[Ti(H2O)6]Cl3 is an octahedral violet colour complex; the violet colour of this
complex is due to d-d transition of a single (d1) electron from t2g lower level to eg higher
level by absorbing corresponding energy of yellow green region of light and
emitted energy corresponding to violet region and hence appears violet in
colour. But on heating it is dehydrated and water molecules (ligand)
removed so in absence of ligand splitting of D orbitals does not occur hence it
becomes colourless.
Similarly anhydrous CuSO4 is white ,
but CuSO4 .5H2O is Blue in Colour.
Related Question:
Related Question:
Which of the
Complex of the following pairs has the highest value of CFSE?
Colour of Complexes due to charge transfer:
Why violet colour of [Ti(H2O)6]Cl3 disapear (colourless) on heating heating ?
Why [Ni(CN)4]-2 is colourless while [Ni(H2O)4]-2 although both have +2 oxidation state and 3d*8 configuration ?
Why [FeF6]3– is colourless whereas [CoF6]3– is coloured ?
Why Fe(CO)5 is colourless while Fe(bipy)(CO)3 is intensely purple in colour ?
Why all the tetrahedral Complexes are high spin Complexes ?
Colour of Complexes due to charge transfer:
Why violet colour of [Ti(H2O)6]Cl3 disapear (colourless) on heating heating ?
Why [Ni(CN)4]-2 is colourless while [Ni(H2O)4]-2 although both have +2 oxidation state and 3d*8 configuration ?
Why [FeF6]3– is colourless whereas [CoF6]3– is coloured ?
Why Fe(CO)5 is colourless while Fe(bipy)(CO)3 is intensely purple in colour ?
Why all the tetrahedral Complexes are high spin Complexes ?
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