is the chemical element
with the symbol Cs
and atomic number
55. It is a soft, silvery-gold alkali metal
with a melting point of , which makes it one of only five metals
that are liquid at or near room temperature
. Caesium is most notably used in atomic clocks
Caesium is the international spelling standardized by the IUPAC, but in North American English, the spelling cesium is more common.
The emission spectrum of caesium has two bright lines in the blue area of the spectrum along with several other lines in the red, yellow, and green areas. This metal is silvery gold in color and is both soft and ductile. Caesium is the second most electropositive and alkaline of the chemical elements and has the second lowest ionization potential (after francium). Caesium is the least abundant of the five non-radioactive alkali metals (francium is the least common alkali metal, but since it is highly radioactive with an estimated 30 grams in the entire Earth's crust at one time, its abundance can be considered zero in practical terms).
Along with gallium, francium, rubidium, and mercury, caesium is among the only metals that are liquid at or near room temperature. Caesium reacts explosively in cold water and also reacts with ice at temperatures above , 157 K).
Caesium hydroxide (CsOH) is a very strong base and will rapidly etch the surface of glass. CsOH is often stated to be the "strongest base", but in fact many compounds such as n-butyllithium and sodium amide are stronger.
Probably the most widespread use of caesium today is in caesium formate
-based drilling fluids
for the oil industry. The high density of the caesium formate brine (up to 2.3 sg
), coupled with the relatively benign nature of 133
Cs , reduces the requirement for toxic high-density suspended solids in the drilling fluid, which is a significant technological, engineering and environmental advantage.
Caesium is also used in atomic clocks
, which are accurate to seconds over many thousands of years. Since 1967, the International System of Measurements
has based its unit of time
, the second
, on the properties of caesium. The International System of Units
(SI) defines the second
as 9,192,631,770 cycles of the radiation
, which corresponds to the transition between two hyperfine energy levels
of the ground state
of the 133
- 134Cs has been used in hydrology as a measure of caesium output by the nuclear power industry. This isotope is used because, while it is less prevalent than either 133Cs or 137Cs, 134Cs can be produced solely by nuclear reactions. 135Cs has also been used in this function.
- Like other elements of group 1, caesium has a great affinity for oxygen and is used as a "getter" in vacuum tubes.
- This metal is also used in photoelectric cells due to its ready emission of electrons.
- Caesium was used as a propellant in early ion engines. It used a method of ionization to strip the outer electron from the propellant by simple contact with tungsten. Caesium use as a propellant was discontinued when Hughes Research Laboratory conducted a study finding xenon gas as a suitable replacement.
- Caesium is used as a catalyst in the hydrogenation of certain organic compounds.
- Radioactive isotopes of caesium are used in the medical field to treat certain types of cancer.
- Caesium fluoride is widely used in organic chemistry as a base and as a source of anhydrous fluoride ion.
- Caesium vapor is used in many common magnetometers.
- Because of their high density, caesium chloride solutions are commonly used in molecular biology for density gradient ultracentrifugation, primarily for the isolation of viral particles, subcellular organelles and fractions, and nucleic acids from biological samples.
- Caesium nitrate is used as an oxidizer to burn silicon in infrared flares such as the LUU-19 flare, because it emits much of its light in the near infrared spectrum.
- Caesium-137 is an extremely common radioisotope used as a gamma-emitter in industrial applications such as:
- moisture density gauges
- leveling gauges
- thickness gauges
- well-logging devices which are used to measure the electron density, which is analogous to the bulk density, of the rock formations.
- Caesium is also used as an internal standard in spectrophotometry.
- Caesium has been used to reduce the radar signature of exhaust plumes in military aircraft.
Caesium (Latin caesius
meaning "blueish grey") was spectroscopically
discovered by Robert Bunsen
and Gustav Kirchhoff
in 1860 in mineral water
. The residues of 44000 liters of mineral water yielded several grams of caesium salt for further analysis. Its identification was based upon the bright blue lines in its spectrum and it was the first element discovered by spectrum analysis
. The first caesium metal was produced in 1882 by electrolysis of caesium chloride by Carl Setterberg. Setterberg received his PhD from Kekule
and Bunsen for this work. Historically, the most important use for caesium has been in research and development, primarily in chemical and electrical applications.
An alkali metal, caesium occurs in lepidolite, pollucite (hydrated silicate of aluminium and caesium) and within other sources. One of the world's most significant and rich sources of this metal is at Bernic Lake in Manitoba. The deposits there are estimated to contain 300,000 metric tons of pollucite at an average of 20% caesium.
It can be isolated by electrolysis of fused caesium cyanide and in a number of other ways.
Exceptionally pure and gas-free caesium can be made by the thermal decomposition of caesium azide.
The primary compounds of caesium are caesium chloride and its nitrate. The price of caesium metal in 1997 was about US$30 per gram, but its compounds are much cheaper. See also Caesium minerals.
Caesium has at least 39 known isotopes, which is more than any other element except francium. The atomic masses of these isotopes range from 112 to 151. Even though this element has a large number of isotopes, it has only one naturally occurring stable isotope, 133Cs. Most of the other isotopes have half-lives from a few days to fractions of a second. The radiogenic isotope 137Cs has been used in hydrologic studies, analogous to the use of 3H. 137Cs is produced from the detonation of nuclear weapons and is produced in nuclear power plants, and was released to the atmosphere most notably from the 1986 Chernobyl meltdown.
This isotope (137Cs) is one of the numerous products of fission, directly issued from the fission of uranium.
Beginning in 1945 with the commencement of nuclear testing, 137Cs was released into the atmosphere where it is not absorbed readily into solution and is returned to the surface of the earth as a component of radioactive fallout. Once 137Cs enters the ground water, it is deposited on soil surfaces and removed from the landscape primarily by particle transport. As a result, the input function of these isotopes cannot be estimated as a function of time. Caesium-137 has a half-life of 30.17 years. It decomposes to barium-137m (a short-lived product of decay) then to a form of nonradioactive barium.
All alkali metals are highly reactive. Caesium, being one of the heavier alkali metals
, is also one of the most reactive and is highly explosive
when it comes in contact with water
. The hydrogen gas produced by the reaction is heated by the thermal energy released at the same time, causing ignition and a violent explosion (the same as all alkali metals) - but caesium is so reactive that this explosive reaction can even be triggered by cold water or ice.
Caesium is highly pyrophoric and ignites spontaneously in air to form caesium hydroxide and various oxides.
Caesium hydroxide is an extremely strong base, and can etch glass.
Caesium compounds are rarely encountered by most persons. All caesium compounds should be regarded as mildly toxic because of its chemical similarity to potassium. Large amounts cause hyperirritability and spasms, but such amounts would not ordinarily be encountered in natural sources, so Cs is not a major chemical environmental pollutant. Rats fed caesium in place of potassium in their diet die, so this element cannot replace potassium in function.
The isotopes 134Cs and 137Cs (present in the biosphere in small amounts as a result of radiation leaks) represent a radioactivity burden which varies depending on location. Radiocaesium does not accumulate in the body as effectively as many other fission products (such as radioiodine and radiostrontium), which are actively accumulated by the body.