiberg, E. (2001) ''Inorganic Chemistry''. Academic Press: San Diego. {{ISBN|978-0-12-352651-9}}.</ref> The liquid is also colorless but can appear as a brownish yellow liquid due to the presence of NO<sub>2</sub> according to the following equilibrium:<ref name=HW/> |
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: N<sub>2</sub>O<sub>4</sub> ⇌ 2 NO<sub>2</sub>{{Pad|2em}}({{Math|Δ''H'' {{=}} +57.23 kJ/mol}}) |
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Higher temperatures push the equilibrium towards nitrogen dioxide. Inevitably, some dinitrogen tetroxide is a component of ] containing nitrogen dioxide. |
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Solid {{chem2|N2O4}} is white, and melts at −11.2 °C.<ref name=HW/> |
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==Production== |
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Nitrogen tetroxide is made by the ] ] of ] (the ]): steam is used as a ] to reduce the combustion temperature. In the first step, the ammonia is oxidized into ]: |
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: 4 NH<sub>3</sub> + 5 O<sub>2</sub> → 4 NO + 6 H<sub>2</sub>O |
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Most of the water is condensed out, and the gases are further cooled; the nitric oxide that was produced is oxidized to nitrogen dioxide, which is then dimerized into nitrogen tetroxide: |
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: 2 NO + O<sub>2</sub> → 2 NO<sub>2</sub> |
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: 2 NO<sub>2</sub> ⇌ N<sub>2</sub>O<sub>4</sub> |
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and the remainder of the water is removed as ]. The gas is essentially pure nitrogen dioxide, which is condensed into dinitrogen tetroxide in a brine-cooled liquefier.<ref>{{cite book |last1=Hebry |first1=TH |last2=Inskeep |first2=GC |title=Modern Chemical Processes: A Series of Articles Describing Chemical Manufacturing Plants |date=1954 |publisher=Reinhold |location=New York |page=219 |url=https://books.google.com/books?id=-L3nAAAAMAAJ |language=en}}</ref> |
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Dinitrogen tetroxide can also be made through the reaction of concentrated nitric acid and metallic copper. This synthesis is practical in a laboratory setting. Dinitrogen tetroxide can also be produced by heating metal nitrates.<ref>{{cite book |last1=Rennie |first1=Richard |title=A Dictionary of Chemistry |date=2016 |publisher=Oxford University Press |isbn=978-0-19-872282-3 |page=178 |url=https://books.google.com/books?id=d1sFCwAAQBAJ&pg=PA178 |language=en}}</ref> The oxidation of copper by nitric acid is a complex reaction forming various nitrogen oxides of varying stability which depends on the concentration of the nitric acid, presence of oxygen, and other factors. The unstable species further react to form nitrogen dioxide which is then purified and condensed to form dinitrogen tetroxide. |
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==Use as a rocket propellant== |
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Nitrogen tetroxide is used as an oxidizing agent in one of the most important rocket propellant systems because it can be stored as a liquid at room temperature. ], a ] ], reported in 1927 that he had experimented in the 1890s with a rocket engine that used spring-loaded nozzles that periodically introduced vaporized nitrogen tetroxide and a ] to a ] for ignition, with the engine putting out 300 pulsating explosions per minute.<ref>{{Cite web |last=Gonzales Obando |first=Diana |date=2021-07-22 |title=Pedro Paulet: el genio peruano que se adelantó a su época y fundó la era espacial |url=https://elcomercio.pe/eldominical/ciencia/pedro-paulet-el-genio-peruano-que-fundo-la-era-espacial-noticia/ |access-date=2022-03-13 |website=] |language=es}}</ref><ref>{{Cite web |last= |first= |date=25 August 1927 |title=Un peruano Pedro Paulet reclama la propiedad de su invento |url=https://elcomercio.pe/bicentenario/1927-l-el-buque-cohete-un-peruano-pedro-paulet-reclama-la-propiedad-de-su-invento-l-bicentenario-noticia/ |access-date=2022-03-13 |website=] |language=es}}</ref> Paulet would go on to visit the German rocket association ] and on March 15, 1928, Valier applauded Paulet's liquid-propelled rocket design in the VfR publication ''Die Rakete'', saying the engine had "amazing power".