7784-36-3

Usage

Uses

1. Used in Electroconductive Polymers Industry:
Arsenic Pentafluoride is used as a doping agent for electroconductive polymers. Its chemical properties make it suitable for enhancing the electrical conductivity of these polymers, which is crucial for various applications in the electronics and materials science industries.
2. Used in Chemical Synthesis:
Arsenic Pentafluoride can be used in the synthesis of various compounds due to its reactivity with other elements and compounds. Its ability to form white clouds in moist air and its enthalpy of vaporization make it a valuable reagent in chemical processes.
3. Used in Research and Development:
Due to its unique chemical properties, Arsenic Pentafluoride can be utilized in research and development for studying the behavior of different materials under specific conditions. This can lead to the discovery of new compounds and applications in various scientific fields.

InChI:InChI=1/AsH3.5FH/h1H3;5*1H/q+3;;;;;/p-5

Upstream product

• 7782-41-4 fluorine 
• 16871-69-5 tetrachloroarsonium(V) hexafluoroarsenate(V) 
• 80485-40-1 dithionitronium hexafluoroarsenate 
• 88203-25-2 H₂NNH₃⁽¹⁺⁾*AsF₆^(1-)=N₂H₅AsF₆ 
• 136750-67-9 {FCNF}⁽¹⁺⁾*AsF₆^(1-)={FCNF}(AsF₆) 
• 86527-33-5 ClF₆⁽¹⁺⁾*AsF₆^(1-)=(ClF₆)(AsF₆) 
• 13709-36-9 xenon difluoride 
• 21501-81-5 H₃O⁽¹⁺⁾*AsF₆^(1-)=H₃O⁽¹⁺⁾AsF₆^(1-) 
• 7790-91-2 chlorine trifluoride 
• 7664-39-3 hydrogen fluoride 
• 7783-70-2 antimony pentafluoride 
• 7784-35-2 arsenic(III) fluoride 
• 7783-41-7 difluoroether 
• 7783-81-5 uranium hexafluoride 

Downstream Products

• 7783-54-2 nitrogen trifluoride 
• 13776-62-0 trans-1,2-difluorodiazine 
• 59544-89-7 SeI₃⁽¹⁺⁾*AsF₆^(1-)=(SeI₃)(AsF₆) 
• 7784-35-2 arsenic(III) fluoride 
• 12005-82-2 silver(I) hexafluoroarsenate 
• 119484-31-0 AsBr₄⁽¹⁺⁾*AsF₆^(1-)={AsBr₄}{AsF₆} 
• 7783-55-3 trifluorophosphane 
• 14720-21-9 gold(III) trifluoride 
• 49756-76-5 XeF₅⁽¹⁺⁾*AsF₆^(1-)=XeF₅AsF₆ 
• 7647-19-0 phosphorus pentafluoride 
• 15195-58-1 manganese tetrafluoride 
• 123168-21-8 bis-(pentafluoro phenyl) fluoro borane 
• 52374-78-4 Se₈⁽²⁺⁾*2AsF₆^(1-)={Se₈(AsF₆)2} 
• 53513-64-7 Se₄⁽²⁺⁾*2AsF₆^(1-)=(Se₄)(AsF₆)2 

Relevant academic research and scientific papers

Synthesis and Raman spectra of [Nd (XeF2)n](AsF6)3 (n = 3, 2.5) and crystal structure of [Nd (XeF2)2.5](AsF6)3

The reaction between Nd(AsF6)3(solv) and excess of XeF2(solv) in anhydrous HF (aHF) yields compounds of the type [Nd(XeF2)n](AsF6)3 (n = 3, 2.5). The first compound is very soluble in aHF while the latter crystallizes from the saturated solution in aHF. Pink needles [Nd(XeF2)2.5] (AsF6)3 crystallize in the space group C2/m with a = 3463.7(8) pm, b = 586.3(2) pm, c = 1010.7(2) pm, β = 103.53(2)°, V = 1.9955(9) nm3, Z = 4, R1 = 0.0379, wR2 = 0.0910, 5341 reflections collected, 2318 independent reflections. The Nd center is coordinated by a tricapped trigonal prism of nine fluorine atoms. The rectangular faces are capped by three coordinated XeF2 molecules. The regular trigonal prisms are formed by six different edge-bridging AsF6 octahedra, connecting the Nd centers to infinite chains. Two of such chains are interconnected by one of the XeF2 molecules forming a double chain.

