| Revision as of 10:51, 16 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,074 edits Saving copy of the {{chembox}} taken from revid 472452296 of page Cadmium_fluoride for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 07:15, 22 May 2024 edit 194.191.255.17 (talk) Fix SMILES with incorrect grammar |
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{{redirect|CdF2|the airport in Canada|Teeswater (Dent Field) Aerodrome}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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{{Chembox |
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| Watchedfields = changed |
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| verifiedrevid = 442572086 |
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| verifiedrevid = 477163492 |
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| Name = Cadmium fluoride |
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| Name = Cadmium fluoride |
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| ImageFile=Fluorite-unit-cell-3D-ionic.png |
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| ImageFile = Fluorite-unit-cell-3D-ionic.png |
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| IUPACName = Cadmium fluoride |
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| OtherNames = Cadmium(II) fluoride, Cadmium difluoride |
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| IUPACName = Cadmium fluoride |
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| OtherNames = Cadmium(II) fluoride, Cadmium difluoride |
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| Section1 = {{Chembox Identifiers |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 23036 |
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| ChemSpiderID = 23036 |
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| InChI = 1/Cd.2FH/h;2*1H/q+2;;/p-2 |
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| InChI = 1/Cd.2FH/h;2*1H/q+2;;/p-2 |
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| SMILES = FF |
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| SMILES = .. |
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| InChIKey = LVEULQCPJDDSLD-NUQVWONBAG |
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| InChIKey = LVEULQCPJDDSLD-NUQVWONBAG |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = LVEULQCPJDDSLD-UHFFFAOYSA-L |
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| StdInChIKey = LVEULQCPJDDSLD-UHFFFAOYSA-L |
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| CASNo = 7790-79-6 |
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| CASNo = 7790-79-6 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| EINECS = 232-222-0 |
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| UNII = M0975E7Z8Z |
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| EINECS = 232-222-0 |
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| PubChem = 24634 |
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| PubChem1 = 71356118 |
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| PubChem1_Comment = dihydrate |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = CdF<sub>2</sub> |
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| Formula = CdF<sub>2</sub> |
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| MolarMass = 150.41 g/mol |
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| MolarMass = 150.41 g/mol |
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| Appearance = grey or white-grey crystals |
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| Appearance = grey or white-grey crystals |
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| Density = 6.33 g/cm<sup>3</sup>, solid |
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| Density = 6.33 g/cm<sup>3</sup>, solid |
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| Solubility = 4.35 g/100 mL |
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| Solubility = 4.35 g/100 mL |
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| SolubleOther = soluble in ]<br /> insoluble in ] alcohol and liquid ] |
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| SolubleOther = soluble in ]<br /> insoluble in ] alcohol and liquid ] |
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| SolubilityProduct = 0.00644<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=5–188|edition=99 |language=English}}</ref> |
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| MeltingPt = 1110 °C |
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| BoilingPt = 1748 °C |
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| MeltingPtC = 1110 |
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| MeltingPt_notes = |
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| BoilingPtC = 1748 |
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| BoilingPt_notes = |
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| MagSus = -40.6·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| CrystalStruct = ] (cubic), ] |
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| CrystalStruct = ] (cubic), ] |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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}} |
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| Section7 = {{Chembox Hazards |
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| Section4 = {{Chembox Thermochemistry |
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| HeatCapacity = |
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| ExternalMSDS = |
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| Entropy = |
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| EUClass = ]<br />]<br />Repr. Cat. 2<br />Highly toxic ('''T+''')<br />Dangerous for the environment ('''N''') |
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| DeltaHf = -167.39 ± 0.23 kcal. mole-1 at 298.15 (K, C?) |
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| EUIndex = 048-006-00-2 |
