Isotopes of helium

Main isotopes of helium
Iso­tope Decay
abun­dance half-life (t1/2) mode pro­duct
3He 0.0002% stable
4He 99.9998% stable
Standard atomic weight (Ar)
  • 4.002602(2)[1]

Although there are nine known isotopes of helium (2He) (standard atomic weight: 4.002602(2)), only helium-3 (3
He
) and helium-4 (4
He
) are stable. All radioisotopes are short-lived, the longest-lived being 6
He
 with a half-life of 806.7 milliseconds. The least stable is 5
He
, with a half-life of 7.6×10−22 s, although it is possible that 2
He
 has an even shorter half-life.

In the Earth's atmosphere, there is one 3
He
 atom for every million 4
He
 atoms.[2] However, helium is unusual in that its isotopic abundance varies greatly depending on its origin. In the interstellar medium, the proportion of 3
He
 is around a hundred times higher.[3] Rocks from the Earth's crust have isotope ratios varying by as much as a factor of ten; this is used in geology to investigate the origin of rocks and the composition of the Earth's mantle.[4] The different formation processes of the two stable isotopes of helium produce the differing isotope abundances.

Equal mixtures of liquid 3
He
 and 4
He
 below 0.8 K will separate into two immiscible phases due to their dissimilarity (they follow different quantum statistics: 4
He
 atoms are bosons while 3
He
 atoms are fermions).[5] Dilution refrigerators take advantage of the immiscibility of these two isotopes to achieve temperatures of a few millikelvins.

Helium-2 (diproton)

Helium-2 or 2
He
, also known as a diproton, is an extremely unstable isotope of helium that consists of two protons with no neutrons. According to theoretical calculations, it would have been much more stable (although still beta-decaying to deuterium) if the strong force had been 2% greater.[6] Its instability is due to spin–spin interactions in the nuclear force, and the Pauli exclusion principle, which forces the two protons to have anti-aligned spins and gives the diproton a negative binding energy.[7]

There may have been observations of 2
He
. In 2000, physicists first observed a new type of radioactive decay in which a nucleus emits two protons at once—perhaps a 2
He
 nucleus.[8][9] The team led by Alfredo Galindo-Uribarri of the Oak Ridge National Laboratory announced that the discovery will help scientists understand the strong nuclear force and provide fresh insights into the creation of elements inside stars. Galindo-Uribarri and co-workers chose an isotope of neon with an energy structure that prevents it from emitting protons one at a time. This means that the two protons are ejected simultaneously. The team fired a beam of fluorine ions at a proton-rich target to produce 18
Ne
, which then decayed into oxygen and two protons. Any protons ejected from the target itself were identified by their characteristic energies. There are two ways in which the two-proton emission may proceed. The neon nucleus might eject a "diproton"—a pair of protons bound together as a 2
He
 nucleus—which then decays into separate protons. Alternatively, the protons may be emitted separately but simultaneously—so-called "democratic decay". The experiment was not sensitive enough to establish which of these two processes was taking place.

More evidence of 2
He
 was found in 2008 at the Istituto Nazionale di Fisica Nucleare, in Italy.[10][11] A beam of 20
Ne
 ions was directed at a target of beryllium foil. This collision converted some of the heavier neon nuclei in the beam into 18
Ne
 nuclei. These nuclei then collided with a foil of lead. The second collision had the effect of exciting the 18
Ne
 nucleus into a highly unstable condition. As in the earlier experiment at Oak Ridge, the 18
Ne
 nucleus decayed into an 16
O
 nucleus, plus two protons detected exiting from the same direction. The new experiment showed that the two protons were initially ejected together, correlated in a quasibound 1S configuration, before decaying into separate protons much less than a nanosecond later.

