Гелий химический элемент как пишется

Helium, ₂He

Helium
Pronunciation	​(HEE-lee-əm)
Appearance	colorless gas, exhibiting a gray, cloudy glow (or reddish-orange if an especially high voltage is used) when placed in an electric field
Standard atomic weight Ar°(He)	4.002602±0.000002 4.0026±0.0001 (abridged)[1]
Helium in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ He ↓ Ne hydrogen ← helium → lithium
Atomic number (Z)	2
Group	group 18 (noble gases)
Period	period 1
Block	s-block
Electron configuration	1s2
Electrons per shell	2
Physical properties
Phase at STP	gas
Melting point	0.95 K ​(−272.20 °C, ​−457.96 °F) (at 2.5 MPa)
Boiling point	4.222 K ​(−268.928 °C, ​−452.070 °F)
Density (at STP)	0.1786 g/L
when liquid (at m.p.)	0.145 g/cm3
when liquid (at b.p.)	0.125 g/cm3
Triple point	2.177 K, ​5.043 kPa
Critical point	5.1953 K, 0.22746 MPa
Heat of fusion	0.0138 kJ/mol
Heat of vaporization	0.0829 kJ/mol
Molar heat capacity	20.78 J/(mol·K)[2]
Vapor pressure (defined by ITS-90) P (Pa) 1 10 100 1 k 10 k 100 k at T (K)     1.23 1.67 2.48 4.21
Atomic properties
Oxidation states	0
Electronegativity	Pauling scale: no data
Ionization energies	1st: 2372.3 kJ/mol 2nd: 5250.5 kJ/mol
Covalent radius	28 pm
Van der Waals radius	140 pm
Spectral lines of helium
Other properties
Natural occurrence	primordial
Crystal structure	​hexagonal close-packed (hcp)
Speed of sound	972 m/s
Thermal conductivity	0.1513 W/(m⋅K)
Magnetic ordering	diamagnetic[3]
Molar magnetic susceptibility	−1.88×10−6 cm3/mol (298 K)[4]
CAS Number	7440-59-7
History
Naming	after Helios, Greek god of the Sun
Discovery	Pierre Janssen, Norman Lockyer (1868)
First isolation	William Ramsay, Per Teodor Cleve, Abraham Langlet (1895)
Main isotopes of helium v e
Iso­tope Decay abun­dance half-life (t1/2) mode pro­duct 3He 0.0002(2)% stable 4He 99.9998(2)% stable
Category: Helium view talk edit | references

Helium (from Greek: ἥλιος, romanized: helios, lit. ‘sun’) is a chemical element with the symbol He and atomic number 2. It is a colorless, odorless, tasteless, non-toxic, inert, monatomic gas and the first in the noble gas group in the periodic table.^[a] Its boiling and melting point are the lowest among all the elements. It is the second lightest and second most abundant element in the observable universe, after hydrogen. It is present at about 24% of the total elemental mass, which is more than 12 times the mass of all the heavier elements combined. Its abundance is similar to this in both the Sun and in Jupiter, due to the very high nuclear binding energy (per nucleon) of helium-4, with respect to the next three elements after helium. This helium-4 binding energy also accounts for why it is a product of both nuclear fusion and radioactive decay. The most common isotope of helium in the universe is helium-4, the vast majority of which was formed during the Big Bang. Large amounts of new helium are created by nuclear fusion of hydrogen in stars.

Helium was first detected as an unknown, yellow spectral line signature in sunlight during a solar eclipse in 1868 by Georges Rayet,^[11] Captain C. T. Haig,^[12] Norman R. Pogson,^[13] and Lieutenant John Herschel,^[14] and was subsequently confirmed by French astronomer Jules Janssen.^[15] Janssen is often jointly credited with detecting the element, along with Norman Lockyer. Janssen recorded the helium spectral line during the solar eclipse of 1868, while Lockyer observed it from Britain. Lockyer was the first to propose that the line was due to a new element, which he named. The formal discovery of the element was made in 1895 by chemists Sir William Ramsay, Per Teodor Cleve, and Nils Abraham Langlet, who found helium emanating from the uranium ore, cleveite, which is now not regarded as a separate mineral species, but as a variety of uraninite.^[16][17] In 1903, large reserves of helium were found in natural gas fields in parts of the United States, by far the largest supplier of the gas today.

Liquid helium is used in cryogenics (its largest single use, absorbing about a quarter of production), and in the cooling of superconducting magnets, with its main commercial application in MRI scanners. Helium’s other industrial uses—as a pressurizing and purge gas, as a protective atmosphere for arc welding, and in processes such as growing crystals to make silicon wafers—account for half of the gas produced. A well-known but minor use is as a lifting gas in balloons and airships.^[18] As with any gas whose density differs from that of air, inhaling a small volume of helium temporarily changes the timbre and quality of the human voice. In scientific research, the behavior of the two fluid phases of helium-4 (helium I and helium II) is important to researchers studying quantum mechanics (in particular the property of superfluidity) and to those looking at the phenomena, such as superconductivity, produced in matter near absolute zero.

On Earth, it is relatively rare—5.2 ppm by volume in the atmosphere. Most terrestrial helium present today is created by the natural radioactive decay of heavy radioactive elements (thorium and uranium, although there are other examples), as the alpha particles emitted by such decays consist of helium-4 nuclei. This radiogenic helium is trapped with natural gas in concentrations as great as 7% by volume, from which it is extracted commercially by a low-temperature separation process called fractional distillation. Terrestrial helium is a non-renewable resource because once released into the atmosphere, it promptly escapes into space. Its supply is thought to be rapidly diminishing.^[19][20] However, some studies suggest that helium produced deep in the earth by radioactive decay can collect in natural gas reserves in larger than expected quantities,^[21] in some cases, having been released by volcanic activity.^[22]

History

Scientific discoveries

The first evidence of helium was observed on August 18, 1868, as a bright yellow line with a wavelength of 587.49 nanometers in the spectrum of the chromosphere of the Sun. The line was detected by French astronomer Jules Janssen during a total solar eclipse in Guntur, India.^[23][24] This line was initially assumed to be sodium. On October 20 of the same year, English astronomer, Norman Lockyer, observed a yellow line in the solar spectrum, which, he named the D₃ because it was near the known D₁ and D₂ Fraunhofer line lines of sodium.^[25][26] He concluded that it was caused by an element in the Sun unknown on Earth. Lockyer and English chemist Edward Frankland named the element with the Greek word for the Sun, ἥλιος (helios).^[27][28]

In 1881, Italian physicist Luigi Palmieri detected helium on Earth for the first time through its D₃ spectral line, when he analyzed a material that had been sublimated during a recent eruption of Mount Vesuvius.^[29]

On March 26, 1895, Scottish chemist Sir William Ramsay isolated helium on Earth by treating the mineral cleveite (a variety of uraninite with at least 10% rare-earth elements) with mineral acids. Ramsay was looking for argon but, after separating nitrogen and oxygen from the gas, liberated by sulfuric acid, he noticed a bright yellow line that matched the D₃ line observed in the spectrum of the Sun.^{[26][31][32][33]} These samples were identified as helium by Lockyer and British physicist William Crookes.^[34][35] It was independently isolated from cleveite, in the same year, by chemists, Per Teodor Cleve and Abraham Langlet, in Uppsala, Sweden, who collected enough of the gas to accurately determine its atomic weight.^{[36][37][24][38]} Helium was also isolated by the American geochemist, William Francis Hillebrand, prior to Ramsay’s discovery, when he noticed unusual spectral lines while testing a sample of the mineral uraninite. Hillebrand, however, attributed the lines to nitrogen.^[39] His letter of congratulations to Ramsay offers an interesting case of discovery, and near-discovery, in science.^[40]

In 1907, Ernest Rutherford and Thomas Royds demonstrated that alpha particles are helium nuclei, by allowing the particles to penetrate the thin, glass wall of an evacuated tube, then creating a discharge in the tube, to study the spectrum of the new gas inside.^[41] In 1908, helium was first liquefied by Dutch physicist Heike Kamerlingh Onnes by cooling the gas to less than 5 K (−268.15 °C; −450.67 °F).^[42][43] He tried to solidify it, by further reducing the temperature, but failed, because helium does not solidify at atmospheric pressure. Onnes’ student Willem Hendrik Keesom was eventually able to solidify 1 cm³ of helium in 1926 by applying additional external pressure.^[44][45]

In 1913, Niels Bohr published his «trilogy»^[46][47] on atomic structure that included a reconsideration of the Pickering–Fowler series as central evidence in support of his model of the atom.^[48][49] This series is named for Edward Charles Pickering, who in 1896 published observations of previously unknown lines in the spectrum of the star ζ Puppis^[50] (these are now known to occur with Wolf–Rayet and other hot stars).^[51] Pickering attributed the observation (lines at 4551, 5411, and 10123 Å) to a new form of hydrogen with half-integer transition levels.^[52][53] In 1912, Alfred Fowler^[54] managed to produce similar lines from a hydrogen-helium mixture, and supported Pickering’s conclusion as to their origin.^[55] Bohr’s model does not allow for half-integer transitions (nor does quantum mechanics) and Bohr concluded that Pickering and Fowler were wrong, and instead assigned these spectral lines to ionised helium, He⁺.^[56] Fowler was initially skeptical^[57] but was ultimately convinced^[58] that Bohr was correct,^[46] and by 1915 «spectroscopists had transferred [the Pickering–Fowler series] definitively [from hydrogen] to helium.»^[49][59] Bohr’s theoretical work on the Pickering series had demonstrated the need for «a re-examination of problems that seemed already to have been solved within classical theories» and provided important confirmation for his atomic theory.^[49]

In 1938, Russian physicist Pyotr Leonidovich Kapitsa discovered that helium-4 has almost no viscosity at temperatures near absolute zero, a phenomenon now called superfluidity.^[60] This phenomenon is related to Bose–Einstein condensation. In 1972, the same phenomenon was observed in helium-3, but at temperatures much closer to absolute zero, by American physicists Douglas D. Osheroff, David M. Lee, and Robert C. Richardson. The phenomenon in helium-3 is thought to be related to pairing of helium-3 fermions to make bosons, in analogy to Cooper pairs of electrons producing superconductivity.^[61]

Extraction and use

After an oil drilling operation in 1903 in Dexter, Kansas produced a gas geyser that would not burn, Kansas state geologist Erasmus Haworth collected samples of the escaping gas and took them back to the University of Kansas at Lawrence where, with the help of chemists Hamilton Cady and David McFarland, he discovered that the gas consisted of, by volume, 72% nitrogen, 15% methane (a combustible percentage only with sufficient oxygen), 1% hydrogen, and 12% an unidentifiable gas.^[24][62] With further analysis, Cady and McFarland discovered that 1.84% of the gas sample was helium.^[63][64] This showed that despite its overall rarity on Earth, helium was concentrated in large quantities under the American Great Plains, available for extraction as a byproduct of natural gas.^[65]

This enabled the United States to become the world’s leading supplier of helium. Following a suggestion by Sir Richard Threlfall, the United States Navy sponsored three small experimental helium plants during World War I. The goal was to supply barrage balloons with the non-flammable, lighter-than-air gas. A total of 5,700 m³ (200,000 cu ft) of 92% helium was produced in the program even though less than a cubic meter of the gas had previously been obtained.^[26] Some of this gas was used in the world’s first helium-filled airship, the U.S. Navy’s C-class blimp C-7, which flew its maiden voyage from Hampton Roads, Virginia, to Bolling Field in Washington, D.C., on December 1, 1921,^[66] nearly two years before the Navy’s first rigid helium-filled airship, the Naval Aircraft Factory-built USS Shenandoah, flew in September 1923.

Although the extraction process using low-temperature gas liquefaction was not developed in time to be significant during World War I, production continued. Helium was primarily used as a lifting gas in lighter-than-air craft. During World War II, the demand increased for helium for lifting gas and for shielded arc welding. The helium mass spectrometer was also vital in the atomic bomb Manhattan Project.^[67]

The government of the United States set up the National Helium Reserve in 1925 at Amarillo, Texas, with the goal of supplying military airships in time of war and commercial airships in peacetime.^[26] Because of the Helium Act of 1925, which banned the export of scarce helium on which the US then had a production monopoly, together with the prohibitive cost of the gas, the Hindenburg, like all German Zeppelins, was forced to use hydrogen as the lift gas. The helium market after World War II was depressed but the reserve was expanded in the 1950s to ensure a supply of liquid helium as a coolant to create oxygen/hydrogen rocket fuel (among other uses) during the Space Race and Cold War. Helium use in the United States in 1965 was more than eight times the peak wartime consumption.^[68]

After the «Helium Acts Amendments of 1960» (Public Law 86–777), the U.S. Bureau of Mines arranged for five private plants to recover helium from natural gas. For this helium conservation program, the Bureau built a 425-mile (684 km) pipeline from Bushton, Kansas, to connect those plants with the government’s partially depleted Cliffside gas field near Amarillo, Texas. This helium-nitrogen mixture was injected and stored in the Cliffside gas field until needed, at which time it was further purified.^[69]

By 1995, a billion cubic meters of the gas had been collected and the reserve was US$1.4 billion in debt, prompting the Congress of the United States in 1996 to phase out the reserve.^[24][70] The resulting Helium Privatization Act of 1996^[71] (Public Law 104–273) directed the United States Department of the Interior to empty the reserve, with sales starting by 2005.^[72]

Helium produced between 1930 and 1945 was about 98.3% pure (2% nitrogen), which was adequate for airships. In 1945, a small amount of 99.9% helium was produced for welding use. By 1949, commercial quantities of Grade A 99.95% helium were available.^[73]

For many years, the United States produced more than 90% of commercially usable helium in the world, while extraction plants in Canada, Poland, Russia, and other nations produced the remainder. In the mid-1990s, a new plant in Arzew, Algeria, producing 17 million cubic meters (600 million cubic feet) began operation, with enough production to cover all of Europe’s demand. Meanwhile, by 2000, the consumption of helium within the U.S. had risen to more than 15 million kg per year.^[74] In 2004–2006, additional plants in Ras Laffan, Qatar, and Skikda, Algeria were built. Algeria quickly became the second leading producer of helium.^[75] Through this time, both helium consumption and the costs of producing helium increased.^[76] From 2002 to 2007 helium prices doubled.^[77]

As of 2012, the United States National Helium Reserve accounted for 30 percent of the world’s helium.^[78] The reserve was expected to run out of helium in 2018.^[78] Despite that, a proposed bill in the United States Senate would allow the reserve to continue to sell the gas. Other large reserves were in the Hugoton in Kansas, United States, and nearby gas fields of Kansas and the panhandles of Texas and Oklahoma. New helium plants were scheduled to open in 2012 in Qatar, Russia, and the US state of Wyoming, but they were not expected to ease the shortage.^[78]

In 2013, Qatar started up the world’s largest helium unit,^[79] although the 2017 Qatar diplomatic crisis severely affected helium production there.^[80] 2014 was widely acknowledged to be a year of over-supply in the helium business, following years of renowned shortages.^[81] Nasdaq reported (2015) that for Air Products, an international corporation that sells gases for industrial use, helium volumes remain under economic pressure due to feedstock supply constraints.^[82]

Characteristics

Atom

In quantum mechanics

In the perspective of quantum mechanics, helium is the second simplest atom to model, following the hydrogen atom. Helium is composed of two electrons in atomic orbitals surrounding a nucleus containing two protons and (usually) two neutrons. As in Newtonian mechanics, no system that consists of more than two particles can be solved with an exact analytical mathematical approach (see 3-body problem) and helium is no exception. Thus, numerical mathematical methods are required, even to solve the system of one nucleus and two electrons. Such computational chemistry methods have been used to create a quantum mechanical picture of helium electron binding which is accurate to within < 2% of the correct value, in a few computational steps.^[83] Such models show that each electron in helium partly screens the nucleus from the other, so that the effective nuclear charge Z_eff which each electron sees is about 1.69 units, not the 2 charges of a classic «bare» helium nucleus.

Related stability of the helium-4 nucleus and electron shell

The nucleus of the helium-4 atom is identical with an alpha particle. High-energy electron-scattering experiments show its charge to decrease exponentially from a maximum at a central point, exactly as does the charge density of helium’s own electron cloud. This symmetry reflects similar underlying physics: the pair of neutrons and the pair of protons in helium’s nucleus obey the same quantum mechanical rules as do helium’s pair of electrons (although the nuclear particles are subject to a different nuclear binding potential), so that all these fermions fully occupy 1s orbitals in pairs, none of them possessing orbital angular momentum, and each cancelling the other’s intrinsic spin. Adding another of any of these particles would require angular momentum and would release substantially less energy (in fact, no nucleus with five nucleons is stable). This arrangement is thus energetically extremely stable for all these particles, and this stability accounts for many crucial facts regarding helium in nature.

