Neon (atomic number 10), located in group 18, is a noble gas characterized by a complete valence shell, which makes it highly stable and largely unreactive under normal conditions. In contrast, sodium (atomic number 11) is an alkali metal found in group 1, characterized by having a single electron in its outermost shell. This configuration makes sodium highly reactive, as it readily loses that one valence electron to achieve a stable electron configuration like that of neon. Therefore, while neon’s full valence shell contributes to its inertness, sodium’s desire to achieve stability through electron loss leads to its strong reactivity, particularly with nonmetals.
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
in 1 paraghraph
1 answer