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Title: Chemistry/Elements/Cesium - LANL: Cesium History, sources, properties, and costs.
Lenntech__Cesium Physical data, chemical properties, health and environmental effects.

USGS_Minerals_Information__Cesium Statistics and information on the worldwide supply, demand, and flow of the element (PDF format).

Visual_Elements__Caesium Image, general and physical information, and key isotopes.

WebElements__Caesium Extensive information on history, uses, occurrence, compounds, and properties.

Wikipedia__Caesium Properties of the element, including its history, applications, and characteristics.

Radiochemistry_of_Cesium Full text of the monograph by M. T. Kinsley (Brookhaven National Laboratory, Upton, New York). [PDF] (February, 1961)


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Cesium /* No Right Click Copyright Mike McGrath (http://website.lineone.net/~mike_mcgrath/) To add more shock to your site, visit www.DHTML Shock.com */ Back to the Periodic Table          Cesium Atomic Number: 55 Atomic Radius: 265.4 pm Atomic Symbol: Cs Melting Point: 28.5 șC Atomic Weight: 132.9054 Boiling Point: 671 șC Electron Configuration: [Xe]6s1 Oxidation States: 1

History

(L. caesius: sky blue) Cesium was discovered spectroscopically in 1860 by Bunsen and Kirchhoff  in mineral water from Durkheim.

Sources

Cesium, an alkali metal, occurs in lepidolite, pollucte (a hydrated silicate of aluminum and cesium), and in other sources. One of the world's richest sources of cesium is located at Bernic Lake, Manitoba. The deposits are estimated to contain 300,000 tons of pollucite, averaging 20% cesium. It can be isolated by elecytrolysis of the fused cyanide and by a number of other methods. Very pure, gas-free cesium can be prepared by thermal decomposition of cesium azide.

Properties

The metal is characterized by a spectrum containing two bright lines in the blue along with several others in the red, yellow, and green wavelengths. It is silvery white, soft, and ductile. It is the most electropositive and most alkaline element. Cesium, gallium, and mercury are the only three metals that are liquid at room temperature. Cesium reacts explosively with cold water, and reacts with ice at temperatures above -116C. Cesium hydroxide, the strongest base known, attacks glass.

Uses

Because of it has great affinity for oxygen, the metal is used as a "getter" in electron tubes. It is also used in photoelectric cells, as well as a catalyst in the hydrogenation of certain organic compounds. The metal has recently found application in ion propulsion systems. Cesium is used in atomic clocks, which are accurate to 5 s in 300 years. Its chief compounds are the chloride and the nitrate.

Isotopes

Cesium has more isotopes than any element--32--with masses ranging from 114 to 145.

Costs

The present price of cesium is about $30/g. Title Picture: puddle of cesium: the pure solid melts at room temperature Sources: CRC Handbook of Chemistry and Physics and the American Chemical Society. Chemistry Division HomeLANL Home Last Updated: 12/15/2003,© Chemistry Operations Operated by the University of California for the US Department of Energy   | Help | Copyright © UC 2003 | Disclaimer  
 

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