Vanadyl nitrate

Source: Wikipedia, the free encyclopedia.
Vanadyl nitrate
Names
Other names
trinitratooxovanadium
Identifiers
3D model (
JSmol
)
ChemSpider
  • InChI=1S/3NO3.O.V/c3*2-1(3)4;;/q3*-1;;+3
    Key: NRKQBMOGOKEWPX-UHFFFAOYSA-N
SMILES
  • [V](O[N+]([O-])=O)(O[N+]([O-])=O)(O[N+]([O-])=O)=O
Properties
VO(NO3)3
Molar mass 252.953 g/mol
Appearance yellow liquid.
Melting point 2 °C (36 °F; 275 K)[1]
Boiling point 86 to 91 °C (187 to 196 °F; 359 to 364 K) at 0.7mm Hg
Hydrolysis
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 oxidant
Related compounds
Related compounds
titanium nitrate, vanadyl perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Vanadyl nitrate, also called vanadium oxytrinitrate or vanadium oxynitrate is an inorganic compound of vanadium in the +5 oxidation state with nitrate ligands and oxygen. The formula is VO(NO3)3. It is a pale yellow viscous liquid.[2]

Production

It is made by soaking

vanadium pentoxide in liquid dinitrogen pentoxide for durations around two days at room temperature. The yield for this method is about 85%.[3]

V2O5 + 3 N2O5 → 2 VO(NO3)3.

Purification can be achieved by vacuum distillation.[3]

Mononitratodioxovanadium (VO2NO3) is an intermediate in this synthesis. It is a brick red solid.[4][5]

Vanadyl nitrate can also be made from vanadyl trichloride VOCl3 and dinitrogen pentoxide.[6]

Structure

VO(NO3)3 has a distorted pentagonal bipyramid shape with idealized Cs (mirror) symmetry. The vanadium oxygen bond (157.2 pm) is typical for

vanadyl(V). Two nitrate groups in the pentagonal plane are bidentate (V-O distances range from 199 to 206 pm). The third nitrate spans the pentagonal plane (197 pm) to the position trans to oxo (223 pm).[7][8]

Properties

Vanadyl nitrate dissolves in dichloromethane, nitromethane, carbon tetrachloride, and saturated hydrocarbons.[1] 1-Hexene, or other unsaturated hydrocarbons ignite upon contact with vanadyl nitrate.[3][9] Upon contact with water, it irreversibly hydrolyzes, releasing nitric acid.[3][10]

The ultraviolet spectrum of the liquid shows an absorption band peaking at 208 nm with a shoulder at 242 nm. At 55 °C the gaseous vanadyl nitrate has absorption bands also at 486, 582 and 658 nm in the visual light spectrum.[10] in the infrared region, liquid vanadyl nitrate absorbs at 1880, 1633, 1612, 1560, 1306, 1205, 1016, 996, 965, 895, 783, 632, 457, 357, 301, 283, 234, 193, 133, 93 and 59 cm−1.[10] Gaseous vanadyl nitrate has absorption bands at 775, 783, 786, 962.5, 994.4, 997.5, 1000.5, 1006.2, 1012, 1016.3, 1020, 1198, 1211, 1216.3, 1564, 1612, 1629, 1632, 1635, 1648 and 1888 cm−1.[2] Many of these bands are due to stretching in nitrogen–oxygen bonds, but 1016.3 cm−1 is due to the double vanadium–oxygen bond. 786 is due to out of phase wagging in N-O, and 775 is due to deformation in O-N=O in the mirror plane.[2]

Reactions

It is a nitrating agent for aromatic compounds. Reactions proceed at room temperature. Often dichloromethane is used as an inert solvent.[1] Nitrotoluene, methyl benzoate and benzoic acid are nitrated by prolonged exposure over a few days.[1] Benzonitrile does not react.[1] [11]

Vanadyl nitrate form a solid pale yellow adduct with boron trifluoride.[3] An adduct is also formed with acetonitrile.[1]


References

  1. ^
    ISSN 0300-922X
    .
  2. ^
    ISSN 0044-2313
    .
  3. ^ a b c d e Harris, Arlo D.; John C. Trebellas (26 April 1962). "AD296097 Experimental Studies of the Reactions of N2O5 with Metal Acid Anhydrides and BF3". Arlington Hall Station: Armed Services Technical Information Agency. Archived from the original on September 24, 2015. Retrieved 30 September 2014.
  4. ^ Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry A Comprehensive Text (5 ed.). John Wiley. p. 814.
  5. ISSN 0022-1902
    .
  6. ISSN 0044-8249
    .
  7. ISSN 0300-9246
    . (free download)
  8. ISBN 9780854044269
    . Retrieved 30 September 2014.
  9. ^ Fedoroff, Basil T; Sheffield, Oliver E. Encyclopedia of Explosives and Related Items Vol 10 of 10- U to Z. Vol. 10. p. V4. Archived from the original on October 1, 2014.
  10. ^
    ISSN 1386-1425
    .
  11. ISBN 9783131720719
    . Retrieved 29 September 2014.

Other reading

  • Gmelin, Syst No 48, Teil A & Teil B (Lieferung 1 & 2) (1967); Teil A (Lieferung 1) & Teil A (Lieferung 2) (1968);& Erganzungwerk (Band2)(1971)
  • M. Schmeisser, "Chemical Abstracts", (1955), 49, 10873
  • L. Bretherick, Ed, "Hazards in the Chemical Laboratory", Royal Society of Chemistry, London, Engl (1979), pg. 1160
Retrieved from "https://en.wikipedia.org/w/index.php?title=Vanadyl_nitrate&oldid=1272799513"