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| DeltaGf = -155.4 ± 0.3 kcal. mole-1 at 298.15 (K, C?) |
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| NFPA-H = |
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| DeltaHc = |
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| NFPA-R = |
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| RPhrases = {{R45}}, {{R46}}, {{R60}}, {{R61}}, {{R25}}, {{R26}}, {{R48/23/25}}, {{R50/53}} |
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| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}} |
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| Section8 = {{Chembox Related |
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| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| OtherAnions = ],<br/>]<br/>] |
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| NFPA-H = |
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| OtherCations = ],<br/>],<br/>] |
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| NFPA-F = |
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| NFPA-R = |
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| GHSPictograms = {{GHS06}}{{GHS08}}{{GHS09}} |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|301|330|340|350|360|372|410}} |
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| 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}} |
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| REL = Ca<ref name=PGCH>{{PGCH|0087}}</ref> |
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| PEL = TWA 0.005 mg/m<sup>3</sup> (as Cd)<ref name=PGCH/> |
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| IDLH = Ca <ref name=PGCH/> |
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}} |
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| Section8 = {{Chembox Related |
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| OtherAnions = ],<br/>]<br/>] |
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| OtherCations = ],<br/>],<br/>],<br/>],<br/>],<br/>] |
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'''Cadmium fluoride''' (CdF<sub>2</sub>) is a mostly water-insoluble source of ] 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 ].<ref>{{cite web|url=http://www.americanelements.com/cdf.html|title=Cadmium Fluoride| access-date=2009-06-06}}</ref> The standard enthalpy has been found to be -167.39 kcal. mole<sup>−1</sup> and the Gibbs energy of formation has been found to be -155.4 kcal. mole<sup>−1</sup>, and the heat of sublimation was determined to be 76 kcal. mole<sup>−1</sup>.<ref>{{cite journal |title=Fluorine Bomb Calorimetry. VII. The Heat of Formation of Cadmium Difluoride. |last1=Rudzitis |first1=Edgars |date=November 1963 |journal=Journal of Physical Chemistry |doi=10.1021/j100805a031 |last2=Feder |first2=Harold |last3=Hubbard |first3=Ward|volume=67 |issue=11 |pages=2388–2390 }}</ref><ref>{{cite journal|title=Knudson and Langmuir Measurements of the Sublimation Pressure of Cadmium (II) Fluoride |last1=Besenbruch |first1=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|volume=69 |issue=9 |pages=3174–3176 }}</ref> |
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==Preparation== |
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Cadmium fluoride is prepared by the reaction of gaseous fluorine or ] with cadmium metal or its ]s, such as the ], ], or ]. |
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It may also be obtained by dissolving ] in 40% ] solution, evaporating the solution and drying in a vacuum at 150 °C. |
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Another method of preparing it is to mix ] and ] solutions, followed by ]. The insoluble cadmium fluoride is filtered from solution.<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> |
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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.<ref>{{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.|last1 = Haendler|first1 = Helmut|date = November 1951|journal = Journal of the American Chemical Society| volume=73|doi = 10.1021/ja01155a064|last2 = Bernard|first2 = Walter}}</ref> |
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== Uses == |
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=== Electronic conductor === |
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CdF<sub>2</sub> can be transformed into an electronic conductor when doped with certain rare earth elements or ] 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 ] F<sup>−</sup> ions. This creates more CdF<sub>2</sub> molecules and releases electrons which are weakly bonded to trivalent dopant ions resulting in n-type conductivity and a hydrogenic donor level.<ref>{{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|volume = 4|issue = 11|pages = 1545–1551|doi = 10.1021/ic50033a004}}</ref> |
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==Safety== |
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Cadmium fluoride, like all cadmium compounds, is toxic and should be used with care. |
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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 ], fluorosis, and even ] in extreme cases. Cadmium fluoride also has the same potential hazards caused by cadmium and fluoride.<ref>{{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 |date = 2011-04-01|access-date = 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 }}</ref> |
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==References== |
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<references/> |
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==External links== |
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{{Cadmium compounds}} |
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{{fluorides}} |
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] |
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] |
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] |