Zirconium nitrate

Zirconium nitrate
bottle of zirconium nitrate 五水硝酸锆
Names
Other names
zirconium tetranitrate, tetranitratozirconium, zirconium(4+) tetranitrate, zirconium(IV) nitrate
Identifiers
13746-89-9 N
ChemSpider 24459 N
Jmol interactive 3D Image
PubChem 162478205
Properties
Zr(NO3)4
Molar mass 339.243591 g/mol
Appearance transparent plates
Density ????2.192
Melting point  °C
Boiling point decompose 100 °C
water, ethanol
Hazards
Main hazards oxidiser
Lethal dose or concentration (LD, LC):
500 mg/m3 (rat, 30 min)[1]
Related compounds
Related compounds
 Zirconyl nitrate, hafnium nitrate, titanium nitrate, zirconium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Zirconium nitrate is a volatile anhydrous transition metal nitrate 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[2] and is class 5.1, meaning oxidising substance.[3]

Formation

Anhydrous Zirconium nitrate can be made from zirconium tetrachloride reacting with dinitrogen pentoxide.[4]

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.[4]

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.[4]

Zirconium is highly resistant to nitric acid even in the presence of other impurities and high temperatures.[5] So zirconium nitrate is not made by dissolving zirconium metal in nitric acid.

Properties

Zirconium nitrate pentahydrate dissolves easily in water and alcohol. In water it is acidic. The pentahydrate crystals have a refractive index of 1.6.[6]

Reactions

In water solution a base such as ammonium hydroxide will cause zirconium hydroxide to precipitate.

Zirconium nitrate can be used as a Lewis acid catalyst in the formation of N-substituted pyrroles.[7]

A mixed aqueous solution of hafnium nitrate and zirconium nitrate can be separated by partitioning the zirconium into tributylphosphate dissolved in kerosene. Zirconium free from hafnium is required for nuclear reactor construction.[8]

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.[9]

Related substances

Related substances are zirconium nitrate complexes. Zr(NO3)3.3H2O+ has a tricapped trigonal pyramid, with the nitrates connected by two oxygen atoms each (bidentate).[4] The pentanitrato complex Zr(NO3)5− has all the nitrate groups bidentate, and has a bicapped square antiprism shape.[4]

NO2[Zr(NO3)3.3H2O]2(NO3)3 crystallizes in the hexagonal system, space group P3C1 with unit cell dimensions a=10.292Å b=10.292Å c=14.84Å volume 1632.2Å3 with 2 formulae per cell, density=2.181.[4]

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 1242.8Å3 with 4 formulae per cell, density=2.855.[4]

(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 β=90° volume 1413.6 Å3 with 4 formulae per cell, density=2.267.[4]

A mixed nitronium, nitrosonium pentanitratozirconate crystallizing in the tetragonal system also exists.[4]

Use

Zirconium nitrate is manufactured by a number of chemical suppliers. It is used as a source of zirconium for other salts,[6] as an analytical standard,[6] or as a preservative.[6] Zirconium nitrate[10] and nitronium pentanitratozirconate can be used as chemical vapour deposition precursors as they are volatile, and decompose above 100 °C to form zirconia.[11] 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.[12]

References

  1. ↑ "Zirconium compounds (as Zr)". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
  2. ↑ "App A". The Code of Federal Regulations of the United States of America. U.S. Government Printing Office. 1988. p. 254.
  3. ↑ Recommendations on the Transport of Dangerous Goods: Model Regulations. United Nations Publications. 2009. p. 430. ISBN 9789211391367.
  4. 1 2 3 4 5 6 7 8 9 Morozov, I. V.; A. A. Fedorova; D. V. Palamarchuk; S. I. Troyanov (2005). "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)". Russian Chemical Bulletin 54 (1): 93–98. doi:10.1007/s11172-005-0222-7. ISSN 1066-5285.
  5. ↑ Wah Chang (10 September 2003). "Zirconium in Nitric Acid Applications" (PDF). Retrieved 13 October 2014.
  6. 1 2 3 4 Patnaik, Pradyot (2003). Handbook of inorganic chemicals. McGraw-Hill. p. 1000. ISBN 0070494398.
  7. ↑ Hasaninejad, Alireza; Mohsen Shekouhy; Mohammad Reza Mohammadizadeh; Abdolkarim Zare (2012). "Zirconium nitrate: a reusable water tolerant Lewis acid catalyst for the synthesis of N-substituted pyrroles in aqueous media". RSC Advances 2 (15): 6174. doi:10.1039/C2RA20294H. ISSN 2046-2069. registration required
  8. ↑ Cox, R. P.; G. H. Beyer (23 December 1955). "Separation of Hafnium from Zirconium using Tributyl Phosphate". Retrieved 13 October 2014.
  9. ↑ Schofield, Kenneth (1980). Aromatic Nitration. CUP Archive. p. 97. ISBN 9780521233620. Retrieved 17 October 2014.
  10. ↑ 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. The Electrochemical Society. 2001. p. 144. ISBN 9781566773195.
  11. ↑ Nienow, Amanda M.; Jeffrey T. Roberts (2006). "Chemical Vapor Deposition of Zirconium Oxide on Aerosolized Silicon Nanoparticles". Chemistry of Materials 18 (23): 5571–5577. doi:10.1021/cm060883e. ISSN 0897-4756.
  12. ↑ Houssa, Michel (2003-12-01). High k Gate Dielectrics. CRC Press. pp. 73, 76–77. ISBN 9781420034141. Retrieved 17 October 2014.
Salts and covalent derivatives of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4− C N O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Co(NO3)3		 Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I Xe(NO3)2
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2		 Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
↓
La Ce(NO3)3,
Ce(NO3)4		 Pr Nd Pm Sm Eu Gd(NO3)3 Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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