• question_answer The hybridisation and magnetic moment of complex $[Cr{{({{H}_{2}}O)}_{6}}]\,C{{l}_{2}}$ is A) $s{{p}^{3}}{{d}^{2}},4.89\,BM$ B) ${{d}^{2}}s{{p}^{3}},4.89\,BM$ C) $ds{{p}^{2}},5.89\,BM$ D) $s{{p}^{3}}{{d}^{2}},3.39\,BM$

Correct Answer: A

Solution :

 $Cr$is in $+2$ oxidation state in$[Cr{{({{H}_{2}}O)}_{6}}C{{l}_{2}}$. The electronic configuration of $C{{r}^{2+}}$ is $3{{d}^{4}}4{{s}^{0}}$ As ${{H}_{2}}O$is a weak field ligand, so pairing will not occur.
 Thus, the hybridisation of ${{\left[ Cr\left( {{H}_{2}}O \right)6 \right]}^{2+}}$ $s{{p}^{3}}{{d}^{2}}$ Magnetic moment $=\sqrt{n\left( n+2 \right)}$ For this complex, $n=4$ $\mu =\sqrt{4\left( 4+2 \right)}$ $=\sqrt{24}$ $=4.89BM$

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