| Revision as of 10:59, 6 December 2010 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Script assisted update of identifiers from ChemSpider, CommonChemistry and FDA for the Chem/Drugbox validation project - Updated: InChI1->InChI StdInChI StdInChIKey.← Previous edit |
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{{chembox |
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{{Chembox |
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| verifiedrevid = 394839802 |
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| Watchedfields = changed |
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| ImageFile = Manganese(II)_chloride_tetrahydrate.jpg| |
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| verifiedrevid = 400833775 |
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| ImageSize = 200px |
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| ImageName = Manganese(II) chloride tetrahydrate |
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| ImageFile = Manganese(II)-chloride-xtal-layer-top-infinite-3D-bs-17.png |
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| ImageCaption = ] of crystal packing |
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| ImageFile1 = Cis-MnCl2(H2O)4.png |
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| ImageCaption1 = molecular structure |
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| ImageFile2 = Manganese(II)_chloride_tetrahydrate.jpg |
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| ImageCaption2 = Tetrahydrate |
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| IUPACName = Manganese(II) chloride<br/>Manganese dichloride |
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| IUPACName = Manganese(II) chloride<br/>Manganese dichloride |
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| OtherNames = Manganous chloride |
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| OtherNames = Manganous chloride<br /> |
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hyperchloride of manganese |
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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 = 22888 |
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| ChemSpiderID = 22888 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| ChEMBL_Ref = {{ebicite|changed|EBI}} |
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| UNII = 6YB4901Y90 |
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| ChEMBL = 1200693 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| InChIKey = GLFNIEUTAYBVOC-NUQVWONBAP |
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| UNII = 6YB4901Y90 |
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| InChI = 1/2ClH.Mn/h2*1H;/q;;+2/p-2 |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| SMILES = ClCl |
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| UNII1 = QQE170PANO |
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| StdInChI = 1S/2ClH.Mn/h2*1H;/q;;+2/p-2 |
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| UNII1_Comment = (tetrahydrate) |
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| InChIKey = GLFNIEUTAYBVOC-NUQVWONBAP |
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| InChI = 1S/2ClH.Mn/h2*1H;/q;;+2/p-2 |
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| SMILES = .. |
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| SMILES_Comment = anhydrous |
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| SMILES1 = Cl()(Cl)()() |
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| SMILES1_Comment = tetrahydrate |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/2ClH.Mn/h2*1H;/q;;+2/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = GLFNIEUTAYBVOC-UHFFFAOYSA-L |
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| StdInChIKey = GLFNIEUTAYBVOC-UHFFFAOYSA-L |
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| InChIKey1 = GLFNIEUTAYBVOC-UHFFFAOYSA-L |
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| CASNo = 7773-01-5 |
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| CASNo = 7773-01-5 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo1_Ref = {{cascite|changed|??}} |
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| CASNo1 = 38639-72-4 |
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| CASNo1_Comment = (dihydrate) |
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| CASNo1 = 20603-88-7 |
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| CASNo1_Comment = (dihydrate) |
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| CASNo2_Ref = {{cascite|correct|CAS}} |
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| CASNo2 = 13446-34-9 |
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| CASNo2_Comment = (tetrahydrate) |
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| CASNo2 = 13446-34-9 |
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| CASNo2_Comment = (tetrahydrate) |
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| EINECS = |
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| EINECS = |
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| PubChem = 24480 |
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| PubChem = 24480 |
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| InChI = |
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| RTECS = OO9625000 |
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}} |
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| RTECS = OO9625000 |
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|Section2={{Chembox Properties |
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}} |
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| Section2 = {{Chembox Properties |
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| Formula = MnCl<sub>2</sub> |
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| Formula = MnCl<sub>2</sub> |
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| MolarMass = 125.844 g/mol (anhydrous)<br/>161.874 g/mol (dihydrate)<br/>197.91 g/mol (tetrahydrate) |
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| MolarMass = 125.844 g/mol (anhydrous)<br/>161.874 g/mol (dihydrate)<br/>197.91 g/mol (tetrahydrate) |
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| Appearance = pink solid (tetrahydrate) |
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| Appearance = pink solid (tetrahydrate) |
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| Density = 2.98 g/cm<sup>3</sup> (anhydrous) <br> 2.27 g/cm<sup>3</sup> (dihydrate) <br> 2.01 g/cm<sup>3</sup> (tetrahydrate) |
