Lead(II) bromide: Difference between revisions
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| ImageFile = Bromid olovnatý.PNG |
| ImageFile = Bromid olovnatý.PNG |
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| ImageSize = |
| ImageSize = |
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| ImageName = Lead(II) bromide |
| 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 |
| IUPACName = Lead(II) bromide |
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| OtherNames = Lead dibromide |
| OtherNames = Lead dibromide |
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|Section1={{Chembox Identifiers |
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| CASNo = 10031-22-8 |
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| CASNo_Ref = {{cascite}} |
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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 = Br[Pb]Br |
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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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| Formula = PbBr<sub>2</sub> |
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| MolarMass = 367.01 g/mol |
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| Appearance = white powder |
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| Density = 6.66 g/cm<sup>3</sup> <ref></ref> |
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| = 916 |
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| BoilingPt_notes = (vaporizes) |
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| Solubility = 0.455 g/100 mL (0 °C) <br> 0. g/100 mL (20 °C) <br> 4.41 g/100 mL (100 °C) |
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| SolubilityProduct = . x 10<sup></sup> |
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| SolubleOther = insoluble in [[alcohol]]; <br> soluble in [[ammonia]], [[alkali]], [[potassium bromide|KBr]], [[sodium bromide|NaBr]] |
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| MagSus = −90.6·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox |
| Section3 = {{Chembox |
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| Structure_ref = <ref name=Lumbreras1986 /> |
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| ExternalMSDS = |
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| CrystalStruct = [[Lead(II) chloride|PbCl<sub>2</sub>]] 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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| LattConst_a = 805.90 pm |
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| = 0 |
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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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| ExternalSDS = |
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| NFPA-H = 3 |
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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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'''Lead(II) bromide''' is the [[inorganic compound]] 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 [[lead]] and [[hydrobromic acid]]. It is typically formed by precipitation from [[lead(II) nitrate]] by the addition of a water-soluble bromide. As a [[chemical compound]] containing lead, it is categorized as ''probably carcinogenic to humans'' (Category 2A), by the [[International Agency for Research on Cancer]] (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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It is typically prepared from treating solutions of lead salts (e.g., ([[lead(II) nitrate]]) 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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PbBr<sub>2</sub> has the same [[crystal structure]] as [[Lead(II) chloride|lead chloride]] ([[cotunnite]]) – they are [[Isomorphism (crystallography)|isomorphous]]. In this structure, Pb<sup>2+</sup> is surrounded by nine Br<sup>−</sup> ions in a distorted [[Tricapped trigonal prismatic molecular geometry|tricapped trigonal prismatic]] 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 = [[Solid State Ionics|Solid State Ion.]] | volume = 20 | issue = 4 | year = 1986 | pages = 295–304 | doi = 10.1016/0167-2738(86)90049-4 }}</ref> |
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Lead bromide was prevalent in the environment as the result of the use of leaded gasoline. [[Tetraethyl lead]] 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 [[1,2-Dibromoethane]], 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 [[International Agency for Research on Cancer]] (IARC). Its release into the environment as a product of leaded gasoline was highly controversial. |
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{{inorganic-compound-stub}} |
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{{bromine compounds}} |
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{{bromides}} |
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[[ |
[[:(II)]] |
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[[el:Βρωμιούχος μόλυβδος]] |
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[[it:Bromuro di piombo]] |
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[[ja:臭化鉛(II)]] |
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[[simple:Lead(II) bromide]] |