Class of improbable chemical compounds only formed at very high pressure or low temperature
Helium is the smallest and the lightest noble gas and one of the most unreactive elements, so it was commonly considered that helium compounds cannot exist at all, or at least under normal conditions.[1] Helium's first ionization energy of 24.57 eV is the highest of any element.[2] Helium has a complete shell of electrons, and in this form the atom does not readily accept any extra electrons nor join with anything to make covalent compounds. The electron affinity is 0.080 eV, which is very close to zero.[2] The helium atom is small with the radius of the outer electron shell at 0.29 Å.[2] Helium is a very hard atom with a Pearson hardness of 12.3 eV.[3] It has the lowest polarizability of any kind of atom, however, very weak van der Waals forces exist between helium and other atoms. This force may exceed repulsive forces, so at extremely low temperatures helium may form van der Waals molecules. Helium has the lowest boiling point (4.2 K) of any known substance.
Repulsive forces between helium and other atoms may be overcome by high pressures. Helium has been shown to form a crystalline compound with sodium under pressure. Suitable pressures to force helium into solid combinations could be found inside planets. Clathrates are also possible with helium under pressure in ice, and other small molecules such as nitrogen.
Other ways to make helium reactive are: to convert it into an ion, or to excite an electron to a higher level, allowing it to form excimers. Ionised helium (He+), also known as He II, is a very high energy material able to extract an electron from any other atom. He+ has an electron configuration like hydrogen, so as well as being ionic it can form covalent bonds. Excimers do not last for long, as the molecule containing the higher energy level helium atom can rapidly decay back to a repulsive ground state, where the two atoms making up the bond repel. However, in some locations such as helium white dwarfs, conditions may be suitable to rapidly form excited helium atoms. The excited helium atom has a 1s electron promoted to 2s. This requires 1,900 kilojoules (450 kcal) per gram of helium, which can be supplied by electron impact, or electric discharge.[4] The 2s excited electron state resembles that of the lithium atom.
^Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry. John Wiley. pp. 140–141.
^ abcDong, Xiao; Oganov, Artem R. (25 April 2014). "Stable Compound of Helium and Sodium at High Pressure". Nature Chemistry. 9 (5): 440–445. arXiv:1309.3827. Bibcode:2017NatCh...9..440D. doi:10.1038/nchem.2716. PMID 28430195. S2CID 20459726.
^Grochala, W. (1 January 2009). "On Chemical Bonding Between Helium and Oxygen" (PDF). Polish Journal of Chemistry. 83 (1): 87–122. Archived from the original (abstract) on 2 February 2017. Retrieved 17 May 2016.
^Cite error: The named reference adli was invoked but never defined (see the help page).
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