Addition of excess aqueous ammonia to a pink coloured aqueous solution of MCl2.6H2O(X) and NH4Cl gives an octahedral complex Y in the presence of air. In aqueous solution, complex Y behaves as 1:3 electrolyte. The reaction of X with excess HCl at room temperature results in the formation of a blue coloured complex Z. The calculated spin only magnetic moment of X and Z is 3.87 B.M., whereas it is zero for complex Y. Among the following options, which statement is incorrect?

Question

Addition of excess aqueous ammonia to a pink coloured aqueous solution of MCl2.6H2O(X) and NH4Cl gives an octahedral complex Y in the presence of air. In aqueous solution, complex Y behaves as 1:3 electrolyte. The reaction of X with excess HCl at room temperature results in the formation of a blue coloured complex Z. The calculated spin only magnetic moment of X and Z is 3.87 B.M., whereas it is zero for complex Y. Among the following options, which statement is incorrect? (A) The hybridization of the central metal ion in Y is d2sp3 (B) Addition of solver nitrate to Y gives only two equivalents of silver chloride (C) When X and Z are in equilibrium at 0°C, the colour of the solution is pink (D) Z is a tetrahedral complex

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="Solution" src="https://cdn.tardigrade.in/q/nta/c-ezobmvue41v1.png" /> X and Z are in equilibrium at 0oC , equilibrium is shifted towards X, making colour of solution pink.

The hybridization of the central metal ion in Y is $d^{2} s p^{3}$

Addition of solver nitrate to Y gives only two equivalents of silver chloride

When X and Z are in equilibrium at 0°C, the colour of the solution is pink

Z is a tetrahedral complex

X and Z are in equilibrium at $0^{o} C$ , equilibrium is shifted towards X, making colour of solution pink.