Moving from the element with atomic number 10 (Neon) to atomic number 11 (Sodium) on the periodic table, there is a significant change in reactivity. Neon, a noble gas, is chemically inert and does not easily form compounds. However, Sodium is an alkali metal and is highly reactive. It readily reacts with water to produce sodium hydroxide and hydrogen gas. Sodium's reactivity is due to its tendency to lose one electron from its outermost shell, leading to increased interactions with other elements.
Moving from the element with atomic number 10 (neon) to atomic number 11 (sodium) on the periodic table, there is a significant change in reactivity. Neon is a noble gas and is known for its inertness, meaning it does not readily react with other elements. Conversely, sodium is an alkali metal and is highly reactive. This change in reactivity is due to the difference in electron configuration. Neon has a full valence electron shell and does not have a strong tendency to gain or lose electrons. Sodium, on the other hand, has one valence electron, which it readily donates, making it highly reactive. The change in reactivity from neon to sodium is thus a result of the change in electron configuration and the desire to achieve a more stable configuration.
