Given below are two statements:Statement I: C | vedclass

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(A) For $[Mn(H_2O)_6]^{2+}$, the configuration is $d^5$ with a weak field ligand $(H_2O)$, resulting in $t_{2g}^3 e_g^2$. The $CFSE$ is $(3 	imes -0.

Vedclass · Accepted Answer

Both Statement $I$ and Statement $II$ are true

Vedclass · Answer

(A) For $[Mn(H_2O)_6]^{2+}$, the configuration is $d^5$ with a weak field ligand $(H_2O)$, resulting in $t_{2g}^3 e_g^2$. The $CFSE$ is $(3 	imes -0.4 \Delta_o) + (2 	imes 0.6 \Delta_o) = 0 \Delta_o$.For $[Cr(H_2O)_6]^{2+}$, the configuration is $d^4$ with a weak field ligand $(H_2O)$, resulting in $t_{2g}^3 e_g^1$. The $CFSE$ is $(3 	imes -0.4 \Delta_o) + (1 	imes 0.6 \Delta_o) = -0.6 \Delta_o$. Since $|-0.6| > 0$, Statement $I$ is true.For potassium ferricyanide, $K_3[Fe(CN)_6]$, the iron is in $+3$ oxidation state $(d^5)$. $CN^-$ is a strong field ligand, leading to $t_{2g}^5 e_g^0$ with $1$ unpaired electron. $\mu = \sqrt{1(1+2)} = \sqrt{3} \approx 1.73 \ B.M.$For sodium ferrocyanide, $Na_4[Fe(CN)_6]$, the iron is in $+2$ oxidation state $(d^6)$. $CN^-$ is a strong field ligand, leading to $t_{2g}^6 e_g^0$ with $0$ unpaired electrons. $\mu = 0 \ B.M.$Since $\sqrt{3} > 0$, Statement $II$ is true.

List-$I$	List-$II$
$A$. Ziegler-Natta	$i$. $Fe_4[Fe(CN)_6]_3$
$B$. Brown ring complex	$ii$. $[Fe(H_2O)_5NO]SO_4$
$C$. Prussian Blue	$iii$. $Al(C_2H_5)_3 + TiCl_4$
$D$. Turnbull Blue	$iv$. $Fe_3[Fe(CN)_6]_2$

List-$I$ (Complex)	List-$II$ (Color)
$A. [Ni(en)_3]^{2+}$	$I. \text{Green}$
$B. [Ni(H_2O)_4(en)]^{2+}$	$II. \text{Blue}$
$C. [Ni(H_2O)_6]^{2+}$	$III. \text{Pale blue}$
$D. [Ni(H_2O)_2(en)_2]^{2+}$	$IV. \text{Violet}$

Similar Questions

Which of the following compounds is not colored yellow?

Match List-$I$ with List-$II$ and select the correct code:

List-$I$ List-$II$

$A$. Ziegler-Natta $i$. $Fe_4[Fe(CN)_6]_3$

$B$. Brown ring complex $ii$. $[Fe(H_2O)_5NO]SO_4$

$C$. Prussian Blue $iii$. $Al(C_2H_5)_3 + TiCl_4$

$D$. Turnbull Blue $iv$. $Fe_3[Fe(CN)_6]_2$

Correct code is:

Match the following complexes in List-$I$ with their colors in List-$II$:
List-$I$ (Complex) List-$II$ (Color)
$A. [Ni(en)_3]^{2+}$ $I. \text{Green}$
$B. [Ni(H_2O)_4(en)]^{2+}$ $II. \text{Blue}$
$C. [Ni(H_2O)_6]^{2+}$ $III. \text{Pale blue}$
$D. [Ni(H_2O)_2(en)_2]^{2+}$ $IV. \text{Violet}$

The complex ion $[Co(en)_2Br_2]^+$ has two optical isomers. Their correct configurations are:

Which of the following orders is not correct?

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