Is the Lewis Structure for SOCl2 Correct?

[phys1618]

Homework Statement

write lewis structure for SOCl2.

Homework Equations

The Attempt at a Solution

.. .. ..
:Cl-S-Cl:
.. | ..
:O:
..

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

 

[Ygggdrasil]

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.

 

[phys1618]

thank you