Further evidence comes from RIKEN in Japan and JINR in Dubna, Russia, where beams of 6
He
 nuclei were directed at a cryogenic hydrogen target to produce 5
He
. It was discovered that the 6
He
 nucleus can donate all four of its neutrons to the hydrogen. The two remaining protons could be simultaneously ejected from the target as a 2
He
 nucleus, which quickly decayed into two protons. A similar reaction has also been observed from 8
He
 nuclei colliding with hydrogen.[12]

2
He
 is an intermediate in the first step of the proton–proton chain reaction. The first step of the proton–proton chain reaction is a two-stage process; first, two protons fuse to form a diproton:

1
1H
 + 1
1H
 → 2
2He
,

followed by the immediate beta-plus decay of the diproton to deuterium:

2
2He
 → 2
1D
 +
e+
 +
ν
e,

with the overall formula

1
1H
 + 1
1H
 → 2
1D
 +
e+
 +
ν
e + 0.42 MeV.

R. A. W. Bradford has considered the hypothetical effect of the binding of the diproton on Big Bang and stellar nucleosynthesis.[6]

Helium-3

A helium-3 atom contains two protons, one neutron, and two electrons

3
He
 is stable and is the only stable isotope other than 1
H
 with more protons than neutrons. (There are many such unstable isotopes, the lightest being 7
Be
 and 8
B
.) There is only a trace amount (0.000137%) of 3
He
 on Earth, primarily present since the formation of the Earth, although some falls to Earth trapped in cosmic dust.[4] Trace amounts are also produced by the beta decay of tritium.[13] In stars, however, 3
He
 is more abundant, a product of nuclear fusion. Extraplanetary material, such as lunar and asteroid regolith, has trace amounts of 3
He
 from solar wind bombardment.

For helium-3 to form a superfluid, it must be cooled to a temperature of 0.0025 K, or almost a thousand times lower than helium-4 (2.17 K). This difference is explained by quantum statistics, since helium-3 atoms are fermions, while helium-4 atoms are bosons, which condense to a superfluid more easily.

Helium-4

A helium-4 atom contains two protons, two neutrons, and two electrons

The most common isotope, 4
He
, is produced on Earth by alpha decay of heavier radioactive elements; the alpha particles that emerge are fully ionized 4
He
 nuclei. 4
He
 is an unusually stable nucleus because its nucleons are arranged into complete shells. It was also formed in enormous quantities during Big Bang nucleosynthesis.

Terrestrial helium consists almost exclusively (99.99986%) of this isotope. Its boiling point of 4.2 K is the lowest of any known substance. When cooled further to 2.17 K, it transforms to a unique superfluid state of zero viscosity. It solidifies only at pressures above 25 atmospheres, where its melting point is 0.95 K.

Heavier helium isotopes

Although all heavier helium isotopes decay with a half-life of less than one second, researchers have created new isotopes through particle accelerator collisions to create unusual atomic nuclei for elements such as helium, lithium and nitrogen. The unusual nuclear structures of such isotopes may offer insight into the isolated properties of neutrons.

The shortest-lived isotope is helium-5 with a half-life of 7.6×10−22 seconds. Helium-6 decays by emitting a beta particle and has a half-life of 0.8 seconds. Helium-7 also emits a beta particle as well as a gamma ray. The most widely studied heavy helium isotope is helium-8. This isotope, as well as helium-6, are thought to consist of a normal helium-4 nucleus surrounded by a neutron "halo" (containing two neutrons in 6
He
 and four neutrons in 8
He
). Halo nuclei have become an area of intense research. Isotopes up to helium-10, with two protons and eight neutrons, have been confirmed. Helium-7 and helium-8 are hyperfragments that are created in certain nuclear reactions. 10
He
, despite being a doubly magic isotope, has a very short half-life as it is not particle-bound and near-instantaneously drips out two neutrons.[14]

