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Hybrid orbitals problem

  1. Oct 8, 2014 #1
    I'm seeing conflicting answers among various textbooks. I would predict that it forms SP3 hybrid orbitals, and yet its bond angles are far from 109.5.

    Edit: H2S, rather.
     
    Last edited: Oct 8, 2014
  2. jcsd
  3. Oct 9, 2014 #2

    Borek

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    Staff: Mentor

    No hybridization at all and pure sp3 are just two ends of a continuum.

    For some highly symmetrical molecules (say, CH4) hybridization of the central atom is a pure sp3. But for some other molecules, like H2S, what we observe is just some partial hybridization, in which bonds are not equivalent.
     
  4. Oct 9, 2014 #3

    DrDu

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    Science Advisor

    Note also that hybridization is not a property of the molecule but entirely your personal choice of a convenient expression for the molecules wavefunction.
    E.g. molecules like ethylene can equally well be described in terms of sp2+p or sp3 hybrids and water in terms of s+p or sp3 or even something intermediate.
    In the case of H2S a description in terms of pure s and p orbitals makes probably more sense than the assumption of sp3 hybrid orbitals as the s and p orbitals in second row atoms differ considerably in size and energy.
     
  5. Oct 10, 2014 #4
    I see. How does one determine whether pure hybridization is a more appropriate model to describe orbital shape?
     
  6. Oct 20, 2014 #5
    What about HCl, are orbitals of chlorine hybridized in that case?
     
  7. Oct 20, 2014 #6

    Borek

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    Staff: Mentor

    No need for that.
     
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