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{{chembox
{{chembox
| Verifiedfields = changed
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| verifiedrevid = 447133598
| Watchedfields = changed
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| Name = Thallium(I) chloride
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| verifiedrevid = 470605497
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| ImageFileL1 = Thallium(I)-chloride-3D-SF-C.png
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| Name = Thallium(I) chloride
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| ImageFileR1 = CsCl polyhedra.png
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| ImageFileL1 = Thallium(I)-chloride-3D-SF-C.png
<!-- | ImageSize1 = 200px -->
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| ImageFileR1 = CsCl polyhedra.png
| ImageFile2 = Thallium(I) chloride.jpg
| IUPACName = Thallium monochloride<br/>Thallium(I) chloride
| ImageFile2 = Thallium(I) chloride.jpg
| ImageSize2 = 240px
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| OtherNames = Thallous chloride
| IUPACName = Thallium monochloride<br/>Thallium(I) chloride
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| Section1 = {{Chembox Identifiers
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| OtherNames = Thallous chloride
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
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|Section1={{Chembox Identifiers
| CASNo = 7791-12-0
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| CASNo_Ref = {{cascite|correct|CAS}}
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| ChEBI_Ref = {{ebicite|correct|EBI}}
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| ChEBI = 37117
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 23044
| ChemSpiderID = 23044
| DrugBank = DB09316
| EC_number = 232-241-4
| UNNumber = 2811 1707
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 37CB58V15B
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| PubChem = 24642
| InChI = 1/ClH.Tl/h1H;/q;+1/p-1
| InChI = 1/ClH.Tl/h1H;/q;+1/p-1
| InChIKey = GBECUEIQVRDUKB-REWHXWOFAE
| InChIKey = GBECUEIQVRDUKB-REWHXWOFAE
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| ChEBI_Ref = {{ebicite|correct|EBI}}
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| ChEBI = 37117
| SMILES = Cl[Tl]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/ClH.Tl/h1H;/q;+1/p-1
| StdInChI = 1S/ClH.Tl/h1H;/q;+1/p-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = GBECUEIQVRDUKB-UHFFFAOYSA-M
| StdInChIKey = GBECUEIQVRDUKB-UHFFFAOYSA-M
| CASNo = 7791-12-0
| SMILES = Cl[Tl]
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| CASNo_Ref = {{cascite|correct|CAS}}
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| PubChem = 24642
}}
}}
| Section2 = {{Chembox Properties
|Section2={{Chembox Properties
| Formula = TlCl
| Formula = TlCl
| MolarMass = 239.82 g/mol
| MolarMass = 239.836 g/mol<ref name=r1>Haynes, p. 4.94</ref>
| Appearance = white, odorless crystalline solid
| Appearance = white, odorless crystalline solid<ref name=r1/>
| Density = 7.004 g/cm<sup>3</sup> (20 °C)
| Density = 7.0 g/cm<sup>3</sup><ref name=r1/>
| Solubility = 3.3 g/L (25 °C)<ref name=r1/>
| Solubility = 0.29 g/100 mL (15.5 °C) <br> 0.318 g/100 mL (20 °C) <br> 2.41 g/100 mL (100 °C) <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref>
| SolubleOther = insoluble in [[alcohol]], [[acetone]], [[ammonium hydroxide|NH<sub>4</sub>OH]]
| SolubleOther = insoluble in [[ethanol|alcohol]]<ref name=r1/>
| MeltingPtC = 430
| MeltingPtC = 431
| BoilingPtC = 720
| BoilingPtC = 720
| MeltingPt_ref = <ref name=r1/>
| Boiling_notes = decomp
| BoilingPt_ref = <ref name=r1/>
