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Usage

Uses

Used in Textile Industry:
CHROMIUM(III) FLUORIDE is used as a mordant for dyeing and printing woolens, which helps to improve the colorfastness and quality of the dyed fabric. It is also used for moth-proofing of woolen materials, providing protection against common fabric-damaging insects.
Used in Metal Polishing:
CHROMIUM(III) FLUORIDE is used as an abrasive in metal polishing, helping to achieve a smooth and shiny surface on various metal objects.
Used in Marble Coloring:
CHROMIUM(III) FLUORIDE is used as a coloring agent for marbles, enhancing their appearance and adding aesthetic value.
Used as a Halogenation Catalyst:
CHROMIUM(III) FLUORIDE is used as a catalyst in halogenation reactions, a chemical process that involves the addition of a halogen (such as fluorine, chlorine, bromine, or iodine) to a molecule.
Used in the Preparation of HFC-134a:
CHROMIUM(III) FLUORIDE is used in the preparation of a mixed-metal fluoride catalyst for the synthesis of HFC-134a, a refrigerant and propellant used in various applications.
Used in Rust-Prevention Paints:
CHROMIUM(III) FLUORIDE is used as a corrosion inhibitor in rust-prevention paints, helping to protect metal surfaces from rust and corrosion.

Preparation

Chromium(III) fluoride may be prepared by heating chromium trichloride under a stream of hydrogen fluoride: The compound may be prepared by the reaction of chromium hydroxide with hydrofluoric acid:

Air & Water Reactions

Water soluble.

Reactivity Profile

Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas.

Hazard

Irritant to skin and eyes, especially in solution.

Health Hazard

TOXIC; inhalation, ingestion or skin contact with material may cause severe injury or death. Contact with molten substance may cause severe burns to skin and eyes. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.

Fire Hazard

Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated.

Flammability and Explosibility

Notclassified

Safety Profile

A poison by ingestion. A corrosive. When heated to decomposition it emits toxic vapors of Cr and F-.

InChI:InChI=1/Cr.3FH/h;3*1H/q+2;;;/p-3

Upstream product

• 7664-39-3 hydrogen fluoride 
• 174002-65-4 H⁽¹⁺⁾*HF₂^(1-)=H₂F₂ 
• 7440-47-3 chromium 
• 10025-73-7 chromium(III) chloride 
• 7732-18-5 water 
• 10102-43-9 nitrogen(II) oxide 
• 123333-98-2 chromium(III) fluoride * x H₂O 
• 123333-98-2 chromium(III) fluoride trihydrate 
• 14884-42-5 chromium pentafluoride 
• 7782-50-5 chlorine 

Downstream Products

• 13709-38-1 lanthanum(III) fluoride 
• 7758-88-5 cerium(III) fluoride 
• 199620-14-9 chromium⁽⁰⁾ hexacarbonyl 
• 10025-73-7 chromium(III) chloride 
• 16671-27-5 {CrF₃(H₂O)3} 
• 14721-18-7 nickel(II) chromite 
• 10049-14-6 uranium(IV) tetrafluoride 
• 7783-81-5 uranium hexafluoride 
• 123333-98-2 chromium(III) fluoride * 5H2O 
• 11113-56-7 chromium(I) fluoride 
• 7783-40-6 magnesium fluoride 
• 7440-47-3 chromium 
• 7664-39-3 hydrogen fluoride 

Relevant academic research and scientific papers

Synthesis of a porous chromium fluoride catalyst with a large surface area

A novel approach to the preparation of a porous chromium fluoride catalyst with a large surface area is reported. The pores were generated by introduction of a siliceous material into the precursor of the catalyst and then removal of the material by reaction with anhydrous hydrogen fluoride. During the reaction, the formation and escape of a volatile gas (SiF4) from the precursor enlarged the surface area of the chromium fluoride. This process provided for the first time a porous chromium fluoride with a surface area of 187 m 2/g and a pore volume of 0.58 cm3/g. Furthermore, the porous chromium fluoride exhibited excellent chemical stability in the presence of HCl, HF, and F2. It was catalytically active for halogen exchange in a fixed-bed fluorination reaction, and it exhibited excellent catalytic performance in mitigating the coke formation on the surface of the catalyst during vapor-phase catalytic fluorination.

Surface characterization of chromia for chlorine/fluorine exchange reactions

The dismutation of CCl2F2 was used to probe the effect of halogenation of chromia by Cl/F exchange reactions to find out the difference between the halogenated inactive and active catalysts. The heterogeneous reactions were performed in a continuous flow Ni reactor and also under simulated reaction conditions in a reactor where after the reaction X-ray photoelectron spectroscopy (XPS) and X-ray excited Auger electron spectroscopy (XAES) analyses are possible without air exposure of the catalyst, i.e., under so-called in situ conditions. The Cr(III) 2p XP spectra, which revealed multiplet splitting features and satellite emission, were used for chemical analysis by using a simple evaluation procedure which neglects this inherent complexity. Chemical analysis was also applied by using chemical state plots for Cr 3s in order to cross-check Cr 2p related results. Both ex and in situ XPS show that as soon as Cr2O3 is exposed to CCl 2F2 at 390?°C fluorination as well as chlorination takes place at the catalyst surface. When the XPS surface composition reaches approximately 4 at. % fluorination and 6 at. % chlorination, maximum catalytic activity was obtained. Application of longer reaction times did not change significantly the obtained surface composition of the activated chromia. The fluorination and chlorination of chromia was further investigated by various HF and HCl treatments. The activated chromia samples and the Cr2O 3, Cr(OH)3, CrF2OH, CrF 3?·H2O, ?±-CrF3, ?2-CrF 3, and CrCl3 reference samples with well-known chemical structures were also characterized by X-ray absorption near edge structure (XANES), time-of-flight secondary ion mass spectroscopy (TOF-SIMS), pyridine-FTIR, wet chemical (F and Cl) analysis, X-ray powder diffraction (XRD), and surface area (BET) analysis. The results suggest that the formation of chromium oxide chloride fluoride species, e.g., chromium oxide halides, at the surface is sufficient to provide catalytic activity. The presence of any CrF3 and/or CrCl3 phases on the activated chromia samples was not found.