<ref>{{cite book |last1=Mejía |first1=Álvaro |url=https://revistas.ucsp.edu.pe/index.php/persona/article/view/209/230 |title=Pedro Paulet, sabio multidisciplinario |publisher=Universidad Católica San Pablo |year=2017 |isbn= |edition= |location= |pages=95–122 |language=es |access-date=}}</ref> Paulet would soon be approached by ] to help develop rocket technology, though he refused to assist and never shared the formula for his propellant.<ref name=":03">{{Cite news |title=El peruano que se convirtió en el padre de la astronáutica inspirado por Julio Verne y que aparece en los nuevos billetes de 100 soles |language=es |work=] |url=https://www.bbc.com/mundo/noticias-america-latina-38197437 |access-date=2022-03-11}}</ref> |
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In early 1944, research on the usability of dinitrogen tetroxide as an oxidizing agent for rocket fuel was conducted by German scientists, although the Germans only used it to a very limited extent as an additive for ] (fuming nitric acid). It became the storable oxidizer of choice for many rockets in both the ] and ] by the late 1950s. It is a ] in combination with a ]-based ]. One of the earliest uses of this combination was on the ] used originally as ] and then as ]s for many spacecraft. Used on the U.S. ] and ] spacecraft and also on the ], it continues to be used as station-keeping propellant on most geo-stationary satellites, and many deep-space probes. It is also the primary oxidizer for Russia's ]. |
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When used as a propellant, dinitrogen tetroxide is usually referred to simply as ''nitrogen tetroxide'' and the abbreviation ''NTO'' is extensively used. Additionally, NTO is often used with the addition of a small percentage of ] that reacts to form ], which inhibits ] of titanium alloys, and in this form, propellant-grade NTO is referred to as '']'' (''MON'') and can be distinguished by its green-blue color. Larger additions of nitric oxide, up to 25-30%, also lower the freezing point of NTO, improving storability in space conditions.<ref>{{Cite encyclopedia |title=Dinitrogen Tetroxide |chapter=N<sub>2</sub>O<sub>4</sub>/N<sub>2</sub>O<sub>3</sub> Mixtures|encyclopedia=Encyclopedia of Oxidizers |publisher=De Gruyter |last= Schmidt |first=Eckart W. |volume=1|date=2022 |pages=437–453 |doi=10.1515/9783110750294-005 |isbn=978-3-11-075029-4}}</ref> Most spacecraft now use MON instead of NTO; for example, the Space Shuttle reaction control system used MON3 (NTO containing 3% NO by weight).<ref>{{Cite web | url=http://www.friends-partners.org/partners/mwade/props/rocindex.htm | title=Rocket Propellant Index | access-date=2005-03-01 | archive-url=https://web.archive.org/web/20080511232517/http://www.friends-partners.org/partners/mwade/props/rocindex.htm | archive-date=2008-05-11 | url-status=dead }}</ref> |
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===The Apollo-Soyuz mishap=== |
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On 24 July 1975, NTO poisoning affected three U.S. ]s on the final descent to Earth after the ] flight. This was due to a switch accidentally left in the wrong position, which allowed the ] thrusters to fire after the cabin fresh air intake was opened, allowing NTO fumes to enter the cabin. One crew member lost consciousness during descent. Upon landing, the crew was hospitalized for five days for chemical-induced ] and ].<ref>, ''Florence, AL - Times Daily newspaper'', August 10, 1975</ref><ref>Sotos, John G., MD. , May 12, 2008, accessed April 1, 2011.</ref> |
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==Power generation using N<sub>2</sub>O<sub>4</sub>== |
