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(B) The thermodynamic stability of a coordination complex is primarily determined by the charge density of the central metal ion. Higher charge on the

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$[Co(NH_3)_6]^{3+} > [Cu(CN)_4]^{2-} > [Ag(CN)_2]^{-}$

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(B) The thermodynamic stability of a coordination complex is primarily determined by the charge density of the central metal ion. Higher charge on the central metal ion leads to stronger electrostatic attraction with the ligands,resulting in higher stability. The oxidation states of the central metal ions in the given complexes are: $Co$ in $[Co(NH_3)_6]^{3+}$ is $+3$. $Cu$ in $[Cu(CN)_4]^{2-}$ is $+2$. $Ag$ in $[Ag(CN)_2]^{-}$ is $+1$. Therefore,the order of stability follows the order of oxidation states: $[Co(NH_3)_6]^{3+} > [Cu(CN)_4]^{2-} > [Ag(CN)_2]^{-}$.

Which among the following is a correct decreasing order of thermodynamic stability of the complexes?

Similar Questions

An aqueous solution of $FeSO_4$ gives tests for both $Fe^{2+}$ and $SO_4^{2-}$ ions,but after the addition of an excess of $KCN$,the solution ceases to give a test for $Fe^{2+}$. This is due to the formation of:

$CuSO_4$ solution reacts with excess of $KCN$ solution to form:

Explain the chelating effect or chelation.

Assertion : The $[Ni(en)_3]Cl_2$ ($en =$ ethylenediamine) has lower stability than $[Ni(NH_3)_6]Cl_2$.
Reason : In $[Ni(en)_3]Cl_2$,the geometry of $Ni$ is trigonal bipyramidal.

The molar ionic conductances of the octahedral complexes:
$(I)$ $PtCl_4 \cdot 5NH_3$
$(II)$ $PtCl_4 \cdot 4NH_3$
$(III)$ $PtCl_4 \cdot 3NH_3$
$(IV)$ $PtCl_4 \cdot 2NH_3$
Follow the order $-$

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