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 this in one big paragraph

Answer 1

Neon (atomic number 10) and sodium (atomic number 11) exhibit significantly different reactivity due to their positions on the periodic table. Neon is located in group 18, which contains the noble gases, known for their complete outer electron shells, making them highly stable and largely inert in chemical reactions. With eight electrons in its outer shell, neon does not readily form bonds, and its lack of reactivity is a key characteristic that sets it apart from other elements. In contrast, sodium is situated in group 1, known as the alkali metals, which possess only one electron in their outermost shell. This single valence electron makes sodium highly reactive, as it readily loses this electron to achieve a stable electron configuration, often forming ionic compounds with nonmetals. The differences in reactivity can also be attributed to the periods they occupy; sodium, being in period 3, is larger in atomic size compared to neon in period 2, resulting in decreased nuclear charge effect on its outer electron, thereby facilitating its loss during chemical reactions. These elemental characteristics—neon's full outer shell contributing to its inertness versus sodium's single valence electron leading to high reactivity—are central to understanding the contrasting behaviors of these two elements.