caesium chloride

{{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 CsBr and CsI and many binary metallic alloys. In contrast, the other alkaline halides have the sodium chloride (rocksalt) structure.Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}} When both ions are similar in size (Cs⁺ ionic radius 174 pm for this coordination number, Cl⁻ 181 pm) the CsCl structure is adopted, when they are different (Na⁺ ionic radius 102 pm, Cl⁻ 181 pm) the sodium chloride structure is adopted. Upon heating to above 445 °C, the normal caesium chloride structure (α-CsCl) converts to the β-CsCl form with the rocksalt structure (space group Fm{{overline|3}}m). The rocksalt structure is also observed at ambient conditions in nanometer-thin CsCl films grown on mica, LiF, KBr and NaCl substrates.{{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 }}

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 °C to 2705 g/L at 100 °C.Lidin, p. 620 The crystals are very hygroscopic and gradually disintegrate at ambient conditions. Caesium chloride does not form hydrates.

In contrast to sodium chloride and potassium chloride, caesium chloride readily dissolves in concentrated hydrochloric acid. Caesium chloride has also a relatively high solubility in formic acid (1077 g/L at 18 °C) and hydrazine; medium solubility in methanol (31.7 g/L at 25 °C) and low solubility in ethanol (7.6 g/L at 25 °C),Plyushev, p. 97 sulfur dioxide (2.95 g/L at 25 °C), ammonia (3.8 g/L at 0 °C), acetone (0.004% at 18 °C), acetonitrile (0.083 g/L at 18 °C), ethylacetate and other complex ethers, butanone, acetophenone, pyridine and chlorobenzene.

Despite its wide band gap of about 8.35 eV at 80 K, caesium chloride weakly conducts electricity, and the conductivity is not electronic but ionic. The conductivity has a value of the order 10⁻⁷ S/cm at 300 °C. It occurs through nearest-neighbor jumps of lattice vacancies, and the mobility is much higher for the Cl⁻ than Cs⁺ vacancies. The conductivity increases with temperature up to about 450 °C, with an activation energy changing from 0.6 to 1.3 eV at about 260 °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.

Caesium chloride completely dissociates upon dissolution in water, and the Cs⁺ cations are solvated in dilute solution. CsCl converts to caesium sulfate upon being heated in concentrated sulfuric acid or heated with caesium hydrogen sulfate at 550–700 °C:

:2 CsCl + H₂SO₄ → Cs₂SO₄ + 2 HCl

:CsCl + CsHSO₄ → Cs₂SO₄ + HCl

Caesium chloride forms a variety of double salts with other chlorides. Examples include 2CsCl·BaCl₂, 2CsCl·CuCl₂, CsCl·2CuCl and CsCl·LiCl, and with interhalogen compounds:

:CsCl + ICl3 -> Cs[ICl4]

File:CsX@DWNT.jpgs.{{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}}]]

Caesium chloride occurs naturally as an impurity in the halide minerals carnallite (KMgCl₃·6H₂O with up to 0.002% CsCl), sylvite (KCl) and kainite (MgSO₄·KCl·3H₂O),Plyushev, pp. 210–211 and in mineral waters. For example, the water of Bad Dürkheim spa, which was used in isolation of caesium, contained about 0.17 mg/L of CsCl.Plyushev, p. 206 None of these minerals are commercially important.

On industrial scale, CsCl is produced from the mineral pollucite, which is powdered and treated with hydrochloric acid at elevated temperature. The extract is treated with antimony chloride, iodine monochloride, or cerium(IV) chloride to give the poorly soluble double salt, e.g.:

:CsCl + SbCl₃ → CsSbCl₄

Treatment of the double salt with hydrogen sulfide gives CsCl:

:2 CsSbCl₄ + 3 H₂S → 2 CsCl + Sb₂S₃ + 8 HCl

High-purity CsCl is also produced from recrystallized {{#tag:ce|Cs[ICl2]}} (and {{#tag:ce|Cs[ICl4]}}) by thermal decomposition:Plsyushev, pp. 357–358

:{{#tag:ce|Cs[ICl2] -> {CsCl} + ICl}}

Only about 20 tonnes of caesium compounds, with a major contribution from CsCl, were being produced annually around the 1970s and 2000s worldwide. Caesium chloride enriched with caesium-137 for radiation therapy applications is produced at a single facility Mayak in the Ural Region of RussiaEnrique Lima "Cesium: Radionuclide" in Encyclopedia of Inorganic Chemistry, 2006, Wiley-VCH, Weinheim. {{doi|10.1002/0470862106.ia712}} and is sold internationally through a UK dealer. The salt is synthesized at 200 °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.