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| Density = 2.977 g/cm<sup>3</sup> (anhydrous) <br> 2.27 g/cm<sup>3</sup> (dihydrate) <br> 2.01 g/cm<sup>3</sup> (tetrahydrate) |
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| MeltingPtC = 654 |
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| MeltingPt = 654 °C (anhydrous) <br> 135 °C (dihydrate) <br> 58 °C (tetrahydrate) |
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| MeltingPt_notes = (anhydrous) <br> dihydrate ] at 135 °C <br> tetrahydrate dehydrates at 58 °C |
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| Melting_notes = |
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| BoilingPt = 1225 °C |
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| BoilingPtC = 1225 |
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| Boiling_notes = |
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| BoilingPt_notes = |
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| Solubility = high<!--72.3 g/100mL (anhydrate) <br> 12.0 g/100mL (dihydrate) <br> 19.8 g/100mL (tetrahydrate)--> |
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| Solubility = 63.4 g/100 ml (0 °C) <br> 73.9 g/100 ml (20 °C) <br> 88.5 g/100 ml (40 °C) <br> 123.8 g/100 ml (100 °C) |
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| SolubleOther = slightly soluble in ], soluble in ] <br> insoluble in ] |
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| SolubleOther = |
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| Solvent = |
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| Solvent = |
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| pKa = |
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| pKa = |
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| pKb = |
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| pKb = |
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| MagSus = +14,350·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = ] |
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| CrystalStruct = ] |
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| Coordination = ] |
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| Coordination = ] |
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| MolShape = |
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| MolShape = |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| EUIndex = Not listed |
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| MainHazards = |
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| MainHazards = |
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| NFPA-H = 2 |
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| NFPA-H = 2 |
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| NFPA-F = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-R = 0 |
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| NFPA-O = |
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| NFPA-S = |
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| RPhrases = |
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| SPhrases = |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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| PEL = |
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| PEL = |
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| LD50 = 250-275 mg/kg (rat, oral){{citation needed|date=July 2015}}<br/>1715 mg/kg (mouse, oral)<ref>{{IDLH|7439965|Manganese compounds (as Mn)}}</ref> |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = ]<br/>]<br/>] |
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| OtherAnions = ]<br/>]<br/>] |
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| OtherCations = ]<br/>]<br/>]<br/>]<br/>]<br/>] |
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| OtherCations = ]<br/>]<br/>]<br/>]<br/>]<br/>] |
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| OtherFunctn = |
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| OtherFunction = |
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| Function = |
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| OtherCpds = ]<br/>] |
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| OtherCompounds = ]<br/>] |
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'''Manganese(II) chloride''' describes a series of compounds with the formula ]]<sub>2</sub>(H<sub>2</sub>O)<sub>x</sub>, where the value of x can be 0, 2, or 4. The ] is the most common form of "manganese(II) chloride". MnCl<sub>2</sub>·4H<sub>2</sub>O, but the anhydrous form and dihydrate MnCl<sub>2</sub>·2H<sub>2</sub>O are also known. Like many Mn(II) species, these salts are pink, the paleness of the color being characteristic of transition metal complexes with ] d<sup>5</sup> configurations.<ref>N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.</ref> |
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'''Manganese(II) chloride''' is the di] salt of ], MnCl<sub>2</sub>. This ] exists in the ] form, as well as the di] (MnCl<sub>2</sub>·2H<sub>2</sub>O) and tetrahydrate (MnCl<sub>2</sub>·4H<sub>2</sub>O), with the tetrahydrate being the most common form. Like many Mn(II) species, these salts are pink, with the paleness of the color being characteristic of transition metal complexes with ] d<sup>5</sup> configurations.<ref>N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.</ref> |
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==Preparation== |
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==Preparation== |
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Manganese chloride is produced by treating ] with concentrated hydrochloric acid. |
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Manganese chloride is produced by treating ] with concentrated hydrochloric acid. |
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:MnO<sub>2</sub> + 4 HCl → MnCl<sub>2</sub> + 2 H<sub>2</sub>O + Cl<sub>2</sub> |
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:MnO<sub>2</sub> + 4 HCl → MnCl<sub>2</sub> + 2 H<sub>2</sub>O + Cl<sub>2</sub> |
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This reaction was once used for the manufacture of ]. By carefully neutralizing the resulting solution with MnCO<sub>3</sub>, one can selectively precipitate iron salts, which are common impurities in manganese dioxide.<ref name=Ullmann>{{citation | first = Arno H. | last = Reidies | contribution = Manganese Compounds | title = Ullmann's Encyclopedia of Industrial Chemistry | publisher = Wiley-VCH | location = Weinheim | year = 2002 | doi = 10.1002/14356007.a16_123 | isbn = 3-527-30385-5}}.</ref> |
