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Revision as of 12:19, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 474201886 of page Caesium_chloride for the Chem/Drugbox validation project (updated: '').		Latest revision as of 15:09, 16 December 2024 edit 209.160.162.114 (talk) →Crystal structureTag: Visual edit
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			{{Redirect|CsCl|other uses|CSCL (disambiguation){{!}}CSCL}}
	{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}}
	{{chembox		{{chembox
			| Verifiedfields = changed
	| verifiedrevid = 443998230
			| Watchedfields = changed
	| Name = Caesium chloride
			| verifiedrevid = 476993274
	| ImageFile = Caesium chloride.jpg
			| Name =
	| ImageName = Cesium chloride
	| ImageFile1 = Caesium-chloride-3D-ionic.png		| ImageFile = Caesium chloride.jpg
			| ImageSize = 230px
	| ImageName1 = Cesium chloride
			| ImageFile1 = CsCl polyhedra.png
	| OtherNames = Cesium chloride
			| ImageSize1 = 230px
	| Section1 = {{Chembox Identifiers
			| ImageFile2 = Caesium-chloride-3D-ionic.png
			| IUPACName = Caesium chloride
			| OtherNames = Cesium chloride
			| Section1 = {{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 22713		| ChemSpiderID = 22713
Line 15:		Line 19:
	| InChI = 1/ClH.Cs/h1H;/q;+1/p-1		| InChI = 1/ClH.Cs/h1H;/q;+1/p-1
	| SMILES = .		| SMILES = .
	| InChIKey = AIYUHDOJVYHVIT-REWHXWOFAO		| InChIKey = AIYUHDOJVYHWHXWOFAO
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/ClH.Cs/h1H;/q;+1/p-1		| StdInChI = 1S/ClH.Cs/h1H;/q;+1/p-1
Line 23:		Line 27:
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
	| EINECS = 231-600-2		| EINECS = 231-600-2
			| PubChem = 24293
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = CsCl		| Formula = CsCl
	| MolarMass = 168.36 g/mol		| MolarMass = 168.36 g/mol
	| Appearance = white solid <br> ]		| Appearance = white solid <br/> ]
	| Density = 3.99 g/cm<sup>3</sup>		| Density = 3.988 g/cm<sup>3</sup><ref name=r1/>
	| Solubility = 1865 g/L<ref>Lide</ref>		| Solubility = 1910 g/L (25 °C)<ref name=r1/>
	| SolubleOther = soluble in ]<ref>Lide, pp. 4–67, 4–1363</ref>		| SolubleOther = soluble in ]<ref name=r1/>
	| MeltingPt = 645 °C		| MeltingPtC = 646
			| MeltingPt_ref =<ref name=r1/>
	| BoilingPt = 1297 °C (vaporizes)
			| BoilingPtC = 1297
	|RefractIndex = 1.64<ref>Lide, p. 10-227</ref>
			| BoilingPt_ref =<ref name=r1>Haynes, p. 4.57</ref>
	|BandGap=8.35 eV (80 K)<ref name=gap>{{cite journal|doi=10.1088/0953-8984/6/12/009|year=1994|last1=Lushchik|first1=A|last2=Feldbach|first2=E|last3=Frorip|first3=A|last4=Ibragimov|first4=K|last5=Kuusmann|first5=I|last6=Lushchik|first6=C|journal=Journal of Physics: Condensed Matter|volume=6|issue=12|pages=2357–2366}}</ref>
			| RefractIndex = 1.712 (0.3 μm)<br/>1.640 (0.59 μm)<br/>1.631 (0.75 μm)<br/>1.626 (1 μm)<br/>1.616 (5 μm)<br/>1.563 (20 μm)<ref>Haynes, p. 10.240</ref>
