Question

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. 2-4 sentences.

Answer 1

Neon, with atomic number 10, is a noble gas located in group 18, which means it has a complete outer electron shell and is largely unreactive, exhibiting minimal chemical reactivity. In contrast, sodium, with atomic number 11, is an alkali metal in group 1 that has a single electron in its outer shell, making it highly reactive as it readily loses that electron to achieve a stable configuration. Therefore, while neon remains chemically inert due to its stable electron configuration, sodium's tendency to react stems from its desire to attain stability through electron loss.