7790-79-6

Usage

Chemical Properties

White powder

Physical properties

Colorless cubic crystal; density 6.33 g/cm3; melts at 1,110°C; vaporizes at 1,748°C; vapor pressure 5 torr at 1,231°C; moderately soluble in water, 4.35 g/100mL at 25°C; soluble in hydrofluoric and other mineral acids; practically insoluble in alcohol and liquid ammonia.

Uses

Different sources of media describe the Uses of 7790-79-6 differently. You can refer to the following data:
1. Cadmium fluoride is used in phosphors, glass and nuclear reactor controls. It is also used in high-temperature lubricants and to start crystals for lasers. It is used in oxygen-sensitive applications such as the production of metallic alloys and it is also used in limited medical treatment protocols. In addition, it can be used in synthetic organic chemistry.
2. Manufacture of phosphors, glass; in nuclear reactor controls.

Definition

Available as pure crystals, 99.89%, d 6.6, mp approx- imately 1110C, soluble in water and acids, insoluble in alkalies.

Preparation

Cadmium fluoride is prepared by the reaction of gaseous fluorine or hydrogen fluoride with cadmium metal or its salt, such as chloride, oxide or sulfide:Cd + F2 → CdF2Cd + 2HF → CdF2 + H2CdO + 2HF → CdF2 + H2OIt also may be obtained by dissolving cadmium carbonate in 40% hydrofluoric acid solution, evaporating the solution and drying in vacuum at 150°C:CdCO3 + 2HF → CdF2 + H2O + CO2It also may be prepared by mixing cadmium chloride and ammonium fluoride solutions, followed by crystallization.

Safety Profile

Confirmed human carcinogen. Poison by subcutaneous route. Violent reaction with K. When heated to decomposition it emits very toxic fumes of Cd and F-. See also FLUORIDES and CADMIUM COMPOUNDS.

Purification Methods

Crystallise it by dissolving it in hot water (25mL/g at room temperature) at 60o, filtering, then cooling. [Kwasnik in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 243 1963.]

InChI:InChI=1/Cd.FH/h;1H/q+2;/p-1

Upstream product

• 7664-39-3 hydrogen fluoride 
• 7440-43-9 cadmium 
• 7787-71-5 bromine trifluoride 
• 15989-98-7 bis(pentafluorophenyl)cadmium 
• 739319-89-2 cadmium(II) carbonate 
• 7782-41-4 fluorine 
• 873196-82-8 [(N,N,N',N'-tetramethylethylenediamine)bis(2-thenoyl-trifluorocetonate)cadmium(II)] 
• 13847-65-9 trifluoroamine oxide 
• 12125-01-8 ammonium fluoride 
• 119255-09-3 bis(difluoromethyl)cadmium 

Downstream Products

• 14215-29-3 cadmium(II) azide 

Relevant academic research and scientific papers

Phase transition and thermal decomposition of [Cd(H2O)6](BF4)2

Phase transition and thermal decomposition of [Cd(H2O)6](BF4)2 were studied by differential scanning calorimetry (DSC), differential thermal analysis (DTA) and thermogravimetry (TG) methods. The solid-solid phas

Phase equilibria in the binary system lead fluoride [PbF2]-cadmium fluoride [CdF2]

Phase dependences in the binary system lead fluoride [PbF2]-cadmium fluoride [CdF2] were examined and the phase diagram of this system was established. The occurrence of solid continuous solutions with a minimum melting point of 750°C and a CdF2 content of 35 mol% was confirmed. Thermal, dilatometric, microscopic and X-ray analytical methods were used during the investigations.

Thermal decomposition and kinetic data of Cd(BF4)2·6H2O

The thermal dehydration and decomposition of Cd(BF4)2·6H2O were studied by means of DTA, TG, DSC and X-ray diffraction methods and the end products of the thermal decomposition were identified. The results of thermal analysis show that the compound is fused first, then it is dehydrated until Cd(BF4)2·3H2O is obtained, which has not been described in the literature so far. The enthalpy of phase transition is ΔHph.tr.=115.6 kJ mol-1. Separation of the compound is difficult since it is highly hygroscopic. Then, dehydration and decomposition take place simultaneously until CdF2 is obtained which is proved by X-ray diffraction. On further increasing the temperature, CdF2 is oxidized to CdO and the characteristic curve assumes a linear character. Based on TG data, kinetic analyses were carried out separately for both parts of the curve: first until formation of the trihydrate and then - until formation of CdF2. The formal kinetic parameters are as follows: for the first phase: E*=45.3 kJ mol-1; rate equation F=α2/3; correlation coefficient 0.9858 for the second phase: E*=230.1 kJ mol-1; rate equation F =(1-α)2/3 [1-(1-α)1/3]-1; correlation coefficient 0.9982.