			| BandGap =8.35 eV (80 K)<ref name=gap>{{cite journal|doi=10.1088/0953-8984/6/12/009|year=1994|last1=Lushchik|first1=A|last2=Feldbach|first2=E|last3=Frorip|first3=A|last4=Ibragimov|first4=K|last5=Kuusmann|first5=I|last6=Lushchik|first6=C|journal=Journal of Physics: Condensed Matter|volume=6|issue=12|pages=2357–2366|title=Relaxation of excitons in wide-gap CsCl crystals|bibcode=1994JPCM....6.2357L|s2cid=250824677 }}</ref>
			| MagSus = -56.7·10<sup>−6</sup> cm<sup>3</sup>/mol<ref>Haynes, p. 4.132</ref>
	}}		}}
	| Section3 = {{Chembox Structure		| Section3 = {{Chembox Structure
			| CrystalStruct = CsCl, ]
	| Coordination = simple cubic (])
			| SpaceGroup = Pm{{overline|3}}m, No. 221<ref name=str>{{cite journal|doi=10.1107/S0567739477000722|title=The transition mechanism between the CsCl-type and NaCl-type structures in CsCl|journal=Acta Crystallographica Section A|volume=33|issue=2|pages=294|year=1977|last1=Watanabe|first1=M.|last2=Tokonami|first2=M.|last3=Morimoto|first3=N.|bibcode=1977AcCrA..33..294W}}</ref>
	| CrystalStruct = ], ''Pm{{overline|3}}m'', ] No. 221, ] cP2
			| LattConst_a = 0.4119 nm
			| UnitCellFormulas = 1
			| UnitCellVolume =0.0699 nm<sup>3</sup>
			| Coordination = Cubic (Cs<sup>+</sup>)<br/>Cubic (Cl<sup>−</sup>)
			}}
			| Section4 = {{Chembox Hazards
			| LD50 = 2600 mg/kg (oral, rat)<ref>. nlm.nih.gov</ref>
			| GHSPictograms = {{GHS07}}{{GHS08}}
			| GHSSignalWord = Warning
			| HPhrases = {{H-phrases|302|341|361|373}}
			| PPhrases = {{P-phrases|201|202|260|264|270|281|301+312|308+313|314|330|405|501}}
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions = ]<br/>]<br/>]		| OtherAnions = ]<br/>]<br/>]<br/>Caesium astatide
	| OtherCations = ]<br/>]<br/>]<br/>]		| OtherCations = ]<br/>]<br/>]<br/>]<br/>]
	}}		}}
	}}		}}
			'''Caesium chloride''' or '''cesium chloride''' is the ] with the formula ]]. This colorless salt is an important source of ] ]s in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chloride ions. Caesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Caesium chloride occurs naturally as impurities in ] (up to 0.002%), ] and ]. Less than 20 ]s of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral ].<ref name=G&W>{{Greenwood&Earnshaw2nd}}</ref>
			Caesium chloride is widely used in ] for separating various types of ]. It is a reagent in ], where it is used to identify ions by the color and morphology of the precipitate. When enriched in ], such as <sup>137</sup>CsCl or <sup>131</sup>CsCl, caesium chloride is used in ] applications such as treatment of ] and diagnosis of ]. Another form of cancer treatment was studied using conventional non-radioactive CsCl. Whereas conventional caesium chloride has a rather low toxicity to humans and animals, the radioactive form easily contaminates the environment due to the high solubility of CsCl in water. Spread of <sup>137</sup>CsCl powder from a 93-gram container in 1987 in ], Brazil, resulted in one of the worst-ever radiation spill accidents killing four and directly affecting 249 people.
