Lead(II) chloride: Difference between revisions

Lead(II) chloride
	; The crystal structure of PbCl2, in the unconventional crystallographic setting Pnam. This corresponds to the standard Pnma setting by switching the labels on the b and c axes.
Names
	IUPAC names Lead(II) chloride; Lead dichloride
	Other names Plumbous chloride; Cotunnite; Dichloroplumbylene
Identifiers
CAS Number	7758-95-4 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:88212 ;
ChemSpider	22867 ;
ECHA InfoCard	100.028.950
EC Number	231-845-5;
PubChem CID	166945;
UNII	4IL61GN3YI ;
CompTox Dashboard (EPA)	DTXSID1041059 ;
	InChI InChI=1S/2ClH.Pb/h2*1H;/q;;+2/p-2 Key: HWSZZLVAJGOAAY-UHFFFAOYSA-L ;
	SMILES Cl[Pb]Cl;
Properties
Chemical formula	PbCl2
Molar mass	278.10 g/mol
Appearance	white odorless solid
Density	5.85 g/cm3
Melting point	501 °C (934 °F; 774 K)
Boiling point	950 °C (1,740 °F; 1,220 K)
Solubility in water	0.99 g/100 mL (20 °C)
Solubility product (Ksp)	1.7×10−5 (20 °C)
Solubility	slightly soluble in dilute HCl, ammonia; ; insoluble in alcohol Soluble in hot water as well as in presence of alkali hydroxide Soluble in concentrated HCl (>6M)
Magnetic susceptibility (χ)	−73.8·10−6 cm3/mol
Refractive index (nD)	2.199
Structure
Crystal structure	Orthorhombic, oP12
Space group	Pnma (No. 62)
Lattice constant	a = 762.040 pm, b = 453.420 pm, c = 904.520 pm
Formula units (Z)	4
Thermochemistry
Std molar; entropy (S⦵298)	135.98 J K−1 mol−1
Std enthalpy of; formation (ΔfH⦵298)	-359.41 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H332, H351, H360, H372, H410
Precautionary statements	P201, P261, P273, P304+P340, P308+P313, P312, P391
NFPA 704 (fire diamond)	3 0 0
	Lethal dose or concentration (LD, LC):
LDLo (lowest published)	140 mg/kg (guinea pig, oral)
Related compounds
Other anions	Lead(II) fluoride; Lead(II) bromide; Lead(II) iodide
Other cations	Lead(IV) chloride; Tin(II) chloride; Germanium(II) chloride
Related compounds	Thallium(I) chloride; Bismuth chloride
Supplementary data page
	Lead(II) chloride (data page)
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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Lead(II) chloride (PbCl₂) is an inorganic compound which is a white solid under ambient conditions. It is poorly soluble in water. Lead(II) chloride is one of the most important lead-based reagents. It also occurs naturally in the form of the mineral cotunnite.

Structure and properties

In solid PbCl₂, each lead ion is coordinated by nine chloride ions in a tricapped triangular prism formation — six lie at the vertices of a triangular prism and three lie beyond the centers of each rectangular 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.^[6] PbCl₂ forms white orthorhombic needles.

Ball-and-stick model of part of the crystal structure of cotunnite
Space-filling model
Coordination geometry of Pb²⁺
Coordination geometry of Cl⁻
Coordination polyhedron of Pb²⁺

In the gas phase, PbCl₂ molecules have a bent structure with the Cl–Pb–Cl angle being 98° and each Pb–-Cl bond distance being 2.44 Å.^[7] Such PbCl₂ is emitted from internal combustion engines that use ethylene chloride-tetraethyllead additives for antiknock purposes.

PbCl₂ is sparingly soluble in water, solubility product K_sp = 1.7×10⁻⁵ at 20 °C. It is one of only 5 commonly water-insoluble chlorides, the other 4 being thallium(I) chloride, silver chloride (AgCl) with K_sp = 1.8×10⁻¹⁰, copper(I) chloride (CuCl) with K_sp = 1.72×10⁻⁷ and mercury(I) chloride (Hg₂Cl₂) with K_sp = 1.3×10⁻¹⁸.^[8]^[9]

Synthesis

Solid lead(II) chloride precipitates upon addition of aqueous chloride sources (HCl, NaCl, KCl) to aqueous solutions of lead(II) compounds, such as lead(II) nitrate and lead(II) acetate:

Pb(NO₃)₂ + 2 HCl → PbCl₂(s) + 2 HNO₃

It also forms by treatment of basic lead(II) compounds such as Lead(II) oxide and lead(II) carbonate.