| RefractIndex = 2.247
| RefractIndex = 2.247 (0.59 µm)<br>2.198 (0.75 µm)<br>2.145 (1 µm)<br>1.891 (5 µm)<br>2.193 (20 µm)<ref>Haynes, p. 10.242</ref>
| MagSus = &minus;57.8·10<sup>−6</sup> cm<sup>3</sup>/mol<ref>Haynes, p. 4.135</ref>
}}
}}
| Section7 = {{Chembox Hazards
|Section3={{Chembox Structure
| CrystalStruct = [[Caesium chloride|CsCl]], [[Pearson symbol|cP2]]
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| ExternalMSDS = http://www.crystran.co.uk/uploads/files/178.pdf
| SpaceGroup = Pm{{overline|3}}m, No. 221<ref name=str2>{{cite journal|doi=10.1002/pssa.2210210251|title=X-ray diffraction study of the systems TlI-CsI, TlI-RbI, and TlI-Tl ''Cl''|journal=Physica Status Solidi A|volume=21|issue=2|pages=K81|year=1974|last1=Müürsepp|first1=T.|last2=Haav|first2=A.|bibcode=1974PSSAR..21...81M}}</ref>
| EUIndex = 081-002-00-9
| LattConst_a = 0.38416 nm
| EUClass = Very toxic ('''T+''')<br/>Dangerous for the environment ('''N''')
| UnitCellFormulas = 1
| RPhrases = {{R26/28}}, {{R33}}, {{R51/53}}
| UnitCellVolume =0.0567 nm<sup>3</sup>
| SPhrases = {{S1/2}}, {{S13}}, {{S28}}, {{S45}}, {{S61}}
| Coordination = Cubic (Tl<sup>+</sup>)<br/>Cubic (Cl<sup>−</sup>)
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| NFPA-H =
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| NFPA-F =
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| NFPA-R =
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| NFPA-O =
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| LD50 = 24 mg/kg, oral, mouse
}}
}}
| Section8 = {{Chembox Related
|Section7={{Chembox Hazards
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| ExternalSDS = http://www.crystran.co.uk/uploads/files/178.pdf
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| OtherAnions = [[Thallium(I) fluoride]]<br/>[[Thallium(I) bromide]]<br/>[[Thallium(I) iodide]]
| GHSPictograms = {{GHS06}}{{GHS08}}{{GHS09}}
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| OtherCations = [[Thallium(III) chloride]]<br/>[[Silver(I) chloride]]<br/>[[Lead(II) chloride]]
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|300|330|373|411}}
| PPhrases = {{P-phrases|260|264|270|271|273|284|301+310|304+340|310|314|320|321|330|391|403+233|405|501}}
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| NFPA-H =
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| NFPA-F =
⚫
| NFPA-R =
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| NFPA-S =
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| LD50 = 24 mg/kg, oral, mouse
}}
|Section8={{Chembox Related
⚫
| OtherAnions = [[Thallium(I) fluoride]]<br/>[[Thallium(I) bromide]]<br/>[[Thallium(I) iodide]]
⚫
| OtherCations = [[Thallium(III) chloride]]<br/>[[Silver(I) chloride]]<br/>[[Lead(II) chloride]]
}}
}}
}}
}}
'''Thallium(I) chloride''' is the [[chemical compound]] with the formula [[Thallium|Tl]][[Chlorine|Cl]]. This colourless solid is an intermediate in the isolation of thallium from its ores. Typically, an acidic solution of [[thallium(I) sulfate]] is treated with [[hydrochloric acid]] to precipitate insoluble thallium(I) chloride. This solid crystallizes in the [[caesium chloride]] motif.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>
'''Thallium(I) chloride''', also known as '''thallous chloride''', is a [[chemical compound]] with the formula TlCl. This colourless salt is an intermediate in the isolation of [[thallium]] from its ores. Typically, an acidic solution of [[thallium(I) sulfate]] is treated with [[hydrochloric acid]] to precipitate insoluble thallium(I) [[chloride]]. This solid crystallizes in the [[caesium chloride]] motif.<ref>Holleman, A. F.; Wiberg, E. ''Inorganic Chemistry''. Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref>