			==Crystal structure==
			{{main|Cubic crystal system}}
			The caesium chloride structure adopts a primitive cubic lattice with a two-atom basis, where both atoms have eightfold coordination. The chloride atoms lie upon the lattice points at the corners of the cube, while the caesium atoms lie in the holes in the center of the cubes; an alternative and exactly equivalent 'setting' has the caesium ions at the corners and the chloride ion in the center. This structure is shared with ] and ] and many binary metallic ]s. In contrast, the other alkaline halides have the ] (rocksalt) structure.<ref>Wells A.F. (1984) ''Structural Inorganic Chemistry'' 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}</ref> When both ions are similar in size (Cs<sup>+</sup> ] 174 pm for this coordination number, Cl<sup>−</sup> 181 pm) the CsCl structure is adopted, when they are different (Na<sup>+</sup> ] 102 pm, Cl<sup>−</sup> 181 pm) the ] structure is adopted. Upon heating to above 445&nbsp;°C, the normal caesium chloride structure (α-CsCl) converts to the β-CsCl form with the rocksalt structure (] ''Fm{{overline|3}}m'').<ref name=str/> The rocksalt structure is also observed at ambient conditions in nanometer-thin CsCl films grown on ], LiF, KBr and NaCl substrates.<ref name=str2>{{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>
			==Physical properties==
			Caesium chloride is colorless in the form of large crystals and white when powdered. It readily dissolves in water with the maximum solubility increasing from 1865 g/L at 20&nbsp;°C to 2705 g/L at 100&nbsp;°C.<ref>Lidin, p. 620</ref> The crystals are very ] and gradually disintegrate at ambient conditions.<ref name=esbi /> Caesium chloride does not form ]s.<ref name=en5 />
			{|class="wikitable" style="text-align:center"
			|+Solubility of CsCl in water<ref>Haynes, p. 5.191</ref>
			!Т (°C)
			!0
			!10
			!20
			!25
			!30
			!40
			!50
			!60
			!70
			!80
			!90
			!100
			|-
			|S (wt%)
			|61.83
			|63.48
			|64.96
			|65.64
			|66.29
			|67.50
			|68.60
			|69.61
			|70.54
			|71.40
			|72.21
			|72.96
			|}
			In contrast to ] and ], caesium chloride readily dissolves in concentrated hydrochloric acid.<ref name=neorganic2 /><ref name=analitcesium /> Caesium chloride has also a relatively high solubility in ] (1077 g/L at 18&nbsp;°C) and ]; medium solubility in ] (31.7 g/L at 25&nbsp;°C) and low solubility in ] (7.6 g/L at 25&nbsp;°C),<ref name=en5 /><ref name=analitcesium /><ref>Plyushev, p. 97</ref> ] (2.95 g/L at 25&nbsp;°C), ] (3.8 g/L at 0&nbsp;°C), ] (0.004% at 18&nbsp;°C), ] (0.083 g/L at 18&nbsp;°C),<ref name=analitcesium /> ] and other complex ]s, ], ], ] and ].<ref name=rare />
			Despite its wide ] of about 8.35 eV at 80 K,<ref name=gap/> caesium chloride weakly conducts electricity, and the conductivity is not electronic but ]. The conductivity has a value of the order 10<sup>−7</sup> S/cm at 300&nbsp;°C. It occurs through nearest-neighbor jumps of lattice vacancies, and the mobility is much higher for the Cl<sup>−</sup> than Cs<sup>+</sup> vacancies. The conductivity increases with temperature up to about 450&nbsp;°C, with an activation energy changing from 0.6 to 1.3 eV at about 260&nbsp;°C. It then sharply drops by two orders of magnitude because of the phase transition from the α-CsCl to β-CsCl phase. The conductivity is also suppressed by application of pressure (about 10 times decrease at 0.4 GPa) which reduces the mobility of lattice vacancies.<ref name=b1/>
			{|class="wikitable collapsible collapsed" style="text-align:center"
			|+Properties of aqueous solutions of CsCl at 20&nbsp;°C<ref>Haynes, p. 5.126</ref><ref>Lidin, p. 645</ref>
			! width="16%" |Concentration, <br/>wt%
			! width="16%" |Density, <br/>kg/L
			! width="16%" |Concentration, <br/>mol/L
