When [Ti(H_2O)_6]Cl_3 is heated at 250^{circ} | vedclass

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(D) The complex $[Ti(H_2O)_6]Cl_3$ contains $Ti^{3+}$ ion which has a $3d^1$ electronic configuration.Due to the presence of one unpaired electron,it

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violet to colourless

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(D) The complex $[Ti(H_2O)_6]Cl_3$ contains $Ti^{3+}$ ion which has a $3d^1$ electronic configuration.Due to the presence of one unpaired electron,it undergoes $d-d$ transition and exhibits a violet colour.Upon heating at $250^{\circ} C$ in the presence of oxygen,it decomposes to form $TiO_2$ where titanium is in the $+4$ oxidation state $(Ti^{4+} : 3d^0)$.Since $Ti^{4+}$ has no unpaired electrons,it does not undergo $d-d$ transition and is colourless.Therefore,the colour change is from violet to colourless.

Column-$I$ (Coordination compound)	Column-$II$ (Central metal atom)
$(a)$ Chlorophyll	$(p)$ Rhodium
$(b)$ Blood pigment	$(q)$ Cobalt
$(c)$ Wilkinson catalyst	$(r)$ Calcium
$(d)$ Vitamin $B_{12}$	$(s)$ Iron
	$(t)$ Magnesium

When $[Ti(H_2O)_6]Cl_3$ is heated at $250^{\circ} C$,the change in colour is from

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