For example, the stability and low energy of the electron cloud state in helium accounts for the element’s chemical inertness, and also the lack of interaction of helium atoms with each other, producing the lowest melting and boiling points of all the elements.

In a similar way, the particular energetic stability of the helium-4 nucleus, produced by similar effects, accounts for the ease of helium-4 production in atomic reactions that involve either heavy-particle emission or fusion. Some stable helium-3 (two protons and one neutron) is produced in fusion reactions from hydrogen, but it is a very small fraction compared to the highly favorable helium-4.

The unusual stability of the helium-4 nucleus is also important cosmologically: it explains the fact that in the first few minutes after the Big Bang, as the «soup» of free protons and neutrons which had initially been created in about 6:1 ratio cooled to the point that nuclear binding was possible, almost all first compound atomic nuclei to form were helium-4 nuclei. Owing to the relatively tight binding of helium-4 nuclei, its production consumed nearly all of the free neutrons in a few minutes, before they could beta-decay, and thus few neutrons were available to form heavier atoms such as lithium, beryllium, or boron. Helium-4 nuclear binding per nucleon is stronger than in any of these elements (see nucleogenesis and binding energy) and thus, once helium had been formed, no energetic drive was available to make elements 3, 4 and 5.^[84] It is barely energetically favorable for helium to fuse into the next element with a lower energy per nucleon, carbon. However, due to lack of intermediate elements, this process requires three helium nuclei striking each other nearly simultaneously (see triple alpha process). There was thus no time for significant carbon to be formed in the few minutes after the Big Bang, before the early expanding universe cooled to the temperature and pressure point where helium fusion to carbon was no longer possible. This left the early universe with a very similar ratio of hydrogen/helium as is observed today (3 parts hydrogen to 1 part helium-4 by mass), with nearly all the neutrons in the universe trapped in helium-4.

All heavier elements (including those necessary for rocky planets like the Earth, and for carbon-based or other life) have thus been created since the Big Bang in stars which were hot enough to fuse helium itself. All elements other than hydrogen and helium today account for only 2% of the mass of atomic matter in the universe. Helium-4, by contrast, makes up about 23% of the universe’s ordinary matter—nearly all the ordinary matter that is not hydrogen.

Gas and plasma phases

Helium is the second least reactive noble gas after neon, and thus the second least reactive of all elements.^[85] It is chemically inert and monatomic in all standard conditions. Because of helium’s relatively low molar (atomic) mass, its thermal conductivity, specific heat, and sound speed in the gas phase are all greater than any other gas except hydrogen. For these reasons and the small size of helium monatomic molecules, helium diffuses through solids at a rate three times that of air and around 65% that of hydrogen.^[26]

Helium is the least water-soluble monatomic gas,^[86] and one of the least water-soluble of any gas (CF₄, SF₆, and C₄F₈ have lower mole fraction solubilities: 0.3802, 0.4394, and 0.2372 x₂/10⁻⁵, respectively, versus helium’s 0.70797 x₂/10⁻⁵),^[87] and helium’s index of refraction is closer to unity than that of any other gas.^[88] Helium has a negative Joule–Thomson coefficient at normal ambient temperatures, meaning it heats up when allowed to freely expand. Only below its Joule–Thomson inversion temperature (of about 32 to 50 K at 1 atmosphere) does it cool upon free expansion.^[26] Once precooled below this temperature, helium can be liquefied through expansion cooling.

Most extraterrestrial helium is found in a plasma state, with properties quite different from those of atomic helium. In a plasma, helium’s electrons are not bound to its nucleus, resulting in very high electrical conductivity, even when the gas is only partially ionized. The charged particles are highly influenced by magnetic and electric fields. For example, in the solar wind together with ionized hydrogen, the particles interact with the Earth’s magnetosphere, giving rise to Birkeland currents and the aurora.^[89]

Liquid phase

Unlike any other element, helium will remain liquid down to absolute zero at normal pressures. This is a direct effect of quantum mechanics: specifically, the zero point energy of the system is too high to allow freezing. Solid helium requires a temperature of 1–1.5 K (about −272 °C or −457 °F) at about 25 bar (2.5 MPa) of pressure.^[90] It is often hard to distinguish solid from liquid helium since the refractive index of the two phases are nearly the same. The solid has a sharp melting point and has a crystalline structure, but it is highly compressible; applying pressure in a laboratory can decrease its volume by more than 30%.^[91] With a bulk modulus of about 27 MPa^[92] it is ~100 times more compressible than water. Solid helium has a density of 0.214±0.006 g/cm³ at 1.15 K and 66 atm; the projected density at 0 K and 25 bar (2.5 MPa) is 0.187±0.009 g/cm³.^[93] At higher temperatures, helium will solidify with sufficient pressure. At room temperature, this requires about 114,000 atm.^[94]

Helium I

Below its boiling point of 4.22 K (−268.93 °C; −452.07 °F) and above the lambda point of 2.1768 K (−270.9732 °C; −455.7518 °F), the isotope helium-4 exists in a normal colorless liquid state, called helium I.^[26] Like other cryogenic liquids, helium I boils when it is heated and contracts when its temperature is lowered. Below the lambda point, however, helium does not boil, and it expands as the temperature is lowered further.

Helium I has a gas-like index of refraction of 1.026 which makes its surface so hard to see that floats of Styrofoam are often used to show where the surface is.^[26] This colorless liquid has a very low viscosity and a density of 0.145–0.125 g/mL (between about 0 and 4 K),^[95] which is only one-fourth the value expected from classical physics.^[26] Quantum mechanics is needed to explain this property and thus both states of liquid helium (helium I and helium II) are called quantum fluids, meaning they display atomic properties on a macroscopic scale. This may be an effect of its boiling point being so close to absolute zero, preventing random molecular motion (thermal energy) from masking the atomic properties.^[26]

Helium II

Liquid helium below its lambda point (called helium II) exhibits very unusual characteristics. Due to its high thermal conductivity, when it boils, it does not bubble but rather evaporates directly from its surface. Helium-3 also has a superfluid phase, but only at much lower temperatures; as a result, less is known about the properties of the isotope.^[26]

Helium II is a superfluid, a quantum mechanical state (see: macroscopic quantum phenomena) of matter with strange properties. For example, when it flows through capillaries as thin as 10⁻⁷ to 10⁻⁸ m it has no measurable viscosity.^[24] However, when measurements were done between two moving discs, a viscosity comparable to that of gaseous helium was observed. Current theory explains this using the two-fluid model for helium II. In this model, liquid helium below the lambda point is viewed as containing a proportion of helium atoms in a ground state, which are superfluid and flow with exactly zero viscosity, and a proportion of helium atoms in an excited state, which behave more like an ordinary fluid.^[96]

In the fountain effect, a chamber is constructed which is connected to a reservoir of helium II by a sintered disc through which superfluid helium leaks easily but through which non-superfluid helium cannot pass. If the interior of the container is heated, the superfluid helium changes to non-superfluid helium. In order to maintain the equilibrium fraction of superfluid helium, superfluid helium leaks through and increases the pressure, causing liquid to fountain out of the container.^[97]

The thermal conductivity of helium II is greater than that of any other known substance, a million times that of helium I and several hundred times that of copper.^[26] This is because heat conduction occurs by an exceptional quantum mechanism. Most materials that conduct heat well have a valence band of free electrons which serve to transfer the heat. Helium II has no such valence band but nevertheless conducts heat well. The flow of heat is governed by equations that are similar to the wave equation used to characterize sound propagation in air. When heat is introduced, it moves at 20 meters per second at 1.8 K through helium II as waves in a phenomenon known as second sound.^[26]

Helium II also exhibits a creeping effect. When a surface extends past the level of helium II, the helium II moves along the surface, against the force of gravity. Helium II will escape from a vessel that is not sealed by creeping along the sides until it reaches a warmer region where it evaporates. It moves in a 30 nm-thick film regardless of surface material. This film is called a Rollin film and is named after the man who first characterized this trait, Bernard V. Rollin.^[26][98][99] As a result of this creeping behavior and helium II’s ability to leak rapidly through tiny openings, it is very difficult to confine. Unless the container is carefully constructed, the helium II will creep along the surfaces and through valves until it reaches somewhere warmer, where it will evaporate. Waves propagating across a Rollin film are governed by the same equation as gravity waves in shallow water, but rather than gravity, the restoring force is the van der Waals force.^[100] These waves are known as third sound.^[101]

Isotopes

There are nine known isotopes of helium, but only helium-3 and helium-4 are stable. In the Earth’s atmosphere, one atom is ³
He for every million that are ⁴
He.^[24] Unlike most elements, helium’s isotopic abundance varies greatly by origin, due to the different formation processes. The most common isotope, helium-4, is produced on Earth by alpha decay of heavier radioactive elements; the alpha particles that emerge are fully ionized helium-4 nuclei. Helium-4 is an unusually stable nucleus because its nucleons are arranged into complete shells. It was also formed in enormous quantities during Big Bang nucleosynthesis.^[102]

Helium-3 is present on Earth only in trace amounts. Most of it has been present since Earth’s formation, though some falls to Earth trapped in cosmic dust.^[103] Trace amounts are also produced by the beta decay of tritium.^[104] Rocks from the Earth’s crust have isotope ratios varying by as much as a factor of ten, and these ratios can be used to investigate the origin of rocks and the composition of the Earth’s mantle.^{[103] 3}
He is much more abundant in stars as a product of nuclear fusion. Thus in the interstellar medium, the proportion of ³
He to ⁴
He is about 100 times higher than on Earth.^[105] Extraplanetary material, such as lunar and asteroid regolith, have trace amounts of helium-3 from being bombarded by solar winds. The Moon’s surface contains helium-3 at concentrations on the order of 10 ppb, much higher than the approximately 5 ppt found in the Earth’s atmosphere.^[106][107] A number of people, starting with Gerald Kulcinski in 1986,^[108] have proposed to explore the moon, mine lunar regolith, and use the helium-3 for fusion.

Liquid helium-4 can be cooled to about 1 K (−272.15 °C; −457.87 °F) using evaporative cooling in a 1-K pot. Similar cooling of helium-3, which has a lower boiling point, can achieve about 0.2 kelvin in a helium-3 refrigerator. Equal mixtures of liquid ³
He and ⁴
He below 0.8 K separate into two immiscible phases due to their dissimilarity (they follow different quantum statistics: helium-4 atoms are bosons while helium-3 atoms are fermions).^[26] Dilution refrigerators use this immiscibility to achieve temperatures of a few millikelvins.^[109]

It is possible to produce exotic helium isotopes, which rapidly decay into other substances. The shortest-lived heavy helium isotope is the unbound helium-10 with a half-life of 2.6(4)×10⁻²² s.^[110] Helium-6 decays by emitting a beta particle and has a half-life of 0.8 second. Helium-7 also emits a beta particle as well as a gamma ray. Helium-7 and helium-8 are created in certain nuclear reactions.^[26] Helium-6 and helium-8 are known to exhibit a nuclear halo.^[26]

Properties

Table of thermal and physical properties of helium gas at atmospheric pressure:^[111][112]

Temperature (K)	Density (kg/m^3)	Specific heat (kJ/kg °C)	Dynamic viscosity (kg/m s)	Kinematic viscosity (m^2/s)	Thermal conductivity (W/m °C)	Thermal diffusivity (m^2/s)	Prandtl Number
100		5.193	9.63E-06	1.98E-05	0.073	2.89E-05	0.686
120	0.406	5.193	1.07E-05	2.64E-05	0.0819	3.88E-05	0.679
144	0.3379	5.193	1.26E-05	3.71E-05	0.0928	5.28E-05	0.7
200	0.2435	5.193	1.57E-05	6.44E-05	0.1177	9.29E-05	0.69
255	0.1906	5.193	1.82E-05	9.55E-05	0.1357	1.37E-04	0.7
366	0.1328	5.193	2.31E-05	1.74E-04	0.1691	2.45E-04	0.71
477	0.10204	5.193	2.75E-05	2.69E-04	0.197	3.72E-04	0.72
589	0.08282	5.193	3.11E-05	3.76E-04	0.225	5.22E-04	0.72
700	0.07032	5.193	3.48E-05	4.94E-04	0.251	6.66E-04	0.72
800	0.06023	5.193	3.82E-05	6.34E-04	0.275	8.77E-04	0.72
900	0.05451	5.193	4.14E-05	7.59E-04	0.33	1.14E-03	0.687
1000		5.193	4.46E-05	9.14E-04	0.354	1.40E-03	0.654

Compounds

Helium has a valence of zero and is chemically unreactive under all normal conditions.^[91] It is an electrical insulator unless ionized. As with the other noble gases, helium has metastable energy levels that allow it to remain ionized in an electrical discharge with a voltage below its ionization potential.^[26] Helium can form unstable compounds, known as excimers, with tungsten, iodine, fluorine, sulfur, and phosphorus when it is subjected to a glow discharge, to electron bombardment, or reduced to plasma by other means. The molecular compounds HeNe, HgHe₁₀, and WHe₂, and the molecular ions He⁺
₂, He²⁺
₂, HeH⁺
, and HeD⁺
have been created this way.^[113] HeH⁺ is also stable in its ground state, but is extremely reactive—it is the strongest Brønsted acid known, and therefore can exist only in isolation, as it will protonate any molecule or counteranion it contacts. This technique has also produced the neutral molecule He₂, which has a large number of band systems, and HgHe, which is apparently held together only by polarization forces.^[26]

Van der Waals compounds of helium can also be formed with cryogenic helium gas and atoms of some other substance, such as LiHe and He₂.^[114]

Theoretically, other true compounds may be possible, such as helium fluorohydride (HHeF) which would be analogous to HArF, discovered in 2000.^[115] Calculations show that two new compounds containing a helium-oxygen bond could be stable.^[116] Two new molecular species, predicted using theory, CsFHeO and N(CH₃)₄FHeO, are derivatives of a metastable FHeO⁻ anion first theorized in 2005 by a group from Taiwan. If confirmed by experiment, the only remaining element with no known stable compounds would be neon.^[117]

Helium atoms have been inserted into the hollow carbon cage molecules (the fullerenes) by heating under high pressure. The endohedral fullerene molecules formed are stable at high temperatures. When chemical derivatives of these fullerenes are formed, the helium stays inside.^[118] If helium-3 is used, it can be readily observed by helium nuclear magnetic resonance spectroscopy.^[119] Many fullerenes containing helium-3 have been reported. Although the helium atoms are not attached by covalent or ionic bonds, these substances have distinct properties and a definite composition, like all stoichiometric chemical compounds.

Under high pressures helium can form compounds with various other elements. Helium-nitrogen clathrate (He(N₂)₁₁) crystals have been grown at room temperature at pressures ca. 10 GPa in a diamond anvil cell.^[120] The insulating electride Na₂He has been shown to be thermodynamically stable at pressures above 113 GPa. It has a fluorite structure.^[121]

Occurrence and production

Natural abundance

Although it is rare on Earth, helium is the second most abundant element in the known Universe, constituting 23% of its baryonic mass. Only hydrogen is more abundant.^[24] The vast majority of helium was formed by Big Bang nucleosynthesis one to three minutes after the Big Bang. As such, measurements of its abundance contribute to cosmological models. In stars, it is formed by the nuclear fusion of hydrogen in proton–proton chain reactions and the CNO cycle, part of stellar nucleosynthesis.^[102]

In the Earth’s atmosphere, the concentration of helium by volume is only 5.2 parts per million.^[122][123] The concentration is low and fairly constant despite the continuous production of new helium because most helium in the Earth’s atmosphere escapes into space by several processes.^{[124][125][126]} In the Earth’s heterosphere, a part of the upper atmosphere, helium and other lighter gases are the most abundant elements.

