Neon, with an atomic number of 10, is a noble gas located in group 18, which makes it largely inert and unreactive due to its complete valence electron shell. In contrast, sodium, which has an atomic number of 11 and is found in group 1, has only one electron in its outermost shell, making it highly reactive as it readily loses that electron to achieve a stable electron configuration. The differences in their reactivity can be attributed to their positions in the periodic table; while neon’s full outer shell provides stability, sodium's tendency to lose its one valence electron leads to its vigorous reactions, particularly with nonmetals. Therefore, the properties of atomic structure and electron configuration explain the contrasting reactivities of these two elements.
How does the reactivity of neon (atomic number 10, period 2, group 18) differ from that of sodium (atomic number 11, period 3, group 1)? Explain your reasoning based on the properties of neon and sodium that you can infer based on their atomic numbers, periods, and groups.(4 points) write it in 3-5 sentences in one paragraph
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