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 them in one big sentence

Answer 1

The reactivity of neon, which is a noble gas in Group 18, is significantly lower than that of sodium, which is an alkali metal in Group 1, due to neon's full valence electron shell that makes it chemically stable and largely inert, while sodium has a single electron in its outermost shell that it readily loses to achieve a stable noble gas configuration, resulting in high reactivity particularly with nonmetals, which can be explained by the trends in atomic structure where neon's higher electronegativity and greater ionization energy compared to sodium's contribute to its lack of tendency to engage in chemical reactions.