In the laboratory, CsCl can be obtained by treating caesium hydroxide, carbonate, caesium bicarbonate, or caesium sulfide with hydrochloric acid:

:CsOH + HCl → CsCl + H₂O

:Cs₂CO₃ + 2 HCl → 2 CsCl + 2 H₂O + CO₂

Caesium chloride is the main precursor to caesium metal by high-temperature reduction:

:2 CsCl (l) + Mg (l) → MgCl₂ (s) + 2 Cs (g)

A similar reaction – heating CsCl with calcium in vacuum in presence of phosphorus – was first reported in 1905 by the French chemist M. L. Hackspill and is still used industrially.

Caesium hydroxide is obtained by electrolysis of aqueous caesium chloride solution:Plyushev, p. 90

: 2 CsCl + 2 H₂O → 2 CsOH + Cl₂ + H₂

Caesium chloride is widely used in centrifugation in a technique known as isopycnic centrifugation. 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). 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.

Caesium chloride is rarely used in organic chemistry. It can act as a phase transfer catalyst reagent in selected reactions. One of these reactions is the synthesis of glutamic acid derivatives

:$\backslash overbrace\{\backslash ce\{CH2=CHCOOCH3\}\}^\backslash text\{Methyl\; acrylate\}\; +\; \backslash ce\{ArCH=N-CH(CH3)-COOC(CH3)3$

->[\ce{TBAB,\ CsCl,\ K2CO3}][\ce{CPME,\ 0^\circ C}]

{ArCH=N-C(C2H4COOCH3)(CH3)-COOC(CH3)3}}

where TBAB is tetrabutylammonium bromide (interphase catalyst) and CPME is a cyclopentyl methyl ether (solvent).

Another reaction is substitution of tetranitromethane

:$\backslash overbrace\{\backslash ce\{C(NO2)4\}\}^\backslash text\{tetranitromethane\}\; +\; \backslash ce\{CsCl\; ->[\backslash ce\{DMF\}]\; \{C(NO2)3Cl\}\; +\; CsNO2\}$

where DMF is dimethylformamide (solvent).

Caesium chloride is a reagent in traditional analytical chemistry used for detecting inorganic ions via the color and morphology of the precipitates. Quantitative concentration measurement of some of these ions, e.g. Mg²⁺, with inductively coupled plasma mass spectrometry, is used to evaluate the hardness of water.

It is also used for detection of the following ions:

The American Cancer Society states that "available scientific evidence does not support claims that non-radioactive cesium chloride supplements have any effect on tumors." The Food and Drug Administration has warned about safety risks, including significant heart toxicity and death, associated with the use of cesium chloride in naturopathic medicine.{{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}}{{dead link|date=May 2025|bot=medic}}{{cbignore|bot=medic}}{{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 = Science-Based Medicine | date = August 2, 2018}}

Caesium chloride composed of radioisotopes such as ¹³⁷CsCl and ¹³¹CsCl, is used in nuclear medicine, including treatment of cancer (brachytherapy) and diagnosis of myocardial infarction. In the production of radioactive 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 strontium titanate, which is insoluble in water. For teletherapy sources, however, the radioactive density (Ci 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.

Caesium chloride is used in the preparation of electrically conducting glasses{{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}} and screens of cathode ray tubes. In conjunction with rare gases CsCl is used in excimer lamps{{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 }} and excimer lasers. Other uses include activation of electrodes in welding; manufacture of mineral water, beer and drilling muds; and high-temperature solders. 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; 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.{{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}} Therefore, it can be useful in electrophysiology experiments in neuroscience.