List of isotopes

nuclide
symbol		 Z(p) N(n) isotopic mass (u) half-life decay
mode(s)[15]		 daughter
isotope(s)[n 1]		 nuclear
spin		 representative
isotopic
composition
(mole fraction)		 range of natural
variation
(mole fraction)
2
He
[n 2]		 2 0 2.015894(2) ≪ 10−9 s[10] p (>99.99%) 2 1
H
 0+(#)
β+ (<0.01%) 2
H
3
He
[n 3]		 2 1 3.0160293191(26) Stable[n 4] 1/2+ 1.34(3)×10−6 4.6×10−10−4.1×10−5
4
He
[n 3]		 2 2 4.00260325415(6) Stable 0+ 0.99999866(3) 0.999959-1
5
He
 2 3 5.01222(5) 700(30)×10−24 s n 4
He
 3/2−
6
He
[n 5]		 2 4 6.0188891(8) 806.7(15) ms β− (99.99%) 6
Li
 0+
β−, α (2.8×10−4%) 4
He
, 2
H
7
He
 2 5 7.028021(18) 2.9(5)×10−21 s
[159(28) keV]		 n 6
He
 (3/2)−
8
He
[n 6]		 2 6 8.033922(7) 119.0(15) ms β− (83.1%) 8
Li
 0+
β−,n (16.0%) 7
Li
β−, fission (0.9%) 5
He
, 3
H
9
He
 2 7 9.04395(3) 7(4)×10−21 s n 8
He
 1/2−(#)
10
He
 2 8 10.05240(8) 2.7(18)×10−21 s 2n 8
He
 0+
  1. ↑ Bold for stable isotopes
  2. ↑ Intermediate in the proton-proton chain reaction
  3. 1 2 Produced during Big bang nucleosynthesis
  4. ↑ This and 1H are the only stable nuclides with more protons than neutrons
  5. ↑ Has 2 halo neutrons
  6. ↑ Has 4 halo neutrons

Notes

Decay chains

Although some helium isotopes, such as 6He and 8He, decay mostly to isotopes of lithium, the major tendency among known isotopes seems to be decay into lighter helium isotopes. Fission, seen only in even-numbered isotopes, is also unusually common.

Decay chains for isotopes with multiple decay modes listed in order of probability:

References

  1. ↑ Meija, J.; et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Report)". Pure Appl. Chem. 88 (3): 265–91. doi:10.1515/pac-2015-0305.
  2. ↑ J. Emsley (2001). Nature's Building Blocks: An A–Z Guide to the Elements. Oxford University Press. p. 178. ISBN 0-19-850340-7.
  3. ↑ G. N. Zastenker; et al. (2002). "Isotopic Composition and Abundance of Interstellar Neutral Helium Based on Direct Measurements". Astrophysics. 45 (2): 131–142. Bibcode:2002Ap.....45..131Z. doi:10.1023/A:1016057812964.
  4. 1 2 "Helium Fundamentals".
  5. ↑ The Encyclopedia of the Chemical Elements. p. 264.
  6. 1 2 Bradford, R. A. W. (27 August 2009). "The effect of hypothetical diproton stability on the universe" (PDF). Journal of Astrophysics and Astronomy. 30 (2): 119–131. doi:10.1007/s12036-009-0005-x.
  7. ↑ Nuclear Physics in a Nutshell, C. A. Bertulani, Princeton University Press, Princeton, N.J., 2007, Chapter 1, ISBN 978-0-691-12505-3.
  8. ↑ Physicists discover new kind of radioactivity, in physicsworld.com Oct 24, 2000.
  9. ↑ Decay of a Resonance in 18Ne by the Simultaneous Emission of Two Protons, Physical Review Letters vol. 86, pp. 43–46 (2001), by J. Gómez del Campo, A. Galindo-Uribarri et al.
  10. 1 2 "New Form of Artificial Radioactivity" Inside Physics Research—Science News Update Number 865 #2, May 29, 2008 by Phil Schewe.
  11. ↑ G. Raciti et al., Physical Review Letters 100, 192503–06 (2008) "Experimental Evidence of 2He Decay from 18Ne Excited States".
  12. ↑ A. A. Korsheninnikov; et al. (2003-02-28). "Experimental Evidence for the Existence of 7
    H
     and for a Specific Structure of 8
    He
    "     (PDF). Physical Review Letters. Bibcode:2003PhRvL..90h2501K. doi:10.1103/PhysRevLett.90.082501.
  13. ↑ K. L. Barbalace. "Periodic Table of Elements: Li—Lithium". EnvironmentalChemistry.com. Retrieved 2010-09-13.
  14. ↑ Clifford A. Hampel (1968). The Encyclopedia of the Chemical Elements. Reinhold Book Corporation. p. 260. ISBN 0278916430.
  15. ↑ "Universal Nuclide Chart". nucleonica. (Registration required (help)).
Isotopes of hydrogen Isotopes of helium Isotopes of lithium
Table of nuclides
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