Talk:Vanadium(III) chloride
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Many vanadium(III) compounds are paramagnetic, but there are also numerous compounds of V(III) that are not. A general rule is, that vanadium compounds with 14 or less valence electrons are paramagnetic (though there are examples of V(III) compounds with (formally) only 10 valence electrons that are diamagnetic: e.g. the dinitrogen adduct of vanadium(III) trialkyls [V(CH2SiMe3)3]2[N2]). Vanadium compounds with 16 valence electrons often pair the electrons, leaving one empty orbital of high energy, and compounds with 18 electrons practically have no choice but to pair the electrons.
[edit] Exactly!
Very interesting point. Yes the traditional V(III) coordination cmpds are all triplet ground states not matter how you look at them. Of course one could wonder if your cmpd is not an imide, i.e. R3V=N-N=VR3. But the point would be worth noting. --Smokefoot 05:20, 1 May 2006 (UTC)
There are crystal structures of these compounds available, the only thing I know from personal experience, is that it is quite easy to remove the dinitrogen (by vacuum), but there is more know about the compound. Maybe interesting for a seperate article (but under which name?).Dirk Beetstra 11:30, 1 May 2006 (UTC)
