Achieve #6 Week 5
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Achieve #6 Week 5
Hi! I was reviewing the homework and realized I don't quite understand why SO2 is a Lewis Acid? The S atom has a lone pair of electrons, so I would thin that it could donate those electrons as a base, but evidently, this line of thinking is wrong. Thanks so much for the help!
Re: Achieve #6 Week 5
SO2 is a Lewis acid because the central atom is double bonded to the two O atoms. There's one sigma bond, and one pi bond for each double bond, and the pi bond is easy to break since it's weaker than the sigma bond.
The electronegativity of oxygen is more than the electronegativity of sulfur, and so the oxygen has a partial negative charge. There's a partial breaking of bonds. The sulfur is deficient in electrons then, and can accept a pair of electrons.
The electronegativity of oxygen is more than the electronegativity of sulfur, and so the oxygen has a partial negative charge. There's a partial breaking of bonds. The sulfur is deficient in electrons then, and can accept a pair of electrons.
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Re: Achieve #6 Week 5
SO2 is a nonmetal oxide and contains lone pairs on the central atom in SO2. Therefore, these lone pairs can interact with a lone pair on another molecule, allowing for the formation of another bond to the central atom. Therefore, this would make SO2 a Lewis acid.
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Re: Achieve #6 Week 5
I thought this was the definition for bases ? Is this an exception to the rule?
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