Xenon electron configuration

The stability of the electronic configuration is indicated by the fact that each element has the highest ionization energy in its period, though the value decreases down the group as a result of increasing size of the atoms. For the heavier elements is it actually smaller than for first-row elements such as O and F with consequences for the chemical reactivities of the noble gases which will be considered in the next section. Nuclear properties, particularly for xenon, have been exploited for nmr spectroscopy and Mdssbauer... 

Duncanson (i) of the molecular orbital bonding concepts of Dewar (2), which he developed to explain the structure of Ag+-olefin complexes, led to the suggestion that ethylene is symmetrically coordinated to the metal. Platinum, atomic number 78, has the electronic configuration of the xenon core (Is 2s 2p 35 3p 3d Z = 54), then... 

Treatment of the chloro-bridged complex [PdCl(7r-C3H5)]2 with cyclo-pentadienylsodium gives 7r-al lyl-rr-cyclopentadienylpalladiu m (II) [Pd(ir-C3H6)(7r-C6H6)] as dark red, voltatile crystals, mp 64° (190). Its nmr spectrum (191) confirms the sandwich structure (L) in which the palladium has the electronic configuration of xenon. 

After this schematic discussion of possible processes around the 4d ionization shell in xenon, Fig. 5.2(h) can be compared with the experimental results shown in Fig. 5.1. The main structures can be related to 4d, photoexcitation/ionization, and autoionization/Auger decay to 5s25p4fa electron configurations can be identified in the energy regions of overlap. 

All argon nuclei have charge +18 electronic units, so that 18 electrons orbit the nucleus of the neutral atom. Its electronic configuration is is22s22p63s23p6, which fills each of these shells. It is these closed, or full, s and p shells of electrons that make Ar and all noble gases inert. Before 1962 it was thought that these elements were absolutely inert, but at that time the first stable compound of xenon, Xe, was discovered. The newly discovered compounds of krypton, Kr, and Xe are extremely interesting to chemists. 

Three places after xenon there follows the remarkable group of the elements of the Rare Earths, because here, beginning with cerium, the Nf or 4f shell (/ — 3, m = —3, —2, —1, o, 1, 2, 3) is filled up. There is thus produced a group of 14 elements from cerium (58) to lutecium (71), which all possess the same electron configuration of the outermost shell as lanthanum and thus also show a great similarity in chemical properties [group of the lanthanides or lanthanons]. 

The formation and properties of the lanthanide complex species can be best understood by summarizing first some of the pertinent general characteristics of these elements. In their ground states, the lanthanide atoms have the characteristic valence-shell electronic configurations 4/"5 d 6 or 4 / + 6 where n = 0 for lanthanum and 14 for lutetium, overlying the closed-shell xenon arrangement. The atoms are large and readily oxidized. In both aqueous or nonaqueous systems and the solid state, oxidation... 

What do the electron configurations of neon, argon, krypton, xenon, and radon have in common ... 

Helium, with electronic configuration l5, is placed in Group 18 because its properties are similar to those of neon, argon, krypton, and xenon. 

With their closed-shell electron configurations the noble gas elements of group 18 were long regarded as chemically inert. However, in 1962 Bartlett noted that the ionization energy of xenon was similar to that of 02, and by reaction with PtF6 attempted to prepare the compound analogous to... 

XeF2 The outer electronic configuration of xenon and fluorine atoms are... 

Write the expected abbreviated electron configuration for the as-yet-undiscovered element with an atomic number of 121. Use Uuo for the symbol of the noble gas below xenon, Xe. (Hint See Figure 11.17.)... 

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