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Question

Select the coloured compound amongst the following:


(Atomic no. Ti=22,Cr=24,Cu=29,Zn=30)

A
TiCl4
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B
CrCl3
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C
ZnCl2
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D
CuCl
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Solution

The correct option is A CrCl3
TiCl4
Electronic configuration of Ti is [Ar]3d24s2.
For Ti4+ - [Ar]3d04s0
Since no electron is present, so it is colourless.

CrCl3
Electronic configuration of Cr is [Ar]3d54s1
For Cr3+ - [Ar]3d34s0.
Since there is a presence of d-electrons, so it is coloured. There is partially filled d-orbital so due to d-d transition colour is imparted to this compound.

ZnCl2
Electronic configuration of Zn - [Ar]3d104s2
For Zn2+ - [Ar]3d104s0
Because of fully filled d orbital, the compound is colourless.

CuCl
Electronic configuration of Cu+ is 3d104s0
Due to fully filled d-orbital, it is colourless.

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