zinc to positive salts are white and cu +2 are coloured why?
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The salts gets colored due to transition metals and the difference in energy band of eg to t2g in partially filled d- orbitals..
Zinc has fully filled d-orbitals even in its excited state. Thus, there is no such transition and even the the eg and t2g are filled so they are white.
Whereas in copper, it dont have fully filled d-orbitals even in its excited state it is partially filled resulting to such an energy difference and thus is transition metal. It's bond thus are colorful.
Hope I helped u with.
Zinc has fully filled d-orbitals even in its excited state. Thus, there is no such transition and even the the eg and t2g are filled so they are white.
Whereas in copper, it dont have fully filled d-orbitals even in its excited state it is partially filled resulting to such an energy difference and thus is transition metal. It's bond thus are colorful.
Hope I helped u with.
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Zn has electronic configuration = 3d104s2
Zn2+ = 3d10
Cu = 3d54s1
Cu2+ = 3d4
In case of Zn fully filled d orbital is present therefore no d-d transition can be possible in this case and it is colorless.
In case of copper because of d-d transition electrons emits light in the visible range and hence they are colored compounds.
Zn2+ = 3d10
Cu = 3d54s1
Cu2+ = 3d4
In case of Zn fully filled d orbital is present therefore no d-d transition can be possible in this case and it is colorless.
In case of copper because of d-d transition electrons emits light in the visible range and hence they are colored compounds.
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