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In the 19th century this reaction ] for the manufacture of ]. By carefully neutralizing the resulting solution with MnCO<sub>3</sub>, one can selectively precipitate iron salts, which are common impurities in manganese dioxide.<ref name=Ullmann>{{citation | first = Arno H. | last = Reidies | contribution = Manganese Compounds | title = Ullmann's Encyclopedia of Industrial Chemistry | publisher = Wiley-VCH | location = Weinheim | year = 2002 | doi = 10.1002/14356007.a16_123 | isbn = 978-3-527-30385-4}}.</ref> |
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] |
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In the laboratory, manganese chloride can be prepared by treating ] metal or ] with ]: |
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:Mn + 2 HCl + 4 H<sub>2</sub>O → MnCl<sub>2</sub>(H<sub>2</sub>O)<sub>4</sub> + H<sub>2</sub> |
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:MnCO<sub>3</sub> + 2 HCl + 3 H<sub>2</sub>O → MnCl<sub>2</sub>(H<sub>2</sub>O)<sub>4</sub> + CO<sub>2</sub> |
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===Structures=== |
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In the laboratory, manganese chloride can be prepared by treating ] metal or ] and ]: |
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Anhydrous MnCl<sub>2</sub> adopts a layered ]-like structure. The tetrahydrate consists of octahedral '']''-Mn(H<sub>2</sub>O)<sub>4</sub>Cl<sub>2</sub> molecules. The trans isomer, which is metastable, is also known.<ref>{{cite journal|title=Crystal structure of manganese dichloride tetrahydrate|author1=Zalkin, Allan|author2=Forrester, J. D.|author3=Templeton, David H.|journal=Inorganic Chemistry|year=1964|volume=3|issue=4|pages=529–33|doi=10.1021/ic50014a017|url=http://www.escholarship.org/uc/item/7vf7p79j}}</ref><ref>A. F. Wells, ''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984.</ref> The dihydrate MnCl<sub>2</sub>(H<sub>2</sub>O)<sub>2</sub> is a ]. Each Mn center is coordinated to four doubly ]s. The octahedron is completed by a pair of mutually trans ]s.<ref>{{cite journal|title=Crystal structures of manganese(II) and iron(II) chloride dihydrate|author1=Morosin, B.|author2=Graeber, E. J.|journal=Journal of Chemical Physics|year=1965|volume=42|issue=3|pages=898–901|doi=10.1063/1.1696078|bibcode=1965JChPh..42..898M}}</ref> |
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:Mn + 2 HCl → MnCl<sub>2</sub> + H<sub>2</sub> |
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:MnCO<sub>3</sub> + 2 HCl → MnCl<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> |
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] |
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==Chemical properties== |
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==Chemical properties== |
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The hydrates dissolve in water to give mildly acidic solutions with a ] of around 4. These solutions consist of the ] <sup>2+</sup>. |
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Anhydrous MnCl<sub>2</sub> is a polymeric solid, which adopts a layered ]-like structure. The tetrahydrate consists of octahedral '']''-Mn(H<sub>2</sub>O)<sub>4</sub>Cl<sub>2</sub> molecules<ref>A. F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984.</ref> The hydrates dissolve in water to give mildly acidic solutions with a ] of around 4. |
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It is a weak ], reacting with ] ions to produce a series of solids containing the following ions <sup><nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup> , and <sup>4<nowiki>−</nowiki></sup>. Both <sup><nowiki>−</nowiki></sup> and <sup>2<nowiki>−</nowiki></sup> are ]ic. |
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It is a weak ], reacting with ] ions to produce a series of salts containing the following ions <sup><nowiki>−</nowiki></sup>, <sup>2<nowiki>−</nowiki></sup>, and <sup>4<nowiki>−</nowiki></sup>. |
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Upon treatment with typical organic ligands, manganese(II) undergoes oxidation by air to give Mn(III) ]. Examples include ])]<sup><nowiki>−</nowiki></sup>, ])<sub>6</sub>]<sup>3<nowiki>−</nowiki></sup>, and ])<sub>3</sub>]. ] forms a labile 2:1 ]: |
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Upon treatment with typical organic ligands, manganese(II) undergoes oxidation by air to give Mn(III) ]. Examples include ])]<sup><nowiki>−</nowiki></sup>, ])<sub>6</sub>]<sup>3<nowiki>−</nowiki></sup>, and ])<sub>3</sub>]. ] forms a labile 2:1 ]: |
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:MnCl<sub>2</sub> + 2 ] → |
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:MnCl<sub>2</sub> + 2 ] → |
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Anhydrous manganese(II) chloride serves as a starting point for the synthesis of a variety of manganese compounds. For example, ] is prepared by reaction of MnCl<sub>2</sub> with a solution of ] in ]. |
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Anhydrous manganese(II) chloride serves as a starting point for the synthesis of a variety of ]s. For example, ] is prepared by reaction of MnCl<sub>2</sub> with a solution of ] in ] (THF). |
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:MnCl<sub>2</sub> + 2 NaC<sub>5</sub>H<sub>5</sub> → Mn(C<sub>5</sub>H<sub>5</sub>)<sub>2</sub> + 2 NaCl |
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:MnCl<sub>2</sub> + 2 NaC<sub>5</sub>H<sub>5</sub> → Mn(C<sub>5</sub>H<sub>5</sub>)<sub>2</sub> + 2 NaCl |
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Similar reactions are used in the preparation of the antiknock compound ].<ref name=Ullmann/> |
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Manganese chloride is a precursor to organomanganese reagents in organic chemistry.<ref>{{cite journal |doi=10.15227/orgsyn.076.0239|title=Regioselective Monoalkylation of Ketones Via Their Manganese Enolates: 2-Benzyl-6-Methylcyclohexanone from 2-Methylcyclohexanone |journal=Organic Syntheses |year=1999 |volume=76 |page=239|author=Gérard Cahiez, François Chau, Bernard Blanchot }}</ref><ref>{{cite journal |doi=10.15227/orgsyn.072.0135|title=Manganese-Copper-Catalyzed Conjugate Addition of Organomagnesium Reagents to a,b-Ethylenic Ketones\: 2-(1,1-Dimethylpentyl)-5-methyl-cyclohexanone from Pulegone |journal=Organic Syntheses |year=1995 |volume=72 |page=135|author=S. Marquais, M. Alami, and G. Cahiez }}</ref> |
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Manganese chloride is mainly used in the production of dry cell batteries. |
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==Applications== |
