Question

# In $$[Co(CN)_6]^{4-}$$ and  $$[Co(CN)_6]^{3-}$$:

A
one is paramagnetic
B
second is diamagnetic
C
one is diamagnetic and second is paramagnetic
D
both A and B

Solution

## The correct option is D both A and BWe know that,$$Co^{+2}$$ ion is present in $$[Co(CN)_{6}]^{-4}$$ while $$Co^{+3}$$ ion is present in $$[Co(CN)_{6}]^{-3}$$.The attached image shows the Electronic Configuration of $$Co^{+2}$$ and $$Co^{+3}$$ ions in the ground state.While in the excited state, and undergoing hybridisation, $$CN^{-}$$ being a strong field ligand forces the inner d electrons to pair up.Due to this, $$Co^{+2}$$ in $$[Co(CN)_{6}]^{-4}$$ has one unpaired electron(i.e. it is paramagnetic) whereas, $$Co^{+3}$$ in $$[Co(CN)_{6}]^{-3}$$ has no unpaired electron(i.e. it is diamagnetic). Hence the given statement is True. So we write $$1$$.ChemistryNCERTStandard XII

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