Caesium chloride has a low toxicity to humans and animals. Its median lethal dose (LD₅₀) in mice is 2300 mg per kilogram of body weight for oral administration and 910 mg/kg for intravenous injection. 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. When taken in large quantities, however, can cause a significant imbalance in potassium and lead to hypokalemia, arrhythmia, and acute cardiac arrest.{{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|bibcode=2010BTER..135....1M|s2cid=19186683}} However, caesium chloride powder can irritate the mucous membranes and cause asthma.

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. However, in the Goiânia accident in Brazil, such a source containing about 93 grams of ¹³⁷CsCl, 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 radiation sickness, 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.[https://web.archive.org/web/20090330064104/http://www.time.com/time/photogallery/0,29307,1887705_1862268,00.html "The Worst Nuclear Disasters"]. Time. 2009.

• List of ineffective cancer treatments

{{reflist|30em|refs=

{{cite book|author1=Plyushev, V.E. |author2=Stepin, B. D|title=Аналитическая химия рубидия и цезия|place=Moscow|publisher=Nauka|year=1975|pages=22–26}}

{{cite web

| url = http://www.cancer.org/Treatment/TreatmentsandSideEffects/ComplementaryandAlternativeMedicine/HerbsVitaminsandMinerals/cesium-chloride

| title = Cesium Chloride

| date = 30 November 2008

| work = Complementary and Alternative Medicine: Herbs, Vitamins, and Minerals

| publisher = American Cancer Society

| access-date = 2011-05-13

| archive-date = 2011-08-17

| archive-url = https://web.archive.org/web/20110817234536/http://www.cancer.org/Treatment/TreatmentsandSideEffects/ComplementaryandAlternativeMedicine/HerbsVitaminsandMinerals/cesium-chloride

| url-status = dead

}}

{{cite book|author=Ehrenreich, Henry |title=Solid state physics: advances in research and applications|url=https://books.google.com/books?id=ljr450_uYlsC&pg=PA30|year=1984|publisher=Academic Press|isbn=978-0-12-607738-4|pages=29–31}}

{{cite book|author1=National Research Council (U.S.). Committee on Radiation Source Use and Replacement; Nuclear and Radiation Studies Board|title=Radiation source use and replacement: abbreviated version|url=https://books.google.com/books?id=3cT2REdXJ98C&pg=PA28|date=January 2008|publisher=National Academies Press|isbn=978-0-309-11014-3|pages=28–}}

{{cite web

| url = http://www.cabot-corp.com/wcm/msds/en-us/CE/CESCHLORDRY-NA-EN.pdf

| title = Cesium Chloride MSDS

| work = Cesium Fine Chemicals

| publisher = Cabot Corporation

| access-date = 2011-04-11

| archive-date = 2011-09-28

| archive-url = https://web.archive.org/web/20110928030137/http://www.cabot-corp.com/wcm/msds/en-us/CE/CESCHLORDRY-NA-EN.pdf

| url-status = dead

}}

{{cite web

| url = http://cartwright.chem.ox.ac.uk/hsci/chemicals/caesium_chloride.html

| title = Chemical Safety Data: Caesium chloride

| work = Hands-on Science (H-Sci) Project: Chemical Safety Database

| publisher = Physical and Theoretical Chemistry Laboratory, Oxford University

| access-date = 2011-04-08

| archive-date = 2011-08-07

| archive-url = https://web.archive.org/web/20110807193524/http://cartwright.chem.ox.ac.uk/hsci/chemicals/caesium_chloride.html

| url-status = dead

}}

{{cite journal|url=http://deepblue.lib.umich.edu/bitstream/2027.42/32170/1/0000225.pdf|pmid=14222401|title=The direct diagnosis of myocardial infarction by photoscanning after administration of cesium-131|year=1964|last1=Carrea|first1=JR|last2=Gleason|first2=G|last3=Shaw|first3=J|last4=Krontz|first4=B|volume=68|pages=627–36|journal=American Heart Journal|doi=10.1016/0002-8703(64)90271-6|issue=5|hdl=2027.42/32170|hdl-access=free}}

