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Hybridization of sulfur

  1. Oct 18, 2013 #1

    Qube

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    Hybridization of carbon

    Pretty sure my professor is wrong once again.

    me8y6yge.jpg

    SO2 should have two double bonds which gives the sulfur a minimal formal charge and two signs bonds. The two sigma bonds imply sp hybridization, not the blatantly wrong circled answer.
     
    Last edited: Oct 18, 2013
  2. jcsd
  3. Oct 18, 2013 #2
    How many valence electrons does sulfur has? What is the structure of SO2?

    The attached question is about C2H2, but the circled answer is wrong. The hybridisation is sp for carbon in C2H2.
     
  4. Oct 18, 2013 #3

    SteamKing

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    It's fortunate that your professor has you around to keep him straight.
     
  5. Oct 18, 2013 #4

    DrDu

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    I am quite tired of repeating here in the forum that atoms don't "have" a certain hybridization in a given molecule over and over.
    Acetylene can perfectly well be described both in terms of sp and sp3 hybrids. In the latter case, the bonds are called descriptively "banana bonds". The energetic difference is usually minute between alternative hybridization schemes in valence bond theory and can only be evaluated using dedicated VB programs.
    In the case of SO2, it is not even necessary to involve hybridization: The bonds to the two oxygens can be explained using two of the p orbitals of sulphur alone.
     
  6. Oct 18, 2013 #5

    Qube

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    Whoops, I was thinking of another question. Yes, the circled answer is still wrong since in the case of the hydrocarbon in the picture the carbon has a hybridization of sp2; there are two bonds with hydrogen and one triple bond between the carbons, giving us a total of 3 sigma bonds.
     
  7. Oct 18, 2013 #6

    Qube

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    I won't be having him around any longer; I think his job security is decreasing by the day (answer?)
     
  8. Oct 18, 2013 #7

    Qube

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    You lost me at banana bond.

    I do understand that hybridization is a model for explaining phenomenon such as the fact carbon forms four bonds instead of two, and that models don't always translate perfectly to the real world, just as the Bohr atom model is still used to explain things even though the model is overly simplistic (or simply incorrect).
     
  9. Oct 18, 2013 #8

    dextercioby

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    Take it easy. in C2H2, the hybridization of C is sp, The molecule is linear (no free electrons) and between the 2 C atoms there's a triple bond.
     
  10. Oct 18, 2013 #9

    Qube

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    You're right sorry I keep thinking of C2H4.
     
  11. Oct 18, 2013 #10

    DrDu

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