Vanadium tetrafluoride

Vanadium(IV) fluoride  | 3D model of vanadium(IV) fluoride | 3D model of vanadium(IV) fluoride

|

Names
IUPAC name

vanadium tetrafluoride

Identifiers

CAS Number

* 10049-16-8

3D model (JSmol)

* Interactive image

ChemSpider |

* 11226730 Y

ECHA InfoCard | 100.030.143
EC Number |

* 233-171-7

PubChem CID

* 44717705

UNII |

* M372NC1A3B Y

UN number | UN2923

CompTox Dashboard (EPA)

* DTXSID50894991

InChI

* InChI=1S/4FH.V/h4*1H;/q;;;;+4/p-4 Y

Key: JTWLHYPUICYOLE-UHFFFAOYSA-J Y

* InChI=1/4FH.V/h4*1H;/q;;;;+4/p-4

Key: JTWLHYPUICYOLE-XBHQNQODAC

SMILES

* [V+4].[F-].[F-].[F-].[F-]

Properties

Chemical formula

| 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]

Solubility in water

| Very soluble[1]
Solubility | Soluble in acetone, acetic acid
Very slightly soluble in SO2Cl2, alcohols, CHCl3[2]
Structure

Crystal structure

| Monoclinic, mP10

Space group

| P21/c, No. 14
Thermochemistry

Std molar
entropy (S⦵298)

| 126 J/mol·K[3]

Std enthalpy of
formation (ΔfH⦵298)

| −1412 kJ/mol[3]

Gibbs free energy (ΔfG⦵)

| −1312 kJ/mol[3]
Hazards
Occupational safety and health (OHS/OSH):

Eye hazards

| Causes serious damage

Skin hazards

| Causes burns
GHS labelling:[4]

Pictograms

Signal word

| Danger

Hazard statements

| H300, H314, H330

Precautionary statements

| 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).

Y verify (what is YN ?)

Infobox references

Chemical compound

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

[edit]

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

[edit]

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−

## References

[edit]

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

## External links

[edit]

* WebElements

* v
* t
* e

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

|

* v
* t
* e

Fluorine compounds

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

| HF |  |  |  | ?HeF2

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4
+BO3 | CF4
CxFy
+CO3 | NF3
FN3
N2F2

N2F4
NF2
?NF5 | OF2
O2F2

O3F2
O4F2
?OF4 | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
S2F4
SF3
SF4
S2F10
SF6
+SO4 | ClF
ClF3
ClF5 | ?ArF2
?ArF4
KF | CaF
CaF2 |  | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
?CrF6 | MnF2
MnF3
MnF4
?MnF5 | FeF2
FeF3
FeF4 | CoF2
CoF3
CoF4 | NiF2
NiF3
NiF4 | CuF
CuF2
?CuF3 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6
+SeO3 | BrF
BrF3
BrF5 | KrF2
?KrF4
?KrF6
RbF | SrF
SrF2 |  | YF3 | ZrF2
ZrF3
ZrF4 | NbF4
NbF5 | MoF4
MoF5
MoF6 | TcF4
TcF

TcF6 | RuF3
RuF

RuF5
RuF6 | RhF3
RhF4
RhF5
RhF6 | PdF2
Pd[PdF6]
PdF4
?PdF6 | Ag2F
AgF
AgF2
AgF3 | CdF2 | InF
InF3 | SnF2
SnF4 | SbF3
SbF5 | TeF4
?Te2F10
TeF6
+TeO3 | IF
IF3
IF5
IF7
+IO3 | XeF2
XeF4
XeF6
?XeF8
CsF | BaF2 |  | LuF3 | HfF4 | TaF5 | WF4
WF5
WF6 | ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6
?OsF

?OsF
8 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
Pt[PtF6]
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
?AuF6
AuF5•F2 | Hg2F2
HgF2
?HgF4 | TlF
TlF3 | PbF2
PbF4 | BiF3
BiF5 | ?PoF2
PoF4
PoF6 | AtF
?AtF3
?AtF5 | RnF2
?RnF