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===Magnetism=== |
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Manganese(II) salts are paramagnetic. As such the presence of such salts profoundly affect ].<ref> |
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The main application is used in the production of dry cell batteries. It is the precursor to the antiknock compound ].<ref name=Ullmann/> |
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===Vesicle characterization with <sup>31</sup>P-NMR=== |
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MnCl<sub>2</sub> is used in ] to determine the size and ] of ] ].<ref> |
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{{Citation |
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{{Citation |
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| last = Frohlich |
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| last1 = Frohlich |
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| first = Margret |
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| first1 = Margret |
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| last2 = Brecht |
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| last2 = Brecht |
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| first2 = Volker |
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| first2 = Volker |
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| last3 = Peschka-Suss |
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| last3 = Peschka-Suss |
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| first3 = Regine |
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| first3 = Regine |
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| title = Parameters influencing the determination of liposome lamellarity by <sup>31P</sup>-NMR |
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| title = Parameters influencing the determination of liposome lamellarity by <sup>31P</sup>-NMR |
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| journal = Chemistry and Physics of Lipids |
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| journal = Chemistry and Physics of Lipids |
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| volume = 109 |
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| volume = 109 |
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| issue = 1 |
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| issue = 1 |
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| pages = 103-112 |
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| pages = 103–112 |
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| date = January 2001 |
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| date = January 2001 |
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| doi = 10.1016/S0009-3084(00)00220-6 |
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| year = 2001 |
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| month = January |
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| pmid = 11163348 |
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| url = http://www.sciencedirect.com/science?_ob=ArticleURL&_udi=B6T2N-423J9WK-9&_user=10&_coverDate=01/31/2001&_rdoc=1&_fmt=high&_orig=search&_origin=search&_sort=d&_docanchor=&view=c&_searchStrId=1527591417&_rerunOrigin=google&_acct=C000050221&_version=1&_urlVersion=0&_userid=10&md5=7433836d10ceaa1aee850a98fefa62dd&searchtype=a |
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}} |
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</ref> When manganese chloride is added to a vesicular solution, Mn<sup>2+</sup> ] ] are released, perturbing the ] of the phospholipids' ] groups and ] the resulting <sup>31</sup>P ]. Only phospholipids located in the outermost ] exposed to Mn<sup>2+</sup> experience this broadening. The effect is negligle for multilamellar vesicles, but for large unilamellar vesicles, a ~50% reduction in signal intensity is observed.<ref> |
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{{Citation |
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| last = Hope |
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| last2 = Bally |
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| last3 = Webb |
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| last4 = Cullis |
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| title = Production of large unilamellar vesicles by a rapid extrusion procedure. Characterization of size distribution, trapped volume and ability to maintain a membrane potential |
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| journal = Biochimica et Biophysica Acta |
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| volume = 812 |
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| pages = 55-65 |
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| date received = April 10th, 1984 |
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| year = 1985 |
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| url = http://www.islandnet.com/~prc/PDFs/073.pdf |
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}} |
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}} |
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</ref> |
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</ref> |
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==Natural occurrence== |
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Scacchite is the natural, anhydrous form of manganese(II) chloride.<ref>{{Cite web|url=https://www.mindat.org/min-3549.html|title=Scacchite}}</ref> |
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==Precautions== |
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==Precautions== |
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], or manganese poisoning, can be caused by long-term exposure to manganese dust or fumes. |
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], or manganese poisoning, can be caused by long-term exposure to manganese dust or fumes. |
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==References== |
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==References== |
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{{reflist}} |
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<references/> |
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==External links== |
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==External links== |
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{{Commons category|Manganese(II) chloride}} |
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