The low solubility of TlCl is exploited in chemical synthesis: treatment of metal chloride [[coordination chemistry|complexes]] with TlPF<sub>6</sub>, gives the corresponding metal [[hexafluorophosphate]] derivative. The resulting TlCl precipitate is separated by filtration of the reaction mixture. The overall methodology is similar to the use of AgPF<sub>6</sub>, except that Tl<sup>+</sup> is much less oxidizing.
The low solubility of TlCl is exploited in chemical synthesis: treatment of metal chloride [[coordination chemistry|complexes]] with TlPF<sub>6</sub>, gives the corresponding metal [[hexafluorophosphate]] derivative. The resulting TlCl precipitate is separated by filtration of the reaction mixture. The overall methodology is similar to the use of AgPF<sub>6</sub>, except that Tl<sup>+</sup> is much less oxidizing.


The crystalline structure is of cubic [[Caesium chloride|CsCl]] type at room temperature, but it lowers to the [[orthorombic]] [[Thallium(I) iodide|thallium iodide]] type upon cooling, the transition temperature being likely affected by the impurities <ref>M Blackman et al "The Polymorphism of Thallium and Other Halides at Low Temperatures" [http://dx.doi.org/10.1088/0370-1328/77/2/331 Proc. Phys. Soc. 77 (1961) 471]</ref><ref>A-V Mudring "Thallium Halides – New Aspects of the Stereochemical Activity of Electron Lone Pairs of Heavier Main-Group Elements" [http://www3.interscience.wiley.com/journal/114066398/abstract Eur. J. Inorg. Chem. 6 (2007) 882]</ref><ref>R. P. Lowndes and C. H. Perry "Molecular structure and anharmonicity in thallium iodide" [http://link.aip.org/link/?JCPSA6/58/271/1 J. Chem. Phys. 58, 271 (1973)]</ref>.
The crystalline structure is of cubic caesium chloride type at room temperature, but it lowers to the [[orthorhombic]] [[Thallium(I) iodide|thallium iodide]] type upon cooling, the transition temperature being likely affected by the impurities.<ref>{{cite journal|doi=10.1088/0370-1328/77/2/331|title=The Polymorphism of Thallium and Other Halides at Low Temperatures|journal=Proceedings of the Physical Society|volume=77|issue=2|pages=471|year=1961|last1=Blackman|first1=M|last2=Khan|first2=I H|bibcode=1961PPS....77..471B}}</ref> Nanometer-thin TlCl films grown on KBr substrates exhibit a [[rocksalt]] structure, while the films deposited on [[mica]] or NaCl are of the regular CsCl type.<ref name=str>{{cite journal|doi=10.1107/S0365110X51001641|title=Polymorphism of cesium and thallium halides|journal=Acta Crystallographica|volume=4|issue=6|pages=487–489|year=1951|last1=Schulz|first1=L. G.|bibcode=1951AcCry...4..487S }}</ref>


A very rare mineral lafossaite, Tl(Cl,Br), is a natural form of thallium(I) chloride.<ref>http://www.mindat.org/min-27521.html</ref>
A very rare mineral [[lafossaite]], {{chem2|Tl(Cl,Br)}}, is a natural form of thallium(I) chloride.<ref>[http://www.mindat.org/min-27521.html Lafossaite]. Mindat.org</ref>


Thallium(I) chloride, like all thallium compounds, is highly toxic, although its insolubility limits its toxicity to a degree.
Thallium(I) chloride, like all thallium compounds, is highly toxic, although its low solubility limits its toxicity.<ref>[http://www.espimetals.com/index.php/722-msds/thallium-chloride/738-thallium-chloride Thallium Chloride Material Safety Data Sheet] {{Webarchive|url=https://web.archive.org/web/20190401160424/http://espimetals.com/index.php/722-msds/thallium-chloride/738-thallium-chloride |date=2019-04-01 }}. espimetals.com</ref>


==References==
==References==
{{reflist}}
{{reflist}}


==Cited sources==
{{inorganic-compound-stub}}
{{Commons category}}
*{{RubberBible92nd}}

{{Thallium compounds}}
{{Thallium compounds}}
{{Chlorides}}


[[Category:Chlorides]]
[[Category:Chlorides]]
[[Category:Thallium compounds]]
[[Category:Thallium(I) compounds]]
[[Category:Metal halides]]
[[Category:Metal halides]]
[[Category:Inorganic compound stubs]]
[[Category:Caesium chloride crystal structure]]

[[ar:كلوريد ثاليوم أحادي]]
[[de:Thallium(I)-chlorid]]
[[fa:کلرید تالیم(I)]]
[[ja:塩化タリウム(I)]]
[[ru:Хлорид таллия(I)]]
[[simple:Thallium(I) chloride]]