Lead dioxide is reduced by chloride as follows:

PbO₂ + 4 HCl → PbCl₂(s) + Cl₂ + 2 H₂O

It also formed by the oxidation of lead metal by copper(II) chloride:

Pb + CuCl₂ → PbCl₂ + Cu

Or most straightforwardly by the action of chlorine gas on lead metal:

Pb + Cl₂ → PbCl₂

Reactions

Addition of chloride ions to a suspension of PbCl₂ gives rise to soluble complex ions. In these reactions the additional chloride (or other ligands) break up the chloride bridges that comprise the polymeric framework of solid PbCl_2(s).

PbCl_2(s) + Cl⁻ → [PbCl₃]⁻_(aq)

PbCl_2(s) + 2 Cl⁻ → [PbCl₄]²⁻_(aq)

PbCl₂ reacts with molten NaNO₂ to give PbO:

PbCl_2(l) + 3 NaNO₂ → PbO + NaNO₃ + 2 NO + 2 NaCl

PbCl₂ is used in synthesis of lead(IV) chloride (PbCl₄): Cl₂ is bubbled through a saturated solution of PbCl₂ in aqueous NH₄Cl forming [NH₄]₂[PbCl₆]. The latter is reacted with cold concentrated sulfuric acid (H₂SO₄) forming PbCl₄ as an oil.^[10]

Lead(II) chloride is the main precursor for organometallic derivatives of lead, such as plumbocenes.^[11] The usual alkylating agents are employed, including Grignard reagents and organolithium compounds:

2 PbCl₂ + 4 RLi → R₄Pb + 4 LiCl + Pb

2 PbCl₂ + 4 RMgBr → R₄Pb + Pb + 4 MgBrCl

3 PbCl₂ + 6 RMgBr → R₃Pb-PbR₃ + Pb + 6 MgBrCl^[12]

These reactions produce derivatives that are more similar to organosilicon compounds, i.e. that Pb(II) tends to disproportionate upon alkylation.

PbCl₂ can be used to produce PbO₂ by treating it with sodium hypochlorite (NaClO), forming a reddish-brown precipitate of PbO₂.

Uses

Molten PbCl₂ is used in the synthesis of lead titanate and barium lead titanate ceramics by cation replacement reactions:^[13]
x PbCl_2(l) + BaTiO_3(s) → Ba_1−xPb_xTiO₃ + x BaCl₂
PbCl₂ is used in production of infrared transmitting glass,^[14] 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.^[15]
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.^[16]
A basic chloride of lead, PbCl₂·Pb(OH)₂, is known as Pattinson's white lead and is used as pigment in white paint.^[17] Lead paint is now banned as a health hazard in many countries by the White Lead (Painting) Convention, 1921.
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 arsenic and tellurium. This is followed by the Parkes process to remove any silver and gold present. There are now Bi, Pb, and Zn in the ore. At 500 °C, it receives treatment from Cl2 gas. First, ZnCl2 forms and is excreted. Pure Bi is left behind after PbCl2 forms and is eliminated. Lastly, BiCl3 would form.^[18]

Toxicity

Like other soluble lead compounds, exposure to PbCl₂ may cause lead poisoning.

