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Is that possible?

  1. Oct 5, 2005 #1
    is this electron configuration possible for non ground state atom:
    1s2 2s2 2p5 3s2 3p5
    Thannx in advance
     
  2. jcsd
  3. Oct 5, 2005 #2

    Gokul43201

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    It will have a very tiny lifetime, probably no longer than nanoseconds - in other words, "NO".

    Why do you ask ?
     
  4. Oct 5, 2005 #3
    How is it even possible to fill up the 3s orbital when the 2p isn't full?
     
  5. Oct 5, 2005 #4
    in my chem quiz there was a question like this ' is it possible to have this electron configuration for an excited atom' ..
    i wrote no ... but the teacher marked me wrong ...
    wut do u think ..?????
     
  6. Oct 5, 2005 #5
    anyone has any clue???
     
  7. Oct 5, 2005 #6

    Gokul43201

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    You start with a full 2p subshell. Then an electron or photon comes by and knocks out one of the 2p electrons. Very soon, an electron from the 3s subshell falls to occupy the vacancy created. But for a very tiny length of time, the stated configuration exists (but it's unfair to say that such a configuration is, in general, "possible").
     
  8. Oct 5, 2005 #7

    Gokul43201

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    You should ask your teacher for his/her reasoning is...and do come back and let us know what it is.
     
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