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Definition: helium from Dictionary of Energy

Chemistry. a gaseous element having the symbol He, the atomic number 2, an atomic weight of 4.002 6 (only hydrogen is lighter), and a boiling point of -268.9°C; it is colorless, odorless, tasteless, and noncombustible. It occurs on earth in natural gas and makes up a small fraction of the atmosphere, and is abundant elsewhere in the universe. Used for filling balloons, as a protective gas in growing silicon, as a coolant for nuclear reactors, in cryogenic applications, and as a rocket fuel.

Summary Article: helium from The Columbia Encyclopedia

(hē'lēəm), gaseous chemical element; symbol He; at. no. 2; at. wt. 4.0026; m.p. below -272 degrees Celsius at 26 atmospheres pressure; b.p. -268.934 degrees Celsius at 1 atmosphere pressure; density 0.1785 grams per liter at STP; valence usually 0.

Properties and Isotopes

Helium is less dense than any other known gas except hydrogen and is about one seventh as dense as air. Extremely unreactive, it is an inert gas in Group 18 of the periodic table. Natural helium is a mixture of two stable isotopes, helium-3 and helium-4. In helium obtained from natural gas about one atom in 10 million is helium-3. The unstable isotopes helium-5, helium-6, and helium-8 have been synthesized. The alpha particles that are emitted from certain radioactive substances are identical to helium-4 nuclei (two protons and two neutrons).

Helium-4 is unusual in that it forms two different kinds of liquids. When it is cooled below 4.22 degrees Kelvin (its boiling point at atmospheric pressure) it condenses to liquid helium-I, which behaves as an ordinary liquid. When liquid helium-I is cooled below about 2.18 degrees Kelvin (at atmospheric pressure), liquid helium-II is formed. Liquid helium-II has a number of unusual properties. It is sometimes called a superfluid because it has extremely low viscosity. It also has extremely high heat conductivity and expands on cooling. It cannot be contained in an open beaker since a thin film of it creeps up the side, over the lip, and flows down the outside. The study of these phenomena is a part of low-temperature physics. When helium-3 is liquefied and cooled it does not exhibit the properties of liquid helium-II; this difference in properties between helium-3 and helium-4 can be explained in terms of quantum mechanics.

Natural Occurrence and Preparation

Helium is rare and costly. Wells in Texas (where the Federal Helium Reserve was established in 1925 near Amarillo), Oklahoma, and Kansas are the principal world source. Crude helium is separated by liquefying the other gases present in the natural gas; it is then either further purified or stored for later purification and use. Some helium is extracted directly from the atmosphere; the gas is also found in certain uranium minerals and in some mineral waters, but not in economic quantities. It has been estimated that helium makes up only about 0.000001% of the combined weight of the earth's atmosphere and crust; it is most concentrated in the exosphere, which is the outermost region of the atmosphere, 600–1500 mi (960–2400 km) above the earth's surface. Helium is abundant in outer space; it makes up about 23% of the mass of the visible universe. It is the end product of energy-releasing fusion processes in stars (see interstellar matter).


Helium's noncombustibility and buoyancy (second only to hydrogen) make it the most suitable gas for balloons and other lighter-than-air craft. A mixture of helium and oxygen is often supplied as a breathing mixture for deep-sea divers and caisson workers and is used in decompression chambers; because helium is less soluble in human blood than nitrogen, its use reduces the risk of caisson disease, or the "bends." Helium can also be used wherever an unreactive atmosphere is needed, e.g., in electric arc welding, in growing crystals of silicon and germanium for semiconductors, and in refining titanium and zirconium metals. It is also used to pressurize the fuel tanks of liquid-fueled rockets. Liquid helium is essential for many low temperature applications (see low-temperature physics).

The Columbia Encyclopedia, © Columbia University Press 2017

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