			! width="17%" |] <br/>(at 589&nbsp;nm)
			! width="18%" |], °C relative to water
			! width="17%" |], <br/>10<sup>−3</sup> Pa·s
			|-
			|0.5
			| –
			|0.030
			|1.3334
			|0.10
			|1.000
			|-
			|1.0
			| 1.0059
			|0.060
			|1.3337
			|0.20
			|0.997
			|-
			|2.0
			| 1.0137
			|0.120
			|1.3345
			|0.40
			|0.992
			|-
			|3.0
			|
			|0.182
			|1.3353
			|0.61
			|0.988
			|-
			|4.0
			|1.0296
			|0.245
			|1.3361
			|0.81
			|0.984
			|-
			|5.0
			|
			|0.308
			|1.3369
			|1.02
			|0.980
			|-
			|6.0
			|1.0461
			|0.373
			|1.3377
			|1.22
			|0.977
			|-
			|7.0
			|
			|0.438
			|1.3386
			|1.43
			|0.974
			|-
			|8.0
			|1.0629
			|0.505
			|1.3394
			|1.64
			|0.971
			|-
			|9.0
			|
			|0.573
			|1.3403
			|1.85
			|0.969
			|-
			|10.0
			|1.0804
			|0.641
			|1.3412
			|2.06
			|0.966
			|-
			|12.0
			|1.0983
			|0.782
			|1.3430
			|2.51
			|0.961
			|-
			|14.0
			|1.1168
			|0.928
			|1.3448
			|2.97
			|0.955
			|-
			|16.0
			|1.1358
			|1.079
			|1.3468
			|3.46
			|0.950
			|-
			|18.0
			|1.1555
			|1.235
			|1.3487
			|3.96
			|0.945
			|-
			|20.0
			|1.1758
			|1.397
			|1.3507
			|4.49
			|0.939
			|-
			|22.0
			|1.1968
			|1.564
			|1.3528
			| –
			|0.934
			|-
			|24.0
			|1.2185
			|1.737
			|1.3550
			| –
			|0.930
			|-
			|26.0
			|
			|1.917
			|1.3572
			| –
			|0.926
			|-
			|28.0
			|
			|2.103
			|1.3594
			| –
			|0.924
			|-
			|30.0
			|1.2882
			|2.296
			|1.3617
			| –
			|0.922
			|-
			|32.0
			|
			|2.497
			|1.3641
			| –
			|0.922
			|-
			|34.0
			|
			|2.705
			|1.3666
			| –
			|0.924
			|-
			|36.0
			|
			|2.921
			|1.3691
			| –
			|0.926
			|-
			|38.0
			|
			|3.146
			|1.3717
			| –
			|0.930
			|-
			|40.0
			|1.4225
			|3.380
			|1.3744
			| –
			|0.934
			|-
			|42.0
			|
			|3.624
			|1.3771
			| –
			|0.940
			|-
			|44.0
			|
			|3.877
			|1.3800
			| –
			|0.947
			|-
			|46.0
			|
			|4.142
			|1.3829
			| –
			|0.956
			|-
			|48.0
			|
			|4.418
			|1.3860
			| –
			|0.967
			|-
			|50.0
			|1.5858
			|4.706
			|1.3892
			| –
			|0.981
			|-
			|60.0
			|1.7886
			|6.368
			|1.4076
			| –
			|1.120
			|-
			|64.0
			|
			|7.163
			|1.4167
			| –
			|1.238
			|}
			==Reactions==
			Caesium chloride completely dissociates upon dissolution in water, and the Cs<sup>+</sup> ]s are ] in dilute solution. CsCl converts to ] upon being heated in concentrated sulfuric acid or heated with ] at 550–700&nbsp;°C:<ref name=neorganic />
			:2 CsCl + H<sub>2</sub>SO<sub>4</sub> → Cs<sub>2</sub>SO<sub>4</sub> + 2 HCl
			:CsCl + CsHSO<sub>4</sub> → Cs<sub>2</sub>SO<sub>4</sub> + HCl
			Caesium chloride forms a variety of double salts with other chlorides. Examples include 2CsCl·BaCl<sub>2</sub>,<ref name=en1 /> 2CsCl·CuCl<sub>2</sub>, CsCl·2CuCl and CsCl·LiCl,<ref name=index /> and with ] compounds:<ref name=en31 />
			:<chem>CsCl + ICl3 -> Cs</chem>
			==Occurrence and production==
			]s.<ref name=chain>{{cite journal|doi=10.1038/nmat4069|pmid=25218060|title=Atomic structure and dynamic behaviour of truly one-dimensional ionic chains inside carbon nanotubes|journal=Nature Materials|volume=13|issue=11|pages=1050–4|year=2014|last1=Senga|first1=Ryosuke|last2=Komsa|first2=Hannu-Pekka|last3=Liu|first3=Zheng|last4=Hirose-Takai|first4=Kaori|last5=Krasheninnikov|first5=Arkady V.|last6=Suenaga|first6=Kazu|bibcode=2014NatMa..13.1050S}}</ref>]]
			Caesium chloride occurs naturally as an impurity in the halide minerals ] (KMgCl<sub>3</sub>·6H<sub>2</sub>O with up to 0.002% CsCl),<ref name=en52 /> ] (KCl) and ] (MgSO<sub>4</sub>·KCl·3H<sub>2</sub>O),<ref>Plyushev, pp. 210–211</ref> and in mineral waters. For example, the water of ] spa, which was used in isolation of caesium, contained about 0.17&nbsp;mg/L of CsCl.<ref>Plyushev, p. 206</ref> None of these minerals are commercially important.
