Superatom

Superatoms are clusters of atoms that seem to exhibit some of the properties of elemental atoms.

Sodium atoms, when cooled from vapor, naturally condense into clusters, more so into clusters of 2, 8, 20, 40, 58 or 82 atoms (the magic numbers), than into the other numbers. The first two of these can be recognized as the numbers of electrons needed to fill s and p orbitals, respectively. The superatom suggestion is that free electrons in the cluster occupy a new set of orbitals that are defined by the entire group of atoms, i.e. cluster, rather than each individual atom separately (non-spherical or doped clusters show deviations in the number of electrons that form a closed shell as the potential is defined by the shape of the positive nuclei.) Superatoms tend to behave chemically in a way that will allow them to have a closed shell of electrons, in this new counting scheme. Therefore, a superatom with one more electron than a full shell should give up that electron very easily, similar to an alkali metal, and a cluster with one electron short of full shell should have a large electron affinity, such as a halogen.

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Aluminum clusters

Certain aluminium clusters have superatom properties. These aluminium clusters are generated as anions (Al_n^- with n = 1,2,3...) in helium gas and reacted with a gas containing iodine. When analyzed by mass spectrometry one main reaction product turns out to be Al₁₃I^-.^[1] These clusters of 13 aluminium atoms with an extra electron added do not appear to react with oxygen when it is introduced in the same gas stream. Assuming each atom liberates its 3 valence electrons, this means that there are 40 electrons present, which is one of the magic numbers noted above for sodium, and implies that these numbers are a reflection of the noble gases. Calculations show that the additional electron is located in the aluminium cluster at the location directly opposite from the iodine atom. The cluster must therefore have a higher electron affinity for the electron than iodine and therefore the aluminium cluster is called a superhalogen. The cluster component in Al₁₃I^- ion is similar to an iodine ion or better still a bromine atom. The related Al₁₃I₂^- cluster is expected to behave chemically like the triiodide ion.

Similarly it has been noted that Al₁₄ clusters with 42 electrons (2 more than the magic numbers) appear to exhibit the properties of an alkaline earth metal which typically adopt +2 valence states. This is only known to occur when there are at least 3 iodine atoms attached to an Al₁₄^- cluster, Al₁₄I₃^-. The anionic cluster has a total of 43 itinerant electrons, but the three Iodine atoms each remove one of the itinerant electrons to leave 40 electrons in the jellium shell.^[2][3]

It is particularly easy and reliable to study atomic clusters of inert gas atoms by computer simulation because interaction between two atoms can be approximated very well by the Lennard-Jones potential. Other methods are readily available and it has been established that the magic numbers are 13, 19, 23, 26, 29, 32, 34, 43, 46, 49, 55, etc. [I. A. Harris et al. Phys. Rev. Lett. Vol. 53, 2391-94 (1984).]

Aluminum clusters

• Al₇ = the property is similar to germanium atoms.
• Al₁₃ = the property is similar to halogen atoms, more specifically, chlorine.
  • Al₁₃I_x^-, where x = 1-13.^[4]
• Al₁₄ = the property is similar to alkaline metals.
  • Al₁₄I_x^-, where x = 1-14.^[4]
• Al₂₃
• Al₃₇

Other clusters

• Li(HF)₃Li = the (HF)₃ interior causes 2 valence electrons from the Li to orbit the entire molecule as if it were an atom's nucleus.^[5]
• VSi₁₆F = has ionic bonding.^[6]
• A cluster of 13 platinum becomes magnetic.^[7]

See also

• Bose-Einstein condensate

References