Lead(II) chloride: Difference between revisions

| verifiedrevid = 443915937

| Name = Lead(II) chloride

| ImageFile = Lead(II) chloride.jpg

| ImageFile1 = Kristallstruktur Blei(II)-chlorid.png

| ImageName = Lead(II) chloride

| IUPACName = Lead(II) chloride<br/>Lead dichloride

| OtherNames = Plumbous chloride<br/>[[Cotunnite]]

| Section1 = {{Chembox Identifiers

| CASNo_Ref = {{cascite}}

| Section2 = {{Chembox Properties

| MolarMass = 278.10 g/mol

| Density = 5.85 g/cm³

| Solubility = 6.73 g/L (0 °C) <br> 9.9 g/L (20 °C) <br> 33.4 g/L (100 °C)

| SolubilityProduct = 1.7{{e|-5}}

| SolubleOther = slightly soluble in dilute [[hydrochloric acid|HCl]], [[ammonia]]; <br> insoluble in [[alcohol]]

| MeltingPt = 501 °C

| BoilingPt = 950 °C

| RefractIndex = 2.199<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>

| Section3 = {{Chembox Structure

| SpaceGroup = Pnma, No. 62

| Section4 = {{Chembox Thermochemistry

| DeltaHf = -359.41 kJ/mol

| Entropy = 135.98 J&thinsp;K⁻¹&thinsp;mol⁻¹

| Section7 = {{Chembox Hazards

| EUClass = Repr. Cat. 1/3<br/>Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''')

| EUIndex = 082-001-00-6

| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}}

| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}

| Section8 = {{Chembox Related

| OtherCpds = [[Thallium(I) chloride]]<br/>[[Bismuth chloride]]

In solid PbCl₂, each lead ion is coordinated by 9 chloride ions – 6 lie at the apices of a trigonal prism and 3 lie beyond the centers of each prism face. The 9 chloride ions are not equidistant from the central lead atom, 7 lie at 280–309 pm and 2 at 370 pm.<ref>Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications ISBN 0-19-855370-6</ref> PbCl₂ forms white orthorhombic needles.

Vaporized PbCl₂ molecules have a bent structure with the Cl-Pb-Cl angle being 98° and each Pb-Cl bond distance being 2.44 Å.<ref>{{cite journal|last1 = Hargittai|first1 = I|last2 = Tremmel|first2 = J|last3 = Vajda|first3 = E|last4 = Ishchenko|first4 = A|last5 = Ivanov|first5 = A|last6 = Ivashkevich|first6 = L|last7 = Spiridonov|first7 = V|title = Two independent gas electron diffraction investigations of the structure of plumbous chloride|journal = Journal of Molecular Structure|volume = 42|pages = 147|year = 1977|doi = 10.1016/0022-2860(77)87038-5}}</ref> Such PbCl₂ is emitted from internal combustion engines that use ethylene chloride-[[tetraethyllead]] additives for antiknock purposes.

The [[solubility]] of PbCl₂ in water is low (9.9 g/L at 20 °C) and for practical purposes it is considered insoluble. Its [[solubility product constant]] (K_sp) is 1.7{{e|-5|}}. It is one of only four commonly insoluble chlorides, the other three being [[silver chloride]] (AgCl) with K_sp = 1.8{{e|−10}}, [[copper(I) chloride]] (CuCl) with K_sp = 1.72{{e|−7}} and [[mercury(I) chloride]] (Hg₂Cl₂) with K_sp = 1.3{{e|−18}}.<ref>CRC Handbook of Chemistry and Physics, 79th Edition, David R. Lide (Ed), p. 8-108</ref><ref>Brown, Lemay, Burnsten. "Chemistry The Central Science". ''Solubility-Product Constants for Compounds at 25 °C.'' (ed 6, 1994). p. 1017</ref>

==Occurrence==

[[File:Cotunnite-3D-balls.png|thumb|left|[[Crystal structure]] of cotunnite, PbCl₂]]

PbCl₂ occurs naturally in the form of the mineral [[cotunnite]]. It is colorless, white, yellow, or green with a density of 5.3–5.8 g/cm³. The hardness on the [[Mohs hardness|Mohs scale]] is 1.5–2. The crystal structure is orthorhombic dipyramidal and the point group is 2/m 2/m 2/m. Each Pb has a coordination number of 9. The composition is 74.50% Pb and 25.50% Cl. Cotunnite occurs near volcanoes: [[Mount Vesuvius|Vesuvius]], Italy; Tarapacá, Chile; and [[Tolbachik]], Russia.<ref>[http://webmineral.com/data/Cotunnite.shtml Cotunnite]</ref><!--

It would be helpful if a geologist looked at that page because the terms are foreign to me--><!--

also, conflicting data w/ the following page (i.e.: hardness): http://rruff.geo.arizona.edu/doclib/hom/cotunnite.pdf-->

<br clear = left/>

Lead(II) chloride [[precipitate]]s from solution upon addition of [[chloride]] sources (HCl, NaCl, KCl) to aqueous solutions of [[lead]](II) compounds such as [[lead(II) nitrate|Pb(NO₃)₂]].