			On industrial scale, CsCl is produced from the mineral ], which is powdered and treated with hydrochloric acid at elevated temperature. The extract is treated with ], ], or cerium(IV) chloride to give the poorly soluble double salt, e.g.:<ref name="kirk" />
			:CsCl + SbCl<sub>3</sub> → CsSbCl<sub>4</sub>
			Treatment of the double salt with ] gives CsCl:<ref name="kirk" />
			:2 CsSbCl<sub>4</sub> + 3 H<sub>2</sub>S → 2 CsCl + Sb<sub>2</sub>S<sub>3</sub> + 8 HCl
			High-purity CsCl is also produced from recrystallized {{#tag:ce|Cs}} (and {{#tag:ce|Cs}}) by thermal decomposition:<ref>Plsyushev, pp. 357–358</ref>
			:{{#tag:ce|Cs -> {CsCl} + ICl}}
			Only about 20 ]s of caesium compounds, with a major contribution from CsCl, were being produced annually around the 1970s<ref name=Ullmann/> and 2000s worldwide.<ref name=Alkali /> Caesium chloride enriched with caesium-137 for ] applications is produced at a single facility ] in the ] of Russia<ref>Enrique Lima "Cesium: Radionuclide" in Encyclopedia of Inorganic Chemistry, 2006, Wiley-VCH, Weinheim. {{doi|10.1002/0470862106.ia712}}</ref> and is sold internationally through a UK dealer. The salt is synthesized at 200&nbsp;°C because of its hygroscopic nature and sealed in a thimble-shaped steel container which is then enclosed into another steel casing. The sealing is required to protect the salt from moisture.<ref name=b2/>
			===Laboratory methods===
			In the laboratory, CsCl can be obtained by treating ], ], caesium bicarbonate, or caesium sulfide with hydrochloric acid:
			:CsOH + HCl → CsCl + H<sub>2</sub>O
			:Cs<sub>2</sub>CO<sub>3</sub> + 2 HCl → 2 CsCl + 2 H<sub>2</sub>O + CO<sub>2</sub>
			==Uses==
			===Precursor to Cs metal===
			Caesium chloride is the main precursor to caesium metal by high-temperature reduction:<ref name=Ullmann/>
			:2 CsCl (l) + Mg (l) → MgCl<sub>2</sub> (s) + 2 Cs (g)
			A similar reaction – heating CsCl with calcium in vacuum in presence of ] – was first reported in 1905 by the French chemist M. L. Hackspill<ref name=hackspill /> and is still used industrially.<ref name=Ullmann/>
			] is obtained by ] of aqueous caesium chloride solution:<ref>Plyushev, p. 90</ref>
			: 2 CsCl + 2 H<sub>2</sub>O → 2 CsOH + Cl<sub>2</sub> + H<sub>2</sub>
			===Solute for ultracentrifugation===
			Caesium chloride is widely used in ] in a technique known as ]. Centripetal and diffusive forces establish a density gradient that allow separation of mixtures on the basis of their molecular density. This technique allows separation of DNA of different densities (e.g. DNA fragments with differing A-T or G-C content).<ref name=Ullmann/> This application requires a solution with high density and yet relatively low viscosity, and CsCl suits it because of its high solubility in water, high density owing to the large mass of Cs, as well as low viscosity and high stability of CsCl solutions.<ref name=kirk/>
			=== Organic chemistry ===
			Caesium chloride is rarely used in organic chemistry. It can act as a ] reagent in selected reactions. One of these reactions is the synthesis of ] derivatives
			:<math chem>\overbrace{\ce{CH2=CHCOOCH3}}^\text{Methyl acrylate} + \ce{ArCH=N-CH(CH3)-COOC(CH3)3
			->
			{ArCH=N-C(C2H4COOCH3)(CH3)-COOC(CH3)3}}</math>
			where TBAB is tetrabutylammonium bromide (interphase catalyst) and CPME is a cyclopentyl methyl ether (solvent).<ref name=rept />
			Another reaction is substitution of ]<ref name=cofgt />
			:<math chem>\overbrace{\ce{C(NO2)4}}^\text{tetranitromethane} + \ce{CsCl -> {C(NO2)3Cl} + CsNO2}</math>
			where DMF is ] (solvent).