Most helium on Earth is a result of radioactive decay. Helium is found in large amounts in minerals of uranium and thorium, including uraninite and its varieties cleveite and pitchblende,^[16][127] carnotite and monazite (a group name; «monazite» usually refers to monazite-(Ce)),^[128][129] because they emit alpha particles (helium nuclei, He²⁺) to which electrons immediately combine as soon as the particle is stopped by the rock. In this way an estimated 3000 metric tons of helium are generated per year throughout the lithosphere.^{[130][131][132]} In the Earth’s crust, the concentration of helium is 8 parts per billion. In seawater, the concentration is only 4 parts per trillion. There are also small amounts in mineral springs, volcanic gas, and meteoric iron. Because helium is trapped in the subsurface under conditions that also trap natural gas, the greatest natural concentrations of helium on the planet are found in natural gas, from which most commercial helium is extracted. The concentration varies in a broad range from a few ppm to more than 7% in a small gas field in San Juan County, New Mexico.^[133][134]

As of 2021 the world’s helium reserves were estimated at 31 billion cubic meters, with a third of that being in Qatar.^[135] In 2015 and 2016 additional probable reserves were announced to be under the Rocky Mountains in North America^[136] and in the East African Rift.^[137]

Modern extraction and distribution

For large-scale use, helium is extracted by fractional distillation from natural gas, which can contain as much as 7% helium.^[138] Since helium has a lower boiling point than any other element, low temperature and high pressure are used to liquefy nearly all the other gases (mostly nitrogen and methane). The resulting crude helium gas is purified by successive exposures to lowering temperatures, in which almost all of the remaining nitrogen and other gases are precipitated out of the gaseous mixture. Activated charcoal is used as a final purification step, usually resulting in 99.995% pure Grade-A helium.^[26] The principal impurity in Grade-A helium is neon. In a final production step, most of the helium that is produced is liquefied via a cryogenic process. This is necessary for applications requiring liquid helium and also allows helium suppliers to reduce the cost of long-distance transportation, as the largest liquid helium containers have more than five times the capacity of the largest gaseous helium tube trailers.^[75][139]

In 2008, approximately 169 million standard cubic meters (SCM) of helium were extracted from natural gas or withdrawn from helium reserves with approximately 78% from the United States, 10% from Algeria, and most of the remainder from Russia, Poland and Qatar.^[140] By 2013, increases in helium production in Qatar (under the company Qatargas managed by Air Liquide) had increased Qatar’s fraction of world helium production to 25%, and made it the second largest exporter after the United States.^[141]
An estimated 54 billion cubic feet (1.5×10⁹ m³) deposit of helium was found in Tanzania in 2016.^[142] A large-scale helium plant was opened in Ningxia, China in 2020.^[143]

In the United States, most helium is extracted from natural gas of the Hugoton and nearby gas fields in Kansas, Oklahoma, and the Panhandle Field in Texas.^[75][144] Much of this gas was once sent by pipeline to the National Helium Reserve, but since 2005 this reserve is being depleted and sold off, and is expected to be largely depleted by 2021,^[141] under the October 2013 Responsible Helium Administration and Stewardship Act (H.R. 527).^[145]

Diffusion of crude natural gas through special semipermeable membranes and other barriers is another method to recover and purify helium.^[146] In 1996, the U.S. had proven helium reserves, in such gas well complexes, of about 147 billion standard cubic feet (4.2 billion SCM).^[147] At rates of use at that time (72 million SCM per year in the U.S.; see pie chart below) this would have been enough helium for about 58 years of U.S. use, and less than this (perhaps 80% of the time) at world use rates, although factors in saving and processing impact effective reserve numbers.

Helium must be extracted from natural gas because it is present in air at only a fraction of that of neon, yet the demand for it is far higher. It is estimated that if all neon production were retooled to save helium, 0.1% of the world’s helium demands would be satisfied. Similarly, only 1% of the world’s helium demands could be satisfied by re-tooling all air distillation plants.^[148] Helium can be synthesized by bombardment of lithium or boron with high-velocity protons, or by bombardment of lithium with deuterons, but these processes are a completely uneconomical method of production.^[149]

Helium is commercially available in either liquid or gaseous form. As a liquid, it can be supplied in small insulated containers called dewars which hold as much as 1,000 liters of helium, or in large ISO containers which have nominal capacities as large as 42 m³ (around 11,000 U.S. gallons). In gaseous form, small quantities of helium are supplied in high-pressure cylinders holding as much as 8 m³ (approx. 282 standard cubic feet), while large quantities of high-pressure gas are supplied in tube trailers which have capacities of as much as 4,860 m³ (approx. 172,000 standard cubic feet).

Conservation advocates

According to helium conservationists like Nobel laureate physicist Robert Coleman Richardson, writing in 2010, the free market price of helium has contributed to «wasteful» usage (e.g. for helium balloons). Prices in the 2000s had been lowered by the decision of the U.S. Congress to sell off the country’s large helium stockpile by 2015.^[150] According to Richardson, the price needed to be multiplied by 20 to eliminate the excessive wasting of helium. In the paper Stop squandering helium published in 2012, it was also proposed to create an International Helium Agency that would build a sustainable market for «this precious commodity».^[151]

Applications

While balloons are perhaps the best known use of helium, they are a minor part of all helium use.^[70] Helium is used for many purposes that require some of its unique properties, such as its low boiling point, low density, low solubility, high thermal conductivity, or inertness. Of the 2014 world helium total production of about 32 million kg (180 million standard cubic meters) helium per year, the largest use (about 32% of the total in 2014) is in cryogenic applications, most of which involves cooling the superconducting magnets in medical MRI scanners and NMR spectrometers.^[153] Other major uses were pressurizing and purging systems, welding, maintenance of controlled atmospheres, and leak detection. Other uses by category were relatively minor fractions.^[152]

Controlled atmospheres

Helium is used as a protective gas in growing silicon and germanium crystals, in titanium and zirconium production, and in gas chromatography,^[91] because it is inert. Because of its inertness, thermally and calorically perfect nature, high speed of sound, and high value of the heat capacity ratio, it is also useful in supersonic wind tunnels^[154] and impulse facilities.^[155]

Gas tungsten arc welding

Helium is used as a shielding gas in arc welding processes on materials that at welding temperatures are contaminated and weakened by air or nitrogen.^[24] A number of inert shielding gases are used in gas tungsten arc welding, but helium is used instead of cheaper argon especially for welding materials that have higher heat conductivity, like aluminium or copper.

Minor uses

Industrial leak detection

One industrial application for helium is leak detection. Because helium diffuses through solids three times faster than air, it is used as a tracer gas to detect leaks in high-vacuum equipment (such as cryogenic tanks) and high-pressure containers.^[156] The tested object is placed in a chamber, which is then evacuated and filled with helium. The helium that escapes through the leaks is detected by a sensitive device (helium mass spectrometer), even at the leak rates as small as 10⁻⁹ mbar·L/s (10⁻¹⁰ Pa·m³/s). The measurement procedure is normally automatic and is called helium integral test. A simpler procedure is to fill the tested object with helium and to manually search for leaks with a hand-held device.^[157]

Helium leaks through cracks should not be confused with gas permeation through a bulk material. While helium has documented permeation constants (thus a calculable permeation rate) through glasses, ceramics, and synthetic materials, inert gases such as helium will not permeate most bulk metals.^[158]

Flight

Because it is lighter than air, airships and balloons are inflated with helium for lift. While hydrogen gas is more buoyant, and escapes permeating through a membrane at a lower rate, helium has the advantage of being non-flammable, and indeed fire-retardant. Another minor use is in rocketry, where helium is used as an ullage medium to displace fuel and oxidizers in storage tanks and to condense hydrogen and oxygen to make rocket fuel. It is also used to purge fuel and oxidizer from ground support equipment prior to launch and to pre-cool liquid hydrogen in space vehicles. For example, the Saturn V rocket used in the Apollo program needed about 370,000 m³ (13 million cubic feet) of helium to launch.^[91]

Minor commercial and recreational uses

Helium as a breathing gas has no narcotic properties, so helium mixtures such as trimix, heliox and heliair are used for deep diving to reduce the effects of narcosis, which worsen with increasing depth.^[159][160] As pressure increases with depth, the density of the breathing gas also increases, and the low molecular weight of helium is found to considerably reduce the effort of breathing by lowering the density of the mixture. This reduces the Reynolds number of flow, leading to a reduction of turbulent flow and an increase in laminar flow, which requires less work of breathing.^[161][162] At depths below 150 metres (490 ft) divers breathing helium–oxygen mixtures begin to experience tremors and a decrease in psychomotor function, symptoms of high-pressure nervous syndrome.^[163] This effect may be countered to some extent by adding an amount of narcotic gas such as hydrogen or nitrogen to a helium–oxygen mixture.^[164]

Helium–neon lasers, a type of low-powered gas laser producing a red beam, had various practical applications which included barcode readers and laser pointers, before they were almost universally replaced by cheaper diode lasers.^[24]

For its inertness and high thermal conductivity, neutron transparency, and because it does not form radioactive isotopes under reactor conditions, helium is used as a heat-transfer medium in some gas-cooled nuclear reactors.^[156]

Helium, mixed with a heavier gas such as xenon, is useful for thermoacoustic refrigeration due to the resulting high heat capacity ratio and low Prandtl number.^[165] The inertness of helium has environmental advantages over conventional refrigeration systems which contribute to ozone depletion or global warming.^[166]

Helium is also used in some hard disk drives.^[167]

Scientific uses

The use of helium reduces the distorting effects of temperature variations in the space between lenses in some telescopes, due to its extremely low index of refraction.^[26] This method is especially used in solar telescopes where a vacuum tight telescope tube would be too heavy.^[168][169]

Helium is a commonly used carrier gas for gas chromatography.

The age of rocks and minerals that contain uranium and thorium can be estimated by measuring the level of helium with a process known as helium dating.^[24][26]

Helium at low temperatures is used in cryogenics, and in certain cryogenics applications. As examples of applications, liquid helium is used to cool certain metals to the extremely low temperatures required for superconductivity, such as in superconducting magnets for magnetic resonance imaging. The Large Hadron Collider at CERN uses 96 metric tons of liquid helium to maintain the temperature at 1.9 K (−271.25 °C; −456.25 °F).^[170]

Medical uses

Helium was approved for medical use in the United States in April 2020 for humans and animals.^[171][172]

As a contaminant

While chemically inert, helium contamination impairs the operation of microelectromechanical systems (MEMS) such that iPhones may fail.^[173]

Inhalation and safety

Effects

Neutral helium at standard conditions is non-toxic, plays no biological role and is found in trace amounts in human blood.

The speed of sound in helium is nearly three times the speed of sound in air. Because the natural resonance frequency of a gas-filled cavity is proportional to the speed of sound in the gas, when helium is inhaled, a corresponding increase occurs in the resonant frequencies of the vocal tract, which is the amplifier of vocal sound.^[24][174] This increase in the resonant frequency of the amplifier (the vocal tract) gives an increased amplification to the high-frequency components of the sound wave produced by the direct vibration of the vocal folds, compared to the case when the voice box is filled with air. When a person speaks after inhaling helium gas, the muscles that control the voice box still move in the same way as when the voice box is filled with air, therefore the fundamental frequency (sometimes called pitch) produced by direct vibration of the vocal folds does not change.^[175] However, the high-frequency-preferred amplification causes a change in timbre of the amplified sound, resulting in a reedy, duck-like vocal quality. The opposite effect, lowering resonant frequencies, can be obtained by inhaling a dense gas such as sulfur hexafluoride or xenon.

Hazards

Inhaling helium can be dangerous if done to excess, since helium is a simple asphyxiant and so displaces oxygen needed for normal respiration.^[24][176] Fatalities have been recorded, including a youth who suffocated in Vancouver in 2003 and two adults who suffocated in South Florida in 2006.^[177][178] In 1998, an Australian girl from Victoria fell unconscious and temporarily turned blue after inhaling the entire contents of a party balloon.^{[179][180][181]}
Inhaling helium directly from pressurized cylinders or even balloon filling valves is extremely dangerous, as high flow rate and pressure can result in barotrauma, fatally rupturing lung tissue.^[176][182]

Death caused by helium is rare. The first media-recorded case was that of a 15-year-old girl from Texas who died in 1998 from helium inhalation at a friend’s party; the exact type of helium death is unidentified.^{[179][180][181]}

In the United States only two fatalities were reported between 2000 and 2004, including a man who died in North Carolina of barotrauma in 2002.^[177][182] A youth asphyxiated in Vancouver during 2003, and a 27-year-old man in Australia had an embolism after breathing from a cylinder in 2000.^[177] Since then two adults asphyxiated in South Florida in 2006,^{[177][178][183]} and there were cases in 2009 and 2010, one a Californian youth who was found with a bag over his head, attached to a helium tank,^[184] and another teenager in Northern Ireland died of asphyxiation.^[185] At Eagle Point, Oregon a teenage girl died in 2012 from barotrauma at a party.^{[186][187][188]} A girl from Michigan died from hypoxia later in the year.^[189]

On February 4, 2015, it was revealed that, during the recording of their main TV show on January 28, a 12-year-old member (name withheld) of Japanese all-girl singing group 3B Junior suffered from air embolism, losing consciousness and falling into a coma as a result of air bubbles blocking the flow of blood to the brain, after inhaling huge quantities of helium as part of a game. The incident was not made public until a week later.^[190][191] The staff of TV Asahi held an emergency press conference to communicate that the member had been taken to the hospital and is showing signs of rehabilitation such as moving eyes and limbs, but her consciousness has not yet been sufficiently recovered. Police have launched an investigation due to a neglect of safety measures.^[192][193]

The safety issues for cryogenic helium are similar to those of liquid nitrogen; its extremely low temperatures can result in cold burns, and the liquid-to-gas expansion ratio can cause explosions if no pressure-relief devices are installed. Containers of helium gas at 5 to 10 K should be handled as if they contain liquid helium due to the rapid and significant thermal expansion that occurs when helium gas at less than 10 K is warmed to room temperature.^[91]

At high pressures (more than about 20 atm or two MPa), a mixture of helium and oxygen (heliox) can lead to high-pressure nervous syndrome, a sort of reverse-anesthetic effect; adding a small amount of nitrogen to the mixture can alleviate the problem.^[194][163]

See also

Notes

References

Bibliography

External links

General

• U.S. Government’s Bureau of Land Management: Sources, Refinement, and Shortage. With some history of helium.
• U.S. Geological Survey publications on helium beginning 1996: Helium
• Where is all the helium? Aga website
• It’s Elemental – Helium
• Chemistry in its element podcast (MP3) from the Royal Society of Chemistry’s Chemistry World: Helium
• International Chemical Safety Cards – Helium; includes health and safety information regarding accidental exposures to helium

More detail

• Helium at The Periodic Table of Videos (University of Nottingham)
• Helium at the Helsinki University of Technology; includes pressure-temperature phase diagrams for helium-3 and helium-4
• Lancaster University, Ultra Low Temperature Physics – includes a summary of some low temperature techniques
• Video: Demonstration of superfluid helium (Alfred Leitner, 1963, 38 min.)

Miscellaneous

• Physics in Speech with audio samples that demonstrate the unchanged voice pitch
• Article about helium and other noble gases

Helium shortage

• America’s Helium Supply: Options for Producing More Helium from Federal Land: Oversight Hearing before the Subcommittee on Energy and Mineral Resources of the Committee on Natural Resources, U.S. House Of Representatives, One Hundred Thirteenth Congress, First Session, Thursday, July 11, 2013
• Helium Program: Urgent Issues Facing BLM’s Storage and Sale of Helium Reserves: Testimony before the Committee on Natural Resources, House of Representatives Government Accountability Office
• Kramer, David (May 22, 2012). «Senate bill would preserve US helium reserve: Measure would give scientists first dibs on helium should a shortage develop. Physics Today web site». Archived from the original on October 27, 2012.
• Richardson, Robert C.; Chan, Moses (2009). «Helium, when will it run out?» (PDF). Archived from the original (PDF) on 2015-06-14.

Helium, ₂He

Helium
Pronunciation	​(HEE-lee-əm)
Appearance	colorless gas, exhibiting a gray, cloudy glow (or reddish-orange if an especially high voltage is used) when placed in an electric field
Standard atomic weight Ar°(He)	4.002602±0.000002 4.0026±0.0001 (abridged)[1]
Helium in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ He ↓ Ne hydrogen ← helium → lithium
Atomic number (Z)	2
Group	group 18 (noble gases)
Period	period 1
Block	s-block
Electron configuration	1s2
Electrons per shell	2
Physical properties
Phase at STP	gas
Melting point	0.95 K ​(−272.20 °C, ​−457.96 °F) (at 2.5 MPa)
Boiling point	4.222 K ​(−268.928 °C, ​−452.070 °F)
Density (at STP)	0.1786 g/L
when liquid (at m.p.)	0.145 g/cm3
when liquid (at b.p.)	0.125 g/cm3
Triple point	2.177 K, ​5.043 kPa
Critical point	5.1953 K, 0.22746 MPa
Heat of fusion	0.0138 kJ/mol
Heat of vaporization	0.0829 kJ/mol
Molar heat capacity	20.78 J/(mol·K)[2]
Vapor pressure (defined by ITS-90) P (Pa) 1 10 100 1 k 10 k 100 k at T (K)     1.23 1.67 2.48 4.21
Atomic properties
Oxidation states	0
Electronegativity	Pauling scale: no data
Ionization energies	1st: 2372.3 kJ/mol 2nd: 5250.5 kJ/mol
Covalent radius	28 pm
Van der Waals radius	140 pm
Spectral lines of helium
Other properties
Natural occurrence	primordial
Crystal structure	​hexagonal close-packed (hcp)
Speed of sound	972 m/s
Thermal conductivity	0.1513 W/(m⋅K)
Magnetic ordering	diamagnetic[3]
Molar magnetic susceptibility	−1.88×10−6 cm3/mol (298 K)[4]
CAS Number	7440-59-7
History
Naming	after Helios, Greek god of the Sun
Discovery	Pierre Janssen, Norman Lockyer (1868)
First isolation	William Ramsay, Per Teodor Cleve, Abraham Langlet (1895)
Main isotopes of helium v e
Iso­tope Decay abun­dance half-life (t1/2) mode pro­duct 3He 0.0002(2)% stable 4He 99.9998(2)% stable
Category: Helium view talk edit | references

Helium (from Greek: ἥλιος, romanized: helios, lit. ‘sun’) is a chemical element with the symbol He and atomic number 2. It is a colorless, odorless, tasteless, non-toxic, inert, monatomic gas and the first in the noble gas group in the periodic table.^[a] Its boiling and melting point are the lowest among all the elements. It is the second lightest and second most abundant element in the observable universe, after hydrogen. It is present at about 24% of the total elemental mass, which is more than 12 times the mass of all the heavier elements combined. Its abundance is similar to this in both the Sun and in Jupiter, due to the very high nuclear binding energy (per nucleon) of helium-4, with respect to the next three elements after helium. This helium-4 binding energy also accounts for why it is a product of both nuclear fusion and radioactive decay. The most common isotope of helium in the universe is helium-4, the vast majority of which was formed during the Big Bang. Large amounts of new helium are created by nuclear fusion of hydrogen in stars.

