12.15 part B

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Christine Wastila 1H
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Joined: Fri Sep 29, 2017 7:04 am

12.15 part B

Postby Christine Wastila 1H » Tue Dec 05, 2017 11:33 am

This is more of a Lewis structure question. Why is the structure for SO2 drawn with a single bond on one of the oxygen + 6 valence electrons and a double bond on the other + 4 valence electrons rather than double bonds on both + 4 valence electrons? I have it with S in the middle + a lone pair and the two oxygens double bonded to it with 4 valence electrons on each (since S can have and expanded octet). Wouldn't that be better because the formal charges on all atoms are zero?

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Re: 12.15 part B

Postby Chem_Mod » Tue Dec 05, 2017 1:03 pm

Hi, Christine,
Both structures are possible. In this case, sulfur is drawn with a positive charge so that upon binding of the chloride, sulfur becomes neutral. This way the interaction between SO2 and Cl- is favorable. Otherwise, the structure is already stable as it is and will not exhibit Lewis base/acid type interaction.

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