China
Africa
Explore chapters and articles related to this topic
N
Published in Splinter Robert, Illustrated Encyclopedia of Applied and Engineering Physics, 2017
[atomic, general] Monatomic elements that were originally considered to be inert due to the oxidation number of zero (0). The six noble gases, all in group 18 (VIIIa) of the periodic table of elements are as follows: helium, neon, argon, krypton, xenon, and radon, all odorless and colorless with minimal chemical reactivity. In the 1960s, there were new discoveries that indicated the potential for chemical links with noble gases; in 1962, the first chemical compound of a noble gas was uncovered: xenon hexafluoroplatinate, by Neil Bartlett (1932–2008), and more thereafter. In the outer shell, all noble gases have the maximum number of electrons allowed: two for Helium, and eight for all the remaining five elements, which is what makes these elements so stable. The term is an English translation from the German word “Edelgas,” introduced by Hugo Erdmann (1862–1910) in 1898 (see Figure N.39).
Noble-Gas Chemistry
Published in Leonid Khriachtchev, Physics and Chemistry at Low Temperatures, 2019
Wojciech Grochala, Leonid Khriachtchev, Markku Rasanen
The chemistry of noble gases began with a room temperature synthesis of the first xenon compound in the solid state, xenon hexafluoroplatinate (XePtF6) by Neil Bartlett.1 The true and indeed very complex nature of the “XePtF6” compound was confirmed by experiments conducted nearly40 years after the initial preparation.2 The history of the breaking of the inertness of the noble gases is certainly complex and fascinating, full of many misleading reports, surprises, and ingenuity.3
An Introduction to Crystal Structures
Published in Elaine A. Moore, Lesley E. Smart, Solid State Chemistry, 2020
Elaine A. Moore, Lesley E. Smart
Interestingly, it was arguments and calculations of this sort that led Neil Bartlett to the discovery of the first noble gas compound, XePtF6. Bartlett had prepared a new complex, O2PtF6, which, by analogy with the diffraction pattern of KPtF6, he formulated as containing the dioxygenyl cation, [O2+][PtF6−]. He realised that the ionisation energies of oxygen and xenon are very similar and that although the radius of the Xe+ ion is slightly different, because the PtF6− anion is very large, the lattice energy of [Xe+][PtF6−] should be very similar to that of the dioxygenyl complex and, therefore, should exist. Accordingly, he mixed xenon and PtF6 and obtained the orange-yellow solid of xenon hexafluoroplatinate—the first noble gas compound. (Although, in fact, the compound turned out not to have the structure that Bartlett predicted because at room temperature XePtF6 reacts with another molecule of PtF6 to give a product containing [XeF]+[PtF6]− and [PtF5]−.)
Theoretical prediction of FNgM3–kHk (Ng = Ar, Kr, Xe, and Rn; M = Cu, Ag and Au; k = 0–2) molecules
Published in Molecular Physics, 2022
Subrahmanya Prasad Kuntar, Ayan Ghosh, Tapan K. Ghanty
Element that has completely filled valence shell are exceedingly averse to participate in a chemical reaction while the species possessing only one electron in the outermost shell are very keen to react, and arguably they are considered as highly reactive species. Former is the case with the noble gas (Ng) atoms present in group 18 of the periodic table. The completely filled valence orbitals make them shy to take part in the electron transfer phenomena with the other atoms. It was hence predicted that the Ng atoms can only be reactive under extreme conditions. Even though Ng atoms have completely filled valence electronic configurations, as we move down along the group in the periodic table the ionisation energy decreases. Consequently, in the heavier Ng atoms, the influence of the nucleus on the valence or the outermost electrons is very less that is because of the increasing ionic radii and the screening of the furthest electrons by the electrons at the crux. With these intuitions, Linus Pauling in 1933 first predicted [1] the existence of xenon compounds with fluorine and oxygen theoretically. This investigation marked as the beginning for the noble gas reaction chemistry as previously the inertness of the noble gas atoms was considered insuperable. In 1962, Neil Bartlett gained an accidental success [2] while separating a stable Xenon compound and observed the first noble gas compound xenon hexafluoroplatinate defeating the entire pigeonhole. Since then Noble gas chemistry [2–9] has become the frontier area of research owing to the versatile applications of Ng atoms in diverse fields. A wide variety of compounds containing different Ng atoms are being theoretically foreseen and observed experimentally. It is vital to quote that the quantum chemical methods are extremely useful in predicting new chemical compounds involving Ng atoms and elucidate their physico-chemical properties. Our aim is to utilise such methods in predicting novel material that forms stable compounds with the Ng atoms.