p41_029 - s subshell, leaving only one remaining electron...

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29. For a given shell with quantum number n the total number of available electron states is 2 n 2 .Thu s ,fo r the ±rst four shells ( n = 1 through 4) the number of available states are 2, 8, 18, and 32 (see Appendix G).Since2+8+18+32=60 < 63, according to the “logical” sequence the ±rst four shells would be completely ±lled in an europium atom, leaving 63 60 = 3 electrons to partially occupy the
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Unformatted text preview: s subshell, leaving only one remaining electron in the only partially lled subshell (the 5 p subshell). In chemical reactions this electron would have the tendency to be transferred to another element, leaving the remaining 62 electrons in chemically stable, completely lled subshells. This situation is very similar to the case of sodium, which also has only one electron in a partially lled shell (the 3 s shell)....
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