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Postby leilawilliams16 » Sun Dec 10, 2017 1:48 pm

Is the lewis structure for SO2 most stable with one or two double bonds? Different sources say different things

Liam Maxwell 2E
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Re: SO2

Postby Liam Maxwell 2E » Sun Dec 10, 2017 3:08 pm

If you apply two double bonds none of the atoms will have a charge since sulfur can have two unpaired electrons due to its expanded octet

Tina Wen 1G
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Re: SO2

Postby Tina Wen 1G » Fri May 11, 2018 2:43 pm

2 double bonds with 2 oxygen atoms and sulfur in the middle with a lone pair is the most stable structure for SO2. Sulfur has the empty 3d orbital that can participate in bonding so it’s okay for sulfur to carry more than 8 electrons.

Jacob Samuels 1E
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Re: SO2

Postby Jacob Samuels 1E » Fri May 11, 2018 2:47 pm

If you’re confused, just remember to prioritize having smaller formal charges and then worry about abiding by the octet rule.

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Re: SO2

Postby MadelynNguyen1F » Sat May 12, 2018 12:19 pm

Two double bonds, because of the formal charges, but the actual structure is a hybrid of all three.

Alondra Juarez section 1E
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Re: SO2

Postby Alondra Juarez section 1E » Sun May 13, 2018 11:34 am

it would be more stable with two double bonds

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