References

^ NIST-data review 1980 Archived 2014-02-11 at the Wayback Machine
^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
^ Sass, Ronald L.; Brackett, E. B.; Brackett, T. E. (1963). "THE CRYSTAL STRUCTURE OF LEAD CHLORIDE". The Journal of Physical Chemistry. 67 (12). American Chemical Society (ACS): 2863–2864. doi:10.1021/j100806a517. ISSN 0022-3654.
^ "Lead compounds (as Pb)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
^ "Classifications - CL Inventory". echa.europa.eu.
^ Wells A. F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
^ Hargittai, I; Tremmel, J; Vajda, E; Ishchenko, A; Ivanov, A; Ivashkevich, L; Spiridonov, V (1977). "Two independent gas electron diffraction investigations of the structure of plumbous chloride". Journal of Molecular Structure. 42: 147–151. Bibcode:1977JMoSt..42..147H. doi:10.1016/0022-2860(77)87038-5.
^ CRC Handbook of Chemistry and Physics, 79th Edition, David R. Lide (Ed), p. 8-108
^ Brown, Lemay, Burnsten. Chemistry The Central Science. "Solubility-Product Constants for Compounds at 25 °C". (ed 6, 1994). p. 1017
^ Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. p. 365. ISBN 978-0-13-039913-7.
^ Lowack, R (1994). "Decasubstituted decaphenylmetallocenes". J. Organomet. Chem. 476: 25–32. doi:10.1016/0022-328X(94)84136-5.
^ Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. p. 524. ISBN 978-0-13-039913-7.
^ Aboujalil, Almaz; Deloume, Jean-Pierre; Chassagneux, Fernand; Scharff, Jean-Pierre; Durand, Bernard (1998). "Molten salt synthesis of the lead titanate PbTiO₃, investigation of the reactivity of various titanium and lead salts with molten alkali-metal nitrites". Journal of Materials Chemistry. 8 (7): 1601. doi:10.1039/a800003d.
^ Dictionary of Inorganic and Organometallic Compounds. Lead(II) Chloride.[1]
^ Stained Glass Terms and Definitions. aurene glass
^ Kirk-Othmer. Encyclopedia of Chemical Technology. (ed 4). p 913
^ Perry & Phillips. Handbook of Inorganic Compounds. (1995). p 213
^ Kirk-Othmer. Encyclopedia of Chemical Technology. (ed 4). p. 241

External links

[1] NIST-data review 1980 Archived 2014-02-11 at the Wayback Machine

[2] Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8

[3] Sass, Ronald L.; Brackett, E. B.; Brackett, T. E. (1963). "THE CRYSTAL STRUCTURE OF LEAD CHLORIDE". The Journal of Physical Chemistry. 67 (12). American Chemical Society (ACS): 2863–2864. doi:10.1021/j100806a517. ISSN 0022-3654.

[IDLH-4] "Lead compounds (as Pb)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).

[5] "Classifications - CL Inventory". echa.europa.eu.

[6] Wells A. F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6

[7] Hargittai, I; Tremmel, J; Vajda, E; Ishchenko, A; Ivanov, A; Ivashkevich, L; Spiridonov, V (1977). "Two independent gas electron diffraction investigations of the structure of plumbous chloride". Journal of Molecular Structure. 42: 147–151. Bibcode:1977JMoSt..42..147H. doi:10.1016/0022-2860(77)87038-5.

[8] CRC Handbook of Chemistry and Physics, 79th Edition, David R. Lide (Ed), p. 8-108

[9] Brown, Lemay, Burnsten. Chemistry The Central Science. "Solubility-Product Constants for Compounds at 25 °C". (ed 6, 1994). p. 1017

[10] Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. p. 365. ISBN 978-0-13-039913-7.

[11] Lowack, R (1994). "Decasubstituted decaphenylmetallocenes". J. Organomet. Chem. 476: 25–32. doi:10.1016/0022-328X(94)84136-5.

[Housecroft_2005_p_524-12] Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. p. 524. ISBN 978-0-13-039913-7.

[Ab-13] Aboujalil, Almaz; Deloume, Jean-Pierre; Chassagneux, Fernand; Scharff, Jean-Pierre; Durand, Bernard (1998). "Molten salt synthesis of the lead titanate PbTiO₃, investigation of the reactivity of various titanium and lead salts with molten alkali-metal nitrites". Journal of Materials Chemistry. 8 (7): 1601. doi:10.1039/a800003d.

[chemnetbase.com-14] Dictionary of Inorganic and Organometallic Compounds. Lead(II) Chloride.[1]

