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Vanadium tetrafluoride

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
EC Number
  • 233-171-7
UNII
UN number UN2923
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
GHS pictograms GHS05: CorrosiveGHS06: Toxic[4]
GHS signal word Danger
H300, H330, H314, H318[4]
P260, P301+310, P303+361+353, P304+340, P305+351+338, P320, P330, P405, P501[4]
Eye hazard Causes serious damage
Skin hazard Causes burns
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

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. 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.[5]

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

2 VF4 → VF3 + VF5

Structure

     V4+;      F

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.[6]

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. External link in |website= (help)
  4. ^ a b c "Vanadium(IV) fluoride, 95%". [www.alfa.com]. Alfa Aesar. Retrieved 2014-06-25. External link in |website= (help)
  5. ^ Otto Ruff, Herbert Lickfett "Vanadinfluoride" Chemische Berichte 1911, vol. 44, pages 2539–2549. doi:10.1002/cber.19110440379
  6. ^ Becker S., Muller B. G. Vanadium Tetrafluoride, Angew. Chem. Intnl. Ed. Engl. 1990, vol. 29, page 406