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Question

Which one of the following complexes will most likely absorb visible light?
[Atomic numbers: $$Sc=21, Ti=22, V=23, Zn=30$$]


A
[Sc(H2O)6]3+
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B
[Ti(NH3)6]4+
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C
[V(NH3)6]2+
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D
[Zn(NH3)6]2+
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Solution

The correct option is A $$[V(NH_3)_6]^{2+}$$
For the absorption of light, transition metal should have electrons in d orbital. When we look at the complexes in the options,
A) $$Sc^{3+}$$ - no electrons in d orbital. So, $$Sc^{3+}$$ doesn't absorb light.
B) $$Ti^{4+}$$ - no electrons in d orbital. So, $$Ti^{4+}$$ doesn't absorb light.
C) $$V^{2+}$$ - three electrons in d orbital. So, $$V^{2+}$$ absorbs light. 
D) $$Zn^{2+}$$ - no empty d orbitals, electrons in d orbitals are filled. So, $$Zn^{2+}$$ doesn't absorb light, so transitions cannot happen.

Chemistry

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