[15] Stained Glass Terms and Definitions. aurene glass

[16] Kirk-Othmer. Encyclopedia of Chemical Technology. (ed 4). p 913

[17] Perry & Phillips. Handbook of Inorganic Compounds. (1995). p 213

[18] Kirk-Othmer. Encyclopedia of Chemical Technology. (ed 4). p. 241

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@@ Line 2: / Line 2: @@
 {{chembox
 | Verifiedfields = changed
-| Watchedfields = changed
+| Watchedfields  = changed
-| verifiedrevid = 444947478
+| verifiedrevid  = 444947478
-| Name = Lead(II) chloride
+| Name           = Lead(II) chloride
-| ImageFile = PbCl2precipiate.jpg
+| ImageFile      = Lead(II) chloride.jpg
-| ImageFile1 = Cotunnite structure.png
+| ImageFile1     = Cotunnite structure.png
+| ImageCaption1  = The crystal structure of PbCl<sub>2</sub>, in the unconventional crystallographic setting Pnam. This corresponds to the standard Pnma setting by switching the labels on the b and c axes.
-| ImageName = Lead(II) chloride precipitation
-| IUPACName = Lead(II) chloride<br/>Lead dichloride
+| ImageName      = Lead(II) chloride
-| OtherNames = Plumbous chloride<br/>[[Cotunnite]]
+| IUPACName      = Lead(II) chloride<br/>Lead dichloride
+| OtherNames     = Plumbous chloride<br/>[[Cotunnite]]<br />Dichloroplumbylene
-|Section1={{Chembox Identifiers
+| Section1       = {{Chembox Identifiers
 | CASNo_Ref = {{cascite|correct|CAS}}
 | CASNo = 7758-95-4
@@ Line 20: / Line 21: @@
 | ChEBI_Ref = {{ebicite|changed|EBI}}
 | ChEBI = 88212
+| EINECS = 231-845-5
 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
 | StdInChIKey = HWSZZLVAJGOAAY-UHFFFAOYSA-L
@@ Line 26: / Line 28: @@
 | StdInChI = 1S/2ClH.Pb/h2*1H;/q;;+2/p-2
  }}
-|Section2={{Chembox Properties
+| Section2       = {{Chembox Properties
 | Formula = PbCl<sub>2</sub>
 | MolarMass = 278.10&nbsp;g/mol
 | Appearance = white odorless solid
 | Density = 5.85&nbsp;g/cm<sup>3</sup>
-| Solubility = 10.8&nbsp;g/L (20&nbsp;°C)<ref>[https://www.nist.gov/data/PDFfiles/jpcrd166.pdf NIST-data review 1980] {{webarchive|url=https://web.archive.org/web/20140211021914/https://www.nist.gov/data/PDFfiles/jpcrd166.pdf |date=2014-02-11 }}</ref>
+| Solubility = 0.99&nbsp;g/100 mL (20&nbsp;°C)<ref>[https://www.nist.gov/data/PDFfiles/jpcrd166.pdf NIST-data review 1980] {{webarchive|url=https://web.archive.org/web/20140211021914/https://www.nist.gov/data/PDFfiles/jpcrd166.pdf |date=2014-02-11 }}</ref>
-| SolubilityProduct = 1.7×10<sup>−4</sup> (20&nbsp;°C)
+| SolubilityProduct = 1.7×10<sup>−5</sup> (20&nbsp;°C)
-| SolubleOther = slightly soluble in dilute [[hydrochloric acid|HCl]], [[ammonia]]; <br> insoluble in [[alcohol]]
+| SolubleOther = slightly soluble in dilute [[hydrochloric acid|HCl]], [[ammonia]]; <br> insoluble in [[ethanol|alcohol]]
+Soluble in hot [[water]] as well as in presence of [[alkali hydroxide]]
+Soluble in concentrated [[hydrochloric acid|HCl]] (>6M)
 | MeltingPtC = 501
 | BoilingPtC = 950
@@ Line 39: / Line 45: @@
 | MagSus = &minus;73.8·10<sup>−6</sup> cm<sup>3</sup>/mol
 }}
-|Section3={{Chembox Structure
+| Section3       = {{Chembox Structure
+| Structure_ref =<ref>{{cite journal | last=Sass | first=Ronald L. | last2=Brackett | first2=E. B. | last3=Brackett | first3=T. E. | title=THE CRYSTAL STRUCTURE OF LEAD CHLORIDE | journal=The Journal of Physical Chemistry | publisher=American Chemical Society (ACS) | volume=67 | issue=12 | year=1963 | issn=0022-3654 | doi=10.1021/j100806a517 | pages=2863–2864}}</ref>