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The tendency of N<sub>2</sub>O<sub>4</sub> to reversibly break into NO<sub>2</sub> has led to research into its use in advanced power generation systems as a so-called dissociating gas.<ref>{{cite tech report |first=Robert J. |last=Stochl |title=Potential performance improvement by using a reacting gas (nitrogen tetroxide) as the working fluid in a closed Brayton cycle |number=TM-79322 |institution=] |year=1979 |url=https://ntrs.nasa.gov/archive/nasa/casi.ntrs.nasa.gov/19800008230.pdf}}</ref> "Cool" dinitrogen tetroxide is compressed and heated, causing it to dissociate into ] at half the molecular weight. This hot nitrogen dioxide is expanded through a turbine, cooling it and lowering the pressure, and then cooled further in a heat sink, causing it to recombine into nitrogen tetroxide at the original molecular weight. It is then much easier to compress to start the entire cycle again. Such dissociative gas ]s have the potential to considerably increase efficiencies of power conversion equipment.<ref>{{cite web|last=Ragheb|first=R.|title=Nuclear Reactors Concepts and Thermodynamic Cycles|url=http://mragheb.com/NPRE%20402%20ME%20405%20Nuclear%20Power%20Engineering/Nuclear%20Reactors%20Concepts%20and%20Thermodynamic%20Cycles.pdf|access-date=1 May 2013}}</ref> |
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The high molecular weight and smaller volumetric expansion ratio of nitrogen dioxide compared to steam allows the turbines to be more compact.<ref>{{Cite journal |last1=Binotti |first1=Marco |last2=Invernizzi |first2=Costante M. |last3=Iora |first3=Paolo |last4=Manzolini |first4=Giampaolo |date=March 2019 |title=Dinitrogen tetroxide and carbon dioxide mixtures as working fluids in solar tower plants |url=https://linkinghub.elsevier.com/retrieve/pii/S0038092X1930091X |journal=Solar Energy |language=en |volume=181 |pages=203–213 |doi=10.1016/j.solener.2019.01.079|s2cid=104462066 }}</ref> |
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N<sub>2</sub>O<sub>4</sub> was the main component of the "nitrin" working fluid in the decommissioned ] portable nuclear reactor which operated from 1985 to 1987.<ref>{{Cite web |last=Paliukhovich |first=V.M. |date=7 May 2023 |title=Safe Decommissioning of Mobile Nuclear Power Plant |url=https://inis.iaea.org/collection/NCLCollectionStore/_Public/33/052/33052291.pdf |url-status=live |archive-url=https://web.archive.org/web/20230507105914/https://inis.iaea.org/collection/NCLCollectionStore/_Public/33/052/33052291.pdf |archive-date=7 May 2023 |access-date=7 May 2023 |website=International Atomic Energy Agency |publisher=Department for Supervision of Industrial and Nuclear Safety |publication-place=Minsk, Belarus}}</ref> |
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==Chemical reactions== |
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===Intermediate in the manufacture of nitric acid=== |
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Nitric acid is manufactured on a large scale via N<sub>2</sub>O<sub>4</sub>. This species reacts with water to give both ] and ]: |
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: N<sub>2</sub>O<sub>4</sub> + H<sub>2</sub>O → HNO<sub>2</sub> + HNO<sub>3</sub> |
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The coproduct HNO<sub>2</sub> upon heating ] to ] and more nitric acid. When exposed to oxygen, NO is converted back into nitrogen dioxide: |
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: 2 NO + O<sub>2</sub> → 2 NO<sub>2</sub> |
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The resulting NO<sub>2</sub> and N<sub>2</sub>O<sub>4</sub> can be returned to the cycle to give the mixture of nitrous and nitric acids again. |
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===Synthesis of metal nitrates=== |
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N<sub>2</sub>O<sub>4</sub> undergoes ] to give , with the former ] ion being a strong oxidant. Various anhydrous ]es can be prepared from N<sub>2</sub>O<sub>4</sub> and base metal.<ref>{{cite journal |last1=Addison |first1=C. Clifford |title=Dinitrogen tetroxide, nitric acid, and their mixtures as media for inorganic reactions |journal=Chemical Reviews |date=February 1980 |volume=80 |issue=1 |pages=21–39 |doi=10.1021/cr60323a002}}</ref> |
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: 2 N<sub>2</sub>O<sub>4</sub> + M → 2 NO + M(NO<sub>3</sub>)<sub>2</sub> |
