| Revision as of 21:14, 7 November 2011 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Script assisted update of identifiers for the Chem/Drugbox validation project (updated: 'StdInChI', 'StdInChIKey', 'CASNo').← Previous edit |
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{{Chembox |
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{{Chembox |
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| verifiedrevid = 459518162 |
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| ImageFile = Bariumferrat-2.JPG |
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| ImageFileL1 = Ba2+.svg |
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| ImageFileL1 = Ba2+.svg |
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| ImageSizeL1 = 121 |
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| ImageSizeL1 = 121 |
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| ImageNameL1 = Structural formula of barium(2+) |
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| ImageNameL1 = Structural formula of barium(2+) |
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| ImageFileR1 = Ferrate ion.svg |
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| ImageFileR1 = Ferrate ion.svg |
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| ImageSizeR1 = 121 |
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| ImageSizeR1 = 121 |
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| ImageNameR1 = Wireframe model of aromatised ferrate |
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| ImageNameR1 = Wireframe model of aromatised ferrate |
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| IUPACName = Barium ferrate(VI) |
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| IUPACName = Barium ferrate(VI) |
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| SystematicName = <!-- Barium dioxoironbis(olate) (substitutive) OR Barium tetraoxidoferrate(2-) (additive) --> |
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| SystematicName = <!-- Barium dioxoironbis(olate) (substitutive) OR Barium tetraoxidoferrate(2-) (additive) --> |
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| OtherNames = Barium ferrate(2-) |
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| OtherNames = Barium ferrate(2-) |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = <!-- blanked - oldvalue: 13773-23-4 --> |
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| CASNo = 13773-23-4 |
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| CASNo_Ref = {{cascite|changed|??}} |
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| CASNo_Ref = {{cascite|changed|??}} |
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| SMILES = .()(=O)=O |
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| ChemSpiderID = 57448624 |
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| SMILES = .()(=O)=O |
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| StdInChI = <!-- blanked - oldvalue: 1S/Ba.Fe.4O/q+2;;;;2*-1 --> |
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| StdInChI = 1S/Ba.Fe.4O/q+2;;;;2*-1 |
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| StdInChI_Ref = {{stdinchicite|correct|??}} |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChIKey = <!-- blanked - oldvalue: JFTTYFWNHKVEMY-UHFFFAOYSA-N --> |
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| StdInChIKey = JFTTYFWNHKVEMY-UHFFFAOYSA-N |
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| StdInChIKey_Ref = {{stdinchicite|correct|??}}}} |
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| StdInChIKey_Ref = {{stdinchicite|changed|??}}}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = BaFeO<sub>4</sub> |
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| Ba = 1 |
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| MolarMass = 257,1646 g/mol |
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| Fe = 1 |
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| Appearance = Dark red, opaque crystals |
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| O = 4 |
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| Solubility = insoluble}} |
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| ExactMass = 257.819841894 g mol<sup>-1</sup> |
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|Section3={{Chembox Structure |
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| Appearance = Dark red, opaque crystals}} |
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| CrystalStruct = orthorhombic |
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}} |
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| SpaceGroup = Pnma, No. 62<ref name="structure" />}}}} |
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'''Barium ferrate ''' is the ] of formula BaFeO<sub>4</sub>. This compound contains ] in the +6 ].<ref>{{cite book |