Preparation and Characterization of the Adduct UO2F2*AsF5

The adduct UO2F2*AsF5 has been prepared as a pale yellow solid by the reaction of UO2F2 with AsF5 in anhydrous hydrogen fluoride.The adduct has been identified by mass balance, chemical analysis, vibrational spectra, X-ray powder diffraction patterns, and thermal analysis.

Syntheses, characterization, and computational study of AsF5 adducts with ketones

Lewis acid-base adducts between AsF5 and the ketones, acetone, cyclopentanone, and adamantanone, were synthesized from SO2 and CH2Cl2 solutions. These adducts, which contain O—As pnictogen bonding interactions, were found to be stable in solutions at room temperature. Raman and NMR spectroscopy of the solid adducts showed a characteristic decrease in the C=O stretching frequency, as well as dramatic deshielding of the 13C resonance of the carbonyl group upon adduct formation. Fluorine-19 NMR spectroscopy showed the two fluorine environments of the O–AsF5 moiety. Optimization of the gas-phase geometry using DFT calculations yielded geometries with essentially planar CC=OAs moieties. NBO analyses of the adducts and the free ketones show the polarization of the C=O bond upon adduct formation. The lowering of the LUMO energies upon adduct formation is more dramatic than what was found for protonation of ketones and reflects the substantially enhanced electrophilicity of the adducted ketones.

The Influence of the Counterions [AsF6]– and [GeF6]2– on the Structure of the [ClSO2NH3]+ Cation

Chlorosulfonamide reacts in the superacidic solutions HF/GeF4 and HF/AsF5 under the formation of ([ClSO2NH3]+)2[GeF6]2– and [ClSO2NH3]+/sup

[Li(XeF2)n](AF6) (A = P, As, Ru, Ir), the first xenon(II) compounds of lithium. Synthesis, Raman spectrum, and crystal structure of [Li(XeF2)3](AsF6)

The reactions between compounds of the type MAF6 (M = alkali metal; A = P, As, V, Ru, Ir, Sb, Nb, Ta) and xenon difluoride were studied in anhydrous hydrogen fluoride solvent. The coordination products [M(XeF 2)n]AsF6 were only observed in the case of LiAF6 (A = P, As, Ru, Ir), and the crystal structure of [Li(XeF 2)3]AsF6 was determined (monoclinic space group P21 with a = 6.901(9) A, b = 13.19(2) A, c = 6.91(1) A, β = 91.84(2), and Z = 2). The coordination sphere of lithium is comprised of six F atoms. The compound series was also characterized by Raman spectroscopy.

On the XeF+/H2O system: Synthesis and characterization of the xenon(II) oxide fluoride cation, FXeOXeFXeF+

The reported synthesis of the H2OF+ cation as a product of the oxidative fluorination of H2O by [XeF][PnF 6] (Pn = As, Sb) in HF solution has been reinvestigated. The system exhibits complex equilibria, producin

Palladium chemistry in anhydrous HF/AsF5 superacid medium

Pd metal dissolves in anhydrous HF (aHF) acidified with AsF5 in the presence of F2 at ≈298 K to give a blue-green solution from which green Pd(AsF6)2 can be isolated. The latter was also prepared by the interaction of PdF2 and AsF5 in aHF or by the reaction between PdO and F2 in aHF acidified with AsF 5. Powdered Pd(AsF6)2 slowly loses AsF 5 in a dynamic vacuum. It can therefore be isolated from solution at T 6)2 were prepared by solvothermal synthesis from a Pd/AsF5/F2/aHF mixture at 393 K. Pd(AsF6)2 is triclinic with a = 500.9(5), b = 538.3(5), c = 864.9(9) pm, α = 74.46(3), β = 89.97(4), γ = 62.47(2)° V = 0.1972(3) nm3, and Z = 1, space group P1 (No. 2). The six-coordinate Pd atoms (coordinated with fluorine) are well separated by isolated AsF6 units. In the 2-175 K temperature range Pd(AsF 6)2 follows the Curie-Weiss law with μeff = 3.53 B.M., Tn = 8 K and θp = -13 K. Because of cation-anion interactions, the AsF6- anions deviate from ideal Oh symmetry. The reduced symmetry can be seen in vibrational spectra, where splitting of the anion vibrational modes can be observed. The oxidation of Pd metal or PdO with F2 in neutral aHF yielded Pd 2F6. No reaction was observed between Pd, PdO or Pd 2F6 and AsF5 in aHF. All attempts to prepare PdFAsF6 were unsuccessful. Wiley-VCH Verlag GmbH & Co. KGaA, 69451 Weinheim, Germany, 2004.

