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Chapter 4: Problem 98

Which atom has a smaller valence shell, lithium (Li) or sodium (Na)? Explain your answer.

Short Answer

Expert verified
Lithium (Li) has a smaller valence shell than sodium (Na). This is because Li is located in period 2 and Na in period 3 of the periodic table, and atomic radii increase moving down a group. Thus, Li's valence shell is closer to its nucleus than Na's valence shell.

Step by step solution

01

Identify the electron configurations

Determine the electron configurations for lithium (Li) and sodium (Na). Li - atomic number: 3 Li electron configuration: 1s² 2s¹ Na - atomic number: 11 Na electron configuration: 1s² 2s² 2p⁶ 3s¹
02

Understand the periodic table trends

Going across a period in the periodic table, atomic radii generally decrease as the elements' effective nuclear charge increases. This is due to the greater attraction between the nucleus and the valence electrons. On the other hand, moving down a group in the periodic table, atomic radii increase as more electron shells are added, causing the outermost electrons to be further away from the nucleus.
03

Compare the positions of Li and Na in the periodic table

Locate lithium (Li) and sodium (Na) in the periodic table. We find that both Li and Na are in Group 1 (alkali metals group), with Li in period 2 and Na in period 3. Since Na is below Li in the same group, it indicates that Na has a larger atomic radius compared to Li, meaning it has a larger valence shell.
04

Conclusion

Based on the analysis of their electron configurations and their positions in the periodic table, we conclude that lithium (Li) has a smaller valence shell than sodium (Na).

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