Helium was first detected as an unknown, yellow spectral line signature in sunlight during a solar eclipse in 1868 by Georges Rayet,^[11] Captain C. T. Haig,^[12] Norman R. Pogson,^[13] and Lieutenant John Herschel,^[14] and was subsequently confirmed by French astronomer Jules Janssen.^[15] Janssen is often jointly credited with detecting the element, along with Norman Lockyer. Janssen recorded the helium spectral line during the solar eclipse of 1868, while Lockyer observed it from Britain. Lockyer was the first to propose that the line was due to a new element, which he named. The formal discovery of the element was made in 1895 by chemists Sir William Ramsay, Per Teodor Cleve, and Nils Abraham Langlet, who found helium emanating from the uranium ore, cleveite, which is now not regarded as a separate mineral species, but as a variety of uraninite.^[16][17] In 1903, large reserves of helium were found in natural gas fields in parts of the United States, by far the largest supplier of the gas today.

Liquid helium is used in cryogenics (its largest single use, absorbing about a quarter of production), and in the cooling of superconducting magnets, with its main commercial application in MRI scanners. Helium’s other industrial uses—as a pressurizing and purge gas, as a protective atmosphere for arc welding, and in processes such as growing crystals to make silicon wafers—account for half of the gas produced. A well-known but minor use is as a lifting gas in balloons and airships.^[18] As with any gas whose density differs from that of air, inhaling a small volume of helium temporarily changes the timbre and quality of the human voice. In scientific research, the behavior of the two fluid phases of helium-4 (helium I and helium II) is important to researchers studying quantum mechanics (in particular the property of superfluidity) and to those looking at the phenomena, such as superconductivity, produced in matter near absolute zero.

On Earth, it is relatively rare—5.2 ppm by volume in the atmosphere. Most terrestrial helium present today is created by the natural radioactive decay of heavy radioactive elements (thorium and uranium, although there are other examples), as the alpha particles emitted by such decays consist of helium-4 nuclei. This radiogenic helium is trapped with natural gas in concentrations as great as 7% by volume, from which it is extracted commercially by a low-temperature separation process called fractional distillation. Terrestrial helium is a non-renewable resource because once released into the atmosphere, it promptly escapes into space. Its supply is thought to be rapidly diminishing.^[19][20] However, some studies suggest that helium produced deep in the earth by radioactive decay can collect in natural gas reserves in larger than expected quantities,^[21] in some cases, having been released by volcanic activity.^[22]

History

Scientific discoveries

The first evidence of helium was observed on August 18, 1868, as a bright yellow line with a wavelength of 587.49 nanometers in the spectrum of the chromosphere of the Sun. The line was detected by French astronomer Jules Janssen during a total solar eclipse in Guntur, India.^[23][24] This line was initially assumed to be sodium. On October 20 of the same year, English astronomer, Norman Lockyer, observed a yellow line in the solar spectrum, which, he named the D₃ because it was near the known D₁ and D₂ Fraunhofer line lines of sodium.^[25][26] He concluded that it was caused by an element in the Sun unknown on Earth. Lockyer and English chemist Edward Frankland named the element with the Greek word for the Sun, ἥλιος (helios).^[27][28]

In 1881, Italian physicist Luigi Palmieri detected helium on Earth for the first time through its D₃ spectral line, when he analyzed a material that had been sublimated during a recent eruption of Mount Vesuvius.^[29]

On March 26, 1895, Scottish chemist Sir William Ramsay isolated helium on Earth by treating the mineral cleveite (a variety of uraninite with at least 10% rare-earth elements) with mineral acids. Ramsay was looking for argon but, after separating nitrogen and oxygen from the gas, liberated by sulfuric acid, he noticed a bright yellow line that matched the D₃ line observed in the spectrum of the Sun.^{[26][31][32][33]} These samples were identified as helium by Lockyer and British physicist William Crookes.^[34][35] It was independently isolated from cleveite, in the same year, by chemists, Per Teodor Cleve and Abraham Langlet, in Uppsala, Sweden, who collected enough of the gas to accurately determine its atomic weight.^{[36][37][24][38]} Helium was also isolated by the American geochemist, William Francis Hillebrand, prior to Ramsay’s discovery, when he noticed unusual spectral lines while testing a sample of the mineral uraninite. Hillebrand, however, attributed the lines to nitrogen.^[39] His letter of congratulations to Ramsay offers an interesting case of discovery, and near-discovery, in science.^[40]

In 1907, Ernest Rutherford and Thomas Royds demonstrated that alpha particles are helium nuclei, by allowing the particles to penetrate the thin, glass wall of an evacuated tube, then creating a discharge in the tube, to study the spectrum of the new gas inside.^[41] In 1908, helium was first liquefied by Dutch physicist Heike Kamerlingh Onnes by cooling the gas to less than 5 K (−268.15 °C; −450.67 °F).^[42][43] He tried to solidify it, by further reducing the temperature, but failed, because helium does not solidify at atmospheric pressure. Onnes’ student Willem Hendrik Keesom was eventually able to solidify 1 cm³ of helium in 1926 by applying additional external pressure.^[44][45]

In 1913, Niels Bohr published his «trilogy»^[46][47] on atomic structure that included a reconsideration of the Pickering–Fowler series as central evidence in support of his model of the atom.^[48][49] This series is named for Edward Charles Pickering, who in 1896 published observations of previously unknown lines in the spectrum of the star ζ Puppis^[50] (these are now known to occur with Wolf–Rayet and other hot stars).^[51] Pickering attributed the observation (lines at 4551, 5411, and 10123 Å) to a new form of hydrogen with half-integer transition levels.^[52][53] In 1912, Alfred Fowler^[54] managed to produce similar lines from a hydrogen-helium mixture, and supported Pickering’s conclusion as to their origin.^[55] Bohr’s model does not allow for half-integer transitions (nor does quantum mechanics) and Bohr concluded that Pickering and Fowler were wrong, and instead assigned these spectral lines to ionised helium, He⁺.^[56] Fowler was initially skeptical^[57] but was ultimately convinced^[58] that Bohr was correct,^[46] and by 1915 «spectroscopists had transferred [the Pickering–Fowler series] definitively [from hydrogen] to helium.»^[49][59] Bohr’s theoretical work on the Pickering series had demonstrated the need for «a re-examination of problems that seemed already to have been solved within classical theories» and provided important confirmation for his atomic theory.^[49]

In 1938, Russian physicist Pyotr Leonidovich Kapitsa discovered that helium-4 has almost no viscosity at temperatures near absolute zero, a phenomenon now called superfluidity.^[60] This phenomenon is related to Bose–Einstein condensation. In 1972, the same phenomenon was observed in helium-3, but at temperatures much closer to absolute zero, by American physicists Douglas D. Osheroff, David M. Lee, and Robert C. Richardson. The phenomenon in helium-3 is thought to be related to pairing of helium-3 fermions to make bosons, in analogy to Cooper pairs of electrons producing superconductivity.^[61]

Extraction and use

After an oil drilling operation in 1903 in Dexter, Kansas produced a gas geyser that would not burn, Kansas state geologist Erasmus Haworth collected samples of the escaping gas and took them back to the University of Kansas at Lawrence where, with the help of chemists Hamilton Cady and David McFarland, he discovered that the gas consisted of, by volume, 72% nitrogen, 15% methane (a combustible percentage only with sufficient oxygen), 1% hydrogen, and 12% an unidentifiable gas.^[24][62] With further analysis, Cady and McFarland discovered that 1.84% of the gas sample was helium.^[63][64] This showed that despite its overall rarity on Earth, helium was concentrated in large quantities under the American Great Plains, available for extraction as a byproduct of natural gas.^[65]

This enabled the United States to become the world’s leading supplier of helium. Following a suggestion by Sir Richard Threlfall, the United States Navy sponsored three small experimental helium plants during World War I. The goal was to supply barrage balloons with the non-flammable, lighter-than-air gas. A total of 5,700 m³ (200,000 cu ft) of 92% helium was produced in the program even though less than a cubic meter of the gas had previously been obtained.^[26] Some of this gas was used in the world’s first helium-filled airship, the U.S. Navy’s C-class blimp C-7, which flew its maiden voyage from Hampton Roads, Virginia, to Bolling Field in Washington, D.C., on December 1, 1921,^[66] nearly two years before the Navy’s first rigid helium-filled airship, the Naval Aircraft Factory-built USS Shenandoah, flew in September 1923.

Although the extraction process using low-temperature gas liquefaction was not developed in time to be significant during World War I, production continued. Helium was primarily used as a lifting gas in lighter-than-air craft. During World War II, the demand increased for helium for lifting gas and for shielded arc welding. The helium mass spectrometer was also vital in the atomic bomb Manhattan Project.^[67]

The government of the United States set up the National Helium Reserve in 1925 at Amarillo, Texas, with the goal of supplying military airships in time of war and commercial airships in peacetime.^[26] Because of the Helium Act of 1925, which banned the export of scarce helium on which the US then had a production monopoly, together with the prohibitive cost of the gas, the Hindenburg, like all German Zeppelins, was forced to use hydrogen as the lift gas. The helium market after World War II was depressed but the reserve was expanded in the 1950s to ensure a supply of liquid helium as a coolant to create oxygen/hydrogen rocket fuel (among other uses) during the Space Race and Cold War. Helium use in the United States in 1965 was more than eight times the peak wartime consumption.^[68]

After the «Helium Acts Amendments of 1960» (Public Law 86–777), the U.S. Bureau of Mines arranged for five private plants to recover helium from natural gas. For this helium conservation program, the Bureau built a 425-mile (684 km) pipeline from Bushton, Kansas, to connect those plants with the government’s partially depleted Cliffside gas field near Amarillo, Texas. This helium-nitrogen mixture was injected and stored in the Cliffside gas field until needed, at which time it was further purified.^[69]

By 1995, a billion cubic meters of the gas had been collected and the reserve was US$1.4 billion in debt, prompting the Congress of the United States in 1996 to phase out the reserve.^[24][70] The resulting Helium Privatization Act of 1996^[71] (Public Law 104–273) directed the United States Department of the Interior to empty the reserve, with sales starting by 2005.^[72]

Helium produced between 1930 and 1945 was about 98.3% pure (2% nitrogen), which was adequate for airships. In 1945, a small amount of 99.9% helium was produced for welding use. By 1949, commercial quantities of Grade A 99.95% helium were available.^[73]

For many years, the United States produced more than 90% of commercially usable helium in the world, while extraction plants in Canada, Poland, Russia, and other nations produced the remainder. In the mid-1990s, a new plant in Arzew, Algeria, producing 17 million cubic meters (600 million cubic feet) began operation, with enough production to cover all of Europe’s demand. Meanwhile, by 2000, the consumption of helium within the U.S. had risen to more than 15 million kg per year.^[74] In 2004–2006, additional plants in Ras Laffan, Qatar, and Skikda, Algeria were built. Algeria quickly became the second leading producer of helium.^[75] Through this time, both helium consumption and the costs of producing helium increased.^[76] From 2002 to 2007 helium prices doubled.^[77]

As of 2012, the United States National Helium Reserve accounted for 30 percent of the world’s helium.^[78] The reserve was expected to run out of helium in 2018.^[78] Despite that, a proposed bill in the United States Senate would allow the reserve to continue to sell the gas. Other large reserves were in the Hugoton in Kansas, United States, and nearby gas fields of Kansas and the panhandles of Texas and Oklahoma. New helium plants were scheduled to open in 2012 in Qatar, Russia, and the US state of Wyoming, but they were not expected to ease the shortage.^[78]

In 2013, Qatar started up the world’s largest helium unit,^[79] although the 2017 Qatar diplomatic crisis severely affected helium production there.^[80] 2014 was widely acknowledged to be a year of over-supply in the helium business, following years of renowned shortages.^[81] Nasdaq reported (2015) that for Air Products, an international corporation that sells gases for industrial use, helium volumes remain under economic pressure due to feedstock supply constraints.^[82]

Characteristics

Atom

In quantum mechanics

In the perspective of quantum mechanics, helium is the second simplest atom to model, following the hydrogen atom. Helium is composed of two electrons in atomic orbitals surrounding a nucleus containing two protons and (usually) two neutrons. As in Newtonian mechanics, no system that consists of more than two particles can be solved with an exact analytical mathematical approach (see 3-body problem) and helium is no exception. Thus, numerical mathematical methods are required, even to solve the system of one nucleus and two electrons. Such computational chemistry methods have been used to create a quantum mechanical picture of helium electron binding which is accurate to within < 2% of the correct value, in a few computational steps.^[83] Such models show that each electron in helium partly screens the nucleus from the other, so that the effective nuclear charge Z_eff which each electron sees is about 1.69 units, not the 2 charges of a classic «bare» helium nucleus.

Related stability of the helium-4 nucleus and electron shell

The nucleus of the helium-4 atom is identical with an alpha particle. High-energy electron-scattering experiments show its charge to decrease exponentially from a maximum at a central point, exactly as does the charge density of helium’s own electron cloud. This symmetry reflects similar underlying physics: the pair of neutrons and the pair of protons in helium’s nucleus obey the same quantum mechanical rules as do helium’s pair of electrons (although the nuclear particles are subject to a different nuclear binding potential), so that all these fermions fully occupy 1s orbitals in pairs, none of them possessing orbital angular momentum, and each cancelling the other’s intrinsic spin. Adding another of any of these particles would require angular momentum and would release substantially less energy (in fact, no nucleus with five nucleons is stable). This arrangement is thus energetically extremely stable for all these particles, and this stability accounts for many crucial facts regarding helium in nature.

For example, the stability and low energy of the electron cloud state in helium accounts for the element’s chemical inertness, and also the lack of interaction of helium atoms with each other, producing the lowest melting and boiling points of all the elements.

In a similar way, the particular energetic stability of the helium-4 nucleus, produced by similar effects, accounts for the ease of helium-4 production in atomic reactions that involve either heavy-particle emission or fusion. Some stable helium-3 (two protons and one neutron) is produced in fusion reactions from hydrogen, but it is a very small fraction compared to the highly favorable helium-4.

The unusual stability of the helium-4 nucleus is also important cosmologically: it explains the fact that in the first few minutes after the Big Bang, as the «soup» of free protons and neutrons which had initially been created in about 6:1 ratio cooled to the point that nuclear binding was possible, almost all first compound atomic nuclei to form were helium-4 nuclei. Owing to the relatively tight binding of helium-4 nuclei, its production consumed nearly all of the free neutrons in a few minutes, before they could beta-decay, and thus few neutrons were available to form heavier atoms such as lithium, beryllium, or boron. Helium-4 nuclear binding per nucleon is stronger than in any of these elements (see nucleogenesis and binding energy) and thus, once helium had been formed, no energetic drive was available to make elements 3, 4 and 5.^[84] It is barely energetically favorable for helium to fuse into the next element with a lower energy per nucleon, carbon. However, due to lack of intermediate elements, this process requires three helium nuclei striking each other nearly simultaneously (see triple alpha process). There was thus no time for significant carbon to be formed in the few minutes after the Big Bang, before the early expanding universe cooled to the temperature and pressure point where helium fusion to carbon was no longer possible. This left the early universe with a very similar ratio of hydrogen/helium as is observed today (3 parts hydrogen to 1 part helium-4 by mass), with nearly all the neutrons in the universe trapped in helium-4.