Coordination of XeF2 to calcium and cadmium hexafluorophosphates(V)

[M(XeF2)5](PF6)2 (M = Ca, Cd) complexes were prepared by the reaction of MF2 and XeF2 under pressure of gaseous PF5 in anhydrous HF as solvent. The coordination sphere of the Ca

Multifunctional cadmium single source precursor for the selective deposition of CdO or CdS by a solution route

We report on the interesting properties of a novel single precursor, Cd(tta)2·tmeda (Htta = 2-thenoyl-trifluoroacetone, tmeda = N,N,N′,N′-tetramethylethylenediamine), ideally suited for the selective and reproducible fabrication of pure quality films of CdS or CdO through a simple solution process. The Royal Society of Chemistry 2005.

XeF2 as a ligand in a coordination compound with the BF 4- anion

The first tetrafluoroborate compound with XeF2 coordinated to a metal center, [Cd(XeF2)](BF4)2, has been synthesized. It crystallizes in monoclinic space group P21/a with a = 8.785(11) A, b = 9.079(2) A, c = 10.718(6) A, β = 110.824(6), and Z = 4. Its crystal structure and that of Cd(BF4) 2 have been solved. The latter crystallizes in orthorhombic space group Pbca. Both syntheses were performed in aHF as solvent, at room temperature, yielding colorless solids. The Raman spectra of the solids are in harmony with the crystallographic findings. [Cd(XeF2)]-(BF 4)2 has been shown to be in equilibrium with XeF 2 and Cd(BF4)2 in aHF.

Cd2NF, an analogue of CdO

Cd2NF, isoelectronic with CdO, has been prepared by ammonolysis of CdF2. Cd2NF has the rock salt structure of CdO and shows electronic properties similar to CdO. First principles calculations shed light on the electronic structure and properties.

Interesting fluorine anion water clusters [F-·(H2O)n] in metal complex crystals

Three crystalline complexes containing fluorine anion water clusters, [Cd(Im)6][F·H2O]2 (1), [Ni(Im)6][F2·(H2O)5] (2) and [Co(Im)6][F·NO3·(H2O)s

Crystal structures of phases observed in [H3O]+/M2+/[SbF6]?system (M?=?Mg, Cr, Mn, Fe, Co, Ni, Cu, Zn, Pd, Cd)

The reactions between the MO (M?=?Be, Mg, Ca, Sr, Ti, V, Nb, Mn, Ni, Cu, Pd, Zn, Hg, Sn, Pb) and SbF5in liquid aHF were investigated. Reactions with the MO (M?=?Mg, Ni, Cu and Zn) yielded H3OM(SbF6)3compounds. Both BeO and PdO didn't show any sign of reactivity meanwhile MO (M?=?V, Nb, Ti) gave products with M in oxidation state higher than two. The rest of the MO (M?=?Ca, Sr, Mn, Hg, Sn, Pb) formed mixtures of M(SbF6)2, H3OSbF6and/or H3OSb2F11. Reactions between H3OSbF6and M(SbF6)2(M?=?Fe, Co, Ni) also gave H3OM(SbF6)3compounds, meanwhile similar attempts with H3OSbF6and M(SbF6)2(M?=?Ca, Mn, Pd, Ag, Cd, Sn) to prepare [H3O]+/M2+/[SbF6]?salts failled. However, slow crystallizations of H3OSbF6and M(SbF6)2(M?=?Mn, Pd, Cd) mixtures resulted in the single crystal growth of new (H3O)3M(SbF6)5phases which crystal structures are not isotypic. Similar procedure with H3OSbF6/Cr(SbF6)2mixture resulted in few light orange crystals of (H3O)3[CrIV(SbF6)6](Sb2F11)·HF. Its crystal structure determination showed the presence of discrete [CrIV(SbF6)6]2?units where each of Cr atoms is found in a homoleptic coordination of six SbF6groups.

Revealing the structural chemistry of the group 12 halide coordination compounds with 2,2′-bipyridine and 1,10-phenanthroline

The coordination compounds of group 12 halides with 2,2′-bipyridine (bpy) and 1,10-phenanthroline (phen), 2[CdF2(bpy)2]·7H2O (1), [ZnI(bpy)2]+·I3 ? (2), [CdI2(bpy)2] (3), [Cd(SiF6)H2O(phen)2]·[Cd(H2O)2(phen)2]2+·F–·0.5(SiF6)2–·9H2O (4), [Hg(phen)3]2+·(SiF6)2–·5H2O (5), [ZnBr2(phen)2] (6), 6[Zn(phen)3]2+·12Br–·26H2O (7) and [ZnI(phen)2]+·I– (8), have been synthesized and characterized by X-ray crystallography, IR spectroscopy, elemental and thermal analysis. Structural investigations revealed that metal : ligand stoichiometry in the inner coordination sphere is 1 : 2 or 1 : 3. A diversity of intra- and intermolecular interactions exists in structures of 1–8, including the rare halogen?halogen and halogen?π interactions. The thermal and spectroscopic properties were correlated with the molecular structures of 1–8. Structural review of all currently known coordination compounds of group 12 halides with bpy and phen is presented.