Tritium Facts (Hydrogen Isotope)

A neutral tritium atom contains one proton, two neutrons, and one electron.
A neutral tritium atom contains one proton, two neutrons, and one electron.

Tritium is the radioactive isotope of the element hydrogen. It is also known as hydrogen-3 or using the shorthand notation T or 3H in chemical formulas and reactions. The nucleus of the tritium atom, called a triton, contains one proton and two neutrons. The word tritium comes from the Greek word tritos, which means “third.”


Ernest Rutherford, Mark Oliphant, and Paul Harteck were the first to produce tritium. They obtained the isotope in 1934 from a sample of deuterium. However, they were unable to isolate it. Luis Alvarez and Robert Cornog isolated tritium and documented its radioactivity in 1939.

Tritium Radioactivity

The other two isotopes of hydrogen, protium and deuterium, are not radioactive. Tritium has a half life of about 4500 days (12.32 years) and undergoes beta decay to form helium 3. The decay is one example of transmutation of one element into another. The reaction is represented by the reaction:

→ 3


The process releases 18.6 keV of energy. The beta particles released by the decay can pass through about 6 millimeters of air, but cannot penetrate human skin.

Tritium Properties

Like protium and deuterium, tritium has the atomic number 1 for hydrogen. Its usual oxidation state is +1. However, its atomic mass is 3.0160492. Tritium bonds with itself or other hydrogen isotopes to form T2 or H2 gas. It combines with oxygen to form a type of heavy water called tritiated water (T2O).

Health Effects

Because it is a low energy beta emitter, tritium poses no danger to humans or animals externally. However, it poses a radiation hazard when inhaled, injected, ingested, or absorbed through the skin. The main health risk associated with beta exposure is an increased risk of cancer. But, hydrogen atoms have a high turnover rate, so half of a tritium exposure is flushed out within 7 to 14 days.

Pure tritiated water is unsafe to drink not only because of the radiation hazard, but also because tritium is much larger than protium and tritiated water is denser than ordinary wate. In a nutshell, it disrupts biochemical reactions. The miniscule natural occurrence of tritium in natural water poses no health risk. However, tritium leaked from nuclear sites and improperly disposed lighting can contaminate water. Several countries have legal limits for tritium in drinking water. In the United States, the limit is 740 Bg/l or a dose of 4.0 millirems per year.

Tritium Uses

Tritium vials mark the hours and hands of this watch. (Autopilot)
Tritium vials mark the hours and hands of this watch. (Autopilot)

Tritium has several uses. It is used as a radioluminescent light for watches, gun sights, and various instruments. Glowing tritium vials contain the gas and a phosphor coating to produce a colored glow for jewelry and keychains. The isotope is a valuable radioactive tracer. Tritium is used for radiocarbon dating of water and wine. Along with deuterium, tritium is used in nuclear weapons and energy production.

Tritium Sources

Tritium occurs naturally and it is synthesized. On Earth, natural tritium is very rare. It forms when cosmic rays interact with nitrogen in the atmosphere to produce carbon-12 and a tritium atom.

There are several methods used to synthesize tritium. In heavy water-moderators reactors, tritium forms when deuterium captures a neutron. It forms in nuclear reactors via neutron activation of lithium-6. Neutron irradiation of boron-10 produces a small amount of tritium. Nuclear fission of uranium-235, uranium-233, and plutonium-239 produce tritium at a rate of about one atom per 10,000 fission events.


  • Alvarez, Luis; Cornog, Robert (1939). “Helium and Hydrogen of Mass 3”. Physical Review. 56 (6): 613. doi:10.1103/PhysRev.56.613
  • Kaufman, Sheldon; Libby, W. (1954). “The Natural Distribution of Tritium”. Physical Review. 93 (6): 1337. doi:10.1103/PhysRev.93.1337
  • Lucas, L. L. & Unterweger, M. P. (2000). “Comprehensive Review and Critical Evaluation of the Half-Life of Tritium”. Journal of Research of the National Institute of Standards and Technology. 105 (4): 541. doi:10.6028/jres.105.043
  • Oliphant, M. L.; Harteck, P.; Rutherford (1934). “Transmutation Effects observed with Heavy Hydrogen”. Nature. 133 (3359): 413. doi:10.1038/133413a0