 | CrystalStruct = [[Orthorhombic]], [[Pearson symbol|oP12]]
-| SpaceGroup = Pnma, No. 62
+| SpaceGroup = Pnma (No. 62)
+| LattConst_a = 762.040 pm
+| LattConst_b = 453.420 pm
+| LattConst_c = 904.520 pm
+| UnitCellFormulas = 4
  }}
-|Section4={{Chembox Thermochemistry
+| Section4       = {{Chembox Thermochemistry
 | DeltaHf = -359.41&nbsp;kJ/mol
-| Entropy = 135.98&nbsp;J&thinsp;K<sup>−1</sup>&thinsp;mol<sup>−1</sup>
+| Entropy = 135.98&nbsp;J{{thin space}}K<sup>−1</sup>{{thin space}}mol<sup>−1</sup>
  }}
-|Section7={{Chembox Hazards
+| Section7       = {{Chembox Hazards
-| EUClass = {{Hazchem T}}{{Hazchem Xn}}{{Hazchem N}}
 | NFPA-H = 3
 | NFPA-F = 0
 | NFPA-R = 0
+| Hazards_ref = <ref>{{cite web |title=Classifications - CL Inventory |url=https://echa.europa.eu/information-on-chemicals/cl-inventory-database/-/discli/details/10492 |website=echa.europa.eu}}</ref>
-| RPhrases = {{R61}}, {{R20/22}}, {{R33}}, {{R62}}, {{R50/53}}
-| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}}
+| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
+| GHSSignalWord = Danger
-| LDLo = 1500 mg/kg (guinea pig, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>
+| HPhrases = {{H-phrases|302|332|351|360|372|410}}
+| PPhrases = {{P-phrases|201|261|273|304+340|308+313|312|391}}
+| LDLo = 140 mg/kg (guinea pig, oral)<ref name=IDLH>{{IDLH|7439921|Lead compounds (as Pb)}}</ref>
  }}
-|Section8={{Chembox Related
+| Section8       = {{Chembox Related
 | OtherAnions = [[Lead(II) fluoride]]<br/>[[Lead(II) bromide]]<br/>[[Lead(II) iodide]]
 | OtherCations = [[Lead(IV) chloride]]<br/>[[Tin(II) chloride]]<br/>[[Germanium(II) chloride]]
@@ Line 66: / Line 79: @@
 ==Structure and properties==
-In solid PbCl<sub>2</sub>, 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&nbsp;pm and 2 at 370&nbsp;pm.<ref>Wells A. F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}</ref> PbCl<sub>2</sub> forms white orthorhombic needles. While Lead(II) chloride is abundant in many natural water reserves, it is unsafe for human consumption and must be filtered out.
+In solid PbCl<sub>2</sub>, each lead ion is coordinated by nine chloride ions in a [[Tricapped trigonal prismatic molecular geometry|tricapped triangular prism formation]] — six lie at the vertices of a triangular prism and three lie beyond the centers of each rectangular prism face. The 9 chloride ions are not equidistant from the central lead atom, 7 lie at 280–309&nbsp;pm and 2 at 370&nbsp;pm.<ref>Wells A. F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}</ref> PbCl<sub>2</sub> forms white orthorhombic needles.
+{{gallery
-Vaporized PbCl<sub>2</sub> molecules have a bent structure with the Cl-Pb-Cl angle being 98° and each Pb-Cl bond distance being 2.44&nbsp;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 PbCl<sub>2</sub> is emitted from internal combustion engines that use ethylene chloride-[[tetraethyllead]] additives for antiknock purposes.
+|File:Cotunnite-3D-balls.png|[[Ball-and-stick model]] of part of the [[crystal structure]] of cotunnite
+|File:Cotunnite-3D-ionic.png|[[Space-filling model]]