All heavier elements (including those necessary for rocky planets like the Earth, and for carbon-based or other life) have thus been created since the Big Bang in stars which were hot enough to fuse helium itself. All elements other than hydrogen and helium today account for only 2% of the mass of atomic matter in the universe. Helium-4, by contrast, makes up about 23% of the universe’s ordinary matter—nearly all the ordinary matter that is not hydrogen.

Gas and plasma phases

Helium is the second least reactive noble gas after neon, and thus the second least reactive of all elements.^[85] It is chemically inert and monatomic in all standard conditions. Because of helium’s relatively low molar (atomic) mass, its thermal conductivity, specific heat, and sound speed in the gas phase are all greater than any other gas except hydrogen. For these reasons and the small size of helium monatomic molecules, helium diffuses through solids at a rate three times that of air and around 65% that of hydrogen.^[26]

Helium is the least water-soluble monatomic gas,^[86] and one of the least water-soluble of any gas (CF₄, SF₆, and C₄F₈ have lower mole fraction solubilities: 0.3802, 0.4394, and 0.2372 x₂/10⁻⁵, respectively, versus helium’s 0.70797 x₂/10⁻⁵),^[87] and helium’s index of refraction is closer to unity than that of any other gas.^[88] Helium has a negative Joule–Thomson coefficient at normal ambient temperatures, meaning it heats up when allowed to freely expand. Only below its Joule–Thomson inversion temperature (of about 32 to 50 K at 1 atmosphere) does it cool upon free expansion.^[26] Once precooled below this temperature, helium can be liquefied through expansion cooling.

Most extraterrestrial helium is found in a plasma state, with properties quite different from those of atomic helium. In a plasma, helium’s electrons are not bound to its nucleus, resulting in very high electrical conductivity, even when the gas is only partially ionized. The charged particles are highly influenced by magnetic and electric fields. For example, in the solar wind together with ionized hydrogen, the particles interact with the Earth’s magnetosphere, giving rise to Birkeland currents and the aurora.^[89]

Liquid phase

Unlike any other element, helium will remain liquid down to absolute zero at normal pressures. This is a direct effect of quantum mechanics: specifically, the zero point energy of the system is too high to allow freezing. Solid helium requires a temperature of 1–1.5 K (about −272 °C or −457 °F) at about 25 bar (2.5 MPa) of pressure.^[90] It is often hard to distinguish solid from liquid helium since the refractive index of the two phases are nearly the same. The solid has a sharp melting point and has a crystalline structure, but it is highly compressible; applying pressure in a laboratory can decrease its volume by more than 30%.^[91] With a bulk modulus of about 27 MPa^[92] it is ~100 times more compressible than water. Solid helium has a density of 0.214±0.006 g/cm³ at 1.15 K and 66 atm; the projected density at 0 K and 25 bar (2.5 MPa) is 0.187±0.009 g/cm³.^[93] At higher temperatures, helium will solidify with sufficient pressure. At room temperature, this requires about 114,000 atm.^[94]

Helium I

Below its boiling point of 4.22 K (−268.93 °C; −452.07 °F) and above the lambda point of 2.1768 K (−270.9732 °C; −455.7518 °F), the isotope helium-4 exists in a normal colorless liquid state, called helium I.^[26] Like other cryogenic liquids, helium I boils when it is heated and contracts when its temperature is lowered. Below the lambda point, however, helium does not boil, and it expands as the temperature is lowered further.

Helium I has a gas-like index of refraction of 1.026 which makes its surface so hard to see that floats of Styrofoam are often used to show where the surface is.^[26] This colorless liquid has a very low viscosity and a density of 0.145–0.125 g/mL (between about 0 and 4 K),^[95] which is only one-fourth the value expected from classical physics.^[26] Quantum mechanics is needed to explain this property and thus both states of liquid helium (helium I and helium II) are called quantum fluids, meaning they display atomic properties on a macroscopic scale. This may be an effect of its boiling point being so close to absolute zero, preventing random molecular motion (thermal energy) from masking the atomic properties.^[26]

Helium II

Liquid helium below its lambda point (called helium II) exhibits very unusual characteristics. Due to its high thermal conductivity, when it boils, it does not bubble but rather evaporates directly from its surface. Helium-3 also has a superfluid phase, but only at much lower temperatures; as a result, less is known about the properties of the isotope.^[26]

Helium II is a superfluid, a quantum mechanical state (see: macroscopic quantum phenomena) of matter with strange properties. For example, when it flows through capillaries as thin as 10⁻⁷ to 10⁻⁸ m it has no measurable viscosity.^[24] However, when measurements were done between two moving discs, a viscosity comparable to that of gaseous helium was observed. Current theory explains this using the two-fluid model for helium II. In this model, liquid helium below the lambda point is viewed as containing a proportion of helium atoms in a ground state, which are superfluid and flow with exactly zero viscosity, and a proportion of helium atoms in an excited state, which behave more like an ordinary fluid.^[96]

In the fountain effect, a chamber is constructed which is connected to a reservoir of helium II by a sintered disc through which superfluid helium leaks easily but through which non-superfluid helium cannot pass. If the interior of the container is heated, the superfluid helium changes to non-superfluid helium. In order to maintain the equilibrium fraction of superfluid helium, superfluid helium leaks through and increases the pressure, causing liquid to fountain out of the container.^[97]

The thermal conductivity of helium II is greater than that of any other known substance, a million times that of helium I and several hundred times that of copper.^[26] This is because heat conduction occurs by an exceptional quantum mechanism. Most materials that conduct heat well have a valence band of free electrons which serve to transfer the heat. Helium II has no such valence band but nevertheless conducts heat well. The flow of heat is governed by equations that are similar to the wave equation used to characterize sound propagation in air. When heat is introduced, it moves at 20 meters per second at 1.8 K through helium II as waves in a phenomenon known as second sound.^[26]

Helium II also exhibits a creeping effect. When a surface extends past the level of helium II, the helium II moves along the surface, against the force of gravity. Helium II will escape from a vessel that is not sealed by creeping along the sides until it reaches a warmer region where it evaporates. It moves in a 30 nm-thick film regardless of surface material. This film is called a Rollin film and is named after the man who first characterized this trait, Bernard V. Rollin.^[26][98][99] As a result of this creeping behavior and helium II’s ability to leak rapidly through tiny openings, it is very difficult to confine. Unless the container is carefully constructed, the helium II will creep along the surfaces and through valves until it reaches somewhere warmer, where it will evaporate. Waves propagating across a Rollin film are governed by the same equation as gravity waves in shallow water, but rather than gravity, the restoring force is the van der Waals force.^[100] These waves are known as third sound.^[101]

Isotopes

There are nine known isotopes of helium, but only helium-3 and helium-4 are stable. In the Earth’s atmosphere, one atom is ³
He for every million that are ⁴
He.^[24] Unlike most elements, helium’s isotopic abundance varies greatly by origin, due to the different formation processes. The most common isotope, helium-4, is produced on Earth by alpha decay of heavier radioactive elements; the alpha particles that emerge are fully ionized helium-4 nuclei. Helium-4 is an unusually stable nucleus because its nucleons are arranged into complete shells. It was also formed in enormous quantities during Big Bang nucleosynthesis.^[102]

Helium-3 is present on Earth only in trace amounts. Most of it has been present since Earth’s formation, though some falls to Earth trapped in cosmic dust.^[103] Trace amounts are also produced by the beta decay of tritium.^[104] Rocks from the Earth’s crust have isotope ratios varying by as much as a factor of ten, and these ratios can be used to investigate the origin of rocks and the composition of the Earth’s mantle.^{[103] 3}
He is much more abundant in stars as a product of nuclear fusion. Thus in the interstellar medium, the proportion of ³
He to ⁴
He is about 100 times higher than on Earth.^[105] Extraplanetary material, such as lunar and asteroid regolith, have trace amounts of helium-3 from being bombarded by solar winds. The Moon’s surface contains helium-3 at concentrations on the order of 10 ppb, much higher than the approximately 5 ppt found in the Earth’s atmosphere.^[106][107] A number of people, starting with Gerald Kulcinski in 1986,^[108] have proposed to explore the moon, mine lunar regolith, and use the helium-3 for fusion.

Liquid helium-4 can be cooled to about 1 K (−272.15 °C; −457.87 °F) using evaporative cooling in a 1-K pot. Similar cooling of helium-3, which has a lower boiling point, can achieve about 0.2 kelvin in a helium-3 refrigerator. Equal mixtures of liquid ³
He and ⁴
He below 0.8 K separate into two immiscible phases due to their dissimilarity (they follow different quantum statistics: helium-4 atoms are bosons while helium-3 atoms are fermions).^[26] Dilution refrigerators use this immiscibility to achieve temperatures of a few millikelvins.^[109]

It is possible to produce exotic helium isotopes, which rapidly decay into other substances. The shortest-lived heavy helium isotope is the unbound helium-10 with a half-life of 2.6(4)×10⁻²² s.^[110] Helium-6 decays by emitting a beta particle and has a half-life of 0.8 second. Helium-7 also emits a beta particle as well as a gamma ray. Helium-7 and helium-8 are created in certain nuclear reactions.^[26] Helium-6 and helium-8 are known to exhibit a nuclear halo.^[26]

Properties

Table of thermal and physical properties of helium gas at atmospheric pressure:^[111][112]

Temperature (K)	Density (kg/m^3)	Specific heat (kJ/kg °C)	Dynamic viscosity (kg/m s)	Kinematic viscosity (m^2/s)	Thermal conductivity (W/m °C)	Thermal diffusivity (m^2/s)	Prandtl Number
100		5.193	9.63E-06	1.98E-05	0.073	2.89E-05	0.686
120	0.406	5.193	1.07E-05	2.64E-05	0.0819	3.88E-05	0.679
144	0.3379	5.193	1.26E-05	3.71E-05	0.0928	5.28E-05	0.7
200	0.2435	5.193	1.57E-05	6.44E-05	0.1177	9.29E-05	0.69
255	0.1906	5.193	1.82E-05	9.55E-05	0.1357	1.37E-04	0.7
366	0.1328	5.193	2.31E-05	1.74E-04	0.1691	2.45E-04	0.71
477	0.10204	5.193	2.75E-05	2.69E-04	0.197	3.72E-04	0.72
589	0.08282	5.193	3.11E-05	3.76E-04	0.225	5.22E-04	0.72
700	0.07032	5.193	3.48E-05	4.94E-04	0.251	6.66E-04	0.72
800	0.06023	5.193	3.82E-05	6.34E-04	0.275	8.77E-04	0.72
900	0.05451	5.193	4.14E-05	7.59E-04	0.33	1.14E-03	0.687
1000		5.193	4.46E-05	9.14E-04	0.354	1.40E-03	0.654

Compounds

Helium has a valence of zero and is chemically unreactive under all normal conditions.^[91] It is an electrical insulator unless ionized. As with the other noble gases, helium has metastable energy levels that allow it to remain ionized in an electrical discharge with a voltage below its ionization potential.^[26] Helium can form unstable compounds, known as excimers, with tungsten, iodine, fluorine, sulfur, and phosphorus when it is subjected to a glow discharge, to electron bombardment, or reduced to plasma by other means. The molecular compounds HeNe, HgHe₁₀, and WHe₂, and the molecular ions He⁺
₂, He²⁺
₂, HeH⁺
, and HeD⁺
have been created this way.^[113] HeH⁺ is also stable in its ground state, but is extremely reactive—it is the strongest Brønsted acid known, and therefore can exist only in isolation, as it will protonate any molecule or counteranion it contacts. This technique has also produced the neutral molecule He₂, which has a large number of band systems, and HgHe, which is apparently held together only by polarization forces.^[26]

Van der Waals compounds of helium can also be formed with cryogenic helium gas and atoms of some other substance, such as LiHe and He₂.^[114]

Theoretically, other true compounds may be possible, such as helium fluorohydride (HHeF) which would be analogous to HArF, discovered in 2000.^[115] Calculations show that two new compounds containing a helium-oxygen bond could be stable.^[116] Two new molecular species, predicted using theory, CsFHeO and N(CH₃)₄FHeO, are derivatives of a metastable FHeO⁻ anion first theorized in 2005 by a group from Taiwan. If confirmed by experiment, the only remaining element with no known stable compounds would be neon.^[117]

Helium atoms have been inserted into the hollow carbon cage molecules (the fullerenes) by heating under high pressure. The endohedral fullerene molecules formed are stable at high temperatures. When chemical derivatives of these fullerenes are formed, the helium stays inside.^[118] If helium-3 is used, it can be readily observed by helium nuclear magnetic resonance spectroscopy.^[119] Many fullerenes containing helium-3 have been reported. Although the helium atoms are not attached by covalent or ionic bonds, these substances have distinct properties and a definite composition, like all stoichiometric chemical compounds.

Under high pressures helium can form compounds with various other elements. Helium-nitrogen clathrate (He(N₂)₁₁) crystals have been grown at room temperature at pressures ca. 10 GPa in a diamond anvil cell.^[120] The insulating electride Na₂He has been shown to be thermodynamically stable at pressures above 113 GPa. It has a fluorite structure.^[121]

Occurrence and production

Natural abundance

Although it is rare on Earth, helium is the second most abundant element in the known Universe, constituting 23% of its baryonic mass. Only hydrogen is more abundant.^[24] The vast majority of helium was formed by Big Bang nucleosynthesis one to three minutes after the Big Bang. As such, measurements of its abundance contribute to cosmological models. In stars, it is formed by the nuclear fusion of hydrogen in proton–proton chain reactions and the CNO cycle, part of stellar nucleosynthesis.^[102]

In the Earth’s atmosphere, the concentration of helium by volume is only 5.2 parts per million.^[122][123] The concentration is low and fairly constant despite the continuous production of new helium because most helium in the Earth’s atmosphere escapes into space by several processes.^{[124][125][126]} In the Earth’s heterosphere, a part of the upper atmosphere, helium and other lighter gases are the most abundant elements.

Most helium on Earth is a result of radioactive decay. Helium is found in large amounts in minerals of uranium and thorium, including uraninite and its varieties cleveite and pitchblende,^[16][127] carnotite and monazite (a group name; «monazite» usually refers to monazite-(Ce)),^[128][129] because they emit alpha particles (helium nuclei, He²⁺) to which electrons immediately combine as soon as the particle is stopped by the rock. In this way an estimated 3000 metric tons of helium are generated per year throughout the lithosphere.^{[130][131][132]} In the Earth’s crust, the concentration of helium is 8 parts per billion. In seawater, the concentration is only 4 parts per trillion. There are also small amounts in mineral springs, volcanic gas, and meteoric iron. Because helium is trapped in the subsurface under conditions that also trap natural gas, the greatest natural concentrations of helium on the planet are found in natural gas, from which most commercial helium is extracted. The concentration varies in a broad range from a few ppm to more than 7% in a small gas field in San Juan County, New Mexico.^[133][134]

As of 2021 the world’s helium reserves were estimated at 31 billion cubic meters, with a third of that being in Qatar.^[135] In 2015 and 2016 additional probable reserves were announced to be under the Rocky Mountains in North America^[136] and in the East African Rift.^[137]

Modern extraction and distribution

For large-scale use, helium is extracted by fractional distillation from natural gas, which can contain as much as 7% helium.^[138] Since helium has a lower boiling point than any other element, low temperature and high pressure are used to liquefy nearly all the other gases (mostly nitrogen and methane). The resulting crude helium gas is purified by successive exposures to lowering temperatures, in which almost all of the remaining nitrogen and other gases are precipitated out of the gaseous mixture. Activated charcoal is used as a final purification step, usually resulting in 99.995% pure Grade-A helium.^[26] The principal impurity in Grade-A helium is neon. In a final production step, most of the helium that is produced is liquefied via a cryogenic process. This is necessary for applications requiring liquid helium and also allows helium suppliers to reduce the cost of long-distance transportation, as the largest liquid helium containers have more than five times the capacity of the largest gaseous helium tube trailers.^[75][139]

In 2008, approximately 169 million standard cubic meters (SCM) of helium were extracted from natural gas or withdrawn from helium reserves with approximately 78% from the United States, 10% from Algeria, and most of the remainder from Russia, Poland and Qatar.^[140] By 2013, increases in helium production in Qatar (under the company Qatargas managed by Air Liquide) had increased Qatar’s fraction of world helium production to 25%, and made it the second largest exporter after the United States.^[141]
An estimated 54 billion cubic feet (1.5×10⁹ m³) deposit of helium was found in Tanzania in 2016.^[142] A large-scale helium plant was opened in Ningxia, China in 2020.^[143]

In the United States, most helium is extracted from natural gas of the Hugoton and nearby gas fields in Kansas, Oklahoma, and the Panhandle Field in Texas.^[75][144] Much of this gas was once sent by pipeline to the National Helium Reserve, but since 2005 this reserve is being depleted and sold off, and is expected to be largely depleted by 2021,^[141] under the October 2013 Responsible Helium Administration and Stewardship Act (H.R. 527).^[145]

Diffusion of crude natural gas through special semipermeable membranes and other barriers is another method to recover and purify helium.^[146] In 1996, the U.S. had proven helium reserves, in such gas well complexes, of about 147 billion standard cubic feet (4.2 billion SCM).^[147] At rates of use at that time (72 million SCM per year in the U.S.; see pie chart below) this would have been enough helium for about 58 years of U.S. use, and less than this (perhaps 80% of the time) at world use rates, although factors in saving and processing impact effective reserve numbers.