{{cite book|chapter = Цезия галогениды|title= Химическая энциклопедия (Chemical encyclopedia)|editor=Knunyants, I. L|place=Moscow|publisher=Soviet Encyclopedia|year=1998|volume=5|page=657|isbn = 978-5-85270-310-1}}

{{cite book|chapter = Цезий|title= Химическая энциклопедия (Chemical encyclopedia)|editor=Knunyants, I. L|place=Moscow|publisher=Soviet Encyclopedia|year=1998|volume=5|pages=654–656

| isbn = 978-5-85270-310-1}}

{{cite web

| url = http://ru.wikisource.org/wiki/%D0%AD%D0%A1%D0%91%D0%95/%D0%A6%D0%B5%D0%B7%D0%B8%D0%B9

| title = ЭСБЕ/Цезий

| work = Brockhaus and Efron Encyclopedic Dictionary|year=1890–1907 | access-date = 2011-04-15

}}

{{cite book |publisher=IAEA| title=The Radiological Accident in Goiânia |year=1988|isbn=978-92-0-129088-5|place=Vienna |url=http://www-pub.iaea.org/MTCD/publications/PubDetAR.asp?pubId=3684}}. See pp. 1–6 for summary and p. 22 for the source description

{{cite journal|title=Cesium 131 Photoscan: Aid in the Diagnosis of Myocardial Infarction|doi=10.1001/jama.1968.03140200025006|year=1968|last1=McGeehan|first1=John T.|journal=JAMA: The Journal of the American Medical Association|volume=204|issue=7|pages=585–589 |pmid=5694480}}

{{cite web

| url = http://msds.chem.ox.ac.uk/CA/caesium_chloride.html

| title = Safety data for caesium chloride

| work = Chemical and Other Safety Information

| publisher = The Physical and Theoretical Chemistry Laboratory Oxford University

| access-date = 2011-04-08

| archive-date = 2010-11-22

| archive-url = https://web.archive.org/web/20101122220928/http://msds.chem.ox.ac.uk/CA/caesium_chloride.html

| url-status = dead

}}

{{cite book

| author = Turova, N. Ya.|title= Неорганическая химия в таблицах

| place =Moscow

| year = 1997

| page = 85}}

{{cite book|author = Plyushev, V.E.

| title = Химия и технология редких и рассеянных элементов

| editor = Bolshakov, K. A.|edition= 2

| place =Moscow

| publisher = Vysshaya Shkola

| year = 1976

| volume = 1

| pages = 101–103|display-authors=etal}}

[http://minerals.usgs.gov/minerals/pubs/commodity/cesium/mcs-2010-cesiu.pdf Cesium]. Mineral Commodity Summaries January 2010. U.S. Geological Survey

{{cite book

|script-title=ru:Вредные вещества в промышленности. Справочник для химиков, инженеров и врачей

|language = ru

|editor = Lazarev N.V. and Gadaskina, I.D.

|edition = 7 |place=St. Petersburg|publisher=Khimiya|year=1977|volume=3|pages=328–329

}}

{{cite book|author1=Lidin, R. A |author2=Molochko V. |author3=Andreeva, L. L. A. | title = Химические свойства неорганических веществ

| edition = 3

| place =Moscow|publisher = Khimiya

| year =2000

| page = 49

| isbn = 978-5-7245-1163-6

}}

{{cite book

| chapter = Бария хлорид|title = Химическая энциклопедия

| editor = Knunyants, I. L|place=Moscow|publisher = Soviet Encyclopedia|year=1988

| volume = 1|page= 463

}}

{{cite book

| chapter = Полигалогениды

| title = Химическая энциклопедия

| editor = Knunyants, I. L

| place =Moscow|publisher = Soviet encyclopedia

| year =1992

| volume = 3

| pages = 1237–1238

| isbn = 978-5-85270-039-1

}}

{{cite book

|title = Consolidated Index of Selected Property Values: Physical Chemistry and Thermodynamics

|editor = National Research Council (U.S.). Office of Critical Tables

|edition = Publication 976

|place=Washington, D.C.