-The [[solubility]] of PbCl<sub>2</sub> in water is low (10.8&nbsp;g/L at 20&nbsp;°C) and for practical purposes it is considered insoluble. Its [[solubility product constant]] (K<sub>sp</sub>) is 1.7{{e|-4|}}. It is one of only four commonly insoluble chlorides, the other three being [[silver chloride]] (AgCl) with K<sub>sp</sub> = 1.8{{e|−10}}, [[copper(I) chloride]] (CuCl) with K<sub>sp</sub> = 1.72{{e|−7}} and [[mercury(I) chloride]] (Hg<sub>2</sub>Cl<sub>2</sub>) with K<sub>sp</sub> = 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&nbsp;°C". (ed 6, 1994). p. 1017</ref>
+|File:Cotunnite-Pb-coordination-geometry-3D-balls.png|[[Coordination geometry]] of Pb<sup>2+</sup>
+|File:Cotunnite-Cl-coordination-geometry-3D-balls.png|Coordination geometry of Cl<sup>−</sup>
+|File:Cotunnite-Pb-coordination-CM-3D-balls.png|Coordination polyhedron of Pb<sup>2+</sup>
+}}
+In the gas phase, PbCl<sub>2</sub> molecules have a bent structure with the Cl–Pb–Cl angle being 98° and each Pb–-Cl bond distance being 2.44&nbsp;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 = 147–151|year = 1977|doi = 10.1016/0022-2860(77)87038-5|bibcode = 1977JMoSt..42..147H}}</ref> Such PbCl<sub>2</sub> is emitted from internal combustion engines that use ethylene chloride-[[tetraethyllead]] additives for antiknock purposes.
-==Occurrence==
-[[File:Cotunnite-3D-balls.png|thumb|left|[[Crystal structure]] of cotunnite, PbCl<sub>2</sub>]]
-PbCl<sub>2</sub> 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/cm<sup>3</sup>. 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. Cotunnite occurs near volcanoes: [[Mount Vesuvius|Vesuvius]], Italy; [[Taapaca|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-->
+PbCl<sub>2</sub> is [[solubility|sparingly soluble]] in water, [[solubility product]] ''K''<sub>sp</sub> = {{val|1.7e-5}} at 20&nbsp;°C. It is one of only 5 commonly water-insoluble chlorides, the other 4 being [[thallium(I) chloride]], [[silver chloride]] (AgCl) with ''K''<sub>sp</sub> = {{val|1.8e-10}}, [[copper(I) chloride]] (CuCl) with ''K''<sub>sp</sub> = {{val|1.72e-7}} and [[mercury(I) chloride]] (Hg<sub>2</sub>Cl<sub>2</sub>) with ''K''<sub>sp</sub> = {{val|1.3e-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&nbsp;°C". (ed 6, 1994). p. 1017</ref>
-{{clear|left}}
 ==Synthesis==
-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(NO<sub>3</sub>)<sub>2</sub>]].
-:Pb(NO<sub>3</sub>)<sub>2(aq)</sub> + 2 [[Sodium chloride|NaCl]]<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 [[Sodium nitrate|NaNO<sub>3</sub>]]<sub>(aq)</sub>
-:[[Lead(II) acetate|Pb(CH<sub>3</sub>COO)<sub>2</sub>]]<sub>(aq)</sub> + [[Hydrochloric acid|HCl]]<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 [[Acetic acid|CH<sub>3</sub>COOH]]<sub>(aq)</sub>
-:basic [[Lead(II) carbonate|PbCO<sub>3</sub>]] + 2 HCl<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + CO<sub>2(g)</sub> + H<sub>2</sub>O<ref name="chemnetbase.com">Dictionary of Inorganic and Organometallic Compounds. ''Lead(II) Chloride.'' [http://www.chemnetbase.com]</ref>
-:Pb(NO<sub>3</sub>)<sub>2(aq)</sub> + 2 HCl<sub>(aq)</sub> → PbCl<sub>2(s)</sub> + 2 HNO<sub>3(aq)</sub>
+Solid lead(II) chloride [[precipitate]]s upon addition of aqueous [[chloride]] sources (HCl, NaCl, KCl) to aqueous solutions of [[lead]](II) compounds, such as [[lead(II) nitrate]] and [[lead(II) acetate]]:
-Treatment of lead dioxide with hydrochloric acid gives lead(II) chloride as well as chlorine gas:
