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{{chembox |
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{{chembox |
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| verifiedrevid = 261672669 |
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| verifiedrevid = 409205963 |
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| ImageFile = Bromid olovnatý.PNG |
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| ImageFile = Bromid olovnatý.PNG |
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| ImageSize = |
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| ImageSize = |
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| ImageName = Lead(II) bromide |
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| ImageName = Lead(II) bromide |
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| ImageFile2 = Lead(II)-bromide-xtal-3x3x3-3D-sf.png |
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| IUPACName = Lead(II) bromide |
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| IUPACName = Lead(II) bromide |
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| OtherNames = Lead dibromide |
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| OtherNames = Lead dibromide |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = 10031-22-8 |
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| CASNo = 10031-22-8 |
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| CASNo_Ref = {{cascite}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = |
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| EINECS = 233-084-4 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = 1O767M99U7 |
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| PubChem = 24831 |
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| ChemSpiderID = 23216 |
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| SMILES = BrBr |
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| StdInChI = 1S/2BrH.Pb/h2*1H;/q;;+2/p-2 |
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| StdInChIKey = ZASWJUOMEGBQCQ-UHFFFAOYSA-L |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = PbBr<sub>2</sub> |
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| Formula = PbBr<sub>2</sub> |
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| MolarMass = 367.01 g/mol |
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| MolarMass = 367.01 g/mol |
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| Appearance = white powder |
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| Appearance = white powder |
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| Density = 6.66 g/cm<sup>3</sup> <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> |
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| Density = 6.66 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref> |
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| MeltingPt = 373 °C |
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| MeltingPtC = 370.6 |
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| BoilingPt = 916 °C (vaporizes) |
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| BoilingPtC = 916 |
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| BoilingPt_notes = (vaporizes) |
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| Solubility = 0.455 g/100 mL (0 °C) <br> 0.844 g/100 mL (20 °C) <br> 4.41 g/100 mL (100 °C) |
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| Solubility = 0.455 g/100 mL (0 °C) <br> 0.973 g/100 mL (20 °C)<ref></ref> <br> 4.41 g/100 mL (100 °C) |
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| SolubilityProduct = 6.60 x 10<sup>-6</sup> |
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| SolubilityProduct = 1.86 x 10<sup>−5</sup> (20 °C) |
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| SolubleOther = insoluble in ]; <br> soluble in ], ], ], ] |
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| SolubleOther = insoluble in ]; <br> soluble in ], ], ], ] |
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| MagSus = −90.6·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Hazards |
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| Section3 = {{Chembox Structure |
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| Structure_ref = <ref name=Lumbreras1986 /> |
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| ExternalMSDS = |
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| CrystalStruct = ] type (orthorhombic) |
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| EUClass = Repr. Cat. 1/3<br/>Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''') |
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| SpaceGroup = Pnma (No. 62) |
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| EUIndex = 082-001-00-6 |
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| NFPA-H = 3 |
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| PointGroup = |
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| LattConst_a = 805.90 pm |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| LattConst_b = 954.0 pm |
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| LattConst_c = 473.19 pm |
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| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}} |
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| LattConst_alpha = |
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| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}} |
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| LattConst_beta = |
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| LattConst_gamma = |
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| LattConst_ref = |
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| LattConst_Comment = |
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| UnitCellVolume = |
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| UnitCellFormulas = 4 |
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| Coordination = |
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| MolShape = |
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| OrbitalHybridisation = |
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| Dipole = |
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| Section8 = {{Chembox Related |
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|Section4={{Chembox Hazards |
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| ExternalSDS = |
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| OtherAnions = ],<br/>],<br/>] |
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| NFPA-H = 3 |
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| OtherCations = ],<br/>]<br/>] |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}} |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|302|332|360|373|410}} |
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| PPhrases = {{P-phrases|201|202|260|261|264|270|271|273|281|301+312|304+312|304+340|308+313|312|314|330|391|405|501}} |
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|Section8={{Chembox Related |
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| OtherAnions = ],<br/>],<br/>] |
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| OtherCations = ],<br/>]<br/>] |
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'''Lead(II) bromide''' is the ] with the formula PbBr<sub>2</sub>. It is a white powder. It is produced in the burning of typical leaded gasolines.<ref name=Ullmann>Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders "Bromine Compounds" in Ullmann's Encyclopedia of Industrial Chemistry" Wiley-VCH, Weinheim, 2000.{{doi|10.1002/14356007.a04_405}}</ref> |
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'''Lead(II) bromide''' is the stable salt of ] and ]. It is typically formed by precipitation from ] by the addition of a water-soluble bromide. As a ] containing lead, it is categorized as ''probably carcinogenic to humans'' (Category 2A), by the ] (IARC). At room temperature it is a white powder. On strong heating, it melts at 367°C to form a colourless liquid that is a weak electrical conductor. The powder is weakly soluble in water (0.455g dissolves in 100g of water at 0°C). However, its solubility rises at higher temperatures and it is about ten times more soluble in boiling water. <ref>{{Greenwood&Earnshaw}}</ref> |
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==Preparation and properties== |
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==References== |
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It is typically prepared from treating solutions of lead salts (e.g., (]) with bromide salts. This process exploits its low solubility in water - only 0.455 g dissolves in 100 g of water at 0 °C. It is about ten times more soluble in boiling water.<ref>{{Greenwood&Earnshaw}}</ref> |
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{{reflist}} |
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PbBr<sub>2</sub> has the same ] as ] (]) – they are ]. In this structure, Pb<sup>2+</sup> is surrounded by nine Br<sup>−</sup> ions in a distorted ] geometry. Seven of the Pb-Br distances are shorter, in the range 2.9-3.3 Å, while two of them are longer at 3.9 Å. The coordination is therefore sometimes described as (7+2).<ref>{{Greenwood&Earnshaw|pages=382}}</ref><ref name=Lumbreras1986>{{ cite journal | title = Structure and ionic conductivity of mixed lead halides PbCl<sub>2x</sub>Br<sub>2(1−x)</sub>. II | first1 = M. | last1 = Lumbreras | first2 = J. | last2 = Protas | first3 = S. | last3 = Jebbari | first4 = G. J. | last4 = Dirksen | first5 = J. | last5 = Schoonman | journal = ] | volume = 20 | issue = 4 | year = 1986 | pages = 295–304 | doi = 10.1016/0167-2738(86)90049-4 }}</ref> |
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{{Lead compounds}} |
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Lead bromide was prevalent in the environment as the result of the use of leaded gasoline. ] was once widely used to improve the combustion properties of gasoline. To prevent the resulting lead oxides from fouling the engine, gasoline was treated with ], which converted lead oxides into the more volatile lead bromide, which was then exhausted from the engine into the environment.<ref name=Ullmann/> |
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==Safety== |
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Like other compounds containing lead, lead(II) bromide is categorized as ''probably carcinogenic to humans'' (Category 2A), by the ] (IARC). Its release into the environment as a product of leaded gasoline was highly controversial. |
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==References== |
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{{Lead compounds}} |
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{{bromine compounds}} |
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{{bromides}} |
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