Cesium chloride Chemical Properties

Melting point:

645 °C (lit.)

Boiling point:

1290 °C

Density 

3.988 g/cm3

vapor density 

5.8 (vs air)

refractive index 

1.6418

Flash point:

1303°C

storage temp. 

Store at +5°C to +30°C.

solubility 

H₂O: 3 M at 20 °C, clear, colorless

form 

beads

color 

White

Specific Gravity

3.988

Odor

Odorless

PH Range

6.0 - 7.5

PH

5.0-7.5 (25℃, 3M in H2O)

Water Solubility 

1860 g/L (20 ºC)

Sensitive 

Hygroscopic

λmax

λ: 260 nm Amax: 0.02
λ: 280 nm Amax: 0.02

Merck 

14,2011

Stability:

Stable. Deliquescent. Incompatible with strong oxidizing agents, strong acids. Protect from moisture.

InChIKey

AIYUHDOJVYHVIT-UHFFFAOYSA-M

CAS DataBase Reference

7647-17-8(CAS DataBase Reference)

NIST Chemistry Reference

Cesium chloride(7647-17-8)

EPA Substance Registry System

Cesium chloride (CsCl) (7647-17-8)

Safety Information

Hazard Codes 

Xn,Xi

Risk Statements 

68-36/38

Safety Statements 

36/37-26-24/25

RIDADR 

2923

WGK Germany 

2

RTECS 

FK9625000

F 

3

TSCA 

Yes

HS Code 

28273980

Hazardous Substances Data

7647-17-8(Hazardous Substances Data)

Toxicity

LD50 i.p. in rats: 1.5 g/kg (Cochran)

MSDS

• Language:English Provider:Caesium chloride
• Language:English Provider:SigmaAldrich
• Language:English Provider:ACROS
• Language:English Provider:ALFA

Cesium chloride Usage And Synthesis

Description

Cesium chloride is the inorganic compound with the formula CsCl. This colorless solid is an important source of caesium ions in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chlorine ions. Cesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Cesium chloride occurs naturally as impurities in carnallite (up to 0.002%), sylvite and kainite. Less than 20 tonnes of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral pollucite.

Cesium Chloride is a chemical reagent used in nuclear and radiologic medical treatments (e.g. Cancer radiation therapy, high pH therapy), in the diagnosis of myocardial infarction, and as a solute for ultracentrifugation.
Cesium chloride is widely used medicine structure in isopycnic centrifugation for separating various types of DNA. It is a reagent in analytical chemistry, where it is used to identify ions by the color and morphology of the precipitate.

Physical properties

White cubic crystal; hygroscopic; density 3.99 g/cm3; melts at 645°C; vaporizes at 1297°C; very soluble in water, soluble in ethanol.

Crystal structure

The Cesium chloride structure is composed of interlocking simple cubic lattices of anions and cations. It is the case that in a cubic 1:1 solid where one atom type is much larger than the other that the Cesium chloride type lattice is obtained, it can be thought of as a combination of basketballs and golf balls packed in a cubic manner with the golf balls in the gaps between the basketballs. If the two atom types are similar in size (imagine field hockey balls packed with tennis balls) then in the cubic lattice the structure will be like that of sodium chloride.

Uses

Cesium chloride is used for the preparation of electrically conducting glasses. It is also used to make solutions for the separation of RNA from DNA by density gradient centrifugation.
Cesium chloride is also widely used in the centrifugation of DNA, in a technique known as isopycnic centrifugation. In this method, a Cesium chloride solution is centrifuged, allowing centrifugal and diffusive forces to establish a concentration gradient (and thus a density gradient) within the centrifuge tube. When DNA is centrifuged in this solution, fragments of DNA will migrate down the tube until they reach a zone where the density of the DNA is equal to the density of the solution. At this point, the DNA will stop migrating. This allows separation of DNA of different densities (e.g. DNA fragments with differing A-T or G-C content). Cesium chloride (non-radioactive) is also promoted as an alternative cancer therapy. These claims are not supported by scientific evidence.
Cesium chloride (CsCl) is a mineral salt that is sometimes taken either by mouth, or by injection into the body, by cancer patients who seek alternative treatments. However, no CsCl products have been approved by FDA to treat cancer or other diseases.

Preparation

Cesium chloride can be prepared by the reaction of caesium hydroxide or caesium carbonate with hydrochloric acid: the resulting salt is purified by recrystallization.

Mechanism of Action

Proponents of cesium chloride therapy claim that it exerts antitumor effects by increasing the intracellular pH of tumor cells. The resulting alkaline environment is thought to prevent cancer cells from undergoing mitosis eventually resulting in cell death. Cesium causes hypokalemia by inhibiting potassium channels used for absorption of dietary potassium and for re-absorption of renal potassium. Cesium may also cause hypokalemia indirectly via loss of potassium due to repetitive diarrhea. Intravenous administration of cesium has been shown to cause arrhythmias in animal models.

