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A quick chemistry Question

  1. Mar 29, 2005 #1
    Hi everyone, i am a new member here. I really liked this web site and i would like to thank everyone who's registered here. I have a quick question in chemistry and i really would like to know the answer of it. the answer would be really appreciated from whoever is going to answer it for me and thanx so much. my question is as the following:

    q. what experimental evidence requires that the emission of energy by an atom be quantized?
    (waiting for ur responses)
    that's it for now... and have a nice day everyone. :smile:
  2. jcsd
  3. Mar 29, 2005 #2


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    What have you studied? Please show us some of your attempts of your brainstorming. Frequently, you have the traces of the answer in your mind, and only you'll do is to gather them.
  4. Mar 29, 2005 #3
    thanks for ur response

    thanx for ur response...the thing is that i am not sure what the question is asking for since i don't fully understand it. i have been studying the atomic theory and the basic concepts concerning isotopes and radioactive substances, that's it so far.... so i don't know if it has to do with isotopes and radioactive substances. and thanx.
  5. Mar 29, 2005 #4


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    Well, I am not sure about so-physics-related-chemistry issues, but look for Balmer, Lyman, Paschen, or Pfund series, characteristic for hydrogen atom. These show clearly that there is a quantized behavior in hydrogen atom. The same approach in other atoms are rather complicated due to interelectronic interactions. However, single-electron ions like Li+ can be calculated, if I am not wrong.
  6. Mar 29, 2005 #5
    hello again

    thanks a lot for ur response...i really appreciate. i am going to look for these series that u gave me but where can i find them just to save some time since i am really busy thes days and i really wanna get this question before this coming thursday since i have a test and i really need help.
    take care. :confused:
  7. Mar 30, 2005 #6


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    Look into Max Planck's work on radiation, and how he figured their energies must be quantized.

    Also look into the photoelectric effect, and the explanation of the effect by Einstein.

    Try Googling "atomic spectra" or "balmer lyman paschen bracket pfund". Chem_tr's already mentioned this and really all you have to do is google the key words.
  8. Jun 7, 2006 #7

    This is one of the quetsions in the SCH4UA courses offered by

    TVontario's Independent Learning Program. Here is a start of an answer for the question by me. I would say that it was Batmers experimentation with hydrogen and specific energy levels analyzed with the spectroscope, revaing bandwidths of colour tied in to the energy levels, and wave engths.

    "Radiant Energy and Spectra
    It has been known for many years that eements gave out specific

    eolectromagetic radiation in the form of spectrao lines. These lines

    are really an element's fingerprints. Each element gives its own

    characteristic line patterns. THe coour playe d II after page 336 in

    the textbook illustrates this well.

    This spectrum was thhought to be associated with waves, the freqency of

    which was governed by the equation

    f=c/ h"lambda" (if I remember rightI don't have a lambda key)

    Where f = frequnecy
    c= the speed of light
    lambad = the wavelength

    read section 1-8 and 1-9
    1-8 is dispersion of visible light

    which goes into how electrons position around the nucleus.

    "Each atom or array of energy acts as as a prisism that is bands are

    absorbed or emited, depending on the 'mater filter' that is the

    'objects that the light is passing through. This goes into newtons

    'optics' stuff. The idea of refraction. Thus wavelengths travel at

    different velocities through a prism. It goess into the spectrograph


    1-9 is atomic emission spectra. Each element has it's own spectrum.
    Batmer 1884 energized atoms of hydrogen gas and eaminded the visible

    radiation with spectorscope he found priminentcoloured lines in the

    hydrogen spectrum.
    red bleu-green blue violet al thse at different ength from 6.653 x

    10-7 to 4.102 x 10-7 (visible light?)
    Planck in 1900 through up the quantum theory started the development of

    a new atom.. einstien confirmed this.
    in 1913 bohr nailed the coffin shut on the debate.

    he electrons in free atoms can will be found in only certain discrete energy states. These sharp energy states are associated with the orbits or shells of electrons in an atom, e.g., a hydrogen atom. One of the implications of these quantized energy states is that only certain photon energies are allowed when electrons jump down from higher levels to lower levels, producing the hydrogen spectrum. The Bohr model successfully predicted the energies for the hydrogen atom, but had significant failures that were corrected by solving the Schrodinger equation for the hydrogen atom.
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