-:[[Lead dioxide|PbO<sub>2]](s)</sub> + 4 HCl → PbCl<sub>2(s)</sub> + [[Chlorine|Cl<sub>2</sub>]] + 2 H<sub>2</sub>O
+:{{chem2|Pb(NO3)2  +  2 HCl  →  PbCl2(s)  + 2 HNO3}}
+It also forms by treatment of basic lead(II) compounds such as [[Lead(II) oxide]] and [[lead(II) carbonate]].
+[[Lead dioxide]] is reduced by chloride as follows:
-Treatment of lead oxide with hydrochloric acid gives lead(II) chloride as well as water
-:[[Lead(II) oxide|PbO<sub>]](s)</sub> + 2 HCl → PbCl<sub>2(s)</sub> + H<sub>2</sub>O
+:{{chem2|PbO2 + 4 HCl → PbCl2(s) + Cl2  + 2 H2O}}
-PbCl<sub>2(s)</sub> also forms by the action of [[chlorine]] gas on lead metal:
+It also  formed by the oxidation of lead metal by [[copper(II) chloride]]:
-:[[Lead|Pb]] + Cl<sub>2</sub> → PbCl<sub>2</sub>
+:{{chem2|Pb + CuCl2  →  PbCl2  +  Cu}}
+Or most straightforwardly by the action of [[chlorine]] gas on lead metal:
+:{{chem2|Pb + Cl2  →  PbCl2}}
 ==Reactions==
@@ Line 101: / Line 112: @@
 :PbCl<sub>2(s)</sub> + 2 Cl<sup>−</sup> → [PbCl<sub>4</sub>]<sup>2−</sup><sub>(aq)</sub>
-PbCl<sub>2</sub> reacts with molten [[sodium nitrite|NaNO<sub>2</sub>]] to give PbO:
+PbCl<sub>2</sub> reacts with molten [[sodium nitrite|NaNO<sub>2</sub>]] to give [[PbO]]:
 :PbCl<sub>2(l)</sub> + 3 NaNO<sub>2</sub> → PbO + NaNO<sub>3</sub> + 2 NO + 2 NaCl
 PbCl<sub>2</sub> is used in synthesis of lead(IV) chloride (PbCl<sub>4</sub>): Cl<sub>2</sub> is bubbled through a saturated solution of PbCl<sub>2</sub> in aqueous NH<sub>4</sub>Cl forming [NH<sub>4</sub>]<sub>2</sub>[PbCl<sub>6</sub>]. The latter is reacted with cold concentrated [[sulfuric acid]] (H<sub>2</sub>SO<sub>4</sub>) forming PbCl<sub>4</sub> as an oil.<ref>{{Housecroft2nd|page=365}}</ref>
-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:
+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 = 25–32|volume = 476|journal = [[J. Organomet. Chem.]]|url = https://zenodo.org/record/1253944}}</ref> The usual alkylating agents are employed, including [[Grignard reagent]]s and organolithium compounds:
 :2 PbCl<sub>2</sub> + 4 RLi → R<sub>4</sub>Pb + 4 LiCl + Pb
 :2 PbCl<sub>2</sub> + 4 RMgBr → R<sub>4</sub>Pb + Pb + 4 MgBrCl
@@ Line 116: / Line 127: @@
 ==Uses==
-*Molten PbCl<sub>2</sub> is used in the synthesis of lead titanate (PbTiO<sub>3</sub>) 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 PbTiO<sub>3</sub>, 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>
+*Molten PbCl<sub>2</sub> is used in the synthesis of [[lead titanate]] 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 PbTiO<sub>3</sub>, 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<sub>2(l)</sub> + BaTiO<sub>3(s)</sub> → Ba<sub>1−x</sub>Pb<sub>x</sub>TiO<sub>3</sub> + xBaCl<sub>2</sub>
+*:''x''&nbsp;PbCl<sub>2(l)</sub> + BaTiO<sub>3(s)</sub> → Ba<sub>1−''x''</sub>Pb<sub>''x''</sub>TiO<sub>3</sub> + ''x''&nbsp;BaCl<sub>2</sub>
-*PbCl<sub>2</sub> 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 PbCl<sub>2</sub> and reheating under controlled conditions. [[Stannous chloride]] (SnCl<sub>2</sub>) is used for the same purpose.<ref>[http://www.thestorefinder.com/glass/library/terms/termsA.html Stained Glass Terms and Definitions. ''aurene glass'']</ref>
