Which one of the following complexes is colored? 1- [Ti(H20)2(OX)2Br21" 2- [Ti(H20)614+ 3- [TI(NH3)2(H20)2Br21+2

Question

Question

Answer 1

Answer #1

The color is due to the d-d transition.

Now we know valence electron configuration of Ti is 3d2 4s2

So out of three choices given ,check out the charge on titanium and then the electrons present in d orbital for d-d transition.

1) H2O has zero oxidation state, ox has -2 and Br is -1 , So Ti would have x-4-2= -1and hence x=+3

Ti (+4 ) would have one electron in d orbital therefore d-d transition is possible and complex is colored.

2) in this case again Ti is +4 t and has zero electron in d orbital, no d-d transition and therefore no colour

3)NH2 has zero oxidation state, H2O also has zero and Br has -1 therefore we solve for Ti as shown

x-2=-2 and x=+4 hence no colour

Answer 2

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