1. Does each element have its own emission spectrum?

2. Does each element have its own absorption spectrum?

3. When you look at the emission or absorption spectrum ofastar, for example, are you seeing the superposition of allstar'sgazes' spectra?

4. When you look at the emission or absorption spectrum ofastar, and you see that it's redshifted or blueshifted, areyoucomparing this spectra to that of the Sun or to that of thatstarat another time?

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Related questions

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?

1. A transformer for an answering machine takes an ACvoltageof 170 V. (maximum, or peak-to-peak) as its input andprovides 7.8V (rms) as its output to the answering machine.

A) What is the rms equivalent to thispeak-to-peakvoltage?

B) Calculate the turns ratio between the primaryandsecondary.

C) When not answering, the machine uses a maximum power of5.0W. What is the current (rms) drawn from the 170 V line?

2. An astronomer is making an observation of anew-discoveredgalactic object. Part of this observation is theanalsis of thelight emitted by the object. It is observed that thislightincludes a clear pattern of the emission spectrum ofatomichydrogen.

Part of that spectrum is the HÎ± line, which on earth hasawavelength of 656.258 nm

(10^-9m). The observed light from this objecthasthis spectral line measured at 659.0 nm.

Explain this discrepancy, quantitatively, using theDopplerEffect.

thank you. Please help me.

Suppose we have reason to suspect that a certain quantum objecthasonly three quantum states. When we excite a collection ofsuchobjects we observe that they emit electromagnetic radiationofthree different energies: 0.9 eV (infrared), 1.9 eV (visible),and 2.8 eV (visible).

(a) Draw a possible energy-level diagram for one of thequantumobjects, which has three bound states. On the diagram,indicate thetransitions corresponding to the emitted photons, andcheck thatthe possible transitions produce the observed photons andnoothers. When you are sure that your energy-level diagramisconsistent with the observed photon energies, enter the energiesofeach level (K+U, which is negative). EnterALLlevels before submitting; all of the energies must be correctto beproperly scored. The energy K+U of theground state is -4eV.