Zirconium nitrate
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| ImageFile = File:Zirconium(IV) nitrate pentahydrate.jpg
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| ImageAlt = sample of zirconium(IV) nitrate pentahydrate
| ImageCaption = Pentahydrate
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| OtherNames = zirconium tetranitrate, tetranitratozirconium, zirconium(4+) tetranitrate, zirconium(IV) nitrate
| Section1 = {{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 13746-89-9
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = L68X591SNQ
| PubChem = 26251
| ChemSpiderID = 24459
| ChemSpiderID_Ref = {{chemspidercite|changedt|chemspider}}
| InChI =1S/4NO3.Zr/c4*2-1(3)4;/q4*-1;+4
| InChIKey =OERNJTNJEZOPIA-UHFFFAOYSA-N
| SMILES = [Zr+4].O=[N+]([O-])[O-].[O-][N+]([O-])=O.[O-][N+]([O-])=O.[O-][N+]([O-])=O }}
| Section2 = {{Chembox Properties
| Formula = Zr(NO3)4
| MolarMass = 339.243591 g/mol
| Appearance = transparent plates
| Density =
| BoilingPt = decompose 100 °C
| Solubility = water, ethanol}}
| Section3 = {{Chembox Hazards
| MainHazards = oxidiser
| FlashPt =
| AutoignitionPt =
| LCLo = 500 mg/m3 (rat, 30 min){{IDLH|7440677|Zirconium compounds (as Zr)}}
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| Section8 = {{Chembox Related
| OtherCompounds = Zirconyl nitrate, hafnium nitrate, titanium nitrate, zirconium perchlorate }}
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Zirconium nitrate is a volatile anhydrous transition metal nitrate salt of zirconium with formula Zr(NO3)4. It has alternate names of zirconium tetranitrate, or zirconium(IV) nitrate.
It has a UN number of UN 2728{{cite book|title=The Code of Federal Regulations of the United States of America|chapter-url=https://books.google.com/books?id=Qrw8AAAAIAAJ&pg=PA254|year=1988|publisher=U.S. Government Printing Office|page=254|chapter=App A}} and is class 5.1, meaning oxidising substance.{{cite book|title=Recommendations on the Transport of Dangerous Goods: Model Regulations|url=https://books.google.com/books?id=hCRzKJXS9iYC&pg=PA430|year=2009|publisher=United Nations Publications|isbn=9789211391367|page=430}}
Formation
The anhydrous salt can be made from zirconium tetrachloride reacting with dinitrogen pentoxide.{{cite journal|last=Morozov|first=I. V.|author2=A. A. Fedorova |author3=D. V. Palamarchuk |author4=S. I. Troyanov |year=2005|title=Synthesis and crystal structures of zirconium(IV) nitrate complexes (NO2)[Zr(NO3)3(H2O)3]2(NO3) 3, Cs[Zr(NO3)5], and (NH4)[Zr(NO3)5](HNO3)|journal=Russian Chemical Bulletin|volume=54|issue=1|pages=93–98|issn=1066-5285|doi=10.1007/s11172-005-0222-7|s2cid=97703681 }}
ZrCl4 + 4 N2O5 → Zr(NO3)4 + 4ClNO2
The product can be purified by sublimation in a vacuum. A contaminating substance in this is nitronium pentanitratozirconate. (NO2)Zr(NO3)5.
Zirconium nitrate pentahydrate Zr(NO3)4·5H2O can be formed by dissolving zirconium dioxide in nitric acid and then evaporating the solution until it is dry. However it is easier to crystallise zirconyl nitrate trihydrate ZrO(NO3)2·3H2O from such a solution.
Zirconium is highly resistant to nitric acid even in the presence of other impurities and high temperatures.{{cite web|url=http://ww.wahchangpresents.com/pdf/zirconium/0005.pdf|title=Zirconium in Nitric Acid Applications|last=Wah Chang|date=10 September 2003|access-date=13 October 2014}} So zirconium nitrate is not made by dissolving zirconium metal in nitric acid.
Properties
Zirconium nitrate pentahydrate dissolves easily in water and alcohol. It is acidic in aqueous solution, and a base such as ammonium hydroxide will cause zirconium hydroxide to precipitate. The pentahydrate crystals have a refractive index of 1.6.{{cite book|last=Patnaik|first=Pradyot|title=Handbook of inorganic chemicals|url=https://archive.org/details/Handbook_of_Inorganic_Chemistry_Patnaik|year=2003|publisher=McGraw-Hill|isbn=0070494398|page=[https://archive.org/details/Handbook_of_Inorganic_Chemistry_Patnaik/page/n1038 1000]}}
Related substances
Related substances are zirconium nitrate complexes. {{Chem2|Zr(NO3)3(H2O)3(+)}} has a tricapped trigonal prismatic structure, with the nitrates connected by two oxygen atoms each (bidentate). The pentanitrato complex {{Chem2|Zr(NO3)5(-)}} has all the nitrate groups bidentate, and has a bicapped square antiprism shape.