|publisher = National Academy of Science

|year=1962

|page = 271}}

{{cite book

| chapter = Cesium and Cesium Compounds

| title = Kirk-Othmer Encyclopedia of Chemical Technology

| edition = 4th

| place =New York

| publisher = John Wiley & Sons

| year =1994

| volume = 5

| pages = 375–376

}}

{{cite book|author1=Halka M. |author2=Nordstrom B. | title = Alkali and Alkaline Earth Metals|url=https://books.google.com/books?id=oZHKEG5V4_0C&pg=PA52|publisher = Infobase Publishing

| year =2010|page = 52

| isbn = 978-0-8160-7369-6

}}Bick, Manfred and Prinz, Horst (2002) "Cesium and Cesium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. Vol. A6, pp. 153–156. {{doi|10.1002/14356007.a06_153}}

{{cite journal

| author = Hackspill, M. L.

| title = Sur une nouvelle prepapratíon du rubidium et du cæsium

| url = http://gallica.bnf.fr/ark:/12148/bpt6k3095m/f106

| language = fr

| journal = Comptes Rendus Hebdomadaires des Séances de l'Académie des Sciences

| year = 1905

| volume =141

| page = 106

}}

{{cite journal

|author1=Kano T. |author2=Kumano T. |author3=Maruoka K. | title = Rate Enhancement of Phase Transfer Catalyzed Conjugate Additions by CsCl

| doi =10.1021/ol900476e

| journal = Organic Letters

| year = 2009

| volume =11

| issue = 9

| pages = 2023–2025

| pmid = 19348469

}}

{{cite book

|author1 = Katritzky A. R.

|author-link1 = Alan R. Katritzky

|author2 = Meth-Cohn O.

|author3 = Rees Ch. W.

|author-link3 = Charles Rees

|series = Comprehensive Organic Functional Group Transformations

|editor = Gilchrist, T. L.

|edition = First

|place = New York

|publisher = Elsevier

|year = 1995

|volume = 6

|title = Synthesis: Carbon with Three or Four Attached Heteroatoms

|page = [https://archive.org/details/comprehensiveorg0000unse/page/283 283]

|isbn = 978-0-08-040604-6

|url-access = registration

|url = https://archive.org/details/comprehensiveorg0000unse/page/283

}}

{{cite book

|title = ГОСТ 52407-2005. Вода питьевая. Методы определения жесткости

|place=Moscow |publisher = Стандартинформ

|year=2006 }}

{{cite journal

|author1=Klenovskii, M.S. |author2=Kel'man, V.A. |author3=Zhmenyak, Yu.V. |author4=Shpenik, Yu.O. | title = Electric-discharge UV radiation source based on a Xe-CsCl vapor-gas mixture

| doi = 10.1134/S1063784210050178

| journal = Technical Physics

| year = 2010

| volume = 55

| issue = 5

| pages = 709–714

|bibcode=2010JTePh..55..709K |s2cid=120781022 }}

{{cite web

| url = http://www.migatronic.ru/content/view/52/46/

| title = Тугоплавкие и химически активные металлы

| publisher = Migatronic

| access-date = 2011-02-24

}}

{{cite book

|chapter = Cesium chloride

|title = Academic Press Dictionary of Science and Technology

|chapter-url = https://archive.org/details/academicpressdic00morr

|chapter-url-access = registration

|editor = Morris, Ch. G.

|place=San Diego

|publisher = Academic Press

|year=1992

|page = [https://archive.org/details/academicpressdic00morr/page/395 395]

|isbn = 978-0-12-200400-1

}}

{{cite book

|title = Industrial Minerals & Rocks: Commodities, Markets, and Uses

|editor1=Kogel, J. E. |editor2=Trivedi, N. C. |editor3=Barker, J. M |edition =7th

|place=Littleton

|publisher = Society for Mining, Metallurgy, and Exploration

|year=2006

|page = 1430

|isbn = 978-0-87335-233-8

}}

}}

{{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}}

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Category:Caesium compounds

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Category:Alkali metal chlorides

Category:Caesium chloride crystal structure