			===Analytical chemistry===
			Caesium chloride is a reagent in traditional ] used for detecting inorganic ions via the color and morphology of the precipitates. Quantitative concentration measurement of some of these ions, e.g. Mg<sup>2+</sup>, with ], is used to evaluate the hardness of water.<ref name=gost />
			{|class="wikitable collapsible collapsed sortable" style="text-align:center"
			! width="14%" |Ion
			! width="20%" |Accompanying reagents
			! Residue
			! Morphology
			! width="14%" |Detection limit (μg)
			|-
			| '''AsO<sub>3</sub><sup>3−</sup>'''
			| ]
			| Cs<sub>2</sub> or Cs<sub>3</sub>
			| Red hexagons
			| 0.01
			|-
			| '''Au<sup>3+</sup>'''
			| ], ]
			| Cs<sub>2</sub>Ag
			| Gray-black crosses, four and six-beamed stars
			| 0.01
			|-
			| '''Au<sup>3+</sup>'''
			| NH<sub>4</sub>SCN
			| Cs
			| Orange-yellow needles
			| 0.4
			|-
			| '''Bi<sup>3+</sup>'''
			| ], ]
			| Cs<sub>2</sub> or 2.5H<sub>2</sub>O
			| Red hexagons
			| 0.13
			|-
			| '''Cu<sup>2+</sup>'''
			| (CH<sub>3</sub>COO)<sub>2</sub>Pb, CH<sub>3</sub>COOH, KNO<sub>2</sub>
			| Cs<sub>2</sub>Pb
			| Small black cubes
			| 0.01
			|-
			| '''In<sup>3+</sup>'''
			| —
			| Cs<sub>3</sub>
			| Small octahedra
			| 0.02
			|-
			| data-sort-value="IrCl" | '''<sup>3−</sup>'''
			| —
			| Cs<sub>2</sub>
			| Small dark-red octahedra
			| –
			|-
			| '''Mg<sup>2+</sup>'''
			| Na<sub>2</sub>HPO<sub>4</sub>
			| CsMgPO<sub>4</sub> or 6H<sub>2</sub>O
			| Small tetrahedra
			| –
			|-
			| '''Pb<sup>2+</sup>'''
			| KI
			| Cs
			| Yellow-green needles
			| 0.01
			|-
			| '''Pd<sup>2+</sup>'''
			| NaBr
			| Cs<sub>2</sub>
			| Dark-red needles and prisms
			| –
			|-
			| data-sort-value="ReCl4" | '''<sup>−</sup>'''
			| —
			| Cs
			| Dark-red rhombs, bipyramids
			| 0.2
			|-
			| data-sort-value="ReCl6" | '''<sup>2−</sup>'''
			| —
			| Cs<sub>2</sub>
			| Small yellow-green octahedra
			| 0.5
			|-
			| '''ReO<sub>4</sub><sup>−</sup>'''
			| —
			| CsReO<sub>4</sub>
			| Tetragonal bipyramids
			| 0.13
			|-
			| '''Rh<sup>3+</sup>'''
			| KNO<sub>2</sub>
			| Cs<sub>3</sub>
			| Yellow cubes
			| 0.1
			|-
			| '''Ru<sup>3+</sup>'''
			| —
			| Cs<sub>3</sub>
			| Pink needles
			| –
			|-
			| data-sort-value="RuCl6" | '''<sup>2−</sup>'''
			| —
			| Cs<sub>2</sub>
			| Small dark-red crystals
			| 0.8
			|-
			| '''Sb<sup>3+</sup>'''
			| —
			| Cs<sub>2</sub>·''n''H<sub>2</sub>O
			| Hexagons
			| 0.16
			|-
			| '''Sb<sup>3+</sup>'''
			| NaI
			| <chem>Cs</chem> or <chem>Cs2</chem>
			| Red hexagons
			| 0.1
			|-
			| '''Sn<sup>4+</sup>'''
			| —
			| Cs<sub>2</sub>
			| Small octahedra
			| 0.2
			|-
			| '''TeO<sub>3</sub><sup>3−</sup>'''
			| HCl
			| Cs<sub>2</sub>
			| Light yellow octahedra
			| 0.3
			|-
			| '''Tl<sup>3+</sup>'''
			| NaI
			| <chem>Cs</chem>
			| Orange-red hexagons or rectangles
			| 0.06
			|}
			It is also used for detection of the following ions:
			{|class="wikitable" style="text-align:center"
			! width="14%" |Ion
			! width="20%" |Accompanying reagents
			! Detection
			! width="14%" |Detection limit (μg/mL)
			|-
			| '''Al<sup>3+</sup>'''
			| K<sub>2</sub>SO<sub>4</sub>
			| Colorless crystals form in neutral media after evaporation
			| 0.01
			|-
			| '''Ga<sup>3+</sup>'''
			| KHSO<sub>4</sub>
			| Colorless crystals form upon heating
			| 0.5
