| 词条 | Cadmium fluoride |
| 释义 |
| Watchedfields = changed | verifiedrevid = 477163492 | Name = Cadmium fluoride | ImageFile =Fluorite-unit-cell-3D-ionic.png | IUPACName = Cadmium fluoride | OtherNames = Cadmium(II) fluoride, Cadmium difluoride |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 23036 | InChI = 1/Cd.2FH/h;2*1H/q+2;;/p-2 | SMILES = F[Cd]F | InChIKey = LVEULQCPJDDSLD-NUQVWONBAG | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/Cd.2FH/h;2*1H/q+2;;/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = LVEULQCPJDDSLD-UHFFFAOYSA-L | CASNo = 7790-79-6 | CASNo_Ref = {{cascite|correct|CAS}} | EINECS = 232-222-0 | PubChem = 24634 | PubChem1 = 71356118 | PubChem1_Comment = dihydrate |Section2={{Chembox Properties | Formula = CdF2 | MolarMass = 150.41 g/mol | Appearance = grey or white-grey crystals | Density = 6.33 g/cm3, solid | Solubility = 4.35 g/100 mL | SolubleOther = soluble in acid insoluble in ethanol alcohol and liquid ammonia | MeltingPtC = 1110 | MeltingPt_notes = | BoilingPtC = 1748 | BoilingPt_notes = | MagSus = -40.6·10−6 cm3/mol }} |Section3={{Chembox Structure | CrystalStruct = Fluorite (cubic), cF12 | SpaceGroup = Fm3m, No. 225 | Section4 = {{Chembox Thermochemistry | HeatCapacity = | Entropy = | DeltaHf = -167.39 ± 0.23 kcal. mole-1 at 298.15 (K, C?) | DeltaGf = -155.4 ± 0.3 kcal. mole-1 at 298.15 (K, C?) | DeltaHc = |Section7={{Chembox Hazards | ExternalSDS = | NFPA-H = | NFPA-F = | NFPA-R = | GHSPictograms = {{GHS06}}{{GHS08}}{{GHS09}} | GHSSignalWord = Danger | HPhrases = {{H-phrases|301|330|340|350|360|372|400|410}} | PPhrases = {{P-phrases|201|202|260|264|270|271|273|281|284|301+310|304+340|308+313|310|314|320|321|330|391|403+233|405|501}} | REL = Ca[1] | PEL = [1910.1027] TWA 0.005 mg/m3 (as Cd)[1] | IDLH = Ca [9 mg/m3 (as Cd)][1] |Section8={{Chembox Related | OtherAnions = Cadmium chloride, Cadmium bromide Cadmium iodide | OtherCations = Zinc fluoride, Mercury(II) fluoride, Copper(II) fluoride, Silver(II) fluoride, Calcium fluoride, Magnesium fluoride }}Cadmium fluoride (CdF2) is a mostly water-insoluble source of cadmium used in oxygen-sensitive applications, such as the production of metallic alloys. In extremely low concentrations (ppm), this and other fluoride compounds are used in limited medical treatment protocols. Fluoride compounds also have significant uses in synthetic organic chemistry.[2] The standard enthalpy has been found to be -167.39 kcal. mole−1 and the Gibbs energy of formation has been found to be -155.4 kcal. mole−1, and the heat of sublimation was determined to be 76 kcal. mole−1.[3][4] PreparationCadmium fluoride is prepared by the reaction of gaseous fluorine or hydrogen fluoride with cadmium metal or its salts, such as the chloride, oxide, or sulfate. It may also be obtained by dissolving cadmium carbonate in 40% hydrofluoric acid solution, evaporating the solution and drying in a vacuum at 150 °C. Another method of preparing it is to mix cadmium chloride and ammonium fluoride solutions, followed by crystallization. The insoluble cadmium fluoride is filtered from solution.[5] Cadmium fluoride has also been prepared by reacting fluorine with cadmium sulfide. This reaction happens very quickly and forms nearly pure fluoride at much lower temperatures than other reactions used.[6] UsesElectronic ConductorCdF2 can be transformed into an electronic conductor when doped with certain rare earth elements or yttrium and treated with cadmium vapor under high temperature conditions. This process creates blue crystals with varying absorption coefficients depending on the concentrations of the dopant. A proposed mechanism explains that the conductivity of these crystals can be explained by a reaction of Cd atoms with Interstitial F− ions. This creates more CdF2 molecules and releases electrons which are weakly bonded to trivalent dopant ions resulting in n-type conductivity and a hydrogenic donor level.[7] SafetyCadmium fluoride, like all cadmium compounds, is toxic and should be used with care. Cadmium fluoride can cause potential health issues if it is not handled properly. It can cause irritation to the skin and the eyes, so gloves and protective eyewear are advised. The MSDS, or Material Safety Data Sheet, also includes warnings for ingestion and inhalation. Under acidic conditions, at high temperatures, and in moist environments, hydrogen fluoride and cadmium vapors may be released into the air. Inhalation may cause irritation of the respiratory system as well as congestion, fluorosis, and even pulmonary edema in extreme cases. Cadmium fluoride also has the same potential hazards caused by cadmium and fluoride.[8] References1. ^1 2 {{PGCH|0087}} 2. ^{{cite web|url=http://www.americanelements.com/cdf.html|title=Cadmium Fluoride| accessdate=2009-06-06}} 3. ^{{cite journal |title=Fluorine Bomb Calorimetry. VII. The Heat of Formation of Cadmium Difluoride. |last=Rudzitis |first=Edgars |date=November 1963 |journal=Journal of Physical Chemistry |doi=10.1021/j100805a031 |last2=Feder |first2=Harold |last3=Hubbard |first3=Ward}} 4. ^{{cite journal|title=Knudson and Langmuir Measurements of the Sublimation Pressure of Cadmium (II) Fluoride |last=Besenbruch |first=G. |date=March 3, 1965 |journal=Journal of Physical Chemistry |doi=10.1021/j100893a505 |first2=A. S. |last2=Kana'an |first3=J. L. |last3=Margrave}} 5. ^Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}} 6. ^{{Cite journal|title = The Reaction of Fluorine with Cadmium and Some of its Binary Compounds. The Crystal Structure, Density and Melting Points of Cadmium Fluoride.|last = Haendler|first = Helmut|date = November 1951|journal = Journal of the American Chemical Society|doi = 10.1021/ja01155a064|last2 = Bernard|first2 = Walter}} 7. ^{{Cite journal|title = Electrical and Optical Properties of Rare Earth Doped Cadmium Fluoride Single Crystals|last = Weller|first = Paul|date = June 1, 1965|journal = Inorganic Chemistry|doi = 10.1021/ic50033a004}} 8. ^{{Cite web|url = http://www.msds.com/servlet/B2BDocumentDisplay?document_version_nri=5827353&manuf_nri=17573&manuf_name=&supplier_nri=17573&page_number=1&search_source=centraldb&CLIENT_session_key=A793323_tylrpwll&CLIENT_language=2|title = Cadmium Fluoride [CdF2]|date = 2011-04-01|accessdate = 2014-12-12|website = MSDS Solutions Center|publisher = Advance Research Chemicals Inc. / A.R.C.}}{{Dead link|date=November 2018 |bot=InternetArchiveBot |fix-attempted=yes }} External links
3 : Fluorides|Metal halides|Cadmium compounds |
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