Chemical Properties

Cesium chloride (CsCl) is an inorganic, colorless, hygroscopic crystalline powder. It has a large mass and is highly soluble in water (1865 g/L). Due to its hygroscopic characteristic, when put in water, it forms a dense solute that is not very viscous. Therefore, it is a good material for equilibrium gradient differential centrifugation where the separation of the particles is size and density dependent.
Cesium Chloride is a type of unit cell that is commonly mistaken as Body-Centered Cubic. This misconception is easy to make, since there is a center atom in the unit cell, but CsCl is really a non-closed packed structure type.

History

Someone has found that CsCl is described as showing a blue glow in the dark. It is interpreted that light can be caused by the collision of subatomic particles that escape from the nucleus of cesium 137 and collide with electrons located on the periphery of the atom, so the energy of the electrons increases, to return to the previous equilibrium state, the electrons release the excess of energy emitting light. It is also explained that because it is a highly active light source used in cancer treatment, blue light can be seen by the naked eye. The blue light is due to fluorescent UV dominant optical emission caused by beta, gamma, and Ba X-ray emissions from within the same excited 137-Cs atoms by a previously unknown atomic phenomenon, now known as Padmanabha Rao effect. But looking at Wikipedia, the IAEA report does not explain whether the blue light emitted by 137-c is fluorescence or Cerenkov radiation.

Uses

Cesium chloride has been used in density gradient centrifugation and for fractionation of nucleic acids, ribosomal subunits, proteins, glycoproteins, and viruses. Cesium chloride can also be used as a raw material to prepare other cesium compounds, such as cesium chloride reacts with nitric acid and oxalate to prepare cesium carbonate. It can be applied to the discharge tube (positive ion provided by the filament surface) fluorescent screen and used as a contrast agent. It effectively prevents activation of caspase-3 and neuronal apoptosis in serum- and potassium-deprived cerebellar granule neurons by inactivating GSK-3β.

Preparation

Cesium chloride (CsCl) is produced by the reaction of cesium metal with chlorine gas (Ca+ + Cl- → CsCl). It is also used in the beer brewing industry, to coat fluorescent screens, and to improve the taste of mineral water.

Uses

Cesium chloride is used in radio and television vacuum tubes. It also is used in ultracentrifuge separations; x-ray fluorescent screens; as radiogrpahic contrast medium, and to prepare cesium and other cesium salts.
Used for the preparation of electrically conducting glasses.
Used to make solutions for the separation of RNA from DNA by density gradient centrifugation.
For molecular genetic applications used in preparing nucleic acids for subsequent hybridization or cloning experiments.

Definition

ChEBI: Caesium chloride is the inorganic chloride salt of caesium; each caesium ion is coordinated by eight chlorine ions. It has a role as a phase-transfer catalyst and a vasoconstrictor agent. It is an inorganic chloride and an inorganic caesium salt.

Application

Cesium chloride has been used in the generation of discontinuous gradient for the purification of Cryptosporidium oocysts and as a component of acetamide medium for fungal selection.
Cesium chloride may be employed in gel-electrophoresis and RNA purification studies. It may be employed for the isolation of bacterial plasmid from Agrobacterium spp.

brand name

Cescan-131 (Abbott).

General Description

Cesium chloride is a cesium halide. Cesium halides can be prepared by reacting cesium carbonate with corresponding hydrohalic acids. Cesium chloride ultracentrifugation method has been reported for the extraction of RNA from cellular fractions.

Health Hazard

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 137CsCl powder from a 93-gram container in 1987 in Goiania, Brazil, resulted in one of the worst-ever radiation spill accidents killing four and directly affecting 249 people.

Flammability and Explosibility

Non flammable

Biochem/physiol Actions

Oral intake of cesium chloride is known to increase the pH in cancer cells. Mild toxicity of cesium chloride might cause hypotension, gastrointestinal distress, numbness and syncope. It also leads to severe hypokalemia, hypomagnesemia, acute heart attack and polymorphic ventricular tachycardia in episodes.

Safety Profile

Moderately toxic by ingestion and intraperitoneal routes. Experimental reproductive effects. Mutation data reported. Reacts violently with BF3. See also CESIUM. When heated to decomposition it emits toxic fumes of Cl-.

Purification Methods

It is soluble in H2O but can be purified by crystallisation from H2O [solublity in g percent: 162.3(0.7o), 182.2(16.2o) and 290(at bp 119.4o)] and dried in high a vacuum. It is soluble in EtOH and is deliquescent; keep it in a tightly closed container. [D.nges in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 951-955 1963.] For further purification of CsCl, a concentrated aqueous solution of the practically pure reagent is treated with an equivalent weight of I2 and Cl2 is bubbled into the solution until preciptation of CsCl2I is complete. Recrystallisation yields a salt which is free from other alkali metals. It is then decomposed to pure CsCl on heating. [Harned & Schupp J Am Chem Soc 52 3886 1930.] It can also be recrystallised from acetone/water, or from water (0.5mL/g) by cooling in a CaCl2/ice bath. Dry it at 78o under vacuum.

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