That reminds me, has anyone attempted a ligand-bonded polymer?
I'm thinking something like, oh, (HOOCCH2)3C-(CH2)n-C(CH2COOH)3, with n maybe 2 to 8. Start with the hexabasic salt (so it's all ionized), then add
something like FeCl3 (or other transition metal salt) to the solution: it should coordinate strongly. Now, the ends will loop around and form
monomers, but those will remain soluble (having a -3 charge), whereas the polymer is charge neutral and probably not all that soluble.
I wonder just how strong the ligand bonds are. I mean, we've got ionic bonds (otherwise known as crystals), covalent bonds both nonpolar
(polyalkenes, etc.) and polar (polyesters, etc.), and pi bonds (cumulenes, polyacetylene, etc.). Why not d orbitals too?
intrigued by this as well .. wanted to try an organic ligand and been trying to make a polystyrene rendition but no joy so will step back and try
another poly- maybe butylamine.. what do you think?yan123 - 7-11-2007 at 04:40
Prof. Makoto Fujita has done lots of work about Molecular Self-Assembly via Coordination.vulture - 8-11-2007 at 01:33
This is basically the basis of supramoleculair chemistry and self-assembly.
Crown ethers are a nice example, that's how you can dissolve KMnO4 in benzene.12AX7 - 8-11-2007 at 12:57
Yeah, crowns and cryptands -- and carcerands -- are cool stuff. I've browsed some of Wikipedia's macrocylic and supermolecular chemistry pages, but
I've never seen scorpionates, neet.
Timchemrox - 8-11-2007 at 21:20
Quote:
Prof. Makoto Fujita has done lots of work about Molecular Self-Assembly via Coordination.
Yes-thank you, and he's willing to correspond via email re specific papers