Helium must be extracted from natural gas because it is present in air at only a fraction of that of neon, yet the demand for it is far higher. It is estimated that if all neon production were retooled to save helium, 0.1% of the world’s helium demands would be satisfied. Similarly, only 1% of the world’s helium demands could be satisfied by re-tooling all air distillation plants.^[148] Helium can be synthesized by bombardment of lithium or boron with high-velocity protons, or by bombardment of lithium with deuterons, but these processes are a completely uneconomical method of production.^[149]

Helium is commercially available in either liquid or gaseous form. As a liquid, it can be supplied in small insulated containers called dewars which hold as much as 1,000 liters of helium, or in large ISO containers which have nominal capacities as large as 42 m³ (around 11,000 U.S. gallons). In gaseous form, small quantities of helium are supplied in high-pressure cylinders holding as much as 8 m³ (approx. 282 standard cubic feet), while large quantities of high-pressure gas are supplied in tube trailers which have capacities of as much as 4,860 m³ (approx. 172,000 standard cubic feet).

Conservation advocates

According to helium conservationists like Nobel laureate physicist Robert Coleman Richardson, writing in 2010, the free market price of helium has contributed to «wasteful» usage (e.g. for helium balloons). Prices in the 2000s had been lowered by the decision of the U.S. Congress to sell off the country’s large helium stockpile by 2015.^[150] According to Richardson, the price needed to be multiplied by 20 to eliminate the excessive wasting of helium. In the paper Stop squandering helium published in 2012, it was also proposed to create an International Helium Agency that would build a sustainable market for «this precious commodity».^[151]

Applications

While balloons are perhaps the best known use of helium, they are a minor part of all helium use.^[70] Helium is used for many purposes that require some of its unique properties, such as its low boiling point, low density, low solubility, high thermal conductivity, or inertness. Of the 2014 world helium total production of about 32 million kg (180 million standard cubic meters) helium per year, the largest use (about 32% of the total in 2014) is in cryogenic applications, most of which involves cooling the superconducting magnets in medical MRI scanners and NMR spectrometers.^[153] Other major uses were pressurizing and purging systems, welding, maintenance of controlled atmospheres, and leak detection. Other uses by category were relatively minor fractions.^[152]

Controlled atmospheres

Helium is used as a protective gas in growing silicon and germanium crystals, in titanium and zirconium production, and in gas chromatography,^[91] because it is inert. Because of its inertness, thermally and calorically perfect nature, high speed of sound, and high value of the heat capacity ratio, it is also useful in supersonic wind tunnels^[154] and impulse facilities.^[155]

Gas tungsten arc welding

Helium is used as a shielding gas in arc welding processes on materials that at welding temperatures are contaminated and weakened by air or nitrogen.^[24] A number of inert shielding gases are used in gas tungsten arc welding, but helium is used instead of cheaper argon especially for welding materials that have higher heat conductivity, like aluminium or copper.

Minor uses

Industrial leak detection

One industrial application for helium is leak detection. Because helium diffuses through solids three times faster than air, it is used as a tracer gas to detect leaks in high-vacuum equipment (such as cryogenic tanks) and high-pressure containers.^[156] The tested object is placed in a chamber, which is then evacuated and filled with helium. The helium that escapes through the leaks is detected by a sensitive device (helium mass spectrometer), even at the leak rates as small as 10⁻⁹ mbar·L/s (10⁻¹⁰ Pa·m³/s). The measurement procedure is normally automatic and is called helium integral test. A simpler procedure is to fill the tested object with helium and to manually search for leaks with a hand-held device.^[157]

Helium leaks through cracks should not be confused with gas permeation through a bulk material. While helium has documented permeation constants (thus a calculable permeation rate) through glasses, ceramics, and synthetic materials, inert gases such as helium will not permeate most bulk metals.^[158]

Flight

Because it is lighter than air, airships and balloons are inflated with helium for lift. While hydrogen gas is more buoyant, and escapes permeating through a membrane at a lower rate, helium has the advantage of being non-flammable, and indeed fire-retardant. Another minor use is in rocketry, where helium is used as an ullage medium to displace fuel and oxidizers in storage tanks and to condense hydrogen and oxygen to make rocket fuel. It is also used to purge fuel and oxidizer from ground support equipment prior to launch and to pre-cool liquid hydrogen in space vehicles. For example, the Saturn V rocket used in the Apollo program needed about 370,000 m³ (13 million cubic feet) of helium to launch.^[91]

Minor commercial and recreational uses

Helium as a breathing gas has no narcotic properties, so helium mixtures such as trimix, heliox and heliair are used for deep diving to reduce the effects of narcosis, which worsen with increasing depth.^[159][160] As pressure increases with depth, the density of the breathing gas also increases, and the low molecular weight of helium is found to considerably reduce the effort of breathing by lowering the density of the mixture. This reduces the Reynolds number of flow, leading to a reduction of turbulent flow and an increase in laminar flow, which requires less work of breathing.^[161][162] At depths below 150 metres (490 ft) divers breathing helium–oxygen mixtures begin to experience tremors and a decrease in psychomotor function, symptoms of high-pressure nervous syndrome.^[163] This effect may be countered to some extent by adding an amount of narcotic gas such as hydrogen or nitrogen to a helium–oxygen mixture.^[164]

Helium–neon lasers, a type of low-powered gas laser producing a red beam, had various practical applications which included barcode readers and laser pointers, before they were almost universally replaced by cheaper diode lasers.^[24]

For its inertness and high thermal conductivity, neutron transparency, and because it does not form radioactive isotopes under reactor conditions, helium is used as a heat-transfer medium in some gas-cooled nuclear reactors.^[156]

Helium, mixed with a heavier gas such as xenon, is useful for thermoacoustic refrigeration due to the resulting high heat capacity ratio and low Prandtl number.^[165] The inertness of helium has environmental advantages over conventional refrigeration systems which contribute to ozone depletion or global warming.^[166]

Helium is also used in some hard disk drives.^[167]

Scientific uses

The use of helium reduces the distorting effects of temperature variations in the space between lenses in some telescopes, due to its extremely low index of refraction.^[26] This method is especially used in solar telescopes where a vacuum tight telescope tube would be too heavy.^[168][169]

Helium is a commonly used carrier gas for gas chromatography.

The age of rocks and minerals that contain uranium and thorium can be estimated by measuring the level of helium with a process known as helium dating.^[24][26]

Helium at low temperatures is used in cryogenics, and in certain cryogenics applications. As examples of applications, liquid helium is used to cool certain metals to the extremely low temperatures required for superconductivity, such as in superconducting magnets for magnetic resonance imaging. The Large Hadron Collider at CERN uses 96 metric tons of liquid helium to maintain the temperature at 1.9 K (−271.25 °C; −456.25 °F).^[170]

Medical uses

Helium was approved for medical use in the United States in April 2020 for humans and animals.^[171][172]

As a contaminant

While chemically inert, helium contamination impairs the operation of microelectromechanical systems (MEMS) such that iPhones may fail.^[173]

Inhalation and safety

Effects

Neutral helium at standard conditions is non-toxic, plays no biological role and is found in trace amounts in human blood.

The speed of sound in helium is nearly three times the speed of sound in air. Because the natural resonance frequency of a gas-filled cavity is proportional to the speed of sound in the gas, when helium is inhaled, a corresponding increase occurs in the resonant frequencies of the vocal tract, which is the amplifier of vocal sound.^[24][174] This increase in the resonant frequency of the amplifier (the vocal tract) gives an increased amplification to the high-frequency components of the sound wave produced by the direct vibration of the vocal folds, compared to the case when the voice box is filled with air. When a person speaks after inhaling helium gas, the muscles that control the voice box still move in the same way as when the voice box is filled with air, therefore the fundamental frequency (sometimes called pitch) produced by direct vibration of the vocal folds does not change.^[175] However, the high-frequency-preferred amplification causes a change in timbre of the amplified sound, resulting in a reedy, duck-like vocal quality. The opposite effect, lowering resonant frequencies, can be obtained by inhaling a dense gas such as sulfur hexafluoride or xenon.

Hazards

Inhaling helium can be dangerous if done to excess, since helium is a simple asphyxiant and so displaces oxygen needed for normal respiration.^[24][176] Fatalities have been recorded, including a youth who suffocated in Vancouver in 2003 and two adults who suffocated in South Florida in 2006.^[177][178] In 1998, an Australian girl from Victoria fell unconscious and temporarily turned blue after inhaling the entire contents of a party balloon.^{[179][180][181]}
Inhaling helium directly from pressurized cylinders or even balloon filling valves is extremely dangerous, as high flow rate and pressure can result in barotrauma, fatally rupturing lung tissue.^[176][182]

Death caused by helium is rare. The first media-recorded case was that of a 15-year-old girl from Texas who died in 1998 from helium inhalation at a friend’s party; the exact type of helium death is unidentified.^{[179][180][181]}

In the United States only two fatalities were reported between 2000 and 2004, including a man who died in North Carolina of barotrauma in 2002.^[177][182] A youth asphyxiated in Vancouver during 2003, and a 27-year-old man in Australia had an embolism after breathing from a cylinder in 2000.^[177] Since then two adults asphyxiated in South Florida in 2006,^{[177][178][183]} and there were cases in 2009 and 2010, one a Californian youth who was found with a bag over his head, attached to a helium tank,^[184] and another teenager in Northern Ireland died of asphyxiation.^[185] At Eagle Point, Oregon a teenage girl died in 2012 from barotrauma at a party.^{[186][187][188]} A girl from Michigan died from hypoxia later in the year.^[189]

On February 4, 2015, it was revealed that, during the recording of their main TV show on January 28, a 12-year-old member (name withheld) of Japanese all-girl singing group 3B Junior suffered from air embolism, losing consciousness and falling into a coma as a result of air bubbles blocking the flow of blood to the brain, after inhaling huge quantities of helium as part of a game. The incident was not made public until a week later.^[190][191] The staff of TV Asahi held an emergency press conference to communicate that the member had been taken to the hospital and is showing signs of rehabilitation such as moving eyes and limbs, but her consciousness has not yet been sufficiently recovered. Police have launched an investigation due to a neglect of safety measures.^[192][193]

The safety issues for cryogenic helium are similar to those of liquid nitrogen; its extremely low temperatures can result in cold burns, and the liquid-to-gas expansion ratio can cause explosions if no pressure-relief devices are installed. Containers of helium gas at 5 to 10 K should be handled as if they contain liquid helium due to the rapid and significant thermal expansion that occurs when helium gas at less than 10 K is warmed to room temperature.^[91]

At high pressures (more than about 20 atm or two MPa), a mixture of helium and oxygen (heliox) can lead to high-pressure nervous syndrome, a sort of reverse-anesthetic effect; adding a small amount of nitrogen to the mixture can alleviate the problem.^[194][163]

See also

Notes

References

Bibliography

External links

General

• U.S. Government’s Bureau of Land Management: Sources, Refinement, and Shortage. With some history of helium.
• U.S. Geological Survey publications on helium beginning 1996: Helium
• Where is all the helium? Aga website
• It’s Elemental – Helium
• Chemistry in its element podcast (MP3) from the Royal Society of Chemistry’s Chemistry World: Helium
• International Chemical Safety Cards – Helium; includes health and safety information regarding accidental exposures to helium

More detail

• Helium at The Periodic Table of Videos (University of Nottingham)
• Helium at the Helsinki University of Technology; includes pressure-temperature phase diagrams for helium-3 and helium-4
• Lancaster University, Ultra Low Temperature Physics – includes a summary of some low temperature techniques
• Video: Demonstration of superfluid helium (Alfred Leitner, 1963, 38 min.)

Miscellaneous

• Physics in Speech with audio samples that demonstrate the unchanged voice pitch
• Article about helium and other noble gases

Helium shortage

• America’s Helium Supply: Options for Producing More Helium from Federal Land: Oversight Hearing before the Subcommittee on Energy and Mineral Resources of the Committee on Natural Resources, U.S. House Of Representatives, One Hundred Thirteenth Congress, First Session, Thursday, July 11, 2013
• Helium Program: Urgent Issues Facing BLM’s Storage and Sale of Helium Reserves: Testimony before the Committee on Natural Resources, House of Representatives Government Accountability Office
• Kramer, David (May 22, 2012). «Senate bill would preserve US helium reserve: Measure would give scientists first dibs on helium should a shortage develop. Physics Today web site». Archived from the original on October 27, 2012.
• Richardson, Robert C.; Chan, Moses (2009). «Helium, when will it run out?» (PDF). Archived from the original (PDF) on 2015-06-14.

У этого термина существуют и другие значения, см. Гелий (значения).

2 Водород ← Гелий → Литий 2He
Внешний вид простого вещества
Инертный газ без цвета, вкуса и запаха
Свойства атома
Имя, символ, номер	Ге́лий/Helium (He), 2
Атомная масса (молярная масса)	4,002602 а. е. м. (г/моль)
Электронная конфигурация	1s2
Радиус атома	? (31)[1] пм
Химические свойства
Ковалентный радиус	28[1] пм
Радиус иона	93[1] пм
Электроотрицательность	4,5 (шкала Полинга)
Электродный потенциал	0
Степени окисления	0
Энергия ионизации (первый электрон)	2361,3(24,47) кДж/моль (эВ)
Термодинамические свойства простого вещества
Плотность (при н. у.)	0,147 (при −270 °C) 0,00017846 (при +20 °C) г/см³
Температура плавления	0,95 (при 2,5 МПа)
Температура кипения	4,215 (для 4He)[2]
Теплота испарения	0,08 кДж/моль
Молярная теплоёмкость	20,79[2] Дж/(K·моль)
Молярный объём	31,8 см³/моль
Кристаллическая решётка простого вещества
Структура решётки	гексагональная
Параметры решётки	a=3,570; c=5,84 Å
Отношение c/a	1,633
Прочие характеристики
Теплопроводность	(300 K) 0,152 Вт/(м·К)

Ге́лий — второй элемент периодической системы химических элементов Д. И. Менделеева с атомным номером 2. Расположен в главной подгруппе восьмой группы, первом периоде периодической системы. Возглавляет группу инертных газов в периодической системе Менделеева. Обозначается символом He (лат. Helium). Простое вещество гелий (CAS-номер: 7440-59-7) — инертный одноатомный газ без цвета, вкуса и запаха.

Гелий — один из наиболее распространённых элементов во Вселенной, он занимает второе место после водорода. Также гелий является вторым по лёгкости (после водорода) химическим веществом.

Гелий добывается из природного газа процессом низкотемпературного разделения — так называемой фракционной перегонкой (см. Фракционная дистилляция в статье Дистилляция).

История

18 августа 1868 года французский учёный Пьер Жансен, находясь во время полного солнечного затмения в индийском городе Гунтур, впервые исследовал хромосферу Солнца. Жансену удалось настроить спектроскоп таким образом, чтобы спектр короны Солнца можно было наблюдать не только при затмении, но и в обычные дни. На следующий же день спектроскопия солнечных протуберанцев наряду с линиями водорода — синей, зелено-голубой и красной — выявила очень яркую жёлтую линию, первоначально принятую Жансеном и другими наблюдавшими её астрономами за линию D натрия. Жансен немедленно написал об этом во Французскую Академию наук. Впоследствии было установлено, что ярко-жёлтая линия в солнечном спектре не совпадает с линией натрия и не принадлежит ни одному из ранее известных химических элементов^[3][4].

Спустя два месяца 20 октября английский астроном Норман Локьер, не зная о разработках французского коллеги, также провёл исследования солнечного спектра. Обнаружив неизвестную жёлтую линию с длиной волны 588 нм (более точно 587,56 нм), он обозначил её D₃, так как она была очень близко расположена к Фраунгоферовым линиям D₁ (589,59 нм) и D₂ (588,99 нм) натрия. Спустя два года Локьер, совместно с английским химиком Эдвардом Франкландом, в сотрудничестве с которым он работал, предложил дать новому элементу название «гелий» (от др.-греч. ἥλιος — «солнце»)^[4].

