Spectrum of Sodium vs. Hydrogen

In summary, the energy levels for sodium are different from those for hydrogen due to the difference in the number of protons and electrons. While sodium has a heavier nucleus and more electrons, the nucleus is "screened" by negative charges, resulting in only one free electron like hydrogen. Additionally, sodium's extra electrons fill up the lowest energy levels, making them unavailable for the valence electron and causing the energy levels to match a subset of hydrogen's levels.
  • #1
roam
1,271
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My question is: Why the energy levels for sodium are different from those for hydrogen even though sodium is described as a "hydrogen-like atom"?

Here I have posted the energy diagrams for sodium, and hydrogen.

So, I have noted that sodium has 11 protons, whereas the hydrogen has only 1 proton. So sodium has a heavier nucleus having a charge 11 times greater than that of hydrogen. And sodium has 11 electrons while hydrogen has only 1.

I wanted to argue that the difference of the number of protons and electrons somehow affects the spin-orbit coupling. But in sodium the nucelus with Z=11 is "screened" by 10 negative charges. So we have 1 free electron, exactly like the hydrogen atom! So shouldn't we end up with the same energy diagram? :confused:

I am very confused about this. Any explanation would be greatly appreciated.
 
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  • #2
It's because Sodium starts out with 10 extra electrons that fill up the lowest shells. Therefore these levels aren't available to the valence electron. Cover over the lowest levels of Hydrogen (principal quantum number 1 and 2), and you'll see that Sodium levels match a subset of Hydrogen levels.
 

Related to Spectrum of Sodium vs. Hydrogen

What is the difference between the spectrum of sodium and hydrogen?

The spectrum of an element refers to the specific wavelengths of light that it emits or absorbs. In the case of sodium and hydrogen, the main difference is the number of spectral lines. Sodium has two prominent lines, while hydrogen has many more lines, creating a more complex spectrum.

Why is the spectrum of sodium simpler than that of hydrogen?

This is due to the difference in the electron configuration of the two elements. Sodium has only one electron in its outermost shell, while hydrogen has one electron in its only shell. This simpler electronic structure of sodium results in fewer possible energy transitions and, therefore, fewer spectral lines.

What is the significance of the spectral lines in the spectrum of sodium and hydrogen?

The spectral lines are significant because they reveal the unique energy levels of each element. Each line corresponds to a specific energy level that an electron can occupy. By analyzing the positions and intensities of these lines, scientists can identify elements and learn about their atomic structure and behavior.

What is the relationship between the spectrum of sodium and hydrogen?

The relationship between the two spectra lies in their atomic structure. Both elements have a single electron in their outermost shell, making them similar in terms of energy levels and transitions. However, the difference in the number of spectral lines is due to the number of electrons in their inner shells.

How does the spectrum of sodium and hydrogen contribute to the field of astronomy?

By studying the spectra of elements like sodium and hydrogen, astronomers can determine the chemical composition and physical properties of celestial bodies. For example, the presence of sodium in a star's spectrum can indicate the temperature and density of its atmosphere. Additionally, the complex hydrogen spectrum can provide insights into the structure and evolution of stars and galaxies.

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