10049-12-4

Basic information

• Product Name: VANADIUM TRIFLUORIDE
• Synonyms: VF3;VANADIUM(III) FLUORIDE;VANADIUM TRIFLUORIDE;Vanadium(III) fluoride 98%;Vanadium(III)fluoride98%;VANADIUM (III) FLOURIDE;Vanadium(III) trifluoride
• CAS NO: 10049-12-4
• Molecular Formula: F₃V
• Molecular Weight: 107.94
• EINECS: 233-169-6
• Mol File: 10049-12-4.mol

Chemical Properties

• Melting Point: 140°C
• Boiling Point: °Cat760mmHg
• Flash Point: °C
• Appearance: /Powder
• Density: 3,36 g/cm3
• Water Solubility: Practically insoluble in water, acetone, and glacial acetic acid
• Sensitive: Moisture Sensitive
• Merck: 14,9922
• CAS DataBase Reference: VANADIUM TRIFLUORIDE(CAS DataBase Reference)
• NIST Chemistry Reference: VANADIUM TRIFLUORIDE(10049-12-4)
• EPA Substance Registry System: VANADIUM TRIFLUORIDE(10049-12-4)

Safety Data

• Hazard Codes: Xi,T
• Statements: 36/37/38-34-32-23/24/25
• Safety Statements: 26-36-45-36/37/39-22
• RIDADR: UN2923
• HazardClass: 8
• PackingGroup: II
• Hazardous Substances Data: 10049-12-4(Hazardous Substances Data)

Usage

Uses

Used in Chemical Industry:
Vanadium trifluoride is used as a catalyst in various chemical reactions, particularly in the production of oxygen-sensitive materials such as metals. Its catalytic properties enable efficient and controlled reactions, making it a valuable component in the chemical industry.
Used in Material Science:
Vanadium trifluoride is employed in the development and synthesis of advanced materials, taking advantage of its unique chemical and physical properties. Its ability to form compounds with various elements contributes to the creation of new materials with specific characteristics and applications.
Used in Oxygen-Sensitive Applications:
Vanadium trifluoride is used as a key component in oxygen-sensitive applications, such as metal production. Its reactivity with oxygen allows for the efficient production of metals and other materials that require controlled oxygen environments.

InChI:InChI=1/3FH.V/h3*1H;/q;;;+3/p-3/rF3V/c1-4(2)3

Upstream product

• 75-71-8 Dichlorodifluoromethane 
• 16984-48-8 fluoride 
• 7718-98-1 vanadium(III) chloride 
• 7782-41-4 fluorine 
• 7783-72-4 vanadium pentafluoride 
• 507-25-5 carbon tetraiodide 
• 7440-62-2 vanadium 
• 7790-91-2 chlorine trifluoride 
• 7664-39-3 hydrogen fluoride 
• 10049-16-8 vanadium(IV) fluoride 
• 7784-35-2 arsenic(III) fluoride 
• 7632-51-1 vanadiumtetrachloride 

Downstream Products

• 7440-62-2 vanadium 

Relevant articles and documents

Synthesis, structure, and magnetic properties of compounds NaMIIZr2F11 (MII = Ti, V, Cu) and a notice on NaPdZr2F11

By synthesizing NaTiZr2F11 in form of red single crystals, it was possible to obtain a complex fluoride with Ti2+ for the first time. It crystallizes like the analogous greenish blue vanadium compound isotypic to AgPdZr2F11 [1] monoclinic, spacegroup C2/m-C2h3 (No. 12) with a = 918.0/911.5 pm, b = 682.6/675.7 pm, c = 780.8/776.6 pm, β = 116.2/116.2° and Z = 2. Colourless NaCuZr2F11 however crystallizes as a result of the Jahn-Teller distortion of Cu2+ triclinic (space group P1-Ci1 (No. 2), a = 552.7 pm, b = 568.2 pm, c = 768.0 pm, α = 111.0°, β = 97.4°, γ = 106.4°) and is - as expected - isotypic to NaAgZr2F11 [1]. Johann Ambrosius Earth 1996.

Thermal dehydration of the fluoride hydrates FeMIIIF5·7H2O (MIII = Al, Fe, V, Cr)

The thermal dehydration of the fluoride hydrates FeAlF5·7H2O, Fe2F5·7H2O, FeVF5·7H2O and FeCrF5·7H2O has been investigated by thermoanalytical, X-ray and i.

(H2O)[V2III F6] and Pyr-VF3:Hydrothermal synthesis, structure determination, and magnetic characterization of new fluorides with the pyrochlore type

Small green triangular crystals of a new tridimensional hydrated vanadium(III) fluoride have been hydrothermally prepared in a simple way by heating a mixture of V:HF:H2O in the molar ratio 1:1:50 at 200°C for 3 days. Its structure was solved by X-ray diffraction in the cubic space group Fd3m (No. 227) with a = 10.4636(2)A. (H2O)[V2IIIF6] presents the structure of the well-known pyrochlore type. The cavities contain water molecules which are lost by heating (T 3 (Pyr-VF3) with the pyrochlore structure is compared to that of the already known Pyr-FeF3 (1). The magnetic behavior of Pyr-VF3 is described.

