Uranyl nitrate

Uranyl nitrate

Uranyl nitrate
Uranyl nitrate as yellow crystals
Ball-and-stick models of the ions present
IUPAC name
Other names
Uranium nitrate
ChemSpider  Y
Jmol-3D images Image
Molar mass 394.04 g/mol
Appearance yellow-green solid
Density 2.81 g/cm3
Melting point
Boiling point (decomposition)
g/100g H2O: 98 (0°C), 122 (20°C), 474 (100°C)[1]
Solubility in tributyl phosphate soluble
Safety data sheet External MSDS
Very Toxic T+
Dangerous for the Environment (Nature) N
R-phrases R51/53
S-phrases (S1/2), S20/21, S45, S61
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
12 mg/kg (dog, oral)
238 (cat, oral)[2]
Related compounds
Other anions
Uranyl chloride
Uranyl sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 Y  (: Y/N?)

Uranyl nitrate (UO2(NO3)2) is a water soluble yellow uranium salt. The yellow-green[3] crystals of uranium nitrate hexahydrate are triboluminescent.

Uranyl nitrate can be prepared by reaction of uranium salts with nitric acid. It is soluble in water, ethanol, acetone, and ether, but not in benzene, toluene, or chloroform.


  • Uses 1
  • Health and environmental issues 2
  • External links 3
  • References 4


During the first half of the 19th century, many photosensitive metal salts had been identified as candidates for photographic processes, among them uranyl nitrate. The prints thus produced were alternately referred to as uranium prints, urbanities, or more commonly uranotypes. The first uranium printing processes were invented by a Scotsman, J. Charles Burnett, between 1855 and 1857, and used this compound as the sensitive salt. Burnett, authored an 1858 article comparing "Printing by the Salts of the Uranic and Ferric Oxides" The basis for the process lies in the ability of the uranyl ion to pick up two electrons and reduce to the lower oxidation state of uranium(IV) under ultraviolet light. Uranotypes can vary from print to print from a more neutral, brown russet to strong Bartolozzi red, with a very long tone grade. Surviving prints are slightly radioactive, a property which serves as a means of non-destructively identifying them. Several other more elaborate photographic processes employing the compound sprung up and vanished throughout the second half of the century with names like Wothlytype, Mercuro-Uranotype and the Auro-Uranium process. Uranium papers were manufactured commercially at least until the end of the 19th century, vanishing in the face of the superior sensitivity and practical advantages of the silver halides. Nevertheless between the 1930s through the 1950s Kodak Books still described a uranium toner (Kodak T-9) using uranium nitrate hexahydrate. Some alternative process photographers including artists Blake Ferris and Robert Schramm continue to make uranotype prints today.

Along with uranyl acetate it is used as a negative stain for viruses in electron microscopy; in tissue samples it stabilizes nucleic acids and cell membranes.

Uranyl nitrate was used to fuel Aqueous Homogeneous Reactors in the 1950s. However it proved too corrosive in this application, and the experiments were abandoned.

Uranyl nitrate is important for nuclear reprocessing; it is the compound of uranium that results from dissolving the decladded spent nuclear fuel rods or yellowcake in nitric acid, for further separation and preparation of uranium hexafluoride for isotope separation for preparing of enriched uranium.

Health and environmental issues

Uranyl nitrate is an oxidizing and highly toxic compound. When ingested, it causes severe kidneys, liver, lungs and brain. It also represents a severe fire and explosion risk when heated or subjected to shock in contact with oxidizable substances.

External links

  • URANIUM DAYS: Notes On Uranium Photography (2007 archive from archive.org)
  • Chemical Database – Uranyl nitrate, solid


  1. ^ http://ibilabs.com/uranium-uranyl-thorium-compounds/uranyl-compounds/uranyl-nitarte-hexahydrate/
  2. ^ "Uranium (soluble compounds, as U)". Immediately Dangerous to Life and Health.  
  3. ^ Roberts, D.E. and Modise, T.S. (2007). Laser removal of loose uranium compound contamination from metal surfaces. Applied Surface Science 253, 5258–5267.
Salts and covalent derivatives of the Nitrate ion
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,
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
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(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,
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