Coordination compounds


> 
> Which of the following complex is diamagnetic? 
> 
> 
> 1. $\ce{[Cr(Cl3)(NMe3)]}$
> 2. $\ce{[Co(EDTA)]-}$
> 3. $\ce{[Cu(CN)(NO2)(NH3)(Py)]}$
> 4. $\ce{[Fe(NH3)6]^2+}$
> 
> 
> 


For (4) I found that since $\ce{NH3}$ is a weak field ligand it cannot pair the electrons of $\ce{Fe^2+}$. Thus, (4) will remain paramagnetic.


But, for the rest of the options, I'm unable to clearly understand if they are paramagnetic or diamagnetic. I need help here.




1) Cr3+ has 3 electrons in 3d orbital. Obviously, it is a tetrahedral splitting, so configuration will be eg2 t2g1 which shows it is paramagnetic.


2) Here you need to know that for Co3+ all complexes are low spin except [CoF6]3- and [Co(H2O)3F3]. So, the complex given will be low spin with all 6 electrons paired & thus it will be diamagnetic.


3) Cu2+ has 3d9 configuration. So, it can never be diamagnetic as one electron will always be unpaired.


4) What you thought is right. But I would like to add that NH3 doesn't always behave like a weak field or strong field ligand. It depends on many factors which can't be explained using CFT.


Hope it helps!


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