Cesium

55 xenon ← caesium → barium Rb ↑ Cs ↓ Fr periodic table
General
Name, Symbol, Number	caesium, Cs, 55
Chemical series	alkali metals
Group, Period, Block	1, 6, s
Appearance	silvery gold
Atomic mass	132.9054519(2) g/mol
Electron configuration	[Xe] 6s1
Electrons per shell	2, 8, 18, 18, 8, 1
Physical properties
Phase	solid
Density (near r.t.)	1.93 g/cm³
Liquid density at m.p.	1.843 g/cm³
Melting point	301.59 K (28.44 °C, 83.19 °F)
Boiling point	944 K (671 °C, 1240 °F)
Critical point	1938 K, 9.4 MPa
Heat of fusion	2.09 kJ/mol
Heat of vaporization	63.9 kJ/mol
Heat capacity	(25 °C) 32.210 J/(mol·K)
Vapor pressure P/Pa 1 10 100 1 k 10 k 100 k at T/K 418 469 534 623 750 940
Atomic properties
Crystal structure	cubic body centered
Oxidation states	1 (strongly basic oxide)
Electronegativity	0.79 (Pauling scale)
Ionization energies	1st: 375.7 kJ/mol
	2nd: 2234.3 kJ/mol
	3rd: 3400 kJ/mol
Atomic radius	260 pm
Atomic radius (calc.)	298 pm
Covalent radius	225 pm
Miscellaneous
Magnetic ordering	no data
Electrical resistivity	(20 °C) 205 nΩ·m
Thermal conductivity	(300 K) 35.9 W/(m·K)
Thermal expansion	(25 °C) 97 µm/(m·K)
Speed of sound (thin rod)	(r.t.) 1.7 m/s
Bulk modulus	1.6 GPa
Mohs hardness	0.2
Brinell hardness	0.14 MPa
CAS registry number	7440-46-2
Notable isotopes
Main article: Isotopes of caesium iso NA half-life DM DE (MeV) DP 133Cs 100% Cs is stable with 78 neutrons 134Cs syn 65.159 Ms (2.0648y) ε 1.229 134Xe β- 2.059 134Ba 135Cs trace 73 Ts (2,300,000y) β- 0.269 135Ba 137Cs syn 948.9 Ms (30.07y) β- 1.176 137Ba

Cesium (also spelled caesium, chemical symbol Cs, atomic number 55) is a member of the group of chemical elements known as alkali metals. Soft and silvery gold in color, it readily liquefies at warm temperatures.

• It is most notably used in atomic clocks.

• It is one of metals that are liquid at or near room temperature: Rubidium (Mp: 38,89°C), Francium (Mp: 27°C), Mercury (Mp: -38,84°C), Gallium (Mp: 29,78°C) and Potassium (Mp: 63,65°C).

• caesium is the spelling used by the IUPAC, although since 1993 it has recognized cesium as a variant as well.

Discovery

Cesium (from the Latin word caesius, meaning "sky blue" or "heavenly blue") was discovered by Robert Bunsen and Gustav Kirchhoff in 1860, when they analyzed the spectrum of mineral water obtained from Dürkheim, Germany. They found two bright blue lines in the spectrum. It was the first element discovered by spectral analysis. Bunsen isolated cesium salts from the spring water, but the metal itself was isolated by Setterberg in 1881.

• Historically, the most important use for caesium has been in research and development, primarily in chemical and electrical applications.

Notable characteristics

The electromagnetic spectrum of caesium has two bright lines in the blue part of the spectrum along with several other lines in the red, yellow, and green. This metal is silvery gold in color and is both soft and ductile. Caesium is also the most electropositive and most alkaline of the stable chemical elements and also has the lowest ionization potential of all the elements, except for francium. Caesium is the least abundant of the five non-radioactive alkali metals. (Technically, francium is the least common alkali metal, but since it is highly radioactive with an estimated 340 to 550 grams in the entire earth at one time, its abundance can be considered zero in practical terms.)

Along with gallium, francium 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 −116°C. Caesium hydroxide (CsOH) is a very strong base and will rapidly etch the surface of glass.

CsOH is often stated to be a "strongest base". That is not correct. Although Caesium might be a strongest inorganic base (after FrOH), it is certainly not *the* strongest base. There are a number of organic compounds that act as a base. For instance, a hexane - cyclic molecule consisted of six C and twelve H atoms is incredibly strong base (pKa value: 52).

There is an account that caesium, reacting with fluorine, takes up more fluorine than it stoichometrically should. It is possible that, after the salt Cs⁺F⁻ has formed, the Cs⁺ ion, which has the same electronic structure as elemental xenon, can like xenon be oxidised further by fluorine and form traces of a higher fluoride such as CsF₃, analogous to XeF₂.

Applications

Caesium is most notably used in atomic clocks, which are accurate to seconds in many thousands of years. Since 1967, the International System of Measurements bases its unit of time, the second, on the properties of caesium. SI defines the second as 9,192,631,770 cycles of the radiation which corresponds to the transition between two energy levels of the ground state of the ¹³³Cs atom.

• 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 group 1 elements, 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.
• In addition, 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 nucleic acids from biological samples.
• More recently this metal has been used in ion propulsion systems.
• Cesium-137 is an extremely common isotope in industrial applications such as:
  • moisture density gauges
  • leveling gauges
  • thickness gauges
  • well-logging devices (used to measure the thickness of rock-strata)

Occurrence

Pollucite, a caesium mineral

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 located 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 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 its chloride and its nitrate. The price of caesium in 1997 was about $US 30 per gram.

See also Caesium minerals.

Isotopes

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 the largest number of isotopes, it has only one naturally occurring stable isotope, ¹³³Cs, the other isotopes (except for the isotopes noted on this page) 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 notably from the 1986 Chernobyl meltdown. Beginning in 1945 with the commencement of nuclear testing, ¹³⁷Cs was released into the atmosphere where it is 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 can be estimated as a function of time. Cesium-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.

Precautions

All alkaline metals are highly reactive. Caesium, being one of the heavier alkaline metals, is also one of the most reactive and is highly explosive when it comes in contact with water (even cold water, or ice). Caesium hydroxide is an extremely strong base, and can attack glass.

Caesium compounds are encountered rarely by most people. 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.

See also

• Cs-137
• Goiânia accident - a major radioactive contamination incident involving a small rod of caesium chloride.
• Caesium compounds

References

ISBN links support NWE through referral fees

• Los Alamos National Laboratory - Cesium

External links

• Video of alkaline metals reacting with water
• WebElements.com – Caesium
• FAQ from alt.cesium newsgroup

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