In the ground state, the outermost shell (n = 1) of helium (He) is filled with e

Question

In the ground state, the outermost shell (n = 1) of helium (He) is filled with electrons, as is the outermost shell (n = 2) of neon (Ne). The full outermost shells of these two elements distinguish them as the first two so-called "noble gases." Suppose that the spin quantum number ms had five possible values, rather than two. Assume that the possible values for the other three quantum numbers are unchanged, and that the Pauli exclusion principal still applies.
(a) Which element would be the first noble gas?


(b) Which element would be the second noble gas?

Explanation / Answer

First noble gas will be still Helium because it depends on atomic number not on the configurations of the electrons

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