Vanadium pentafluoride

Vanadium(V) fluoride

Names
IUPAC name

Vanadium(V) fluoride

Other names

Vanadium pentafluoride

Identifiers

CAS Number

* 7783-72-4 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 10329757

EC Number |

* 232-023-9

PubChem CID

* 13416578

UNII |

* 1GNN7H50UE Y

InChI

* InChI=1S/5FH.V/h5*1H;/q;;;;;+5/p-5

Key: NFVUDQKTAWONMJ-UHFFFAOYSA-I

SMILES

* [F-].[F-].[F-].[F-].[F-].[V+5]

Properties

Chemical formula

| VF5
Molar mass | 145.934
Appearance  | colorless solid
Density | 2.502 g/cm3 (solid)
Melting point |  19.5 °C (67.1 °F; 292.6 K)
Boiling point |  48.3 °C (118.9 °F; 321.4 K)
Related compounds

Other anions

* Vanadium(V) chloride

Other cations

| Niobium(V) fluoride
Tantalum(V) fluoride
Phosphorus pentafluoride

Related Vanadium compounds

| Vanadium(V) oxide
Vanadium(II) fluoride
Vanadium(III) fluoride
Vanadium(IV) fluoride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Vanadium(V) fluoride is the inorganic compound with the chemical formula VF5. It is a colorless volatile liquid[1] that freezes near room temperature. It is a highly reactive compound, as indicated by its ability to fluorinate organic substances.[2]

## Contents

* 1 Properties and structure
* 2 Synthesis
* 3 Characteristics and reactivity
* 4 References
* 5 Other reading

## Properties and structure

The compound is exclusively a monomer in the gas phase.[3] In the gas phase it adopts D3h symmetric trigonal bipyramidal geometry as indicated by electron diffraction.[4] As a solid, VF5 forms a polymeric structure with fluoride-bridged octahedral vanadium centers.[3][5]

The formation enthalpy of VF5 is -1429.4 ± 0.8 kJ/mol.[6]

## Synthesis

Vanadium pentafluoride can be prepared by fluorination of vanadium metal:[7][1]

2 V + 5 F2 → 2 VF5

Alternatively, disproportionation of vanadium tetrafluoride yields equal amounts of the solid trifluoride and the volatile pentafluoride:[8][9][1]

2 VF4 → VF3 \+ VF5

This conversion is conducted at 650 °C. It can also be synthesized by using elemental fluorine to fluorinate industrial concentrates and raw materials so as to produce VF5 on an industrial scale. VF5 can be synthesized from the reaction of raw materials such as metallic Vanadium, ferrovanadium, vanadium (V) oxide and vanadium tetrafluoride with elemental fluorine.[10]

VF5 ionises in the liquid state as reflected by the high values of Trouton's constant and electrical conductivities.[11]

## Characteristics and reactivity

Interest in this highly corrosive compound began in the fifties when there were extensive studies of its physicochemical properties.[10] It is a powerful fluorinating and oxidizing agent. It oxidizes elemental sulfur to sulfur tetrafluoride:

S + 4 VF5 → 4 VF4 \+ SF4

Like other electrophilic metal halides, it hydrolyzes, first to the oxyhalide:

VF5 \+ H2O → VOF3 \+ 2 HF

Then to the binary oxide:

2 VOF3 \+ 3 H2O → V2O5 \+ 6 HF

Hydrolysis is accelerated in the presence of base. Despite its tendency to hydrolyze, it can be dissolved in alcohols.

It is a Lewis acid, as illustrated by its formation of the hexafluorovanadate:[12][13][14]

VF5 \+ KF → KVF6

Vanadium pentafluoride is a weaker acid and mainly undergoes oxidative and fluorinating reactions.[15]

The compound fluorinates unsaturated polyfluoroolefins into polyfluoroalkanes.[10]

The compound dissolves without reaction in liquid Cl2 and Br2. VF5 is moderately soluble in HF.