?RnF

FrF  | RaF2 |  | LrF3 | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
| LaF3 | CeF3
CeF4 | PrF3
PrF4 | NdF2
NdF3
NdF4 | PmF3 | SmF2
SmF3 | EuF2
EuF3 | GdF3 | TbF3
TbF4 | DyF2
DyF3
DyF4 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3
AcF3 | ThF3
ThF4 | PaF4
PaF5 | UF3
UF4
UF5
UF6 | NpF3
NpF4
NpF5
NpF6 | PuF3
PuF4
PuF5
PuF6 | AmF2
AmF3
AmF4
?AmF6 | CmF3
CmF4
?CmF6 | BkF3
BkF
4 | CfF3
CfF4 | EsF3
EsF4
?EsF6 | Fm  | Md  | No

PF6−, AsF6−, SbF6− compounds|

* AgPF6
* KAsF6
* LiAsF6
* NaAsF6
* HPF6
* HSbF6
* NH4PF6
* LiSbF6
* KPF6
* KSbF6
* LiPF6
* NaPF6
* NaSbF6
* TlPF6

AlF6− compounds|

* (NH4)3[AlF6]
* Cs2AlF5
* Li3AlF6
* K3AlF6
* Na3AlF6

chlorides, bromides, iodides
and pseudohalogenides|

* BaClF
* SiIBrClF
* CFN
* ClFO2

SiF62-, GeF62- compounds|

* BaSiF6
* BaGeF6
* (NH4)2SiF6
* Na2[SiF6]
* K2[SiF6]
* Li2GeF6
* Li2SiF6

Oxyfluorides|

* BrOF3
* BrO2F
* BrO3F
* LaOF
* ThOF2
* VOF

* TcO

* WOF

* YOF
* ClOF3
* ClO2F3

Organofluorides|

* CBrF3
* CBr2F2
* CBr3F
* CClF3
* CCl2F2
* CCl3F
* CF2O
* CF3I
* CHF3
* CH2F2
* CH3F
* C2Cl3F3
* C2H3F
* C6H5F
* C7H5F3
* C15F33N
* C3H5F
* C6H11F

with transition metal,
lanthanide, actinide, ammonium|

* VOF3
* CrOF4
* CrF2O2
* NH4F
* (NH4)3CrF6
* (NH4)3GaF6
* (NH4)2GeF6
* (NH4)3FeF6
* (NH4)3InF6
* NH4NbF6
* (NH4)2SnF6
* NH4TaF6
* (NH4)3VF6
* (NH4)2ZrF6
* CsXeF7
* Li2SnF6
* Li2TiF6
* LiWF6
* Li2ZrF6
* K2TiF6
* Rb2TiF6
* Na2TiF6
* Na2ZrF6
* K2NbF7
* K2TaF7
* K2ZrF6
* UO2F2

nitric acids|

* FNO
* FNO2
* FNO3

bifluorides|

* KHF2
* NaHF2
* NH4HF2

thionyl, phosphoryl,
and iodosyl|

* F2OS
* F3OP
* PSF3
* IOF3
* IO3F
* IOF5
* IO2F
* IO2F3

Chemical formulas
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[H300]: H300: Fatal if swallowed
*[H314]: H314: Causes severe skin burns and eye damage
*[H330]: H330: Fatal if inhaled
*[P260]: P260: Do not breathe dust/fume/gas/mist/vapours/spray.
*[P301+P310]: P301+P310: IF SWALLOWED: Immediately call a POISON CENTER or doctor/physician.
*[P303+P361+P353]: P303+P361+P353: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water [or shower].
*[P304+P340]: P304+P340: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing.
*[P305+P351+P338]: P305+P351+P338: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do. Continue rinsing.
*[P320]: P320: Specific treatment is urgent (see ... on this label).
*[P330]: P330: Rinse mouth.
*[P405]: P405: Store locked up.
*[P501]: P501: Dispose of contents/container to ...
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