Lewis Dot Structure of SO2 (Sulfur Dioxide)
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Uploader Comments (kentchemistry)
Top Comments
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Isnt there too many electrons on sulfur? There's 10... 4 bonds and 2 dots?
4 months ago 6
All Comments (18)
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What about ressonance structures? Wouldn't it be more stable if we considered ressonance? Nice video, bro!
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im very new to chem. can anybody explain to me y it just cant be SO such as double bond with S=O. i really hope someone could reply me fast. thx :)
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THERE ARE EXCEPTIONS TO THE OCTET RULE. For the love of god, learn / research your shit, then come open your mouth here.
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@kentchemistry Don't you just love keyboard warriors / ignorant know it alls...
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@HaCk3Erx Elements in the 3rd period or higher (period = row) can have expanded octets (more than 8 electrons in the valence orbital), so this is why it's sound for 10 electrons to be on sulfur.
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Thank you! This was a very helpful review for me as a second semester gen chem. student.
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@ExplosPlankton i think if you draw it with resonance then there is one
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The only scrutiny I can make is that the bond angle for molecules with the bent geometry is LESS THAN 120 degrees. Everything else is right...
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your lewis structure is wrong! that one pair of e- on sulfur would create a bent molecule! dumbass
jvboy88 1 month ago
@jvboy88 What are you talking about 1:19 it say bent shape. Nice comment.
kentchemistry 1 month ago 6
Other sources say there's only one double bond in SO2.
ExplosPlankton 3 months ago
@ExplosPlankton
While there are other possible structures, based on the formal charge SO2 has 2 double bonds. It is the better model.
kentchemistry 3 months ago
You just learned the octet rule was only partially true.
It is only valid for period 1 and 2 elements. Beyond that it can get more complex.
Sulfur is in period 3 it can break the octet rule, 3rd energy level is 3s, 3p and 3d. It can hold up to 18 electrons by hybridizing up to 9 orbitals.
Imagine a d5sp3 hybrid. What shape is that?
kentchemistry 4 months ago