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(B) The magnetic moment is given as $0 \, B.M.$,which implies that there are no unpaired electrons in the titanium ion. For an octahedral complex,the

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$[Ti(H_2O)_6]Cl_4$

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(B) The magnetic moment is given as $0 \, B.M.$,which implies that there are no unpaired electrons in the titanium ion. For an octahedral complex,the coordination number is $6$. In the complex $[Ti(H_2O)_6]Cl_4$,the oxidation state of $Ti$ is calculated as $x + 6(0) = +4$,so $Ti$ is in the $+4$ oxidation state. The electronic configuration of $Ti$ $(Z=22)$ is $[Ar] 3d^2 4s^2$. For $Ti^{4+}$,the configuration is $[Ar] 3d^0$,which has $0$ unpaired electrons. Therefore,the magnetic moment is $0 \, B.M.$

An aqueous solution of titanium chloride,when subjected to magnetic measurement,measured zero magnetic moment. Assuming the octahedral complex in aqueous solution,the formula of the complex is

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