## References

1. ↑ 1.0 1.1 1.2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 989. ISBN 978-0-08-037941-8.
2. ↑ Canterford, J. H.; O'Donnell, Thomas A. (1967-03-01). "Reactivity of transition metal fluorides. IV. Oxidation-reduction reactions of vanadium pentafluoride". Inorganic Chemistry 6 (3): 541–544. doi:10.1021/ic50049a025. ISSN 0020-1669.
3. ↑ 3.0 3.1 Brownstein, S.; Latremouille, G. (1974-06-15). "Complex Fluoroanions in Solution. V. Vanadium Pentafluoride". Canadian Journal of Chemistry 52 (12): 2236–2241. doi:10.1139/v74-323. ISSN 0008-4042.
4. ↑ Hagen, Kolbjoern.; Gilbert, Michael M.; Hedberg, Lise.; Hedberg, Kenneth. (1982-07-01). "Molecular structure of gaseous vanadium pentafluoride, VF5". Inorganic Chemistry 21 (7): 2690–2693. doi:10.1021/ic00137a031. ISSN 0020-1669.
5. ↑ Brownstein, S. (1980-06-01). "The structure of VF5 in solution". Journal of Fluorine Chemistry 15 (6): 539–540. doi:10.1016/S0022-1139(00)85231-8.
6. ↑ Nikitin, M. I.; Zbezhneva, S. G. (2014-12-16). "Thermochemistry of vanadium fluorides: The formation enthalpies of vanadium fluorides" (in en). High Temperature 52 (6): 809–813. doi:10.1134/S0018151X14060108. ISSN 0018-151X. Bibcode: 2014HTemp..52..809N.
7. ↑ Trevorrow, L. E.; Fischer, J.; Steunenberg, R. K. (1957). "The Preparation and Properties of Vanadium Pentafluoride". Journal of the American Chemical Society 79 (19): 5167–5168. doi:10.1021/ja01576a023. Bibcode: 1957JAChS..79.5167T.
8. ↑ Ruff, Otto; Lickfett, Herbert (1911). "Vanadinfluoride". Berichte der Deutschen Chemischen Gesellschaft 44 (3): 2539–2549. doi:10.1002/cber.19110440379. https://zenodo.org/record/1426465.
9. ↑ Cavell, R. G.; Clark, H. C. (1963). "Thermochemistry of vanadium fluorides". Transactions of the Faraday Society 59: 2706. doi:10.1039/TF9635902706.
10. ↑ 10.0 10.1 10.2 Krasil'nikov, V. A.; Andreev, G. G.; Karelin, A. I.; Guzeeva, T. I.; Furin, G. G.; Bardin, V. V.; Avramenko, A. A. (1995-10-17). "ChemInform Abstract: Synthesis and Use of Vanadium Pentafluoride." (in en). ChemInform 26 (42): no. doi:10.1002/chin.199542022. ISSN 1522-2667.
11. ↑ Clark, H. C.; Emeléus, H. J. (January 1958). "40. Chemical reactions with vanadium, niobium, and tantalum pentafluorides" (in en). J. Chem. Soc.: 190–195. doi:10.1039/jr9580000190.
12. ↑ Nikolsky, B. P. [Никольский, Б.П.] et al, eds. (1971). Справочник химика [The Chemist's Handbook] Script error: The function "in_lang" does not exist.. 3rd (corrected) ed. Leningrad: Khimiya.
13. ↑ Knunyants, I. L. [Кнунянц, И.Л.] et al, eds. (1995). Химическая энциклопедия [A Chemical Encyclopedia] Script error: The function "in_lang" does not exist.. Moscow: Soviet Encyclopedias. ISBN 978-5-85270-092-6
14. ↑ Lidin, R. A. [Лидин Р.А.] et al (2000). Химические свойства неорганических веществ: Учеб. пособие для вузов [Chemical Properties of Inorganic Substances: A University Textbook] Script error: The function "in_lang" does not exist.. 3rd (corrected) ed. Мoscow: Khimiya. ISBN 978-5-7245-1163-6
15. ↑ Fowler, Brian R.; Moss, Kenneth C. (1979-12-01). "An N.M.R. study of the solution chemistry of vanadium pentafluoride". Journal of Fluorine Chemistry 14 (6): 485–494. doi:10.1016/S0022-1139(00)82524-5. Bibcode: 1979JFluC..14..485F.

## Other reading

* Arnold F. Holleman, Nils Wiberg: Lehrbuch der Anorganischen Chemie, 102. Auflage, de Gruyter, Berlin 2007, S. 1545, ISBN 978-3-11-017770-1.

* v
* t
* e

Vanadium compounds

Vanadium(0)|

* V(CO)6

Vanadium(II)|

* VBr2
* VCl2
* VO
* VS

Vanadium(III)|

* VBr3
* VCl3
* VF3
* VI3
* VN
* V2O3
* V2(SO4)3
* V2S3

Vanadium(IV)|

* VC
* VO2
* VS2
* VCl4
* VF4

| Organovanadium(IV) compounds|

* VO(C5H7O2)2

|

Vanadyl(IV) compounds|

* VOSO4

Vanadium(V)|

* V2O5
* VOCl3
* VOF3
* VF5
* V2S5

| Vanadyl(V) compounds|

* VO(ClO4)3

|

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

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