Cesium

Base Information

• Chemical Name: Cesium
• CAS No.: 7440-46-2
• Molecular Formula: Cs
• Molecular Weight: 132.905
• Hs Code.: 28051990
• European Community (EC) Number: 231-155-4
• UN Number: 1407
• Wikipedia: Caesium
• Wikidata: Q1108
• Mol file: 7440-46-2.mol

Synonyms:Cesium-133

Chemical Property of Cesium

Chemical Property:

• Appearance/Colour: silvery, light ductile metal
• Vapor Pressure: 1 mm Hg ( 279 °C)
• Melting Point: 28.5 °C(lit.)
• Boiling Point: 705 °C(lit.)
• PSA: 0.00000
• Density: 1.873 g/mL at 25 °C(lit.)
• LogP: 0.11250
• Storage Temp.: 2-8°C
• Sensitive.: moisture sensitive
• Solubility.: H2O: soluble
• Water Solubility.: reacts with H2O to evolve H2; soluble liquid NH3 [MER06]
• Hydrogen Bond Donor Count: 0
• Hydrogen Bond Acceptor Count: 0
• Rotatable Bond Count: 0
• Exact Mass: 132.90545196
• Heavy Atom Count: 1
• Complexity: 0
• Transport DOT Label: Dangerous When Wet

Purity/Quality:

98%min ^*data from raw suppliers

Cesium (99.9+%) (prescored ampoule) ^*data from reagent suppliers

Safty Information:

• Pictogram(s): Dangerous fire and explosion risk, ignites spontaneously in moist air, may explode in contact with sulfur or phosphorus, reacts violently with oxidizing materials, causes burns in contact with skin.
• Hazard Codes: Xi,C,F
• Statements: 36/38-34-14/15-11
• Safety Statements: 26-45-43-36/37/39-16-8

MSDS Files:

SDS file from LookChem

Total 1 MSDS from other Authors

Useful:

• Chemical Classes: Metals -> Elements, Metallic
• Canonical SMILES: [Cs]
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• Recent EU Clinical Trials: Phase III clinical trial to evaluate the efficacy and safety of chondroitin sulphate and glucosamine sulphate in combination versus placebo in patients with osteoarthritis of the knee.
• Description: Cesium was discovered in 1860 by Robert Bunsen and Gustav Kirchoff. It is used in the most accurate atomic clocks. Cesium melts at 28.41°C (just below body temperature) and occurs in Earth’s crust at 2.6 ppm. Cesium is the rarest of the naturally occurring alkali metals as the isotope 133Cs. Its compounds are correspondingly rare. Granites contain about 1 ppm cesium and sedimentary rocks contain approximately 4 ppm cesium. The most common commercial source of cesium is pollucite, which contains between 5 and 32% cesium oxide. Radioactive forms of cesium (134Cs and 137Cs) can also be found in the environment. They are produced during nuclear fission, and are used in cancer treatment.
• Physical properties: Like the other alkali metals, cesium is a soft-solid silvery metal, but much softer than theothers. It is the least electronegative and most reactive of the Earth metals. Cesium has anoxidation state of +1, and because its atoms are larger than Li, Na, and K atoms, it readilygives up its single outer valence electron. The single electron in the P shell is weakly attachedto its nucleus and thus available to combine with many other elements. It is much too reactiveto be found in its metallic state on Earth.Cs has a melting point of 29°C, which is lower than the body temperature of humans(37°C), and thus a chunk of cesium will melt in a person’s hand with disastrous results. Sinceit reacts with moisture on skin as well as with the air to release hydrogen, it will burn vigorously through the palm of one’s hand.Cesium’s boiling point is 669.3°C and its density is 1.837 g/cm3. Mercury is the only metalwith a lower melting point than cesium. It is extremely dangerous when exposed to air, water,and organic compounds or to sulfur, phosphorus, and any other electronegative elements. Itmust be stored in a glass container containing an inert atmosphere or in kerosene.Cesium reacts with water in ways similar to potassium and rubidium metals. In additionto hydrogen, it forms what is known as superoxides, which are identified with the generalformula CsO2. When these superoxides react with carbon dioxide, they release oxygen gas,which makes this reaction useful for self-contained breathing devices used by firemen andothers exposed to toxic environments.
• Uses: Because of some of its longer-lived isotopes, cesium has become valuable for its ability toproduce a steady stream of beta particles (β) as electrons.Light is strong enough to “knock off” electrons from cesium, which makes this phenomenon useful as a coating for photoelectric cells and electric eye devices. Cesium iodide (CsI)is used in scintillation counters (Geiger counters) to measure levels of external radiation. It isalso useful as a “getter” to remove air molecules remaining in vacuum tubes.In 1960 the International Committee of Weights and Measures selected radioactive cesium-137 (with a half-life of about 33 years) as the standard for measuring time. They equated thesecond with the radiation emitted by a Cs-137 atom that is excited by a small energy source.Thus, the second is now defined as 9,192,631,770 vibrations of the radiation emitted by anatom of Cs-137. There are about 200 atomic clocks around the world that collaborate theirefforts to maintain this extremely accurate clock that never needs winding or batteries.62 | The History and Use of Our Earth’s Chemical ElementsCesium is used as a hydrogenation catalyst to enhance and assist the reaction in the conversion of liquid oils to solids forms (e.g., in the production of margarine).In a molten state, it is used as a heat-transfer fluid in plants generating electric power.Cesium is used experimentally as a plasma to produce a source of ions to power outer spacevehicles using ion engines.Cesium is used in military infrared devices and signal lamps as well as in other opticaldevices.Cesium is used as a chemical reagent and reducing agent in industry and the laboratory. Itcan also be used as an antidote for arsenic poisoning. In photoelectric cells, as a "getter" in vacuum tubes; in photoemitter devices, scintillation counters. Adsorbent in CO2 purifn; scavenger of gases and impurities in metallurgy. For doping catalysts. For construction and operation of one type of atomic clock based on the vibrational frequency (9,192.76 megacycles/sec) of 133Cs. 137Cs in process control instruments, sewage and sludge sterilization. Cesium is used in photovoltaic cells, vacuum tubes, scintillation counters, and atomic clocks.

