Atomic Properties of Cs
- Atomic Number of Cs
- 55
- Atomic Mass of Cs
- 132.9100 u
- Electron Configuration
- [Xe] 6s1
- Electronegativity
- 0.79
- Block
- s-block
- Group
- 1
- Period
- 6
Cesium (Cs) is element 55 on the periodic table. Atomic mass of Cs: 132.9100 u. Cs is in period 6, group 1. Melting point of Cs: 301.70 K.Density of Cs: 1.93 g/cm³.
The element that defines time itself—and explodes in water
Cesium has no known biological role. Behaves like potassium in the body. Cesium-137 contamination persists for decades.
Discovered by Gustov Kirchoff, Robert Bunsen in Germany, 1860
Name origin: Latin: coesius (sky blue); for the blue lines of its spectrum.
Soft silvery-white metallic element belonging to group 1 of the periodic table. One of the three metals which are liquid at room temperature. Cs-133 is the natural, and only stable, isotope. Fifteen other radioisotopes exist. Caesium reacts explosively with cold water, and ice at temperatures above 157K. Caesium hydroxide is the strongest base known. Caesium is the most electropositive, most alkaline and has the least ionization potential of all the elements. Known uses include the basis of atomic clocks, catalyst for the hydrogenation of some organic compounds, and in photoelectric cells. Caesium was discovered by Gustav Kirchoff and Robert Bunsen in Germany in 1860 spectroscopically. Its identification was based upon the bright blue lines in its spectrum. The name comes from the latin word caesius, which means sky blue. Caesium should be considered highly toxic. Some of the radioisotopes are even more toxic.
Cesium has 1 naturally occurring isotope, plus 1 notable radioactive isotope.
| Isotope | Atomic Mass (u) | Abundance | Half-Life | Decay Mode |
|---|---|---|---|---|
| 13355Cs (Cs-133)Cesium-133 isotope | 132.905452 | 100.00% | — | — |
| 13755Cs (Cs-137)Cesium-137 isotope | 136.9070896 | 0% | 30.17 years | β⁻ |
Data source: NIH PubChem (aggregated from IUPAC, NIST)
Isotopes of Cesium have important real-world applications in science and industry.
Nuclear fission of 235U (or other fissionable materials) yields 137Cs as a product. Although 137Cs is not naturally present in the environment, it can be collected from nuclear reactor processing and then used as an environmental tracer. 137Cs adheres tightly to porous sediments and will follow the movement of the sediment. By exposing sediments to 137Cs and allowing this combination to move dynamically, gamma ray spectrometry can then be used to measure the activity of 137Cs and monitor the movement of the radioactive sediments [404], [405], [406]. 137Cs dating of sediments not older than 60 years is useful in natural and artificial lakes and other environments because of its widespread production and release during atmospheric nuclear weapons testing, which began in the late 1940s, plus subsequent releases, such as during the accident at the Chernobyl nuclear reactor in April 1986. The 137Cs concentration profile in a sediment core can be matched with the historical record of 137Cs release to determine the approximate age profile of the sediment [406], [407].
High-energy gamma rays from 137Cs serve as food irradiation devices to remove bacteria and other harmful microorganisms (living single celled organisms such as virus, algae and fungus) from food. Although 137Cs is not used commercially for large-scale food irradiation, it has been proposed that it can be used this way. Gamma rays from the radioactive 137Cs destroy the DNA of organisms to enable foods to last longer (i.e. irradiation of fruits and vegetables stops the ripening process) and be contamination free [408], [409].
Used as a 'getter' to remove air traces in vacuum and cathode-ray tubes. Also used in producing photoelectric devices and atomic clocks. Since it ionizes readily, it is used as an ion rocket motor propellant.
Found in pollucite [(Cs4Al4Si9O26).H2O] and as trace in lepidolite.
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