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. write your answer in 3-5 sentences in one paragraph

Answer 1

Neon, with an atomic number of 10, is a noble gas found in group 18, which makes it highly stable and largely inert due to its complete valence electron shell. This stability results in very low reactivity, as neon does not readily form bonds with other elements. In contrast, sodium, with an atomic number of 11 and located in group 1, has only one valence electron, which it readily loses to achieve a stable electron configuration, resulting in a high level of reactivity. The tendency of sodium to react with other elements, especially nonmetals like chlorine, contrasts sharply with neon's lack of reactivity, illustrating how their positions in the periodic table dictate their chemical behavior.