Интересно, что письма Жансена и Локьера пришли во Французскую Академию наук в один день — 24 октября 1868 года, однако письмо Локьера, написанное им четырьмя днями ранее, пришло на несколько часов раньше. На следующий день оба письма были зачитаны на заседании Академии. В честь нового метода исследования протуберанцев Французская академия решила отчеканить медаль. На одной стороне медали были выбиты портреты Жансена и Локьера над скрещенными ветвями лавра, а на другой — изображение мифического бога Солнца Аполлона, правящего в колеснице четверкой коней, скачущей во весь опор^[4].

В 1881 году итальянец Луиджи Пальмиери опубликовал сообщение об открытии им гелия в вулканических газах (фумаролах). Он исследовал светло-желтое маслянистое вещество, оседавшее из газовых струй на краях кратера Везувия. Пальмиери прокаливал этот вулканический продукт в пламени бунзеновской горелки и наблюдал спектр выделявшихся при этом газов. Ученые круги встретили это сообщение с недоверием, так как свой опыт Пальмиери описал неясно. Спустя многие годы в составе фумарол действительно были найдены небольшие количества гелия и аргона^[4].

Только через 27 лет после своего первоначального открытия гелий был обнаружен на Земле — в 1895 году шотландский химик Уильям Рамзай, исследуя образец газа, полученного при разложении минерала клевеита, обнаружил в его спектре ту же ярко-жёлтую линию, найденную ранее в солнечном спектре. Образец был направлен для дополнительного исследования известному английскому ученому-спектроскописту Уильяму Круксу, который подтвердил, что наблюдаемая в спектре образца жёлтая линия совпадает с линией D₃ гелия. 23 марта 1895 года Рамзай отправил сообщение об открытии им гелия на Земле в Лондонское королевское общество, а также во Французскую академию через известного химика Марселена Бертло^[4].

Шведские химики П. Клеве и Н. Ленгле смогли выделить из клевеита достаточно газа, чтобы установить атомный вес нового элемента^{[источник не указан 1252 дня]}.

В 1896 году Генрих Кайзер, Зигберт Фридлендер, а еще через два года Эдвард Бэли окончательно доказали присутствие гелия в атмосфере^[4][5][6].

Еще до Рамзая гелий выделил также американский химик Фрэнсис Хиллебранд, однако он ошибочно полагал, что получил азот^[6] и в письме Рамзаю признал за ним приоритет открытия.

Исследуя различные вещества и минералы, Рамзай обнаружил, что гелий в них сопутствует урану и торию. Но только значительно позже, в 1906 году, Резерфорд и Ройдс установили, что альфа-частицы радиоактивных элементов представляют собой ядра гелия. Эти исследования положили начало современной теории строения атома^[7].

Только в 1908 году нидерландскому физику Хейке Камерлинг-Оннесу удалось получить жидкий гелий дросселированием (см. Эффект Джоуля — Томсона), после того как газ был предварительно охлажден в кипевшем под вакуумом жидком водороде. Попытки получить твёрдый гелий еще долго оставались безуспешными даже при температуре в 0,71 K, которых достиг ученик Камерлинг-Оннеса — немецкий физик Виллем Хендрик Кеезом. Лишь в 1926 году, применив давление выше 35 атм и охладив сжатый гелий в кипящем под разрежением жидком гелии, ему удалось выделить кристаллы^[8].

В 1932 году Кеезом исследовал характер изменения теплоёмкости жидкого гелия с температурой. Он обнаружил, что около 2,19 K медленный и плавный подъём теплоёмкости сменяется резким падением и кривая теплоёмкости приобретает форму греческой буквы λ (лямбда). Отсюда температуре, при которой происходит скачок теплоёмкости, присвоено условное название «λ-точка»^[8]. Более точное значение температуры в этой точке, установленное позднее — 2,172 K. В λ-точке происходят глубокие и скачкообразные изменения фундаментальных свойств жидкого гелия — одна фаза жидкого гелия сменяется в этой точке на другую, причем без выделения скрытой теплоты; имеет место фазовый переход II рода. Выше температуры λ-точки существует так называемый гелий-I, а ниже её — гелий-II^[8].

В 1938 году советский физик Пётр Леонидович Капица открыл явление сверхтекучести жидкого гелия-II, которое заключается в резком снижении коэффициента вязкости, вследствие чего гелий течёт практически без трения^[8][9]. Вот что он писал в одном из своих докладов про открытие этого явления^[10]:

… такое количество тепла, которое фактически переносилось, лежит за пределами физических возможностей, что тело ни по каким физическим законам не может переносить больше тепла, чем его тепловая энергия, помноженная на скорость звука. С помощью обычного механизма теплопроводности тепло не могло переноситься в таком масштабе, как это наблюдалось. Надо было искать другое объяснение.
И вместо того, чтобы объяснить перенос тепла теплопроводностью, то есть передачей энергии от одного атома к другому, можно было объяснить его более тривиально — конвекцией, переносом тепла в самой материи. Не происходит ли дело так, что нагретый гелий движется вверх, а холодный опускается вниз, благодаря разности скоростей возникают конвекционные токи, и таким образом происходит перенос тепла. Но для этого надо было предположить, что гелий при своем движении течет без всякого сопротивления. У нас уже был случай, когда электричество двигалось без всякого сопротивления по проводнику. И я решил, что гелий так же движется без всякого сопротивления, что он является не сверхтеплопроводным веществом, а сверхтекучим. …
… Если вязкость воды равняется 10⁻² П, то это в миллиард раз более текучая жидкость, чем вода …

Происхождение названия

От греч. ἥλιος — «Солнце» (см. Гелиос). Любопытен тот факт, что в названии элемента было использовано характерное для металлов окончание «-ий» (по лат. «-um» — «Helium»), так как Локьер предполагал, что открытый им элемент является металлом. По аналогии с другими благородными газами логично было бы дать ему имя «гелион» («Helion»)^[4]. В современной науке название «гелион» закрепилось за ядром лёгкого изотопа гелия — гелия-3.

Распространённость

Во Вселенной

Гелий занимает второе место по распространённости во Вселенной после водорода — около 23 % по массе^[11]. Однако на Земле гелий редок. Практически весь гелий Вселенной образовался в первые несколько минут после Большого Взрыва^[12][13], во время первичного нуклеосинтеза. В современной Вселенной почти весь новый гелий образуется в результате термоядерного синтеза из водорода в недрах звёзд (см. протон-протонный цикл, углеродно-азотный цикл). На Земле он образуется в результате альфа-распада тяжёлых элементов (альфа-частицы, излучаемые при альфа-распаде — это ядра гелия-4)^[14]. Часть гелия, возникшего при альфа-распаде и просачивающегося сквозь породы земной коры, захватывается природным газом, концентрация гелия в котором может достигать 7 % от объёма и выше.

Земная кора

В рамках восьмой группы гелий по содержанию в земной коре занимает второе место (после аргона)^[15].

Содержание гелия в атмосфере (образуется в результате распада Ac, Th, U) — 5,27·10⁻⁴ % по объёму, 7,24·10⁻⁵ % по массе^[2][6][14]. Запасы гелия в атмосфере, литосфере и гидросфере оцениваются в 5·10¹⁴ м³^[2]. Гелионосные природные газы содержат как правило до 2 % гелия по объёму. Исключительно редко встречаются скопления газов, гелиеносность которых достигает 8 — 16 %^[14].

Среднее содержание гелия в земном веществе — 0,003 мг/кг или 0,003 г/т^[14]. Наибольшая концентрация гелия наблюдается в минералах, содержащих уран, торий и самарий: клевеите, фергюсоните, самарските, гадолините, монаците (монацитовые пески в Индии и Бразилии), торианите. Содержание гелия в этих минералах составляет 0,8 — 3,5 л/кг, а в торианите оно достигает 10,5 л/кг^[6][14]. Этот гелий является радиогенным и содержит лишь изотоп ⁴He, он образуется из альфа-частиц, излучаемых при альфа-распаде урана, тория и их дочерних радионуклидов.

Определение

Качественно гелий определяют с помощью анализа спектров испускания (характеристические линии 587,56 нм и 388,86 нм), количественно — масс-спектрометрическими и хроматографическими методами анализа, а также методами, основанными на измерении физических свойств (плотности, теплопроводности и др.)^[2].

Физические свойства

Гелий — практически инертный химический элемент.

Простое вещество гелий — нетоксично, не имеет цвета, запаха и вкуса. При нормальных условиях представляет собой одноатомный газ. Его точка кипения (T = 4,215 K для ⁴He) наименьшая среди всех простых веществ; твёрдый гелий получен лишь при давлениях выше 25 атмосфер — при атмосферном давлении он не переходит в твёрдую фазу даже при крайне близких к абсолютному нулю температурах. Экстремальные условия также необходимы для создания немногочисленных химических соединений гелия, все они нестабильны при нормальных условиях.

Химические свойства

Гелий — наименее химически активный элемент восьмой группы таблицы Менделеева (инертные газы) ^[16]. Многие соединения гелия существуют только в газовой фазе в виде так называемых эксимерных молекул, у которых устойчивы возбуждённые электронные состояния и неустойчиво основное состояние. Гелий образует двухатомные молекулы He₂⁺, фторид HeF, хлорид HeCl (эксимерные молекулы образуются при действии электрического разряда или ультрафиолетового излучения на смесь гелия с фтором или хлором).

Энергия связи молекулярного иона гелия He₂⁺ составляет 58 ккал/моль, равновесное межъядерное расстояние 1,09 Å.^[17]

Известно химическое соединение гелия LiHe (возможно, имелось в виду соединение LiHe₇)^[18][19].

Свойства в газовой фазе

При нормальных условиях гелий ведёт себя практически как идеальный газ. При всех условиях гелий является моноатомным веществом. При нормальных условиях, плотность составляет 0,17847 кг/м³, обладает тепло­проводностью 0,1437 ^Вт⁄_(м·К) — бо́льшей, чем у всех других газов за исключением водорода, а его удельная теплоёмкость чрезвычайно высока (с_р = 5,23 ^кДж⁄_(кг·К), для сравнения — 14,23 ^кДж⁄_(кг·К) для Н₂).

При пропускании тока через заполненную гелием трубку наблюдаются разряды различных цветов, зависящих главным образом от давления газа в трубке. Обычно видимый свет спектра гелия имеет жёлтую окраску. По мере уменьшения давления происходит смена цветов — розового, оранжевого, жёлтого, ярко-жёлтого, жёлто-зелёного и зелёного. Это связано с присутствием в спектре гелия нескольких серий линий, расположенных в диапазоне между инфракрасной и ультрафиолетовой частями спектра, важнейшие линии гелия в видимой части спектра лежат между 706,52 нм и 447,14 нм^[8]. Уменьшение давления приводит к увеличению длины свободного пробега электрона, то есть к возрастанию его энергии при столкновении с атомами гелия. Это приводит к переводу атомов в возбуждённое состояние с бо́льшей энергией, в результате чего и происходит смещение спектральных линий от инфракрасного к ультрафиолетовому краю.

Хорошо изученный спектр гелия имеет два резко различных набора серий линий — единичных (¹S₀) и триплетных (³S₁), поэтому в конце 19 века Локьер, Рунге и Пашен предположили, что гелий состоит из смеси двух газов; один из них имел в спектре жёлтую линию 587,56 нм, другой — зелёную 501,6 нм. Этот второй газ они предложили назвать астерием (Asterium) от греч. звёздный. Однако Рамзай и Траверс показали, что спектр гелия зависит от условий: при давлении газа 7—8 мм рт.ст. наиболее ярка жёлтая линия; при уменьшении давления увеличивается интенсивность зелёной линии. Спектры атома гелия были объяснены Гейзенбергом в 1926 г.^[20] (см. Обменное взаимодействие). Спектр зависит от взаимного направления спинов электронов в атоме — атом с противоположно направленными спинами (дающий зелёную линию в оптических спектрах) получил название парагелия, с сонаправленными спинами (с жёлтой линией в спектре) назван ортогелием. Линия парагелия — одиночки, линии ортогелия — весьма узкие триплеты. Атом гелия в нормальных условиях находится в одиночном (синглетном) состоянии. Чтобы атом гелия перевести в триплетное состояние, нужно затратить работу в 19,77 эВ. Переход атома гелия из триплетного состояния в синглетное сам по себе осуществляется чрезвычайно редко. Такое состояние, из которого переход в более глубокое сам по себе маловероятен, носит название метастабильного. Вывести атом из метастабильного состояния в стабильное можно, подвергая атом внешнему воздействию, например, электронным ударом или при столкновении с другим атомом с передачей последнему непосредственно энергии возбуждения.^[21] В атоме парагелия (синглетного состояния гелия) спины электронов направлены противоположно, и суммарный спиновый момент равен нулю. В триплетном состоянии (ортогелий) спины электронов сонаправлены, суммарный спиновый момент равен единице. Принцип Паули запрещает двум электронам находиться в состоянии с одинаковыми квантовыми числами, поэтому электроны в низшем энергетическом состоянии ортогелия, имея одинаковые спины, вынуждены иметь различные главные квантовые числа: один электрон находится на 1s-орбитали, а второй — на более удалённой от ядра 2s-орбитали (состояние оболочки 1s2s). У парагелия оба электрона находятся в 1s-состоянии (состояние оболочки 1s²).

Спонтанный интеркомбинационный (то есть сопровождающийся изменением суммарного спина) переход с излучением фотона между орто- и парагелием чрезвычайно сильно подавлен, однако возможны безызлучательные переходы при взаимодействии с налетающим электроном или другим атомом.

В бесстолкновительной среде (например, в межзвёздном газе) спонтанный переход из нижнего состояния ортогелия 2³S₁ в основное состояние парагелия 1⁰S₁ возможен путём излучения одновременно двух фотонов или в результате однофотонного магнитно-дипольного перехода (M1). В этих условиях расчётное время жизни атома ортогелия за счёт двухфотонного распада 2³S₁ → 1⁰S₁ + 2γ составляет 2,49·10⁸ с, или 7,9 года^[22]. Первые теоретические оценки^[23] показывали^[24], что время жизни за счёт магнитно-дипольного перехода на порядки больше, то есть что доминирует двухфотонный распад. Лишь через три десятилетия, после неожиданного открытия запрещённых триплетно-синглетных переходов некоторых гелиеподобных ионов в спектрах солнечной короны^[25] было обнаружено^[26], что однофотонный магнитно-дипольный распад 2³S₁-состояния значительно более вероятен; время жизни при распаде по этому каналу составляет «всего» 8·10³ с^[27].

Следует отметить, что время жизни первого возбуждённого состояния атома парагелия 2⁰S₁ также крайне велико по атомным масштабам. Правила отбора для этого состояния запрещают однофотонный переход 2⁰S₁ → 1⁰S₁ + γ^[28], а для двухфотонного распада время жизни составляет 19,5 мс^[22].

Гелий менее растворим в воде, чем любой другой известный газ. В 1 л воды при 20 °C растворяется около 8,8 мл (9,78 при 0 °C, 10,10 при 80 °C), в этаноле — 2,8 мл/л (15 °C), 3,2 мл/л (25 °C). Скорость его диффузии сквозь твёрдые материалы в три раза выше, чем у воздуха, и приблизительно на 65 % выше, чем у водорода.

Коэффициент преломления гелия ближе к единице, чем у любого другого газа. Этот газ имеет отрицательный коэффициент Джоуля — Томсона при нормальной температуре среды, то есть он нагревается, когда ему дают возможность свободно увеличиваться в объёме. Только ниже температуры инверсии Джоуля — Томсона (приблизительно 40 К при нормальном давлении) он остывает во время свободного расширения. После охлаждения ниже этой температуры гелий может быть превращён в жидкость при расширительном охлаждении. Такое охлаждение производится при помощи детандера.

Свойства конденсированных фаз

В 1908 году Х.Камерлинг-Оннес впервые смог получить жидкий гелий. Твёрдый гелий удалось получить лишь под давлением 25 атмосфер при температуре около 1 К (В. Кеезом, 1926). Кеезом также открыл наличие фазового перехода гелия-4 (⁴He) при температуре 2,17K; назвал фазы гелий-I и гелий-II (ниже 2,17 K). В 1938 году П. Л. Капица обнаружил, что у гелия-II отсутствует вязкость (явление сверхтекучести). В гелии-3 сверхтекучесть возникает лишь при температурах ниже 0,0026 К. Сверхтекучий гелий относится к классу так называемых квантовых жидкостей, макроскопическое поведение которых может быть описано только с помощью квантовой механики. В 2004 году появилось сообщение об открытии сверхтекучести твёрдого гелия (т. н. эффект суперсолид) при исследовании его в торсионном осцилляторе. Однако многие исследователи сходятся во мнении, что обнаруженный в 2004 году эффект не имеет ничего общего со сверхтекучестью кристалла. В настоящее время продолжаются многочисленные экспериментальные и теоретические исследования, целью которых является понимание истинной природы данного явления.

