Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: confused on December 21, 2004, 07:40:12 PM
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Could anyone please explain to me the bonding in Buckminsterfullerene? Specifically I was wondering what happens to the free valency in each carbon atom, or whether double bonds are involved. This would be a huge help to me if anyone can help, so far diagrams I have seen have been quite unhelpful in this regard.
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Free valence is either in double bonds creating a delocalised electron cloud reaching over the whole molecule (sorta like aromatic sphere) or subsitueted, usually by hydrogen etc. C50H50 and C60H60
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Why does a double bond create delocalised electrons?
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double bond doesn't create delocalized electrons, but conjucated double bonds can create aromatic systems where excessive electrons become delocalized.
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the 2p orbitals (that contain electrons) of the carbon atoms overlap with adjacent ones to form a region of equivalent energy level such that the electrons are free to move within without promotting or demoting its energy level.
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Is this a pi oribital then?
Btw, thanks for all the replies guys :)
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yes, it's a pi bond that extends over a carbon chain.
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Isn't it C60?...
:punch:
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Isn't it C60?...
There are diffrent sized buckyballs ranging from C28 to around C240. C60 Being the most common one.
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Perhaps this might help
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That's not the complete "fullerene zoo", I'm afraid:) - that page gives you a better idea...though it's not complete either.
http://www.jcrystal.com/steffenweber/gallery/Fullerenes/Fullerenes.html