Hydrogen ion cluster

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A hydrogen molecular ion cluster or hydrogen cluster ion is a positively charged cluster of hydrogen molecules. The hydrogen molecular ion (H+
2) and trihydrogen ion (H+
3) are well defined molecular species. However hydrogen also forms singly charged clusters (H+
n) with n up to 120.

Contents

Experiments

Hydrogen ion clusters can be formed in liquid helium or with lesser cluster size in pure hydrogen. H+
6 is far more common than higher even numbered clusters. [1] H+
6 is stable in solid hydrogen. The positive charge is balanced by a solvated electron. It is formed when ionizing radiation impinges on solid hydrogen, and so is formed in radioactive solid tritium. In natural hydrogen treated with radiation, the positive charge transfers to HD molecules, in preference to H
2, with the ultimate most stable arrangement being HD(HD)+HD. [2] H+
6 can migrate through solid hydrogen by linking a hydrogen molecule at one end and losing it at the other: H
2 + H+
6 → H+
6 + H
2. This migration stops once an HD molecule is added resulting in a lower energy level. [3] HD or D
2 is added in preference over H
2. [4]

Clampitt and Gowland found clusters with an odd number of hydrogen atoms H+
3+2n [5] and later showed that H+
15 was relatively stable. H+
3 formed the core of this cluster with six H
2 molecules surrounding it. [6] Hiroka studied the stability of the odd numbered clusters in gas up to H+
21. [7] Bae determined that H+
15 was especially stable amongst the odd numbered clusters. [8]

Kirchner discovered even numbered atomic clusters in gas at lower concentrations than the odd numbered atom clusters. H+
6 was twenty times less abundant than H+
5. H+
4, H+
8 and H+
10 were detected at lesser amounts than H+
6. [9] Kurosaki and Takayanagi showed that H+
6 is much more stable than other even clusters and showed antiprismatic symmetry of order 4 (D
2d molecular symmetry). [10] This turnstile structured molecule was computationally found to be more energetically stable than a ring of five hydrogen atoms around a proton. [11]

Negative hydrogen clusters have not been found to exist. H−
3 is theoretically unstable, but D−
3 in theory is bound at 0.003 eV. [8]

Decay

H+
6 in the free gas state decays by giving off H atoms and H
2 molecules. Different energies of decay occur with levels averaging at 0.038 eV and peaking at 0.14 eV. [9]

Formation

Hydrogen molecular ion clusters can be formed through different kinds of ionizing radiation. High energy electrons capable of ionizing the material can perform this task. When hydrogen dissolved in liquid helium is irradiated with electrons their energy must be sufficient to ionize helium to produce significant hydrogen clusters. Irradiation of solid hydrogen by gamma rays or X-rays also produces H+
6. [12]

Positive ion clusters are also formed when compressed hydrogen expands though a nozzle. [13]

Kirchner's theory for the formation of even numbered clusters was that neutral H
3 molecules reacted with the H+
3 ion (or other odd clusters) to make H+
6. [9]

Properties

Solvation of H+
6 in solid hydrogen had little effect on its spectrum. [10]

Use

SRI International studied solid ionic hydrogen fuel. They believed that a solid containing H+
3 and H− ions could be manufactured. If it could be made it would have a higher energy than other rocket fuels with only 2% concentration of ions. However they could not contain the H− in a stable way, but determined that other negative ions would do as well. [8] This theoretical impulse exceeds that of solid and liquid fuel rockets. [8] SRI developed a cluster ion gun that could make positive and negative ion clusters at a current of 500  pA. [8]

Nuclear fusion using ion clusters can impact far more atoms than single ions in one hit. This concept is called cluster ion fusion (CIF). Lithium deuteride (LiD) is a potential starter material for generating the ions. [8]

Related Research Articles

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<span class="mw-page-title-main">Covalent bond</span> Chemical bond by sharing of electron pairs

A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs. The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding. For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. In organic chemistry, covalent bonding is much more common than ionic bonding.

<span class="mw-page-title-main">Molecule</span> Electrically neutral group of two or more atoms

A molecule is a group of two or more atoms held together by attractive forces known as chemical bonds; depending on context, the term may or may not include ions which satisfy this criterion. In quantum physics, organic chemistry, and biochemistry, the distinction from ions is dropped and molecule is often used when referring to polyatomic ions.

<span class="mw-page-title-main">Noble gas</span> Group of low-reactive, gaseous chemical elements

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<span class="mw-page-title-main">Ionization</span> Process by which atoms or molecules acquire charge by gaining or losing electrons

Ionization is the process by which an atom or a molecule acquires a negative or positive charge by gaining or losing electrons, often in conjunction with other chemical changes. The resulting electrically charged atom or molecule is called an ion. Ionization can result from the loss of an electron after collisions with subatomic particles, collisions with other atoms, molecules, electrons, positrons, protons, antiprotons and ions, or through the interaction with electromagnetic radiation. Heterolytic bond cleavage and heterolytic substitution reactions can result in the formation of ion pairs. Ionization can occur through radioactive decay by the internal conversion process, in which an excited nucleus transfers its energy to one of the inner-shell electrons causing it to be ejected.