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'''Barium ferrate''' is the ] of formula BaFeO<sub>4</sub>. This is a rare compound containing ] in the +6 ].<ref>{{Cite book|title=Longman A-level course in chemistry|last=Briggs|first=J. G. R.|publisher=] South Asia|year=2005|isbn=978-981-4105-08-8|edition=4th|pages=536}}</ref> The ferrate(VI) ion has two unpaired electrons, making it ].<ref name=":0">{{Cite book|title=Inorganic chemistry|last1=Wiberg|first1=Egon|authorlink1=Egon Wiberg|last2=Wiberg|first2=Nils|last3=Holleman|first3=Arnold|publisher=]|year=2001|isbn=978-0-12-352651-9|pages=1457–1458}}</ref> It is isostructural with ], and contains the tetrahedral </nowiki>]]<sup>2−</sup> anion.<ref>{{Cite book|title=Structural inorganic chemistry|last=Wells|first=A.F.|publisher=]|year=1986|isbn=978-0-19-855370-0|edition=5th|location=Oxford }}</ref> |
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| title = Longman A-level course in chemistry |
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| author = J. G. R. Briggs |
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| edition = 4th |
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| publisher = Pearson Education South Asia |
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| year = 2005 |
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| isbn = 9814105082 |
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| page = 536 |
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}}</ref> It is isostructural with ], and contains the tetrahedral ]]<sup>2−</sup> anion.<ref> Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6 </ref> |
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==Structure== |
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==Preparation and chemistry== |
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The ] anion is paramagnetic due to its two ]s and it has a ].<ref name=":0" /> |
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Anhydrous barium ferrate can be prepared by precipitation from a solution containing ] and ].<ref>Preparation and Analysis of Barium Ferrate(VI) J. R. Gump, W. F. Wagner, and J. M. Scheyer Analytical chemistry. (1954), 26, 12, 1957 ; {{doi|10.1021/ac60096a027}}</ref> Barium ferrate is an ] and has been proposed as an oxidising reagent for use in organic syntheses.<ref>Barium Ferrate Monohydrate BaFeO<sub>4</sub>.H<sub>2</sub>O, A Versatile Reagent for the Oxidation of Organic Compounds under Aprotic Conditions, H. Firouzabadi D. Mohajer M. Entezari-moghaddam Synthetic Communications, 16, 6 1986 ,723 - 731, {{doi|10.1080/00397918608057745}}</ref> |
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] has been used to determine the orthorhombic unit cell structure<ref name="structure">{{Cite journal|last1=Ni|first1=Xiao-Min|last2=Ji|first2=Ming-Rong|last3=Yang|first3=Zhi-Ping|last4=Zheng|first4=Hua-Gui|year=2004|title=Preparation and structure characterization of nanocrystalline BaFeO<sub>4</sub>|journal=]|volume=261|issue=1|pages=82–86|doi=10.1016/j.jcrysgro.2003.09.024|bibcode=2004JCrGr.261...82N }}</ref> (lattice vectors a ≠ b ≠ c, interaxial angles α=β=γ=90°)<ref>{{Cite web|url=http://www.iucr.org/education/pamphlets/13/full-text|title=IUCr|website=www.iucr.org|access-date=2016-04-29}}</ref> of nanocrystalline BaFeO<sub>4</sub>. It crystallized in the Pnma ] (point group: D<sub>2h</sub>) with lattice parameters ''a'' = 0.8880 nm, ''b'' = 0.5512 nm and ''c'' = 0.7214 nm.<ref name="structure" /> The accuracy of the X-Ray diffraction data has been verified by the lattice fringe intervals from ] (HRTEM) and cell parameters calculated from ] (SAED).<ref name="structure" /> |
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==References== |
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=== Characterization === |
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{{Reflist}} |
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] absorbance peaks of barium ferrate are observed at 870, 812, 780 cm<sup>−1</sup>.<ref name=":2">{{Cite journal|last1=Henry-Chase|first1=Adonica|last2=Bhushan Tewari|first2=Brij|year=2013|title=Use to Ferrate (VI) A Green Chemical for the Environment Remediation|url=http://www.bolivianchemistryjournal.org/QUIMICA%202013%20PDF/3_Environmental_remediation.pdf|journal=]|volume=30|issue=1|pages=13–23|issn=0250-5460}}</ref> |
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]|volume=109|issue=1 |pages=67–70|doi=10.1016/s0378-7753(02)00041-1|bibcode=2002JPS...109...67L }}</ref>]] |
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BaFeO<sub>4</sub> follows the ] and has a ] of (2.92 ± 0.03) × 10<sup>−23</sup> A m<sup>2</sup> (3.45 ± 0.1 ]) with a ] of −89 K.<ref>{{Cite journal|last1=Audette|first1=R. J.|last2=Quail|first2=J. W.|title=Potassium, rubidium, cesium, and barium ferrates(VI). Preparations, infrared spectra, and magnetic susceptibilities|journal=]|volume=11|issue=8|pages=1904–1908|doi=10.1021/ic50114a034|year=1972}}</ref> |
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{{Inorganic-compound-stub}} |
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== Preparation and chemistry == |
