Vanadyl perchlorate

Vanadyl perchlorate
Names
Other names
tripercloratooxovanadium
Identifiers
CAS Number
  • 67632-69-3 ☒N
3D model (JSmol)
  • Interactive image
InChI
  • InChI=1S/3ClHO4.O.V/c3*2-1(3,4)5;;/h3*(H,2,3,4,5);;/q;;;;+3/p-3
    Key: XTDRROXTBUWEJW-UHFFFAOYSA-K
  • O=[V](OCl(=O)(=O)=O)(OCl(=O)(=O)=O)OCl(=O)(=O)=O
Properties
Chemical formula
 VO(ClO4)3
Molar mass 356.29 g/mol
Appearance golden yellow liquid or crystals.
Melting point 21-22 °C
Boiling point 33.5 °C in vacuum
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 oxidant
Related compounds
Related compounds
 niobium perchlorate, vanadyl nitrate, chromyl perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound

Vanadyl perchlorate or vanadyl triperchlorate is a golden yellow coloured liquid or crystalline compound of vanadium, oxygen and perchlorate group. The substance consists of molecules covalently bound and is quite volatile; it ignites organic solvents on contact and explodes at temperatures above 80 °C.[1]

Formation

Vanadyl perchlorate can be made by reacting vanadium pentoxide with dichlorine heptoxide at 5 °C. It is purified by distillation under a vacuum and recrystallisation at 21 °C.[1]

A solution of vanadium(V) perchlorate can be made by dissolving vanadium pentoxide in perchloric acid.[2]

The reaction of vanadium pentoxide and dichlorine hexoxide could produce VO(ClO4)3:[3]

2 V2O5 + 12 Cl2O6 → 4 VO(ClO4)3 + 12 ClO2 + 3 O2

Properties

It can react with vanadium oxychloride to form another vanadyl perchlorate (VO2ClO4): [3]

4 VO(ClO4)3 + 2 VOCl3 → 6 VO2ClO4 + 6 ClO2 + 3 Cl2 + 3 O2

Related

Other perchlorates include pervanadyl perchlorate, also known as dioxovanadium perchlorate, which contains VO2+ ions,[4] vanadyl diperchlorate, oxovanadium perchlorate or vanadium(IV) perchlorate, and VO(ClO4)2, which dissolves in water.[5][6] Vanadic perchlorate, also known as vanadium(III) perchlorate solution in water, is a green-tinged blue colour, significantly different to most other V(III) solutions, which are complexed.[7]