Latest revision as of 01:52, 1 May 2024

Thallium(I) chloride
Names
IUPAC names
Thallium monochloride
Thallium(I) chloride
Other names
Thallous chloride
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
DrugBank
ECHA InfoCard 100.029.311 Edit this at Wikidata
EC Number
  • 232-241-4
UNII
UN number 2811 1707
  • InChI=1S/ClH.Tl/h1H;/q;+1/p-1 checkY
    Key: GBECUEIQVRDUKB-UHFFFAOYSA-M checkY
  • InChI=1/ClH.Tl/h1H;/q;+1/p-1
    Key: GBECUEIQVRDUKB-REWHXWOFAE
  • Cl[Tl]
Properties
TlCl
Molar mass 239.836 g/mol[1]
Appearance white, odorless crystalline solid[1]
Density 7.0 g/cm3[1]
Melting point 431 °C (808 °F; 704 K)[1]
Boiling point 720 °C (1,328 °F; 993 K)[1]
3.3 g/L (25 °C)[1]
Solubility insoluble in alcohol[1]
−57.8·10−6 cm3/mol[2]
2.247 (0.59 µm)
2.198 (0.75 µm)
2.145 (1 µm)
1.891 (5 µm)
2.193 (20 µm)[3]
Structure
CsCl, cP2
Pm3m, No. 221[4]
a = 0.38416 nm
0.0567 nm3
1
Cubic (Tl+)
Cubic (Cl−)
Hazards
GHS labelling:
GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Danger
H300, H330, H373, H411
P260, P264, P270, P271, P273, P284, P301+P310, P304+P340, P310, P314, P320, P321, P330, P391, P403+P233, P405, P501
Lethal dose or concentration (LD, LC):
24 mg/kg, oral, mouse
Safety data sheet (SDS) http://www.crystran.co.uk/uploads/files/178.pdf
Related compounds
Other anions
 Thallium(I) fluoride
Thallium(I) bromide
Thallium(I) iodide
Other cations
 Thallium(III) chloride
Silver(I) chloride
Lead(II) chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Thallium(I) chloride, also known as thallous chloride, is a chemical compound with the formula TlCl. This colourless salt is an intermediate in the isolation of thallium from its ores. Typically, an acidic solution of thallium(I) sulfate is treated with hydrochloric acid to precipitate insoluble thallium(I) chloride. This solid crystallizes in the caesium chloride motif.[5]

The low solubility of TlCl is exploited in chemical synthesis: treatment of metal chloride complexes with TlPF6, gives the corresponding metal hexafluorophosphate derivative. The resulting TlCl precipitate is separated by filtration of the reaction mixture. The overall methodology is similar to the use of AgPF6, except that Tl+ is much less oxidizing.

The crystalline structure is of cubic caesium chloride type at room temperature, but it lowers to the orthorhombic thallium iodide type upon cooling, the transition temperature being likely affected by the impurities.[6] Nanometer-thin TlCl films grown on KBr substrates exhibit a rocksalt structure, while the films deposited on mica or NaCl are of the regular CsCl type.[7]

A very rare mineral lafossaite, Tl(Cl,Br), is a natural form of thallium(I) chloride.[8]

Thallium(I) chloride, like all thallium compounds, is highly toxic, although its low solubility limits its toxicity.[9]

References

[edit]
  1. ^ a b c d e f g Haynes, p. 4.94
  2. ^ Haynes, p. 4.135
  3. ^ Haynes, p. 10.242
  4. ^ Müürsepp, T.; Haav, A. (1974). "X-ray diffraction study of the systems TlI-CsI, TlI-RbI, and TlI-Tl Cl". Physica Status Solidi A. 21 (2): K81. Bibcode:1974PSSAR..21...81M. doi:10.1002/pssa.2210210251.
  5. ^ Holleman, A. F.; Wiberg, E. Inorganic Chemistry. Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  6. ^ Blackman, M; Khan, I H (1961). "The Polymorphism of Thallium and Other Halides at Low Temperatures". Proceedings of the Physical Society. 77 (2): 471. Bibcode:1961PPS....77..471B. doi:10.1088/0370-1328/77/2/331.
  7. ^ Schulz, L. G. (1951). "Polymorphism of cesium and thallium halides". Acta Crystallographica. 4 (6): 487–489. Bibcode:1951AcCry...4..487S. doi:10.1107/S0365110X51001641.
  8. ^ Lafossaite. Mindat.org
  9. ^ Thallium Chloride Material Safety Data Sheet Archived 2019-04-01 at the Wayback Machine. espimetals.com

Cited sources

[edit]
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