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Homework Help: Lewis Structure.

  1. Sep 1, 2009 #1
    1. The problem statement, all variables and given/known data
    write lewis structure for SOCl2.

    2. Relevant equations

    3. The attempt at a solution
    .. .. ..
    .. | ..

    what i did was put S in the middle with a single bond on both side for Cl, each Cl has six dot. S has two at the top. I havve a single bond at the bottom of S to connect to O. O has six dot.
    i wanted to know if i can also write another structure. like take one set of electron away frm Oxygen and put a double bond connect sulfur and oxygen, instead of a single bond? please let me know if the top diagram is correct also. Thank you
  2. jcsd
  3. Sep 2, 2009 #2


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    From the Lewis structure you drew, the oxygen would have a formal charge of -1 and the sulfur would have a formal charge of +1. In order to eliminate these formal charges you can use a lone pair from the oxygen to form a double bond with the sulfur. This leaves none of the atoms with a formal charge, but it leaves sulfur with 10 electrons in its valence shell. This would normally be a problem, but because sulfur is in the third period of the periodic table, it can violate the octet rule by using its d-orbitals to expand its valence shell and hold more than eight electrons.

    So the structure with a double bond between the sulfur and oxygen would be the correct Lewis structure.
  4. Sep 2, 2009 #3
    thank you
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