Изотопы

Природный гелий состоит из двух стабильных изотопов: ⁴He (изотопная распространённость — 99,99986 %) и гораздо более редкого ³He (0,00014 %; содержание гелия-3 в разных природных источниках может варьироваться в довольно широких пределах). Известны ещё шесть искусственных радиоактивных изотопов гелия.

Получение

В промышленности гелий получают из гелийсодержащих природных газов (в настоящее время эксплуатируются главным образом месторождения, содержащие > 0,1 % гелия). От других газов гелий отделяют методом глубокого охлаждения, используя то, что он сжижается труднее всех остальных газов. Охлаждение производят дросселированием в несколько стадий очищая его от CO₂ и углеводородов. В результате получается смесь гелия, неона и водорода. Эту смесь, т. н. сырой гелий, (He — 70-90 % об.) очищают от водорода (4-5 %) с помощью CuO при 650—800 К. Окончательная очистка достигается охлаждением оставшейся смеси кипящим под вакуумом N₂ и адсорбцией примесей на активном угле в адсорберах, также охлаждаемых жидким N₂. Производят гелий технической чистоты (99,80 % по объёму гелий) и высокой чистоты (99,985 %).

В России газообразный гелий получают из природного и нефтяного газов. В настоящее время гелий извлекается на гелиевом заводе ООО «Газпром добыча Оренбург»^[29] в Оренбурге из газа с низким содержанием гелия (до 0,055 % об.), поэтому российский гелий имеет высокую себестоимость. Актуальной проблемой является освоение и комплексная переработка природных газов крупных месторождений Восточной Сибири с высоким содержанием гелия (0,15-1 % об.), что позволит намного снизить его себестоимость.

По производству гелия лидируют США (140 млн м³ в год), затем — Алжир (16 млн м³). Россия занимает третье место в мире — 6 млн м³ в год. Мировые запасы гелия составляют 45,6 млрд м³.

В 2003 г. производство гелия в мире составило 110 млн м3, в том числе в США — 87 млн м3, Алжире — 16 млн м3, России — более 6 млн м3, Польше — около 1 млн м3.^[30]

Транспортировка

Для транспортировки газообразного гелия используются стальные баллоны (ГОСТ 949-73) коричневого цвета, помещаемые в специализированные контейнеры. Для перевозки можно использовать все виды транспорта при соблюдении соответствующих правил перевозки газов.

Для перевозки жидкого гелия применяются специальные транспортные сосуды типа СТГ-10, СТГ-25 и т. п. светло-серого цвета объёмом 10, 25, 40, 250 и 500 литров, соответственно. При выполнении определённых правил транспортировки может использоваться железнодорожный, автомобильный и другие виды транспорта. Сосуды с жидким гелием обязательно должны храниться в вертикальном положении.

Применение

Уникальные свойства гелия широко используются в промышленности и народном хозяйстве:

• в металлургии в качестве защитного инертного газа для выплавки чистых металлов^{[источник не указан 214 дней]}
• в пищевой промышленности зарегистрирован в качестве пищевой добавки E939, в качестве пропеллента и упаковочного газа
• используется в качестве хладагента для получения сверхнизких температур (в частности, для перевода металлов в сверхпроводящее состояние)
• для наполнения воздухоплавающих судов (дирижабли и аэростаты) — при незначительной по сравнению с водородом потере в подъемной силе гелий в силу негорючести абсолютно безопасен
• в дыхательных смесях для глубоководного погружения (см. Баллон для дайвинга)
• для наполнения воздушных шариков и оболочек метеорологических зондов
• для заполнения газоразрядных трубок
• в качестве теплоносителя в некоторых типах ядерных реакторов
• в качестве носителя в газовой хроматографии
• для поиска утечек в трубопроводах и котлах (см. Гелиевый течеискатель)
• как компонент рабочего тела в гелий-неоновых лазерах
• нуклид ³He активно используется в технике нейтронного рассеяния в качестве поляризатора и наполнителя для позиционно-чувствительных нейтронных детекторов
• нуклид ³He является перспективным топливом для термоядерной энергетики

В геологии

Гелий — удобный индикатор для геологов. При помощи гелиевой съёмки^[31] можно определять на поверхности Земли расположение глубинных разломов. Гелий, как продукт распада радиоактивных элементов, насыщающих верхний слой земной коры, просачивается по трещинам, поднимается в атмосферу. Около таких трещин и особенно в местах их пересечения концентрация гелия более высокая. Это явление было впервые установлено советским геофизиком И. Н. Яницким во время поисков урановых руд. Эта закономерность используется для исследования глубинного строения Земли и поиска руд цветных и редких металлов^[32].

В астрономии

В честь гелия назван астероид (895) Гелио (англ.)русск., открытый в 1918 году.

Биологическая роль

На данный момент биологическая роль не выяснена.

Физиологическое действие

• Хотя инертные газы обладают наркозным действием, это воздействие у гелия и неона при атмосферном давлении не проявляется, в то время как при повышении давления раньше возникают симптомы «нервного синдрома высокого давления» (НСВД)^[33].

• Вдыхание гелия вызывает кратковременное повышение тембра голоса (обратное эффекту вдыхания ксенона).

Стоимость

• В 2009 г. цены частных компаний на газообразный гелий находились в пределах 2,5—3 $/м³^[34].
• В 2010 г. цена в Европе на сжиженный гелий была около 11 евро за литр. В 2012 году — 23 евро за литр

Интересные факты

• Гелий — вещество с самой низкой температурой кипения. Гелий кипит при температуре −269 °C^[35].

См. также

• Гелий-3 — лёгкий нерадиоактивный изотоп гелия.
• Эффект Померанчука — аномальный характер плавления (или затвердевания) лёгкого изотопа гелия ³He
• Гелиеметрия — наука, изучающая прохождение гелия через различные среды.
• Жидкий гелий
• Твёрдый гелий

Примечания

Ссылки

	Гелий на Викискладе?

• Гелий на Webelements
• Гелий в Популярной библиотеке химических элементов
• Гелиевая съемка
• Гелиевая съемка на Рустамовской площади и Айском блоке в Башкирии

	гелий в Викисловаре?

Изотопы гелия
Гипотетические: 2He: Гелий-2 (Дипротон) Стабильные: 3He: Гелий-3, 4He: Гелий-4 Нестабильные (менее суток): 5He: Гелий-5, 6He: Гелий-6, 7He: Гелий-7, 8He: Гелий-8, 9He: Гелий-9, 10He: Гелий-10 см. также. Гелий, Таблица нуклидов

Периодическая система химических элементов Д. И. Менделеева
	1	2															3	4	5	6	7	8	9	10	11	12	13	14	15	16	17	18
1	H		He
2	Li	Be		B	C	N	O	F	Ne
3	Na	Mg		Al	Si	P	S	Cl	Ar
4	K	Ca		Sc	Ti	V	Cr	Mn	Fe	Co	Ni	Cu	Zn	Ga	Ge	As	Se	Br	Kr
5	Rb	Sr		Y	Zr	Nb	Mo	Tc	Ru	Rh	Pd	Ag	Cd	In	Sn	Sb	Te	I	Xe
6	Cs	Ba	La	Ce	Pr	Nd	Pm	Sm	Eu	Gd	Tb	Dy	Ho	Er	Tm	Yb	Lu	Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg	Tl	Pb	Bi	Po	At	Rn
7	Fr	Ra	Ac	Th	Pa	U	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr	Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Uut	Fl	Uup	Lv	Uus	Uuo
Щелочные металлы  Щёлочноземельные металлы  Лантаноиды Актиноиды Переходные металлы Другие металлы Металлоиды Другие неметаллы Галогены Инертные газы

• https://ru.wikipedia.org/wiki/%D0%93%D0%B5%D0%BB%D0%B8%D0%B9
• http://www.favorit-nn.ru/articles/?child_id=6

---

Ге́лий (He) — 2 элемент периодической системы элементов, газ.

Гелий — практически инертный химический элемент. Возглавляет группу инертных газов в периодической таблице. Нетоксичен, не имеет цвета, запаха и вкуса. При нормальных условиях представляет собой одноатомный газ. Его точка кипения (T = 4,216 K) наименьшая среди всех элементов; твёрдый гелий получен лишь при давлениях выше 25 атмосфер — при атмосферном давлении он не переходит в твёрдую фазу даже при абсолютном нуле. Экстремальные условия также необходимы для создания немногочисленных химических соединений гелия, все они нестабильны при стандартных температуре и давлении. Природный гелий состоит из двух стабильных изотопов: ⁴He (изотопная распространённость — 99,99986 %) и гораздо более редкого ³He (0,00014 %; содержание гелия-3 в разных природных источниках может варьировать в довольно широких пределах). Известны ещё шесть искусственных радиоактивных изотопов гелия.

Гелий занимает второе место по распространённости во Вселенной и лёгкости (после водорода). Однако на Земле гелий редок. Практически весь гелий Вселенной образовался в первые несколько минут после Большого Взрыва, во время первичного нуклеосинтеза. В современной Вселенной почти весь новый гелий образуется в результате термоядерного синтеза из водорода в недрах звёзд. На Земле он образуется в результате альфа-распада тяжёлых элементов (альфа-частицы, излучаемые при альфа-распаде — это ядра гелия-4). Часть гелия, возникшего при альфа-распаде и просачивающегося сквозь породы земной коры, захватывается природным газом, концентрация гелия в котором может достигать 7 % от объёма. Гелий добывается из природного газа процессом низкотемпературного разделения — так называемой фракционной перегонкой (см. Фракционная дистилляция в статье Дистилляция).

История

Открытие гелия началось с 1868 года, когда при наблюдении солнечного затмения два астронома — француз П. Ж. Жансен и англичанин Д. Н. Локьер — независимо друг от друга обнаружили в спектре солнечной короны жёлтую линию (она получила название D₃-линии), которую нельзя было приписать ни одному из известных в то время элементов. В 1871 году Локьер объяснил её происхождение присутствием на Солнце нового элемента. В 1895 году англичанин У. Рамзай выделил из природной радиоактивной руды клевеита газ, в спектре которого присутствовала та же D₃-линия.

Происхождение названия

Локьер дал гелию имя, отражающее историю его открытия (от греч. Ήλιο (Helio) — солнце). Поскольку Локьер полагал, что обнаруженный элемент — металл, он использовал в латинском названии элемента окончание «-ium» (соответствует русскому окончанию «-ий»), которое обычно употребляется в названии металлов. Таким образом, гелий задолго до своего открытия на Земле получил имя, которое окончанием отличает его от названий остальных инертных газов.

Получение

В настоящее время гелий выделяют из природных гелийсодержащих газов, пользуясь методом глубокого охлаждения (гелий сжижается труднее всех остальных газов). Месторождения таких газов имеются в России, США, Канаде, Китае, Алжире, Польше и Катаре. Гелий содержится также в некоторых минералах (монаците, торианите и других), при этом из 1 кг минерала при нагревании можно выделить до 10 л гелия.

Свойства в газовой фазе

Гелий —— наименее химически активный элемент восьмой группы (инертные газы) таблицы Менделеева. Многие соединения гелия существуют только в газовой фазе в виде так называемых эксимерных молекул, у которых устойчивы возбужденные электронные состояния и неустойчиво основное состояние. Гелий образует двухатомные молекулы He₂, фторид HeF, хлорид HeCl (эксимерные молекулы образуются при действии электрического разряда или УФ излучения на смесь гелия газа и фтора (хлора)). При стандартных температуре и давлении гелий ведёт себя практически как идеальный газ. Фактически при всех условиях гелий моноатомный. Он обладает теплопроводностью большей, чем у других газов, кроме водорода, и его удельная теплоёмкость чрезвычайно высока. Гелий также менее растворим в воде, чем любой другой известный газ. Скорость его диффузии сквозь твёрдые материалы в три раза выше, чем у воздуха, и приблизительно на 65 % выше, чем у водорода. Примерный диаметр молекулы He₂ — 0,20 нм. Коэффициент преломления гелия ближе к единице, чем у любого другого газа. Этот газ имеет отрицательный коэффициент Джоуля-Томсона при нормальной температуре среды, то есть он нагревается, когда ему дают возможность свободно увеличиваться в объёме. Только ниже температуры инверсии Джоуля-Томсона (приблизительно 40 К при нормальном давлении) он остывает во время свободного расширения. После охлаждения ниже этой температуры, гелий может быть превращён в жидкость при расширительном охлаждении. Такое охлаждение производится при помощи детандера.

Свойства конденсированных фаз

В 1908 году Х.Камерлинг-Оннес впервые смог получить жидкий гелий. Твёрдый гелий удалось получить лишь под давлением 25 атмосфер при температуре около 1 К (В.Кеезом, 1926). Кеезом также открыл наличие фазового перехода гелия-IV при температуре 2,17K; назвал фазы гелий-I и гелий-II (ниже 2,17K). В 1938 году П. Л. Капица обнаружил, что у гелия-II отсутствует вязкость (явление сверхтекучести). В гелии-3 сверхтекучесть возникает лишь при температурах ниже 0,0026 К. Сверхтекучий гелий относится к классу так называемых квантовых жидкостей, макроскопическое поведение которых может быть описано только с помощью квантовой механики. В 2004 году появилось сообщение об открытии сверхтекучести твёрдого гелия, однако интерпретация этого явления не до конца понятна.

Применение

Гелий используют для создания инертной и защитной атмосферы при сварке, резке и плавке металлов, при перекачивании ракетного топлива, для наполнения дирижаблей и аэростатов, как компонент активной среды гелий-неоновых лазеров. Гелий-3 используется для наполнения газовых нейтронных детекторов, как рабочее тело гелиевых течеискателей. Жидкий гелий, самая холодная жидкость на Земле, — уникальный хладагент в экспериментальной физике, позволяющий использовать сверхнизкие температуры в научных исследованиях (например, при изучении электрической сверхпроводимости). Благодаря тому, что гелий очень плохо растворим в крови, его используют как составную часть газовой смеси, подаваемой для дыхания водолазам — замена азота воздуха на гелий предотвращает кессонную болезнь (при вдыхании обычного воздуха содержащийся в нём азот под повышенным давлением растворяется в крови, а при падении давления выделяется из неё в виде пузырьков, закупоривающих мелкие сосуды).

Ссылки

• Гелий на Webelements
• Гелий в Популярной библиотеке химических элементов
• «Гелий» — статья в Физической энциклопедии

Периодическая система элементов

H

He

Li

Be

B

C

N

O

F

Ne

Na

Mg

Al

Si

P

S

Cl

Ar

K

Ca

Sc

Ti

V

Cr

Mn

Fe

Co

Ni

Cu

Zn

Ga

Ge

As

Se

Br

Kr

Rb

Sr

Y

Zr

Nb

Mo

Tc

Ru

Rh

Pd

Ag

Cd

In

Sn

Sb

Te

I

Xe

Cs

Ba

*

Hf

Ta

W

Re

Os

Ir

Pt

Au

Hg

Tl

Pb

Bi

Po

At

Rn

Fr

Ra

**

Rf

Db

Sg

Bh

Hs

Mt

Ds

Rg

Uub

Uut

Uuq

Uup

Uuh

Uus

Uuo

*

La

Ce

Pr

Nd

Pm

Sm

Eu

Gd

Tb

Dy

Ho

Er

Tm

Yb

Lu

**

Ac

Th

Pa

U

Np

Pu

Am

Cm

Bk

Cf

Es

Fm

Md

No

Lr

---

Википедия Гелий адрес Викисловарь — адрес Викицитатник — адрес Викиучебник — адрес Викитека — адрес Викиновости — адрес Викиверситет — адрес Викигид — адрес

Выделить Гелий и найти в: Вокруг света адрес Академик адрес Астронет адрес Элементы адрес Научная Россия адрес Кругосвет адрес Научная Сеть Традиция — адрес Циклопедия — адрес Викизнание — адрес

Google Bing Yahoo Яндекс Mail.ru Рамблер Нигма.РФ Спутник Google Scholar Апорт Онлайн-переводчик Архив Интернета Научно-популярные фильмы на Яндексе Документальные фильмы

Список ru-вики Вики-сайты на русском языке Список крупных русскоязычных википроектов Каталог wiki-сайтов Русскоязычные wiki-проекты Викизнание:Каталог wiki-сайтов Научно-популярные сайты в Интернете Лучшие научные сайты на нашем портале Лучшие научно-популярные сайты Каталог научно-познавательных сайтов НАУКА В РУНЕТЕ: каталог научных и научно-популярных сайтов

---

• Страница 0 — краткая статья
• Страница 1 — энциклопедическая статья
• Разное — на страницах: 2 , 3 , 4 , 5
• Прошу вносить вашу информацию в «Гелий 1», чтобы сохранить ее

Комментарии читателей: