Neon, ionization energy

I. Note that in the case of both beryllium and neon, ionization energies increase as one moves from f to I2 to I3. 

The first three ionization energies (f, I2, and I3) for beryllium and neon are given in the following table ... 

The only compound formed would be BeCl2. The Be atom readily loses 2 electrons to form the stable Be2+ ion. The third ionization energy is too high to form Be3+. The electron affinity of neon is very low because it has a stable octet of electrons in its valence shell and the ionization energies of neon are too high. 

The electron affinity of neon is very low because it has a stable octet of electrons in its valence shell and the ionization energies of neon are too high. 

Fig. 2.13 Ionization energy-electron affinity curves for oxygen, fluorine, neon, and clilorine.

Table 2.1. Ionization energies in neon (from [PNS822 and [Moo7 If, for some atomic ionization energies, see [Set>79]).

Neon, and the elements directly below it in the periodic table or the Solid State Table, form the simplest closed-shell systems. The electronic structure of the inert-gas solid, which is face-ccntercd cubic, is essentially that of the isolated atoms, and the interactions between atoms are well described by an overlap interaction that includes a correlation energy contribution (frequently described as a Van der Waals interaction). The total interaction, which can be conveniently fitted by a two-parameter Lennard-Jones potential, describes the behavior of both the gas and the solid. Electronic excitations to higher atomic states become excitons in the solid, and the atomic ionization energy becomes the band gap. Surprisingly, as noted by Pantelides, the gap varies with equilibrium nearest-neighbor distance, d, as d... 

What role does electron-electron repulsion play in the trend in ionization energies from lithium to neon ... 

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