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Barium ferrate(VI) can be prepared by both wet and dry synthetic methods. Dry synthesis is usually performed using a thermal technique,<ref name=":2" /> such as by heating ] and ] in the presence of ] to about 800 to 900 °C.<ref>{{cite book|title = Textbook of Coordination Chemistry|first = R. K.|last = Sharma|publisher = ]|location = New Delhi|year = 2007|isbn = 9788183562232|page = 124|chapter-url = https://books.google.com/books?id=YpRvQd_7dgwC&pg=PA124|chapter = Stabilisation of Fe (VI)}}</ref> |
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:{{chem|Ba(OH)|2}} + {{chem|Fe(OH)|2}} + {{chem|O|2}} → {{chem|BaFeO|4}} + 2 {{chem|H|2|O}} |
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<!-- Note that the Sharma text book describes this as a reaction of barium hexahydroxoferrate, Ba32, but gets the formula and stoichiometry of the reaction wrong. The solid state chemistry can be taken as 6Ba(OH)2 + 4Fe(OH)3 + 2Fe(OH)2 + 5O2 → 6BaFeO4 + 14H2O, but the above is a simpler version --> |
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Wet methods employ both chemical and electrochemical techniques. For example, the ferrate anion forms when a suitable iron ] is placed in ] and a strong ], such as ], is added.<ref name = Wulfsberg>{{cite book|title = Principles of Descriptive Inorganic Chemistry|first = Gary|last = Wulfsberg|publisher = ]|location = Sausalito, CA|year = 1991|isbn = 9780935702668|pages = 142–143|chapter-url = https://books.google.com/books?id=JoNUVLrNg14C&pg=PA142|chapter = pH and the stability of high oxidation states; Syntheses of oxo anions and their use as oxidizing agents}}</ref> |
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:2 {{chem|Fe(OH)|3}} + 3 {{chem|OCl|-}} + 4 {{chem|OH|-}} → 2 {{chem|FeO|4|2-}} + 5 {{chem|H|2|O}} + 3 {{chem|Cl|-}} |
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Barium ferrate is then precipitated from solution by adding a solution of a ] salt.<ref name = Wulfsberg /> Addition of a soluble barium salt to an alkali metal ferrate solution produces a maroon precipitate of barium ferrate, a crystal which has the same structure as ] and has approximately the same solubility.<ref name = Gump /> Barium ferrate has also been prepared by adding ] to a mixture sodium hypochlorite and ] at room temperature (or 0 °C).<ref>{{Cite journal|last1=Herber|first1=Rolfe H.|last2=Johnson|first2=David|title=Lattice dynamics and hyperfine interactions in M<sub>2</sub>FeO<sub>4</sub> (M = K<sup>+</sup>, Rb<sup>+</sup>, Cs<sup>+</sup>) and M'FeO4 (M' = Sr<sup>2+</sup>, Ba<sup>2+</sup>)|journal=]|volume=18|issue=10|pages=2786–2790|doi=10.1021/ic50200a030|year=1979}}</ref> The purity of the product can be improved by carrying out the reaction at low temperature in the absence of carbon dioxide and by rapidly filtering and drying the precipitate, reducing the coprecipitation of ] and ] as impurities.<ref name = Gump>{{Cite journal|last1=Gump|first1=J. R.|last2=Wagner|first2=W. F.|last3=Schreyer|first3=J. M.|year=1954|title=Preparation and analysis of barium ferrate(VI)|journal=]|volume=26|issue=12|pages=1957|doi=10.1021/ac60096a027|issn=0003-2700}}</ref> |
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== Uses == |
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Barium ferrate is an ] and is used as an oxidizing reagent in organic syntheses. Its other applications include removal of color, removal of cyanide, killing bacteria and contaminated and waste water treatment.<ref name=":2" /> |
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Salts of ferrate(VI) are energetic cathode materials in "super-iron" batteries. Cathodes containing ferrate(VI) compounds are referred to as "super-iron" cathodes due to their highly oxidized iron basis, multiple electron transfer, and high intrinsic energy. Among all ferrate(VI) salts, barium ferrate sustains unusually facile charge transfer, which is important for the high power domain of ].<ref name=":3" /> |
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== Reactions == |
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Barium ferrate is the most stable of the ferrate(VI) compounds. It can be prepared in its purest state and has the most definite composition. Barium ferrate can be easily decomposed by all soluble acids, including carbonic acid. If carbon dioxide is passed through water on which hydrated barium ferrate is suspended, barium ferrate will decompose completely to form ], ferric hydroxide and oxygen gas. Alkaline sulfates decompose barium ferrate that has not been dried, forming barium sulfate, ferric hydroxide and oxygen gas. |
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== See also == |
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* ] |
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* ] |
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* ] |
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==References== |
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{{Reflist}} |
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{{Barium compounds}} |
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{{Barium compounds}} |
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{{iron compounds}} |
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