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 your answer in 3-5 sentences

Answer 1

Neon (atomic number 10), a noble gas in group 18, is chemically inert and exhibits very low reactivity due to its full outer electron shell, which provides stability. In contrast, sodium (atomic number 11), an alkali metal in group 1, has one electron in its outermost shell, making it highly reactive as it readily loses that electron to achieve a stable electronic configuration. The difference in reactivity between the two elements can be attributed to their positions in the periodic table: neon’s complete valence shell prevents it from forming bonds, while sodium's propensity to lose an electron facilitates a range of chemical reactions. Thus, sodium's reactivity is significantly higher than that of neon.