Vanadium tetrafluoride

Vanadium(IV) fluoride
3D model of vanadium(IV) fluoride
3D model of vanadium(IV) fluoride
3D model of vanadium(IV) fluoride
3D model of vanadium(IV) fluoride
Names
IUPAC name
vanadium tetrafluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.143 Edit this at Wikidata
EC Number
  • 233-171-7
UNII
UN number UN2923
  • InChI=1S/4FH.V/h4*1H;/q;;;;+4/p-4 checkY
    Key: JTWLHYPUICYOLE-UHFFFAOYSA-J checkY
  • InChI=1/4FH.V/h4*1H;/q;;;;+4/p-4
    Key: JTWLHYPUICYOLE-XBHQNQODAC
  • [V+4].[F-].[F-].[F-].[F-]
Properties
F4V
Molar mass 126.9351 g·mol−1
Appearance Lime green powder, hygroscopic[1]
Odor Odorless
Density 3.15 g/cm3 (20 °C)[1]
2.975 g/cm3 (23 °C)[2]
Melting point 325 °C (617 °F; 598 K)
at 760 mmHg decomposes[1]
Boiling point Sublimes[1]
Very soluble[1]
Solubility Soluble in acetone, acetic acid
Very slightly soluble in SO2Cl2, alcohols, CHCl3[2]
Structure
Monoclinic, mP10
P21/c, No. 14
Thermochemistry
126 J/mol·K[3]
−1412 kJ/mol[3]
−1312 kJ/mol[3]
Hazards
Occupational safety and health (OHS/OSH):
Eye hazards
 Causes serious damage
Skin hazards
 Causes burns
GHS labelling:[4]
GHS05: Corrosive GHS06: Toxic
Danger
H300, H314, H330
P260, P301+P310, P303+P361+P353, P304+P340, P305+P351+P338, P320, P330, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Vanadium(IV) fluoride (VF4) is an inorganic compound of vanadium and fluorine. It is paramagnetic yellow-brown solid that is very hygroscopic.[2] Unlike the corresponding vanadium tetrachloride, the tetrafluoride is not volatile because it adopts a polymeric structure.[5] It decomposes before melting.

Preparation and reactions

VF4 can be prepared by treating VCl4 with HF:

VCl4 + 4 HF → VF4 + 4 HCl

It was first prepared in this way.[6]

It decomposes at 325 °C, undergoing disproportionation to the tri- and pentafluorides:[2]

2 VF4 → VF3 + VF5

Structure

The structure of VF4 is related to that of SnF4. Each vanadium centre is octahedral, surrounded by six fluoride ligands. Four of the fluoride centers bridge to adjacent vanadium centres.[7]

  •   V4+;   F−
      V4+;   F−

References

  1. ^ a b c d e Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
  2. ^ a b c d Kwasnik, W. (1963). Brauer, Georg (ed.). Handbook of Preparative Inorganic Chemistry (UK ed.). London: Academic Press. pp. 252–253.
  3. ^ a b c Anatolievich, Kiper Ruslan. "vanadium(IV) fluoride". chemister.ru. Retrieved 2014-06-25.
  4. ^ "Vanadium(IV) fluoride, 95%". alfa.com. Alfa Aesar. Retrieved 2014-06-25.
  5. ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, p. 716, ISBN 0-471-19957-5
  6. ^ Otto Ruff, Herbert Lickfett "Vanadinfluoride" Chemische Berichte 1911, vol. 44, pages 2539–2549. doi:10.1002/cber.19110440379
  7. ^ Becker S., Muller B. G. Vanadium Tetrafluoride, Angew. Chem. Intnl. Ed. Engl. 1990, vol. 29, page 406