Why is Cr3+ inert?
Hello, Why is Cr3+ inert and reacts very slowly? Thanks, LG
How do you determine the oxidation numbers of metal atoms in complexes?
Hello, I'm not sure how to determine the oxidation numbers of metal atoms in complexes, because the main group number doesn't tell me how many electrons it should have, does it? Thanks; LG
Magnetism of TaCl5 and ReCl3?
Hello, Can someone tell me how I can determine the magnetism of these two materials? Can I determine this from their structure? TaCl5 has edge-sharing dimmers and ReCl3 has triller cluster bonds. Is it possible that ReCl3 is diamagnetic due to metal-metal bonding? If so, why? Thanks, best regards
Metal-metal bonds in complexes?
Hello, are all complexes that contain metal-metal bonds diamagnetic? e.g. ZrI3, WCl2….. Thanks for the answer 🙂
Vaska complex trans position?
Hello, can someone answer the question why trans-(Ir(PPh3)2(Cl)(CO)) has this exact structure? I think what they're getting at is that it's trans and not cis… why can't it be cis? Thanks, regards
Is ZrI3 diamagnetic?
Hello, I don't understand the following: It is claimed that ZrI3 contains a d1 ion. How does this come about? Then it is said that it is diamagnetic because "all the spins are paired again", I guess because we have Zr-Zr bonds, right? I suspect it would be more paramagnetic if it contains a d1…
Do only transition metals occupy d orbitals?
Hello, do only transition metals have occupied d-orbitals? If so, why? Thanks, LG
Oxidation state of cobalt?
What is the oxidation state of cobalt in the following transition metal complex: [Co(CO3)(NO)] CO3 is -2, but I don't know what the oxidation number of NO is in this case, since it can act as both NO+ and NO-. Thank you for any help!
Why is Fe^2+ stable?
Isn't it said that transition metals with a half-filled or fully filled d-orbital are more stable? Like the octet rule for the main groups? If the 2 electrons from the 4s orbital are now split off from the Fe, there will still be 1 electron "too much" left in the d-orbital, so that Fe has…
Irregularities in the electron configuration of TM?
In subgroup IV and subgroup IX, for example in chromium or copper, an electron is raised from the s-orbital to the energetically higher d-orbital to create a (half-)full d-orbital. But why doesn't this happen with tungsten? And why does rhodium add an electron from the s orbital to fully occupy only three orbitals?