			|-
			| '''Cr<sup>3+</sup>'''
			| KHSO<sub>4</sub>
			| Pale-violet crystals precipitate in slightly acidic media
			| 0.06
			|}
			===Medicine===
			The ] states that "available scientific evidence does not support claims that non-radioactive cesium chloride supplements have any effect on tumors."<ref name=asc/> The ] has warned about safety risks, including significant heart toxicity and death, associated with the use of cesium chloride in naturopathic medicine.<ref>{{cite web | url = https://www.fda.gov/Drugs/GuidanceComplianceRegulatoryInformation/PharmacyCompounding/ucm614211.htm | title = FDA alerts health care professionals of significant safety risks associated with cesium chloride | publisher = Food and Drug Administration | date = July 23, 2018}}</ref><ref>{{cite web | url = https://sciencebasedmedicine.org/fda-blacklists-cesium-chloride-ineffective-and-dangerous-naturopathic-cancer-treatment/ | title = FDA blacklists cesium chloride, ineffective and dangerous naturopathic cancer treatment | website = ] | date = August 2, 2018}}</ref>
			===Nuclear medicine and radiography===
			Caesium chloride composed of ]s such as <sup>137</sup>CsCl and <sup>131</sup>CsCl,<ref name=usgs/> is used in ], including treatment of ] (]) and diagnosis of ].<ref name=deepblue/><ref name=jama/> In the production of ] sources, it is normal to choose a chemical form of the radioisotope which would not be readily dispersed in the environment in the event of an accident. For instance, radiothermal generators (RTGs) often use ], which is insoluble in water. For ] sources, however, the radioactive density (] in a given volume) needs to be very high, which is not possible with known insoluble caesium compounds. A thimble-shaped container of radioactive caesium chloride provides the active source.
			===Miscellaneous applications===
			Caesium chloride is used in the preparation of electrically conducting ]es<ref name=usgs /><ref>{{cite journal | author = Tver'yanovich, Y. S. | title = Optical absorption and composition of the nearest environment of neodymium in glasses based on the gallium-germanium-chalcogen system|year = 1998 | journal = Glass Phys. Chem. | volume = 24 | page = 446 |display-authors=etal}}</ref> and screens of cathode ray tubes.<ref name=Ullmann/> In conjunction with rare gases CsCl is used in ]s<ref name=jtph /><ref name=xurm>{{cite journal
			|author1=Klenovskii, M.S. |author2=Kel'man, V.A. |author3=Zhmenyak, Yu.V. |author4=Shpenik, Yu.O. | title = Luminescence of XeCl* and XeBr* exciplex molecules initiated by a longitudinal pulsed discharge in a three-component mixture of Xe with CsCl and CsBr vapors
			| doi = 10.1134/S0030400X13010141
			| journal = Optics and Spectroscopy
			| year = 2013
			| volume = 114
			| issue = 2
			| pages = 197–204
			|bibcode=2013OptSp.114..197K |s2cid=123684289 }}</ref> and ]s. Other uses include activation of electrodes in welding;<ref name=migatronic /> manufacture of mineral water, beer<ref name=dict /> and ]s;<ref name=cabot /> and high-temperature solders.<ref name=imr /> High-quality CsCl single crystals have a wide transparency range from UV to the infrared and therefore had been used for cuvettes, prisms and windows in optical spectrometers;<ref name=Ullmann/> this use was discontinued with the development of less hygroscopic materials.
