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Molecular structure question

  1. Jan 17, 2012 #1
    I am not a chemist. I have a molecular structure question.

    Is it possible to bind two positively charged molecules together by having two electrons bounce up and down in the space between them?

    M1+ e e M2+

    imagine the e, electrons oscillating up and down. Either in sync and 180 degree out of phase.

    Is there any simulation software that I could use to simulate a situation like this? Thanks.

    Ed Pell
     
  2. jcsd
  3. Jan 17, 2012 #2
    You may want to check out the literature on electrides and solvated electrons, as they're the closest thing I can think of that might be applicable, based on your description. The idea is that the electron serves as an anion to a cation in lieu of a typical counterion. I don't think most of them are stable under standard temperature and pressure, although I believe there are one or two that have been found.

    If you can share more about your idea, I might be able to add more to this brief comment.
     
  4. Jan 17, 2012 #3
    Are you asking if its possible to have two positively charged species bound together? Or particularly by electrons bouncing up and down?

    Hydrogen molecule ion, H2+ is the simplest molecule and is an example of the former. The latter is not really how electrons behave, they dont just jump around a molecule like a classical particle might.
     
  5. Jan 18, 2012 #4
    Hey edpell,

    This is more an electron structure question.

    M1+ e e M2+

    This a charge neutral scenario. When stuff is bonded you must offset the all protons and electrons in the molecule to determine the resultant charge - though experimentally it is possible to determine if one of the molecule's constituents has more charge than the other. Here you seem to be suggesting that the 2 e's are not negating the positive charge of the 2 M's but are instead through their synchronicity/phase relationship are forming a bond between the two positively charged M's - remember electrons themselves are repulsive.

    Generally electron positions - determined by probability density functions - are well understood, even in molecules i.e. cuprite, methane. The quantum nature of electrons means we can not know exactly where we will find them in the atom/molecule when we look for them let alone what they were doing before we looked i.e. oscillating.



    ch@rlatan.
     
  6. Jan 21, 2012 #5
    You gave a very complicated description of a covalent bond, however electrons will not "bounce" in the way you suggested - they occupy a molecular orbital and their position is uncertain (read more about wavefunctions).
     
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