References

  1. ^ a b Fedoroff, Basil T; Sheffield, Oliver E. Encyclopedia of Explosives and Related Items Vol 10 of 10- U to Z, Page V5 (PDF). Vol. 10. p. 136.
  2. ^ Kustin, Kenneth; Toppen, David L. (June 1973). "Reduction of vanadium(V) by L-ascorbic acid". Inorganic Chemistry. 12 (6): 1404–1407. doi:10.1021/ic50124a038.
  3. ^ a b Schmeisser, Martin (1955). "Die Chemie der anorganischen Acylnitrate (ein Problem des Nitrylchlorids) und Acylperchlorate (ein Problem des Dichlorhexoxyds)". Angewandte Chemie. 67 (17–18): 493–501. Bibcode:1955AngCh..67..493S. doi:10.1002/ange.19550671708. ISSN 0044-8249.
  4. ^ Ramsey, J. B.; Heldman, M. J. (July 1936). "Kinetics of the Trivalent Vanadium—Iodine Reaction". Journal of the American Chemical Society. 58 (7): 1153–1157. doi:10.1021/ja01298a026.
  5. ^ Iannuzzi, Melanie M.; Rieger, Philip H. (December 1975). "Nature of vanadium(IV) in basic aqueous solution". Inorganic Chemistry. 14 (12): 2895–2899. doi:10.1021/ic50154a006.
  6. ^ Wuethrich, K.; Connick, Robert E. (March 1967). "Nuclear magnetic resonance relaxation of oxygen-17 in aqueous solutions of vanadyl perchlorate and the rate of elimination of water molecules from the first coordination sphere". Inorganic Chemistry. 6 (3): 583–590. doi:10.1021/ic50049a035.
  7. ^ Furman, Sydney C.; Garner, Clifford S. (April 1950). "Absorption Spectra of Vanadium(III) and Vanadium(IV) Ions in Complexing and Non-complexing Media". Journal of the American Chemical Society. 72 (4): 1785–1789. doi:10.1021/ja01160a105.
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Salts and covalent derivatives of the perchlorate ion
HClO4 He
LiClO4 Be(ClO4)2 B(ClO4)−4
B(ClO4)3 		ROClO3 N(ClO4)3
NH4ClO4
NOClO4
NO2ClO4 		H3OClO4 FClO4 Ne
NaClO4 Mg(ClO4)2 Al(ClO4)3
Al(ClO4)−4
Al(ClO4)2−5
Al(ClO4)3−6 		Si P S ClO−4
ClOClO3
Cl2O7 		Ar
KClO4 Ca(ClO4)2 Sc(ClO4)3 Ti(ClO4)4 VO(ClO4)3
VO2(ClO4) 		Cr(ClO4)3 Mn(ClO4)2 Fe(ClO4)2
Fe(ClO4)3 		Co(ClO4)2
Co(ClO4)3 		Ni(ClO4)2 Cu(ClO4)2 Zn(ClO4)2 Ga(ClO4)3 Ge As Se BrOClO3 Kr
RbClO4 Sr(ClO4)2 Y(ClO4)3 Zr(ClO4)4 Nb(ClO4)5 MoO2(ClO4)2 Tc Ru Rh(ClO4)3 Pd(ClO4)2 AgClO4 Cd(ClO4)2 In(ClO4)3 Sn(ClO4)4 Sb(ClO4)3 TeO(ClO4)2 I(OClO3)3 Xe(OClO3)2
CsClO4 Ba(ClO4)2 * Lu(ClO4)3 Hf(ClO4)4 Ta(ClO4)5
TaO(ClO4)3
TaO2ClO4 		WO(ClO4)4 ReO3ClO4 Os Ir Pt Au(ClO4)−4 Hg2(ClO4)2
Hg(ClO4)2 		Tl(ClO4)
Tl(ClO4)3 		Pb(ClO4)2 Bi(ClO4)3 Po At Rn
FrClO4 Ra ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* La(ClO4)3 Ce(ClO4)x Pr(ClO4)3 Nd(ClO4)3 Pm Sm(ClO4)3 Eu(ClO4)3 Gd(ClO4)3 Tb(ClO4)3 Dy(ClO4)3 Ho(ClO4)3 Er(ClO4)3 Tm(ClO4)3 Yb(ClO4)3
** Ac Th(ClO4)4 Pa UO2(ClO4)2 Np Pu Am Cm Bk Cf Es Fm Md No
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Vanadium compounds
Vanadium(0)
  • V(CO)6
Vanadium(II)
  • VF2
  • VBr2
  • VCl2
  • VI2
  • VO
  • VS
  • VSO4
Vanadium(III)
  • VBr3
  • VCl3
  • VF3
  • VI3
  • VN
  • V2O3
  • V2(SO4)3
  • V2S3
Organovanadium(III) compounds
  • V(C9H11)3
    • Vanadium(IV)
    • VC
    • VO2
    • VOCl2
    • V(S2)2
    • VCl4
    • VF4
    Organovanadium(IV) compounds
  • VO(C5H7O2)2
    • Vanadyl(IV) compounds
    • VOSO4
    Vanadium(V)
    • V2O5
    • VOCl3
    • VOF3
    • VO2F
    • VF5
    • VCl5
    • NH4VO3
    • VOPO4
    • VO+2
    Vanadyl(V) compounds
    • VO(ClO4)3
    • VO(NO3)3