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Why is the angle of SO2 120 degrees?!
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So SO2 has 2 bonding pairs and 1 non-bonding pair! So 3 pairs in total!
So it's 120 - 2.5 = 117.5o but why is it 120o ?!
I don't get the explanation about the extra repulsion thing in this case!
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Like water for instance it has 2 bonding pairs and 2 non-bonding pairs, so 4 pairs in total!
109.5-(2.5x2)= 104.5o which is right!
So it's 120 - 2.5 = 117.5o but why is it 120o ?!
I don't get the explanation about the extra repulsion thing in this case!
Like water for instance it has 2 bonding pairs and 2 non-bonding pairs, so 4 pairs in total!
109.5-(2.5x2)= 104.5o which is right!
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#2
This is because the extra repulsion you get from the double bond cancels out the the lone pair repulsion 
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(Original post by ThatMadClown)
This is because the extra repulsion you get from the double bond cancels out the the lone pair repulsion
This is because the extra repulsion you get from the double bond cancels out the the lone pair repulsion
The book says that double bonds must be treated the same as single bonds so why isn't that the same case with SO2?!
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#4
(Original post by Adorable98)
Yeah, but why wouldn't that be the same case with O=C=O ? It's 180 but wouldn't there be more rupilsion?!
The book says that double bonds must be treated the same as single bonds so why isn't that the same case with SO2?!
Yeah, but why wouldn't that be the same case with O=C=O ? It's 180 but wouldn't there be more rupilsion?!
The book says that double bonds must be treated the same as single bonds so why isn't that the same case with SO2?!
There are no additional lone pairs of electrons after it makes its bonds with oxygen.
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(Original post by RMNDK)
Because carbon only has 4 valence electrons.
There are no additional lone pairs of electrons after it makes its bonds with oxygen.
Because carbon only has 4 valence electrons.
There are no additional lone pairs of electrons after it makes its bonds with oxygen.
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#6
You must remember that due to the 'shape' of pi bonds, the p-orbital overlap is above and below the plane and does NOT affect the shape of the molecule/ion. Thus, SO2 has 3 electron pairs around the sulfur atom; two are bonding and one is a lone pair. The lp repels the bp more so the bond angle is about 120 deg. Two lp as in H2O would reduce the BOND ANGLE EVEN MORE.The explanation above about the electron density of the double bonds canceling out is absolutely rubbishTHE ALCHEMISTDoc Dickson
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(Original post by thealchemist666)
You must remember that due to the 'shape' of pi bonds, the p-orbital overlap is above and below the plane and does NOT affect the shape of the molecule/ion. Thus, SO2 has 3 electron pairs around the sulfur atom; two are bonding and one is a lone pair. The lp repels the bp more so the bond angle is about 120 deg. Two lp as in H2O would reduce the BOND ANGLE EVEN MORE.The explanation above about the electron density of the double bonds canceling out is absolutely rubbishTHE ALCHEMISTDoc Dickson
You must remember that due to the 'shape' of pi bonds, the p-orbital overlap is above and below the plane and does NOT affect the shape of the molecule/ion. Thus, SO2 has 3 electron pairs around the sulfur atom; two are bonding and one is a lone pair. The lp repels the bp more so the bond angle is about 120 deg. Two lp as in H2O would reduce the BOND ANGLE EVEN MORE.The explanation above about the electron density of the double bonds canceling out is absolutely rubbishTHE ALCHEMISTDoc Dickson
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