Neon atom orbital energies

The one-electron molecular-orbital energies resulted from the calculations when the oxygen atom of the cluster is replaced by substitution neon was show in Fig. 6 on the right side. 

We represent each electron with an arrow. Different electron spins m value of -5 or +5) are indicated by arrows pointing downward or upward. Because each line represents one orbital, each line may hold a maximum of two arrows. If two arrows are present, they must be pointing in opposite directions. The energy level diagram representing the neon atom is shown in Figure 4.10. 

The 3r electron of sodium is much more important in the description of sodium s chemical reactions than the other electrons are. There are two reasons why this is true. We know from the stability of neon atoms that the s 2s 2p configuration is very stable, so these electrons are not lost or shared in chemical reactions involving sodium. These electrons are called the noble gas inner core of sodium. Another reason is that an electron in the larger 3s orbital is less strongly attracted to the nuclear charge than electrons in smaller orbitals in the first and second principal energy levels. As a result, the 3s electron is easier to remove. 

Several excited states of the neon atom are important in the operation of a helium-neon laser. In these excited states, one electron of the neon atom is promoted from the 2p level to a higher energy orbital. 

There is thus a wide, continuous, and unfilled band of valence orbital energies. If we have a crystal of noble gas atoms (He, Ne, Ar, Kr, Xe, and Rn) on the other hand, every orbital taking part in the interaction arises from an orbital that was filled in the atom. Since the number of MOs created by the interaction must be the same as the original number of orbitals, all orbitals will be filled. The orbitals above the gap receive no electrons at T = 0. For example, in the case of neon, the valence band created from the 2s and 2p orbitals will be filled with 12 electrons. 

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