Helium

  • helium, 2he
    helium discharge tube.jpg
    helium
    pronunciationm/ (hee-lee-əm)
    appearancecolorless 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, std(he)4.002602(2)[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
    hydrogenheliumlithium
    atomic number (z)2
    groupgroup 18 (noble gases)
    periodperiod 1
    blocks-block
    element category  noble gas
    electron configuration1s2
    electrons per shell2
    physical properties
    phase at stpgas
    melting point0.95 k ​(−272.20 °c, ​−457.96 °f) (at 2.5 mpa)
    boiling point4.222 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 point2.177 k, ​5.043 kpa
    critical point5.1953 k, 0.22746 mpa
    heat of fusion0.0138 kj/mol
    heat of vaporization0.0829 kj/mol
    molar heat capacity20.78 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 states0
    electronegativitypauling scale: no data
    ionization energies
    • 1st: 2372.3 kj/mol
    • 2nd: 5250.5 kj/mol
    covalent radius28 pm
    van der waals radius140 pm
    color lines in a spectral range
    spectral lines of helium
    other properties
    natural occurrenceprimordial
    crystal structurehexagonal close-packed (hcp)
    hexagonal close-packed crystal structure for helium
    speed of sound972 m/s
    thermal conductivity0.1513 w/(m·k)
    magnetic orderingdiamagnetic[3]
    magnetic susceptibility−1.88·10−6 cm3/mol (298 k)[4]
    cas number7440-59-7
    history
    namingafter helios, greek titan of the sun
    discoverypierre janssen, norman lockyer (1868)
    first isolationwilliam ramsay, per teodor cleve, abraham langlet (1895)
    main isotopes of helium
    iso­tope abun­dance half-life (t1/2) decay mode pro­duct
    3he 0.0002% stable
    4he 99.9998% stable
    category category: helium
    | references

    helium (from greek: ἥλιος, romanizedhelios, 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, the first in the noble gas group in the periodic table. its boiling point is the lowest among all the elements. helium is the second lightest and second most abundant element in the observable universe (hydrogen is the lightest and most abundant). 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. this is 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. most helium in the universe is helium-4, the vast majority of which was formed during the big bang. large amounts of new helium are being created by nuclear fusion of hydrogen in stars.

    helium is named for the greek titan of the sun, helios. it was first detected as an unknown, yellow spectral line signature in sunlight, during a solar eclipse in 1868 by georges rayet,[5] captain c. t. haig,[6] norman r. pogson,[7] and lieutenant john herschel,[8] and was subsequently confirmed by french astronomer, jules janssen.[9] 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 two swedish chemists, 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.[10][11] in 1903, large reserves of helium were found in natural gas fields in parts of the united states, which is 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), particularly in the cooling of superconducting magnets, with the main commercial application being 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.[12] 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. previously, terrestrial helium—a non-renewable resource, because, once released into the atmosphere it readily escapes into space—was thought to be in increasingly short supply.[13][14] however, recent studies suggest that helium produced deep in the earth by radioactive decay can collect in natural gas reserves in larger than expected quantities,[15] in some cases, having been released by volcanic activity.[16]

  • history
  • characteristics
  • compounds
  • occurrence and production
  • applications
  • as a contaminant
  • inhalation and safety
  • see also
  • references
  • bibliography
  • external links

Helium, 2He
Helium discharge tube.jpg
Helium
Pronunciationm/ (HEE-lee-əm)
Appearancecolorless 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, std(He)4.002602(2)[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
hydrogenheliumlithium
Atomic number (Z)2
Groupgroup 18 (noble gases)
Periodperiod 1
Blocks-block
Element category  Noble gas
Electron configuration1s2
Electrons per shell2
Physical properties
Phase at STPgas
Melting point0.95 K ​(−272.20 °C, ​−457.96 °F) (at 2.5 MPa)
Boiling point4.222 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 point2.177 K, ​5.043 kPa
Critical point5.1953 K, 0.22746 MPa
Heat of fusion0.0138 kJ/mol
Heat of vaporization0.0829 kJ/mol
Molar heat capacity20.78 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 states0
ElectronegativityPauling scale: no data
Ionization energies
  • 1st: 2372.3 kJ/mol
  • 2nd: 5250.5 kJ/mol
Covalent radius28 pm
Van der Waals radius140 pm
Color lines in a spectral range
Spectral lines of helium
Other properties
Natural occurrenceprimordial
Crystal structurehexagonal close-packed (hcp)
Hexagonal close-packed crystal structure for helium
Speed of sound972 m/s
Thermal conductivity0.1513 W/(m·K)
Magnetic orderingdiamagnetic[3]
Magnetic susceptibility−1.88·10−6 cm3/mol (298 K)[4]
CAS Number7440-59-7
History
Namingafter Helios, Greek Titan of the Sun
DiscoveryPierre Janssen, Norman Lockyer (1868)
First isolationWilliam Ramsay, Per Teodor Cleve, Abraham Langlet (1895)
Main isotopes of helium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
3He 0.0002% stable
4He 99.9998% stable
Category Category: Helium
| references

Helium (from Greek: ἥλιος, romanizedHelios, 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, the first in the noble gas group in the periodic table. Its boiling point is the lowest among all the elements. Helium is the second lightest and second most abundant element in the observable universe (hydrogen is the lightest and most abundant). 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. This is 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. Most helium in the universe is helium-4, the vast majority of which was formed during the Big Bang. Large amounts of new helium are being created by nuclear fusion of hydrogen in stars.

Helium is named for the Greek Titan of the Sun, Helios. It was first detected as an unknown, yellow spectral line signature in sunlight, during a solar eclipse in 1868 by Georges Rayet,[5] Captain C. T. Haig,[6] Norman R. Pogson,[7] and Lieutenant John Herschel,[8] and was subsequently confirmed by French astronomer, Jules Janssen.[9] 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 two Swedish chemists, 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.[10][11] In 1903, large reserves of helium were found in natural gas fields in parts of the United States, which is 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), particularly in the cooling of superconducting magnets, with the main commercial application being 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.[12] 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. Previously, terrestrial helium—a non-renewable resource, because, once released into the atmosphere it readily escapes into space—was thought to be in increasingly short supply.[13][14] However, recent studies suggest that helium produced deep in the earth by radioactive decay can collect in natural gas reserves in larger than expected quantities,[15] in some cases, having been released by volcanic activity.[16]