Please use the links on the Experiment page on theserverto complete the questions below and submit themforgrading.
Please use the Bohr model simulator at MichiganStateUniversity to complete the table below:
initial orbital | ending orbital | Wavelength (nm) |
3 | 2 | |
4 | 2 | |
| 2 | 434 |
| 2 | 410.2 |
7 | 2 | 397 |
4 | 3 | |
5 | 3 | |
See the spectrum of any element at http://jersey.uoregon.edu/vlab/elements/Elements.html
Bohr Model Simulation McGraw-Hill (Java)
Explore :LightEmission and Absorption Tutorial(NortonPublishing)
Explore :BohrModelof the Atom Tutorial (Norton Publishing)
Hydrogen Line Spectrum Quicktime Movie (1M)McGraw-Hill
You can generate your own spectra with the MiniSpectroscopyJavaApplet
Line Spectrum Flash Tutorial
1. What is the job of a spectroscope?
2. Why is the helium spectrum have so many morelinesthan the hydrogen spectrum?
3. Would you expect the spectrum of He+ tobehave as many lines as the spectrum of He? Please explainyouranswer? (He+ is the ion formed when Helosesone electron.t
4. The H2+ ion has onlyoneelectron. Would the spectrum of the H2+ionresemble the spectrum for any of the following:H2, H,He+, He? Please explainyour answer.
5. Which of the following can be expected to giveaspectrum most closely like that of the H atom: Li,Li+,Li+2 ?
6. Spectrum wavelengths are sometimes measuredinAngstrom units. Please convert 675 nm to Angstroms. (1Angstrom =10-10 meters. 1 nm =10-9meters.)
7. If an electron is in energy level 4, whatdifferentwavelengths can it make in coming back to energy level 2.(Please remember that the fall down is not always done in justonedrop.)
8. An electron which falls all the way down toenergylevel 1 would give off much more energetic light. Whyweretransitions which ended at energy level 1 were not studied bytheunaided eye?
