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