Chapter 5, Problem 118A

Interpretation Introduction

Interpretation:

The ground state electronic configuration for sodium needs to be determined and how this is related to the bright lines needs to be explained.

Concept introduction:

Atomic emission spectroscopy is used to determine the element’s quantity in the sample by using the intensity of liquid emitted at a particular wavelength.

Answer to Problem 118A

The ground state electronic configuration of sodium metal is $1s^{1}2s^{2}2p^{6}3s^1$. The two bright lines are produced when the electron of sodium atom drops from the excited states (higher energy states) to the lower energy states.

Explanation of Solution

Sodium shows two bright lines having wavelengths of $\text{588}\text{.9590}\text{nm}$ and $\text{589}\text{.9524}\text{nm}$. The ground state electronic configuration cab be determined by including every orbital before $3s^1$. The last electron of the sodium metal is in the $3s^1$ orbital. Therefore, the electronic configuration is $1s^{1}2s^{2}2p^{6}3s^1$. The two bright lines are produced when sodium atom drops from the excited states (higher energy states) to the lower energy states. This occurs when an electron in the higher energy orbitals drops into the lower energy states.

Conclusion

The ground state electronic configuration of sodium metal is $1s^{1}2s^{2}2p^{6}3s^1$. The two bright lines are produced when the electron of sodium atom drops from the excited states (higher energy states) to the lower energy states.