Multiple lines in H2 and Hg emission spectra

[hagopbul]

I was doing a test about rydberg constants using H2 and Hg light spectrum

And in the spectrograph I found that H2 have three spectra and the Hg have 5 spectra
And I DON'T KNOW WHY H2 have 3 lines and Hg have 5 lines? (Scientifically).

I know it is the numbers of the electrons that determine the number of the spectrum lines but how exactly?
Can anyone help me please

 

[Retsam]

Well it is the number of possible transitions that determine the number of spectrum lines you will see, and also the energy supplied to the atoms. If for example we imagine an atom has 3 energy levels, then the possible electron transitions would be :

n3 => n1 5 J
n3 => n2 3 J
n2 => n1 2 J

These energy levels are not proper values i have just made them up for the example. I have noted next to them the energy difference between each pair of shells. So if we supply energy to the electrons in an atom they may be excited to say the n3 state then they have gained 5J of energy. Now the electron will dexcite at some random time and could make either the n3 to n2 transition which means it will emit light of energy 3J, or make the n3 to n1 transition and emit light of 5J. The frequency of light depends on the energy change in the transition.

f = E/h

 

[denian]

The number of spectral lines observed in a spectrum is determined by the electronic transitions that occur within the atoms or molecules being studied. In the case of H2 and Hg, both are made up of multiple atoms, but the number of electrons in each atom is different.

H2 is made up of two hydrogen atoms, each with one electron. When energy is applied to the H2 molecule, the outer electron can transition between different energy levels, resulting in three possible spectral lines. This is because the electron in H2 can occupy three different energy levels: the ground state (lowest energy), the first excited state, and the second excited state. The transitions between these energy levels produce the three observed spectral lines.

On the other hand, Hg is a single atom with 80 electrons. As the number of electrons increases, the number of possible energy levels also increases. This results in a more complex spectrum with more spectral lines. In the case of Hg, there are five possible energy levels that the electrons can occupy, resulting in five observed spectral lines.

In summary, the number of spectral lines observed in a spectrum is determined by the number of electrons and the energy levels available to them. H2, with only two atoms and a simpler electronic structure, has fewer spectral lines compared to Hg, which has a larger number of electrons and a more complex electronic structure. I hope this explanation helps to clarify the difference in the number of spectral lines observed in the H2 and Hg emission spectra.