By J. E. Spice and J. E. Spice (Auth.)
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The crowding together of the levels becomes much more pronounced with even larger values of η than are shown on the diagram, until eventually successive levels coincide. At this point the electron may be said to have escaped from the atom altogether. Thus, the distance between a given level and these coincident levels represents the energy required to remove from the atom an electron which is initially in the given level. When this is the lowest possible level for the most readily removed electron, the energy is called the ionisation energy (see Fig.
16, which is not drawn strictly to scale. The crowding together of the levels becomes much more pronounced with even larger values of η than are shown on the diagram, until eventually successive levels coincide. At this point the electron may be said to have escaped from the atom altogether. Thus, the distance between a given level and these coincident levels represents the energy required to remove from the atom an electron which is initially in the given level. When this is the lowest possible level for the most readily removed electron, the energy is called the ionisation energy (see Fig.
18), but the importance of the spin quantum number is made clear in the next section. ELECTRONIC STRUCTURES OF ATOMS The Pauli Exclusion Principle In 1925, the German physicist Pauli suggested that no two electrons in any atom could have all four quantum numbers the same. H e based this generalisation (known as the Pauli Exclusion Principle) both on theoretical considerations and on experimental evidence. The operation of the quantum rules restricts the possible combinations of quantum numbers, and the addition of the Pauli principle now sets a limit on the number of electrons which can be contained in each of the sub-levels mentioned above.