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(D) The central metal ion is $Co^{3+}$. The atomic number of $Co$ is $27$,so the electronic configuration of $Co^{3+}$ is $[Ar] 3d^6$.$NH_3$ is a stro

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(D) The central metal ion is $Co^{3+}$. The atomic number of $Co$ is $27$,so the electronic configuration of $Co^{3+}$ is $[Ar] 3d^6$.$NH_3$ is a strong field ligand,which causes pairing of electrons in the $3d$ orbitals.In the presence of $NH_3$,the $6$ electrons in the $3d$ subshell pair up in the first three orbitals ($t_{2g}$ set).Thus,all $3d$ electrons are paired,and there are no unpaired electrons in the $[Co(NH_3)_6]^{3+}$ complex.

$A. sp^3$	$(i). [Co(NH_3)_6]^{3+}$
$B. dsp^2$	$(ii). [Ni(CO)_4]$
$C. sp^3d^2$	$(iii). [Pt(NH_3)_2Cl_2]$
$D. d^2sp^3$	$(iv). [CoF_6]^{3-}$
	$(v). [Fe(CO)_5]$

What is the number of unpaired electrons in $[Co(NH_3)_6]^{3+}$ complex?

Similar Questions

Match the following hybridization in Column $I$ with the corresponding coordination complexes in Column $II$.
$A. sp^3$ $(i). [Co(NH_3)_6]^{3+}$
$B. dsp^2$ $(ii). [Ni(CO)_4]$
$C. sp^3d^2$ $(iii). [Pt(NH_3)_2Cl_2]$
$D. d^2sp^3$ $(iv). [CoF_6]^{3-}$
$(v). [Fe(CO)_5]$

If an iron $(III)$ complex with the formula $[Fe(NH_3)_{x}(CN)_{y}]^{-}$ has no electron in its $e_g$ orbital, then the value of $x+y$ is

The example of $dsp^2$ hybridisation is

The number of unpaired electrons responsible for the paramagnetic nature of the following complex species are respectively $:$
$[Fe(CN)_6]^{3-}, [FeF_6]^{3-}, [CoF_6]^{3-}, [Mn(CN)_6]^{3-}$

In the crystal of $CuSO_4 \cdot 5H_2O$,the copper atom is coordinated by:

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