RyanJ Posted March 16, 2006 Share Posted March 16, 2006 Hi all, Is it possible to have more then 3 bonds, I have heard of 1, 2, and 3 but I have never heard of a bond number greater then that… does anyone know if its possible and have any resource links for more information? (Maybe explain a little about them too if possible). Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
Tartaglia Posted March 16, 2006 Share Posted March 16, 2006 Yes quadruple metal-metal bonds are known. They usually involve one of sigma symmetry (ie no node), 2 of pi symmetry (ie one node) and one of delta symmetry (two nodes). The last is face on face d orbital overlap Link to comment Share on other sites More sharing options...
RyanJ Posted March 16, 2006 Author Share Posted March 16, 2006 Yes quadruple metal-metal bonds are known. They usually involve one of sigma symmetry (ie no node), 2 of pi symmetry (ie one node) and one of delta symmetry (two nodes). The last is face on face d orbital overlap Ah, so it is possible! Do you have any article or resource links that have some infromation about them, the Wikipedia entry is less then impressive right now. Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
Tartaglia Posted March 16, 2006 Share Posted March 16, 2006 http://www.pnas.org/cgi/content/abstract/81/8/2592 http://www.tntech.edu/chemistry/Inorganic/Chem4110/Student/08%20MMQBShow.ppt http://en.wikipedia.org/wiki/Covalent_bond Look well down the page of the last Link to comment Share on other sites More sharing options...
RyanJ Posted March 16, 2006 Author Share Posted March 16, 2006 http://www.pnas.org/cgi/content/abstract/81/8/2592http://www.tntech.edu/chemistry/Inorganic/Chem4110/Student/08%20MMQBShow.ppt http://en.wikipedia.org/wiki/Covalent_bond Look well down the page of the last Thanks for the links, I will read them when I get home Thanks again, Ryan Jones Link to comment Share on other sites More sharing options...
Borek Posted March 16, 2006 Share Posted March 16, 2006 http://en.wikipedia.org/wiki/Quintuple_Bond http://pubs.acs.org/cen/news/83/i39/8339notw1.html Best, Borek -- Chemical calculators at www.chembuddy.com equation balancer and stoichiometry calculator www.pH-meter.info Link to comment Share on other sites More sharing options...
ecoli Posted March 17, 2006 Share Posted March 17, 2006 I don't think it's possible in terms of Lewis structures, though. Link to comment Share on other sites More sharing options...
karicha9 Posted March 17, 2006 Share Posted March 17, 2006 I don't think it's possible in terms of Lewis structures, though. It is more than possible if you remember the fact that the bonds will be between two metals. You are right in one regard, though. Lewis structures are poor determinants of structure for anything beyond simple compounds. Link to comment Share on other sites More sharing options...
Mercurial Posted March 17, 2006 Share Posted March 17, 2006 I have read that someone has shown the existence via IR spec of a CH5(+) ion. Is it interesting? sure... is it useful at all? probably not.. and now I just realized that I completely misread your question. Oh well, so my foolish reply stays, hope this is interesting as well. Link to comment Share on other sites More sharing options...
Tartaglia Posted March 17, 2006 Share Posted March 17, 2006 The first metal metal quadruple bond was made by F. A. Cotton in the mid 1960's. He also use to claim credit for the first metal-metal covalent bond too, but that was published in an obscure Russian journal. This didn't however stop him from doing this for years until my PhD supervisor, who still has a "God like" status in the chemistry world told him not to. Link to comment Share on other sites More sharing options...
RyanJ Posted March 18, 2006 Author Share Posted March 18, 2006 Interesting stuff... these bonds can't be stable though can they, I found a reference On Wikipedia) that said there were 7 bonds found but was only stable near absolute zero. Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
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