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where M = ], ], or ]. |
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If metal nitrates are prepared from N<sub>2</sub>O<sub>4</sub> in completely anhydrous conditions, a range of covalent metal nitrates can be formed with many transition metals. This is because there is a thermodynamic preference for the nitrate ion to bond covalently with such metals rather than form an ionic structure. Such compounds must be prepared in anhydrous conditions, since the nitrate ion is a much weaker ligand than water, and if water is present the simple nitrate of the ] will form. The anhydrous nitrates concerned are themselves covalent, and many, e.g. anhydrous ], are volatile at room temperature. Anhydrous titanium nitrate sublimes in vacuum at only 40 °C. Many of the anhydrous transition metal nitrates have striking colours. This branch of chemistry was developed by ] and Norman Logan at the ] in the UK during the 1960s and 1970s when highly efficient desiccants and ]es started to become available. |
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===With organic compounds=== |
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In even slightly basic solvents, N<sub>2</sub>O<sub>4</sub> adds to ]s radically, giving mixtures of ]s and ]s. Pure or in entirely nonbasic solvents, the compounds autoionizes as above, to give ]s and ]s.<ref>{{cite book|title=Nitrosation|first=D. L. H.|last=Williams|publisher=]|location=Cambridge, UK|year=1988|isbn=0-521-26796-X|url=https://archive.org/details/nitrosation0000will|url-access=registration|pages=49–50}}</ref> |
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==References== |
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{{reflist}} |
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== Further reading == |
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*{{Cite encyclopedia |title=Dinitrogen Tetroxide |encyclopedia=Encyclopedia of Oxidizers |publisher=De Gruyter |last= Schmidt |first=Eckart W. |volume=1|date=2022 |pages=367–624 |doi=10.1515/9783110750294-005 |isbn=978-3-11-075029-4}} |
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*{{Cite thesis |last=Head |first=Andrew W. |title=Nitrogen Tetroxide to Mixed Oxides of Nitrogen: History, Usage, Synthesis, and Composition Determination |date=2021 |degree=MSc |publisher=Purdue University |url=https://hammer.purdue.edu/articles/thesis/Nitrogen_Tetroxide_to_Mixed_Oxides_of_Nitrogen_History_Usage_Synthesis_and_Composition_Determination/17003098/1 |doi=10.25394/PGS.17003098.V1}} |
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* Nitrogen Dioxide in Workplace Atmospheres, osha.gov, May 1987, revised May 2001 |
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==External links== |
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{{Commons}} |
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* |
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* : Nitrogen tetroxide |
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* {{Webarchive|url=https://web.archive.org/web/20160310185602/http://encyclopedia.airliquide.com/encyclopedia.asp?btnformula.x=0&btnformula.y=0&countryid=19&formula=n2o4&gasid=0&languageid=11&unnumber=#MSDS |date=2016-03-10 }} |
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* {{cite web|last=Poliakoff|first=Martyn|title=The Chemistry of Lunar Lift-Off: Our Apollo 11 40th Anniversary Special|url=http://www.periodicvideos.com/videos/feature_lunar_liftoff.htm|work=]|publisher=]|author-link=Martyn Poliakoff|year=2009}} |
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{{nitrogen compounds}} |
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{{Oxides}} |
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{{oxygen compounds}} |
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{{Authority control}} |
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{{DEFAULTSORT:Dinitrogen Tetroxide}} |
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] |
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] |
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] |
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] |