Structural and magnetochemical studies of SrVF5

Single crystals of SrVF5 were obtained by heating a mixture of the component fluorides at 850°C for 5 d (a = 707.2(1), b = 727.1(1), c = 1471.4(2) pm, β = 94.96(1)°; space group P21/c, Z = 8). The X-ray structure determination confirmed its helical SrFeF5 type of chain structure, in which the octahedra sharing cis corners are considerably distorted (average V-F: 193,7 pm). The compound is weakly antiferromagnetic; there is indication of three-dimensional ordering only at the lowest temperature measured (TN ≈ 2 K). The flat susceptibility maximum near 6 K is attributed to lowdimensional preordering. As studied at a single crystal the behaviour is anisotropic, indicating spin orientation about along [100], normal to the chain axis [010].

The crystal structures of the vanadium weberites Na2MIIVIIIF7 (MII = Mn, Ni, Cu) and of NaVF4

At single crystals of the vanadium(III) compounds NaVF4 (a = 790.1, b = 531.7, c = 754.0 pm, β = 101.7°; P21/c, Z = 4), Na2NiVF7 (a = 726.0, b = 1031.9, c = 744.6 pm; Imma, Z = 4) and Na2CuVF7 (a = 717.6, b = 1043.5, c = 754.6 pm; Pmnb, Z = 4) X-ray structure determinations were performed, at Na2MnVF7 (a = 746.7, c = 1821.6 pm; P3221, Z = 6) a new refinement. NaVF4 crystallizes in the layer structure type of NaNbO2F2. The fluorides Na2MIIVF7 represent new orthorhombic (MII = Ni; Cu) resp. trigonal (MII = Mn) weberites. The average distances within the [VF6] octahedra of the four compounds are in good agreement with each other and with data of related fluorides (V-F: 193.3 pm). The differences between mean bond lengths of terminal and bridging F ligands are 5% in NaVF4, but less than 1% in the weberites. Details and data for comparison are discussed.

SENSITIZED LUMINESCENCE OF VF5 UNDER THE ACTION OF THE EMISSION OF A PULSED CO2 LASER.

Study of sensitized visible luminescence of VF//5, which accompanies its dissociation, under the action of emission from a pulsed CO//2 laser is described.

Cooperative radiative and nonradiative effects in K2NaScF6 codoped with V3+ and Er3+.

K2NaScF6 crystals codoped with V3+ and Er3+ exhibit some novel cooperative near-IR to visible upconversion processes at cryogenic temperatures. V3+ mainly acts as a broadband sensitizer. The V3+ 3T1g --> 3T2g excitation between 13,500 and 15,500 cm(-1), after fast relaxation to V3+ 1T2g, can be transferred to Er3+ 4I(11/2), and then upconversion takes place. Four upconversion mechanisms are identified and characterized. For narrow-band laser excitation the overall efficiency of the upconversion processes is low. However, at 12 K for broadband excitation, such as in a lamp, between 12,000 and 14,500 cm(-1) the number of emitted visible photons is roughly doubled by codoping V3+ in addition to Er3+. Copyright 2004 American Institute of Physics

Decomposition of dichlorodifluoromethane with simultaneous halogen fixation by vanadium oxide supported on magnesium oxide

Dichlorodifluoromethane (CCl2F2, 1% in He) decomposition with simultaneous halogen fixation by vanadium oxide supported on magnesium oxide was studied at 723 K in a flow apparatus. The pretreatment condition and vanadium loading of supported vanadium oxide samples affected the CCl2F2 decomposition efficiency. Through characterization studies (XRD, IR, Raman, and XPS) and reference experiments, Mg 3(VO4)2 was revealed to be the active species to initiate CCl2F2 decomposition, leading to MgF 2, MgCl2, and CO2 formation. The model experiments also suggested a detailed mechanism that VOCl3 was formed from Mg3(VO4)2 by a reaction with CCl 2F2 or the major intermediate compound CCl4, and that VOCl3 reacted with MgO to regenerate Mg3(VO 4)2 and to promote chlorine fixation as MgCl2.

New Fluorozirconates and -hafnates with V2+ and Ti2+

During investigations of the systems MF2/KF/MF4 e.g. MF2/NaF/MF4 (M2+ = Ti2+, V2+, M4+= Zr4+ Hf4+) we obtained blue crystals of VZrF6, VHfF6, KVZrF7, blue-green crystals of NaVHf2F11, yellow crystals of TiHfF6 and NaTiHf2F11, and yellow to rubyred crystals of TiZrF6, respectively. According to single crystal data, VZrF6 VHfF6 and TiZrF6 crystalizes in the ordered ReO3-type (cubic, Fm3m, a = 812,1(5), 804,2(8), and 821,0(2) pm, Z = 4). TiHfF6 crystalizes in a high-temperature-modification (cubic, ReO3-type, Pm3m, a = 392,3(2) pm, Z = 2). KVZrF7 is isotyic to KPdZrF7 (orthorhombic, Pnna, a = 1109,8(6), b = 788,0(7), c = 648,0(15) pm, Z = 4). NaTiHf2F11 and NaVHf2F11 crystalizes monoclinic (C2/m, a = 910,5(7), b = 675,9(7), c = 773,6(5) pm, β= 116,10(6)° and a = 917,7(5), b = 685,7(5), c = 752,4 pm, β= 118,28(1)°, Z = 2, respectively) and are also isotypic to already known AgPdZr2F11. WILEY-VCH Verlag GmbH, D-69451 Weinheim, 2001.

Reactivity of Tin Difluoride

A new value of the enthalpy of formation of tin difluoride was used to calculate the thermodynamic parameters of reactions of SnF2 with elemental substances and several metal oxides. SnF2 can act as an oxidizer and is useful for the synthesis of higher fluorides of group III-V transition metals, including those that have previously been prepared only by reactions with elemental fluorine (TiF4, NbF5, TaF5). The fact that such reactions occur was verified experimentally.