Electron Energy Levels
1. What causes the lines to be produced in this way?
The different electron energy levels caused in hydrogen cause these lines in the spectrum to be produced in this way because the wavelengths that are released when the electron move back to the ground state is specific and it varies accordingly.
2. Into which energy level are electrons dropping into to make these visible lines?
The electrons are dropping back to the ground state which is the bottom most energy level to makes these visible lines.
3. What happens when the electrons drop into the 1st energy level? What happens when electrons drop into the 3rd, 4th and 5th energy levels?
The wavelength of the electrons becomes closer together and smaller as the electrons drop into the 3rd,
4th and 5th energy levels.
4. Between which energy levels are the electron transitions the largest?
The outermost and the innermost energy levels will have the largest energy transition.
5. The lines on an emission spectrum get closer together towards the violet end of the spectrum. What is this called and why does it happen?
This is called convergence and it happens because the lines become closer together as their energy increases, the energy of shells is increasing by diminishing amounts.
6. Click on the emission spectrums for each of the first 20 elements. What do you notice about the different spectrums as the atoms contain more electrons? Are any of the spectrums the same or are they unique?
The lines in the spectrum increases as the atoms contain more electrons and all of the spectrums are unique as each element has a different amount of electrons.
7. Click to show absorption spectrums. What is the difference? What is a continues spectrum compared to a line spectrum?
The difference is that there are several black lines in the absorption spectrum where the coloured lines are in the emission spectrum. A continuous spectrum displays all the colours in a smooth gradation from one end to the other. However, a line spectrum only displays certain strips out of the continuous spectrum.
The different electron energy levels caused in hydrogen cause these lines in the spectrum to be produced in this way because the wavelengths that are released when the electron move back to the ground state is specific and it varies accordingly.
2. Into which energy level are electrons dropping into to make these visible lines?
The electrons are dropping back to the ground state which is the bottom most energy level to makes these visible lines.
3. What happens when the electrons drop into the 1st energy level? What happens when electrons drop into the 3rd, 4th and 5th energy levels?
The wavelength of the electrons becomes closer together and smaller as the electrons drop into the 3rd,
4th and 5th energy levels.
4. Between which energy levels are the electron transitions the largest?
The outermost and the innermost energy levels will have the largest energy transition.
5. The lines on an emission spectrum get closer together towards the violet end of the spectrum. What is this called and why does it happen?
This is called convergence and it happens because the lines become closer together as their energy increases, the energy of shells is increasing by diminishing amounts.
6. Click on the emission spectrums for each of the first 20 elements. What do you notice about the different spectrums as the atoms contain more electrons? Are any of the spectrums the same or are they unique?
The lines in the spectrum increases as the atoms contain more electrons and all of the spectrums are unique as each element has a different amount of electrons.
7. Click to show absorption spectrums. What is the difference? What is a continues spectrum compared to a line spectrum?
The difference is that there are several black lines in the absorption spectrum where the coloured lines are in the emission spectrum. A continuous spectrum displays all the colours in a smooth gradation from one end to the other. However, a line spectrum only displays certain strips out of the continuous spectrum.