NO2[Zr(NO3)3·3H2O]2(NO3)3 crystallizes in the hexagonal system, space group P{{overline|3}}c1, with unit cell dimensions a = 10.292 Å, b = 10.292 Å, c = 14.84 Å, volume 1632.2 Å3 with 2 formulae per unit cell, density = 2.181.
CsZr(NO3)5 crystallizes in the monoclinic system, space group P21/n, with unit cell dimensions a = 7.497 Å, b = 11.567 Å, c = 14.411 Å, β=96.01°, volume 1242.8 Å3 with 4 formulae per cell, density = 2.855.
(NH4)Zr(NO3)5·HNO3 crystallizes in the orthorhombic system, space group Pna21 with unit cell dimensions a=14.852 Å, b = 7.222 Å, c = 13.177 Å, volume 1413.6 Å3 with 4 formulae per cell, density = 2.267.
A mixed nitronium, nitrosonium pentanitratozirconate crystallizing in the tetragonal system also exists.
Use
Zirconium nitrate is manufactured by a number of chemical suppliers. It is used as a source of zirconium for other salts, as an analytical standard, or as a preservative. Zirconium nitrate{{cite book|title=Fundamental Gas-phase and Surface Chemistry of Vapor-phase Deposition II and Process Control, Diagnostics and Modeling in Semiconductor Manufacturing IV: Proceedings of the International Symposium|url=https://books.google.com/books?id=WIvujcjCez4C&pg=PA144|year=2001|publisher=The Electrochemical Society|isbn=9781566773195|page=144}} and nitronium pentanitratozirconate can be used as chemical vapour deposition precursors as they are volatile, and decompose above 100 °C to form zirconia.{{cite journal|last=Nienow|first=Amanda M.|author2=Jeffrey T. Roberts|year=2006|title=Chemical Vapor Deposition of Zirconium Oxide on Aerosolized Silicon Nanoparticles|journal=Chemistry of Materials|volume=18|issue=23|pages=5571–5577|issn=0897-4756|doi=10.1021/cm060883e}} At 95 °C, zirconium nitrate sublimes with a pressure of 0.2 mm of Hg and can be deposited as zirconium dioxide on silicon at 285 °C. It has the advantage in that it is a single source, meaning it does not have to be mixed with other materials like oxygen, and decomposes at a relatively low temperature, and does not contaminate the surface with other elements such as hydrogen or fluorine.{{cite book|last=Houssa|first=Michel|title=High k Gate Dielectrics|url=https://books.google.com/books?id=mIOoUAkIaJ0C&pg=PA73|access-date=17 October 2014|date=2003-12-01|publisher=CRC Press|isbn=9781420034141|pages=73, 76–77}}
Zirconium free from hafnium is required for nuclear reactor construction. One way to achieve this is via a mixed aqueous solution of hafnium nitrate and zirconium nitrate, which can be separated by partitioning the zirconium into tributylphosphate dissolved in kerosene.{{cite web|last=Cox|first=R. P.|author2=G. H. Beyer|date=23 December 1955|title=Separation of Hafnium from Zirconium using Tributyl Phosphate|url=http://lib.dr.iastate.edu/cgi/viewcontent.cgi?article=1116&context=ameslab_iscreports|access-date=13 October 2014}}
Zirconium nitrate can be used as a Lewis acid catalyst in the formation of N-substituted pyrroles.{{cite journal|last=Hasaninejad|first=Alireza|author2=Mohsen Shekouhy|author3=Mohammad Reza Mohammadizadeh|author4=Abdolkarim Zare|year=2012|title=Zirconium nitrate: a reusable water tolerant Lewis acid catalyst for the synthesis of N-substituted pyrroles in aqueous media|journal=RSC Advances|volume=2|issue=15|page=6174|doi=10.1039/C2RA20294H|bibcode=2012RSCAd...2.6174H |issn=2046-2069}} registration required
Anhydrous zirconium nitrate can nitrate some organic aromatic compounds in an unusual way. Quinoline is nitrated to 3-nitroquinoline and 7-nitroquinoline. Pyridine is nitrated to 3-nitropyridine and 4-nitropyridine.{{cite book|last=Schofield|first=Kenneth|url=https://books.google.com/books?id=N-08AAAAIAAJ&pg=PA97|title=Aromatic Nitration|publisher=CUP Archive|year=1980|isbn=9780521233620|page=97|access-date=17 October 2014}}