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(C) The magnetic moment (spin only) is given by $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.$1. [CoCl_4]^{2-}: Co^{

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$[Cr(H_2O)_6]^{2+}, [Fe(H_2O)_6]^{2+}$

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(C) The magnetic moment (spin only) is given by $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.$1. [CoCl_4]^{2-}: Co^{2+} (d^7)$ is a tetrahedral complex. The configuration is $e^4 t_2^3$,so $n = 3$.$2. [Fe(H_2O)_6]^{2+}: Fe^{2+} (d^6)$ is an octahedral complex. The configuration is $t_{2g}^4 e_g^2$,so $n = 4$.$3. [Mn(H_2O)_6]^{2+}: Mn^{2+} (d^5)$ is an octahedral complex. The configuration is $t_{2g}^3 e_g^2$,so $n = 5$.$4. [Cr(H_2O)_6]^{2+}: Cr^{2+} (d^4)$ is an octahedral complex. The configuration is $t_{2g}^3 e_g^1$,so $n = 4$.Comparing the number of unpaired electrons,both $[Fe(H_2O)_6]^{2+}$ and $[Cr(H_2O)_6]^{2+}$ have $n = 4$,thus they have the same magnetic moment.

The pair in which both the species have the same magnetic moment (spin only) is

Similar Questions

The metal complex that is diamagnetic is (Atomic number: $Fe = 26, Cu = 29$)

Among $(i)$ $[Cr(en)_{3}]^{3+}$,$(ii)$ $trans-[Cr(en)_{2}Cl_{2}]^{+}$,$(iii)$ $cis-[Cr(en)_{2}Cl_{2}]^{+}$,$(iv)$ $[Co(NH_{3})_{4}Cl_{2}]^{+}$,the optically active complexes are:

The two complexes given below are $............$.

The magnetic moment of $[Fe(H_2O)_6]^{3+}$ is $5.92 \ BM$,whereas the magnetic moment of $[Fe(CN)_6]^{3-}$ is $1.74 \ BM$. Explain why.

For a $t_{2g}^6 e_g^2$ system,the value of the magnetic moment $(\mu)$ is equal to ..... $B.M.$

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