Technology Process of Cesium

There total 60 articles about Cesium which guide to synthetic route it. The literature collected by LookChem mainly comes from the sharing of users and the free literature resources found by Internet computing technology. We keep the original model of the professional version of literature to make it easier and faster for users to retrieve and use. At the same time, we analyze and calculate the most feasible synthesis route with the highest yield for your reference as below:

synthetic route:

Reference yield: 90.0%

cesium azide (22750-57-8) → caesium (7440-46-2)

Guidance literature:

In neat (no solvent); byproducts: caesium nitride, caesium silicate; CsN3 was decomposed at 390 °C forming Cs and a yellowish gray residue (contains ca. 70% Cs-nitride beside Cs-silicate and not-reacting Cs-azide);;

Reference yield: 70.0%

cesium dichromate → cesium oxide (20281-00-9) + caesium (7440-46-2)

Guidance literature:

With zirconium; In neat (no solvent); a mixture of Cs2Cr2O7 and Zr powder (weigt ratio = 1:10) was pressed to rods and heated in high vacuum at 380 °C forming Cs and Cs-oxide;;

Reference yield: 50.0%

caesium carbonate (534-17-8) → caesium (7440-46-2)

Guidance literature:

With iron; In neat (no solvent); Cs2CO3 was heated with excess of Fe at 1000 °C for 1 h forming metallic Cs; the evolution of gas started at 650 °C and increased up to 1000°C;; the obtained metal is partially oxidized;;

upstream raw materials:

cesium azide

dicesium

caesium bromide

cesium chloride

Downstream raw materials:

cesium hydroxide

cesium chloride

cesium monoxide radical

oxygen

Refernces

• 1、 Liew, Li-Anne,Moreland, John,Gerginov, Vladislav. "Wafer-level filling of microfabricated atomic vapor cells based on thin-film deposition and photolysis of cesium azide". . . Retrieved 2007.
• 2、 Lee, Jeihyun,Lee, Hyunbok,Jeon, Pyungeun,Jeong, Kwangho,Gun Kim, Tae,Won Kim, Jeong,Yi, Yeonjin. "Direct evidence of n-type doping in organic light-emitting devices: N free Cs doping from CsN3". . . Retrieved 2012.
• 3、 Husain, David,Plane, John M. C.,Xiang, Chen Cong. "". . . Retrieved 1985.
• 4、 Liebhafsky, H. A.,Winslow, A. F.. "". . p. 1128 - 1132. Retrieved 1947.
• 5、 Kawamura, Yoshiko,Yamauchi, Jun. "ESR Study of paramagnetic Nickel Species Obtained by Reduction and Oxidation of Bis(1,3,5-triphenylformazanato)nickel(II)". . p. 3041 - 3048. Retrieved 1995.
• 6、 Saltykov, Vyacheslav,Nuss, Juergen,Jansen, Martin. "Cs10Tl6SiO4, Cs10Tl 6GeO4, and Cs10Tl6SnO3 - First oxotetrelate thallides, double salts containing "hypoelectronic" [Tl6]6- clusters". . p. 1163 - 1168. Retrieved 2011/09/13.