Periodic Table

Cesium

Alkali Metal

Quick Facts about Cesium

Xe
  • solid- state of matter at room temperature
  • Stable- has at least one stable isotope
  • +1- common oxidation states in compounds
  • BCC- crystal structure, atomic arrangement in solid form
Ba

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.

Why Cesium Matters

The element that defines time itself—and explodes in water

In Your Home

  • Your phone/computer time syncs to cesium atomic clocks via GPS satellites
  • Night vision devices may use cesium-based photocathodes

Industry Uses

TimekeepingCesium-133 oscillations define the SI second (9,192,631,770 Hz)
Oil & GasCesium formate drilling fluids—densest aqueous solution available
SpaceIon thrusters use cesium or xenon for spacecraft propulsion
MedicalCs-131 brachytherapy seeds for prostate cancer treatment

In Your Body

✗ Not essential

Cesium has no known biological role. Behaves like potassium in the body. Cesium-137 contamination persists for decades.

Safety: Radioactive cesium-137 from nuclear accidents is dangerous

Discovery of Cesium

Discovered by Gustov Kirchoff, Robert Bunsen in Germany, 1860

Name origin: Latin: coesius (sky blue); for the blue lines of its spectrum.

History & Events

1860
Named from Latin 'caesius' meaning sky blue
1860
First element discovered by spectroscopy (1860)
1860
Discovered by Bunsen and Kirchhoff
1967
Defines the SI second since 1967

About Cesium

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.

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

Physical Properties of Cs

Phase (STP)
solid
Melting Point of Cs
301.70 K
Boiling Point of Cs
944.00 K
Density of Cs
1.9300 g/cm3

Thermal Properties

Heat of Fusion
2.09 kJ/mol
Heat of Vaporization
68.30 kJ/mol
Specific Heat
0.24 J/g·K
Molar Heat Capacity
32.21 J/mol·K
Thermal Conductivity
35.90 W/m·K

Atomic Radii

Calculated
260 pm
Covalent
232 pm
Van der Waals
343 pm
Metallic
235 pm

Common Misconceptions

Wrong:Cesium is blue like its name suggests.
Correct:The metal is silvery-gold. 'Caesius' (sky blue) refers to the blue spectral lines Bunsen and Kirchhoff used to discover it.
Wrong:Atomic clocks contain dangerous amounts of cesium.
Correct:Cesium atomic clocks use tiny amounts of stable Cs-133, not radioactive Cs-137. They're safe laboratory instruments.
Wrong:Cesium-137 contamination comes from cesium mining.
Correct:Cs-137 is a nuclear fission product—it doesn't exist in nature. Chernobyl and Fukushima spread it; it persists for ~30 years (half-life).

Isotopes of Cesium

Cesium has 1 naturally occurring isotope, plus 1 notable radioactive isotope.

IsotopeAtomic Mass (u)AbundanceHalf-LifeDecay Mode
13355Cs (Cs-133)Cesium-133 isotope132.905452100.00%
13755Cs (Cs-137)Cesium-137 isotope136.90708960%30.17 yearsβ⁻

Data source: NIH PubChem (aggregated from IUPAC, NIST)

Isotope Applications

Isotopes of Cesium have important real-world applications in science and industry.

Geochronology & Dating

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].

Industrial Applications

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].

Abundance

Earth's Crust
3.0 mg/kg
Seawater
3.00×10-4 mg/L

Uses

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.

Sources

Found in pollucite [(Cs4Al4Si9O26).H2O] and as trace in lepidolite.

Geochemistry

Goldschmidt
litophile
Geochemical Class
alkali metal

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