			CsCl is a potent inhibitor of HCN channels, which carry the h-current in excitable cells such as neurons.<ref>{{cite journal|last=Biel|first=Martin|author2=Christian Wahl-Schott |author3=Stylianos Michalakis |author4=Xiangang Zong |s2cid=8090694|title=Hyperpolarization-Activated Cation Channels: From Genes to Function|journal=Physiological Reviews|year=2009|doi=10.1152/physrev.00029.2008|volume=89|issue=3|pages=847–85|pmid=19584315}}</ref> Therefore, it can be useful in electrophysiology experiments in neuroscience.
			==Toxicity==
			Caesium chloride has a low toxicity to humans and animals.<ref name=csd /> Its ] (LD<sub>50</sub>) in mice is 2300&nbsp;mg per kilogram of body weight for oral administration and 910&nbsp;mg/kg for intravenous injection.<ref name=msds /> The mild toxicity of CsCl is related to its ability to lower the concentration of potassium in the body and partly substitute it in biochemical processes.<ref name=vredno /> When taken in large quantities, however, can cause a significant imbalance in potassium and lead to ], ], and acute ].<ref>{{cite journal|last1=Melnikov|first1=P|last2=Zanoni|first2=LZ|title=Clinical effects of cesium intake|journal=Biological Trace Element Research|date=June 2010|volume=135|issue=1–3|pages=1–9|pmid=19655100|doi=10.1007/s12011-009-8486-7|s2cid=19186683}}</ref> However, caesium chloride powder can irritate the ]s and cause ].<ref name=cabot />
			Because of its high solubility in water, caesium chloride is highly mobile and can even diffuse through concrete. This is a drawback for its radioactive form which urges a search for less chemically mobile radioisotope materials. Commercial sources of radioactive caesium chloride are well sealed in a double steel enclosure.<ref name=b2/> However, in the ] in ], such a source containing about 93&nbsp;grams of <sup>137</sup>CsCl, was stolen from an abandoned hospital and forced open by two scavengers. The blue glow emitted in the dark by the radioactive caesium chloride attracted the thieves and their relatives who were unaware of the associated dangers and spread the powder. This resulted in one of the worst radiation spill accidents in which 4 people died within a month from the exposure, 20 showed signs of ], 249 people were contaminated with radioactive caesium chloride, and about a thousand received a dose exceeding a yearly amount of background radiation. More than 110,000 people overwhelmed the local hospitals, and several city blocks had to be demolished in the cleanup operations. In the first days of the contamination, stomach disorders and nausea due to radiation sickness were experienced by several people, but only after several days one person associated the symptoms with the powder and brought a sample to the authorities.<ref name=iaea/><ref>. '']''. 2009.</ref>
			==See also==
			*]
			==References==
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			==Bibliography==
			{{Commons category|Caesium chloride}}
			*{{RubberBible92nd}}
			*{{cite book|author1=Lidin, R. A |author2=Andreeva, L. L. |author3=Molochko V. A. |title= Константы неорганических веществ: справочник (Inorganic compounds: data book)|place=Moscow|year=2006|isbn = 978-5-7107-8085-5}}
			*{{cite book|author1=Plyushev, V. E. |author2=Stepin B. D.|script-title=ru:Химия и техtestнология соединений лития, рубидия и цезия|language=ru|place=Moscow|publisher=Khimiya|year=1970}}
			{{Caesium compounds}}
			{{Chlorides}}
			{{Authority control}}
			{{DEFAULTSORT:Caesium Chloride}}
			]
			]
			]
			]
			]