New Coordination Compounds of Cd(AsF6)2 with HF and XeF2

Two new coordination compounds of cadmium with HF and XeF2 as ligands have been synthesized. Solid white [Cd(HF)](AsF6) 2 is obtained from an anhydrous HF (aHF) solution of Cd(AsF 6)2. It crystallizes in a monoclinic P21/c space group with a = 9.4687(14) A, b = 9.2724(11) A, c = 10.5503(18) A, β = 104.887(7)°, and Z = 4. The coordination sphere of Cd consists of 7 + 2 fluorine atoms, which are in a capped trigonal-prismatic arrangement. The reaction between Cd(AsF6)2 and XeF 2 in aHF yields a solid white product at room temperature having the composition [Cd(XeF2)4](AsF6)2 after the excess XeF2 and solvent have been removed under dynamic vacuum. [Cd(XeF2)4](AsF6)2 crystallizes in the orthorhombic space group P21212 1, with a = 8.6482(6) A, b = 13.5555(11) A, c = 16.6312(14) A, and Z = 4. The coordination sphere of Cd consists of eight fluorine atoms, which are at the corners of a trigonal prism with two capped side faces.

Syntheses, structures and properties of 1-ethyl-3-methylimidazolium salts of fluorocomplex anions

Fluoroacid-base reactions of a room-temperature ionic liquid, 1-ethyl-3-methylimidazolium fluorohydrogenate (EMIm(HF)2.3F, EMIm = 1-ethyl-3-methylimidazolium cation), and Lewis fluoroacids (BF3, PF5, AsF5, NbF5, TaF5 and WF6) give EMIm salts of the corresponding fluorocomplex anions, EMImBF4, EMImPF6, EMImAsF6, EMImNbF6, EMImTaF6 and EMImWF7, respectively. Attempts to prepare EMImVF6 by both the acid-base reaction of EMIm(HF)2.3F with VF5 and the metathesis of EMImCl with KVF6 failed due to the strong oxidizing power of the pentavalent vanadium, whereas EMImSbF6 was successfully prepared only by the metathesis of EMImCl and KSbF6. EMImBF4, EMImSbF6, EMImNbF6, EMImTaF6 and EMImWF7 are liquids at room temperature whereas EMImPF6 and EMImAsF6 melts at around 330 K. Raman spectra of the obtained salts showed the existence of the EMIm cation and corresponding fluorocomplex anions. IR spectroscopy revealed that strong hydrogen bonds are not observed in these salts. EMImAsF6 (mp 326 K) and EMImSbF6 (mp 283 K) are isostructural with the previously reported EMImPF6. The melting point of the hexafluorocomplex EMIm salt decreases with the increase of the size of the anion (PF6- 6- 6- 6- ≈ TaF6-).

Thermodynamic properties and decomposition of lithium hexafluoroarsenate, LiAsF6

The heat capacity of lithium hexafluoroarsenate is determined in the temperature range 50-750 K by adiabatic and differential scanning calorimetry techniques. The thermodynamic properties of LiAsF6 under standard conditions are evaluated: Cp0 (298.15 K)= 162.5 ± 0.3 J/(K mol), S0(298.15 K) = 173.4 ± 0.4 J/(K mol), Φ0(298.15 K) = 81.69 ± 0.20 J/(K mol), and H 0(298.15 K) - H0(0) = 27 340 ± 60 J/mol. The C p(T) curve is found to contain a lambda-type anomaly with a peak at 535.0 ± 0.5 K, which is due to the structural transformation from the low-temperature, rhombohedral phase to the high-temperature, cubic phase. The enthalpy and entropy of this transformation are 5.29 ± 0.27 kJ/mol and 10.30 ± 0.53 J/(K mol), respectively. The thermal decomposition of LiAsF6 is studied. It is found that LiAsF6 decomposes in the range 715-820 K. The heat of decomposition, determined in the range 765-820 K using a sealed crucible and equal to the internal energy change ΔU r(T), is 31.64 ± 0.08 kJ/mol.