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.

Structural and magnetochemical studies of Ba5Mn3F19 and related compounds AII5MIII3F19

Single crystal structure determinations by X-ray methods were performed at the following compounds, crystallizing tetragonally body-centred (Z = 4): Sr5V3F19 (a = 1423.4(2), c = 728.9(1) pm), Sr5Cr3F19 (a = 1423.5(2), c = 728.1(1) pm), Ba5Mn3F19 (a =1468.9(1), c =770.3(1) pm, Ba5Fe3F19 (a =1483.5(1), c =766.7 (1) pm), and Ba5Ga3F19 (a = 1466.0(2), c = 760.1(2) pm). Only Ba5Mn3F19 was refined in space group I4cm (mean distances for elongated octahedra Mn1-F: 185/207pm equatorial/axial; for compressed octahedra Mn2-F: 199/182 pm), the remaining compounds in space group I4/m. In all cases the octahedral ligand spheres of the M1 atoms showed disorder, the [M1F6] octahedra being connected into chains in one part of the compounds and into dimers in the other. The magnetic properties of the V, Cr and Mn compounds named above and of Pb5Mn3F19 and Sr5Fe3F19 as well were studied; the results are discussed in context with the in part problematic structures.

Synthesis and crystal structure of CuIIMoIVF6 and CrIINbIVF6 (LT form)

The fluorides CuMoF6 and CrNbF6 are triclinic, isostructural with CuSnF6.Their crystal structures were solved in the space group P1, by the Rietveld method using the data of their X-ray powder patterns. Both crystal structures can be described as a three-dimensional framework of alternating 6 corner-sharing [M11F6] and [M′IVF6] octahedra (MII = Cr, Cu; M′IV = Nb, Mo) with ferrodistortive Jahn-Teller ordering.

Optical properties of chromium-doped fluoroindate glasses

This work reports on the optical properties of Cr3+ ions in the pseudoternary system InF3-GdF3-GaF3. Linear properties, investigated through absorption and emission spectra, provide information on the crystal field, the frequency, and number of phonons emitted during the absorption to the 4T2 band and the emission to the 4A2 ground state, and the Fano antiresonance line shape in the vicinity of the 4A2→2E transition. A study of the nonlinear refractive index as a function of the wavelength, carried out with the Z-scan technique, provides spectroscopic data about electronic transitions starting from the excited state.

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.

Crystal Structure Determinations of Four Monoclinic Weberites Na2M(II)M(III)F7 (M(II)=Fe, Co; M(III)=V, Cr)

By solid state reaction of the binary fluorides single crystals of the following weberites were prepared and their monoclinic structure (space group C2/C, Z=16) determined by X-ray methods: Na2FeVF7 (a=1271.0(3), b=742.9(1), c=2471.6(5) pm, β=100.03(3)°; R1=0.043 (1545 Reflexe); Fe-F=203.8, V-F 193.0 pm); Na2FeCrF7 (a=1262.5(3), b=739.1(1), c=2460.5(5) pm, β=99.93(3)°; R1=0.029 (2340); Fe-F=203.6, Cr-F=190.5 pm); Na2CoVF7 (a=1270.3(5), b=739.1(3), c=2465(10) pm, β=100.02(3)°; R1=0.028 (2250); Co-F=201.6, V-F=193.6 pm); Na2CoCrF7 (a=1257.8(3), b=733.5(1), c=2441.5(50 pm, β=99.64(3)°; R1=0.030 (2227); Co-F=201.2, Cr-F=190.2 pm). Concerning the above average distances within the distorted [MF6] octahedra and the shape of [NaF8] coordination details are given and discussed.

On the Thermal Decomposition of N2H6 and the New Compound N2H6CrF5

Thermal decomposition of N2H6 has been investigated by thermoanalytical, X-ray and IR spectroscopic methods.Under quasi-isobaric conditions the decomposition takes place in several steps.The intermediate N2H6CrF5 has been found which crystallizes monoclinically with a = 555.0 pm, b = 1084.6 pm, c = 77.0 pm, β = 91.76 deg .N2H6CrF5 decomposes via an amorphous intermediate to give pure rhomboedrical CrF3 as the final product.One of the intermediate has been identified as chromium fluoride ammoniate CrF3*0.4 NH3.No hydrolysis reactions have been observed.Keywords: Hydrazinium Pentafluorochromates(III), Fluorochromates(III), Thermal Decomposition, IR Spectra, X-Ray

Synthesis and thermal decomposition of (NH4)2[MIIIF5(H2O)] (M = Al, Fe and Cr)

Ammonium pentafluorometallate monohydrates were prepared by different methods and characterized by chemical analysis, IR spectrometry and X-ray diffraction. Unit cell parameters were determined for the Fe and Cr compounds, which were found to be isostruct