1. Neon (Ne) and sodium (Na) exhibit contrasting reactivity due to their respective positions on the periodic table. Sodium, located in Group 1 as an alkali metal, is highly reactive because it possesses a single electron in its outer shell that it can readily lose to form a Na⁺ ion, thus achieving stability. In contrast, neon resides in Group 18 among the noble gases and remains completely unreactive. This lack of reactivity is attributed to neon's full outer shell containing eight electrons, which renders it stable and non-reactive. The electron configuration for sodium is 1s² 2s² 2p⁶ 3s¹, while neon's configuration is 1s² 2s² 2p⁶. The presence of an unpaired electron in sodium increases its likelihood of reacting, whereas neon's complete outer shell prevents any such reactions. Consequently, the high reactivity of sodium starkly contrasts with the stability of neon, illustrating the diverse behaviors of elements across different groups.

Question

2. Neon (Ne) and sodium (Na) demonstrate significant differences in reactivity, primarily due to their positions on the periodic table. Sodium, classified as an alkali metal in Group 1, is very reactive because it has one electron in its outer shell that it can easily lose to form a Na⁺ ion, achieving a more stable state. Conversely, neon is found in Group 18, the noble gases, and is entirely unreactive. This is because neon has a complete outer shell with eight electrons, which makes it stable and resistant to reactions. Sodium's electron configuration is 1s² 2s² 2p⁶ 3s¹, while neon's is 1s² 2s² 2p⁶. The single unpaired electron in sodium increases its reactivity, while neon’s filled outer shell ensures it remains inert. Thus, sodium's high reactivity contrasts sharply with neon's stability, highlighting the distinct behaviors of elements in different groups.

Answer 1

Both passages effectively explain the contrasting reactivity of neon (Ne) and sodium (Na) based on their positions in the periodic table, their electron configurations, and the concept of stability relating to electron arrangement. Here’s a concise summary of the key points made in both texts:

1. Position in the Periodic Table:

   • Sodium (Na) is in Group 1 (alkali metals) and is highly reactive.
   • Neon (Ne) is in Group 18 (noble gases) and is inert.

2. Electron Configuration:

   • Sodium has the electron configuration: 1s² 2s² 2p⁶ 3s¹. It has one unpaired electron in its outer shell, which it readily loses to form a Na⁺ ion for stability.
   • Neon has the electron configuration: 1s² 2s² 2p⁶. Its outer shell is full with eight electrons, indicating stability and non-reactivity.

3. Reactivity:

   • Sodium's single unpaired electron makes it more likely to react.
   • Neon’s full outer shell imparts stability and a lack of reactivity.

4. Conclusion:

   • The reactivity of sodium sharply contrasts with the stability of neon, showcasing the varying behaviors of elements across different groups in the periodic table.

This comparison highlights fundamental concepts in chemistry related to electron configuration, group characteristics, and the notion of chemical reactivity based on atomic structure.