+*PbCl<sub>2</sub> is used in production of infrared transmitting glass,<ref name="chemnetbase.com">Dictionary of Inorganic and Organometallic Compounds. ''Lead(II) Chloride.''[http://www.chemnetbase.com]</ref> and ornamental glass called [[aurene glass]]. Aurene glass has an iridescent surface formed by spraying with PbCl<sub>2</sub> and reheating under controlled conditions. [[Stannous chloride]] (SnCl<sub>2</sub>) 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 PbCl<sub>2</sub> 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, PbCl<sub>2</sub>·Pb(OH)<sub>2</sub>, 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> [[Lead paint]] is now banned as a health hazard in many countries by the [[White Lead (Painting) Convention, 1921]].
-*PbCl<sub>2</sub> 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 Cl<sub>2</sub> gas at 500&nbsp;°C. ZnCl<sub>2</sub> forms first and is removed. Then PbCl<sub>2</sub> forms and is removed leaving pure Bi. BiCl<sub>3</sub> would form last.<ref>Kirk-Othmer. ''Encyclopedia of Chemical Technology''. (ed 4). p. 241</ref>
+*PbCl<sub>2</sub> 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 [[arsenic]] and [[tellurium]]. This is followed by the [[Parkes process]] to remove any silver and gold present. There are now Bi, Pb, and Zn in the ore. At 500&nbsp;°C, it receives treatment from Cl2 gas. First, ZnCl2 forms and is excreted. Pure Bi is left behind after PbCl2 forms and is eliminated. Lastly, BiCl3 would form.<ref>Kirk-Othmer. ''Encyclopedia of Chemical Technology''. (ed 4). p. 241</ref>
 ==Toxicity==
-Like other lead containing compounds, exposure to PbCl<sub>2</sub> may cause [[lead poisoning]].
+Like other soluble lead compounds, exposure to PbCl<sub>2</sub> may cause [[lead poisoning]].
+{{Clear}}
 ==References==
@@ Line 131: / Line 144: @@
 ==External links==
 {{Commons category|Lead(II) chloride}}
-*[https://web.archive.org/web/20051012214505/http://www-cie.iarc.fr/htdocs/monographs/suppl7/leadandleadcompounds.html IARC Monograph: "Lead and Lead Compounds"]
+* [https://web.archive.org/web/20051012214505/http://www-cie.iarc.fr/htdocs/monographs/suppl7/leadandleadcompounds.html IARC Monograph: "Lead and Lead Compounds"]
-*[https://web.archive.org/web/20051120060034/http://www-cie.iarc.fr/htdocs/announcements/vol87.htm IARC Monograph: "Inorganic and Organic Lead Compounds"]
+* [https://web.archive.org/web/20051120060034/http://www-cie.iarc.fr/htdocs/announcements/vol87.htm IARC Monograph: "Inorganic and Organic Lead Compounds"]
-*[https://web.archive.org/web/20080111154608/http://www.npi.gov.au/database/substance-info/profiles/50.html National Pollutant Inventory – Lead and Lead Compounds Fact Sheet]
+* [https://web.archive.org/web/20080111154608/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]
+* [https://www.atsdr.cdc.gov/csem/csem.html Case Studies in Environmental Medicine – Lead Toxicity]
-*[http://www.atsdr.cdc.gov/tfacts13.html ToxFAQs: Lead]
+* [https://www.atsdr.cdc.gov/toxfaqs/tfacts13.pdf ToxFAQs: Lead]
 {{Lead compounds}}
+{{Chlorides}}
-[[Category:Lead compounds]]
+[[Category:Lead(II) compounds]]
 [[Category:Chlorides]]
 [[Category:Metal halides]]

v t e Lead compounds
Pb(II)	Pb(BiO₃)₂ PbBr₂ Pb(C₅H₅)₂ Pb(C₂H₃O₂)₂ PbC₂O₄ PbC₃₂H₁₆N₈ PbCl₂ Pb(ClO₄)₂ PbCO₃ PbCrO₄ PbF₂ PbHAsO₄ PbI₂ Pb(C ₁₁H ₂₃COO) ₂ Pb(NO₃)₂ Pb(N₃)₂ PbO Pb(OH)₂ PbPo PbP₇ Pb₃(PO₄)₂ PbS Pb(SCN)₂ PbSe PbSO₄ PbSeO₄ PbTe PbTiO₃ PbGeO₃ C ₃₆H ₇₀PbO ₄ PbO2−2 PbC₂ (hypothetical)
Pb(II,IV)	Pb₃O₄
Pb(IV)	Pb(C₂H₃O₂)₄ PbCl₄ PbF₄ PbH₄ PbO₂ PbS₂ plumbate Pb(OH)₄ (hypothetical)