:Pb(NO₃)_2(aq) + 2 [[Sodium chloride|NaCl]]_(aq) → PbCl_2(s) + 2 [[Sodium nitrate|NaNO₃]]_(aq)

:[[Lead(II) acetate|Pb(CH₃COO)₂]]_(aq) + [[Hydrochloric acid|HCl]]_(aq) → PbCl_2(s) + 2 [[Acetic acid|CH₃COOH]]_(aq)

:basic [[Lead(II) carbonate|PbCO₃]] + 2 HCl_(aq) → PbCl_2(s) + CO_2(g) + H₂O<ref name="chemnetbase.com">Dictionary of Inorganic and Organometallic Compounds. ''Lead(II) Chloride.'' [http://www.chemnetbase.com]</ref>

:Pb(NO₃)_2(aq) + 2 HCl_(aq) → PbCl_2(s) + 2 HNO_3(aq)

Treatment of lead dioxide with hydrochloric acid gives lead(II) chloride as well as chlorine gas:

:[[Lead dioxide|PbO_2]](s) + 4 HCl → PbCl_2(s) + [[Chlorine|Cl₂]] + 2 H₂O

Treatment of lead oxide with hydrochloric acid gives lead(II) chloride as well as water

:[[Lead oxide|PbO_]](s) + 2 HCl → PbCl_2(s) + H₂O

PbCl_2(s) also forms by the action of [[chlorine]] gas on lead metal:

:[[Lead|Pb]] + Cl₂ → PbCl₂

:PbCl_2(s) + [[Chloride|Cl^-]] → [PbCl₃]^-_(aq)

:PbCl_2(s) + 2 Cl^- → [PbCl₄]^2-_(aq)

PbCl₂ reacts with molten [[sodium nitrite|NaNO₂]] to give PbO:

Lead(II) chloride is the main [[wiktionary:Precursor|precursor]] for [[organometallic]] derivatives of lead, such as [[plumbocene]]s.<ref>{{cite journal|last1 = Lowack|first1 = R|doi = 10.1016/0022-328X(94)84136-5|title = Decasubstituted decaphenylmetallocenes|year = 1994|pages = 25|volume = 476|journal = [[J. Organomet. Chem.]]}}</ref> The usual alkylating agents are employed, including [[Grignard reagent]]s and organolithium compounds:

*Molten PbCl₂ is used in the synthesis of lead titanate (PbTiO₃) and [[barium]] lead titanate ceramics by cation replacement reactions:<ref name=Ab>{{cite journal|last1 = Aboujalil|first1 = Almaz|last2 = Deloume|first2 = Jean-Pierre|last3 = Chassagneux|first3 = Fernand|last4 = Scharff|first4 = Jean-Pierre|last5 = Durand|first5 = Bernard|title = Molten salt synthesis of the lead titanate PbTiO3, investigation of the reactivity of various titanium and lead salts with molten alkali-metal nitrites|journal = Journal of Materials Chemistry|volume = 8|pages = 1601|year = 1998|doi = 10.1039/a800003d|issue = 7}}</ref>

:xPbCl_2(l) + BaTiO_3(s) → Ba_1-xPb_xTiO₃ + xBaCl₂

*PbCl₂ is used in production of infrared transmitting glass,<ref name="chemnetbase.com"/> and ornamental glass called [[aurene glass]]. Aurene glass has an iridescent surface formed by spraying with PbCl₂ and reheating under controlled conditions. [[Stannous chloride]] (SnCl₂) is used for the same purpose.<ref>[http://www.thestorefinder.com/glass/library/terms/termsA.html Stained Glass Terms and Definitions. ''aurene glass'']</ref>

*Pb is used in HCl service even though the PbCl₂ formed is slightly soluble in HCl. Addition of 6–25% of [[antimony]] (Sb) increases corrosion resistance.<ref>Kirk-Othmer. "Encyclopedia of Chemical Technology". (ed 4). p 913</ref>

*A basic chloride of lead, PbCl₂·Pb(OH)₂, is known as Pattinson's white lead and is used as pigment in white paint.<ref>Perry & Phillips. "Handbook of Inorganic Compounds". (1995). p 213</ref>

*PbCl₂ is an intermediate in refining [[bismuth]] (Bi) ore. The ore containing Bi, Pb, and Zn is first treated with molten [[caustic soda]] to remove traces of acidic elements such as [[arsenic]] and [[tellurium]]. This is followed by the Parkes desilverization process to remove any silver and gold present. The ore now contains Bi, Pb, and Zn. It is treated with Cl₂ gas at 500 °C. ZnCl₂ forms first and is removed. Then PbCl₂ forms and is removed leaving pure Bi. BiCl₂ would form last.<ref>Kirk-Othmer. "Encyclopedia of Chemical Technology". (ed 4). p 241</ref>

Like other lead containing compounds, exposure to PbCl₂ may cause [[lead poisoning]].

*[http://www-cie.iarc.fr/htdocs/monographs/suppl7/leadandleadcompounds.html IARC Monograph: "Lead and Lead Compounds"]

*[http://www-cie.iarc.fr/htdocs/announcements/vol87.htm IARC Monograph: "Inorganic and Organic Lead Compounds"]

*[http://www.npi.gov.au/database/substance-info/profiles/50.html National Pollutant Inventory – Lead and Lead Compounds Fact Sheet]

*[http://www.atsdr.cdc.gov/HEC/CSEM/lead/ Case Studies in Environmental Medicine – Lead Toxicity]

*[http://www.atsdr.cdc.gov/tfacts13.html ToxFAQs: Lead]

[[Category:Lead compounds]]

[[cs:Chlorid olovnatý]]

[[de:Blei(II)-chlorid]]

[[it:Cloruro di piombo]]

[[nl:Lood(II)chloride]]

[[ja:塩化鉛]]

[[pl:Chlorek ołowiu(II)]]

[[pt:Cloreto de chumbo (II)]]