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<span class="mw-page-title-main">Mass spectral interpretation</span>

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<span class="mw-page-title-main">Ion</span> Particle, atom or molecule with a net electrical charge

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References

  1. ↑ Sattler, Klaus D. (2010). "Electron Impact Ionization of Hydrogen Clusters Embedded in Helium". Clusters and Fullerenes. Handbook of Nanophysics. CRC Press. pp. 20–15–20–17. ISBN   978-1-4200-7554-0.
  2. ↑ Ching Yeh Lin; Andrew T.B. Gilbert; Mark A. Walter (6 May 2011). "Interstellar Solid Hydrogen". The Astrophysical Journal. 736 (2): 91. arXiv: 1105.1861 . Bibcode:2011ApJ...736...91L. doi:10.1088/0004-637X/736/2/91. S2CID   50907532.
  3. ↑ Takayuki Kumada; Yuta Shimizu; Takahiro Ushida; Jun Kumagai (October–December 2008). "H atom, e−, and H+
    6     ions produced in irradiated solid hydrogens: An electron spin resonance study". Radiation Physics and Chemistry. 77 (10–12). Elsevier: 1318–1322. Bibcode:2008RaPC...77.1318K. doi:10.1016/j.radphyschem.2008.05.026.
  4. ↑ J. Kumagai; H. Inagaki; S. Kariya; T. Ushida; Y. Shimizu; T. Kumada (14 July 2007). "Electron spin resonance study on H+
    6    , H
    5    D+
    , H
    4    D+
    2    , and H
    2    D+
    4     in solid parahydrogen". J Chem Phys. 127 (2): 024505. Bibcode:2007JChPh.127b4505K. doi:10.1063/1.2748046. PMID   17640135.
  5. ↑ R. Clampitt, L. Gowland; Gowland, L. (August 1969). "Clustering of Cold Hydrogen Gas on Protons". Nature. 223 (5208): 815–816. Bibcode:1969Natur.223..815C. doi:10.1038/223815a0. S2CID   4172620.
  6. ↑ R. Clampitt; D. K. Jefferies (11 April 1970). "Ion Clusters". Nature. 226 (5241): 141–142. Bibcode:1970Natur.226..141C. doi:10.1038/226141a0. PMID   16057136. S2CID   43445356.
  7. ↑ Hiroka, K. (1987). "A determination of the stabilities of H+
    3    (H
    2    )
    n     with n = 1−9 from measurements of the gas-phase ion equilibria H+
    3    (H
    2    )
    n−1    +H
    2     = H+
    3    (H
    2    )
    n    ". The Journal of Chemical Physics. 87 (7). American Institute of Physics: 4048–4055. Bibcode:1987JChPh..87.4048H. doi:10.1063/1.452909. ISSN   0021-9606.
  8. 1 2 3 4 5 6 Bae, Young K.; Phillip C. Cosby (September 1990). "Ionic Solid Hydrogen Fuel: Production and Properties of Hydrogen Ion and Energetic Neutral Clusters" (PDF). Astronautics Laboratory. Archived from the original on October 8, 2012. Retrieved 17 June 2011.
  9. 1 2 3 Kirchner, Nicholas J.; Michael T. Bowers (1987). "An experimental study of the formation and reactivity of ionic hydrogen clusters: The first observation and characterization of the even clusters H+
    4    , H+
    6    , H+
    8    , and H+
    10    ". Journal of Chemical Physics. 86 (3): 1301–1310. Bibcode:1987JChPh..86.1301K. doi:10.1063/1.452219.
  10. 1 2 Kurosaki, Yuzuru; Toshiyuki. Takayanagi (21 August 1998). "A direct isomerization path for the H+
    6     cluster. An ab initio molecular orbital study". Chemical Physics Letters. 293 (1–2). Elsevier Science B.V.: 59–64. Bibcode:1998CPL...293...59K. doi:10.1016/S0009-2614(98)00721-0.
  11. ↑ Qiang Hao; Andrew C. Simmonett; Yukio Yamaguchi; Fang De-Cai; Henry F. Schaeffer (23 October 2009). "Structures and Energetics of H+
    6     Clusters"    . The Journal of Physical Chemistry A. 113 (48). Washington DC: American Chemical Society: 13608–13620. Bibcode:2009JPCA..11313608H. doi:10.1021/jp905928u. ISSN   1089-5639. PMID   19852448.
  12. ↑ Takayuki Kumada; Hiroto Tachikawa; Toshiyuki Takayanagi (2005). "H+
    6     in irradiated solid para-hydrogen and its decay dynamics: reinvestigation of quartet electron paramagnetic resonance lines assigned to H−
    2    ". Physical Chemistry Chemical Physics. 7 (5): 776–784. Bibcode:2005PCCP....7..776K. doi:10.1039/b415179h. ISSN   1463-9076. PMID   19791361.
  13. ↑ Ekinci, Y; E. L. Knuth; J. P. Toennies (5 October 2006). "A mass and time-of-flight spectroscopy study of the formation of clusters in free-jet expansions of normal D
    2    "    . Journal of Chemical Physics. 125 (13): 133409–133420. Bibcode:2006JChPh.125m3409E. doi:10.1063/1.2217942. PMID   17029483.
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