explain why Cu+ ion is not coloured??plz explain in detail
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Transition metals are metals which has partially filled d-orbitals.
In Cu+, configuration is [Ar]4s3d10. So in this case, d-orbital is completely filled, and thus has no unpaired electrons. Thus there are no chances of electron transitions.
For coloring to takes place, there needs to be resonance or unpaired electrons which lacks in Cu+.
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In Cu+, configuration is [Ar]4s3d10. So in this case, d-orbital is completely filled, and thus has no unpaired electrons. Thus there are no chances of electron transitions.
For coloring to takes place, there needs to be resonance or unpaired electrons which lacks in Cu+.
*if this helps, please mark as Brainliest*
Answered by
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D block elements of periodic table are called as Transition
elements. -->Transition elements have partially filled d orbitals.
-->The colour for the elements of D block is due to transition of electrons which is called as d -Transition for which presence of partially filled d electrons is must.
Copper Cu , has 29 electrons.
so electronic configuration will be 1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰
but in case of Cu+ ion, 28 electrons so:
electronic configuration will be 1s²2s²2p⁶3s²3p⁶3d¹⁰
Cu+ion will loose its 4s¹ electron, and as it has filled 3d¹⁰ orbital,therefore no transition and hence cu+ ion will not have any colour.
-->The colour for the elements of D block is due to transition of electrons which is called as d -Transition for which presence of partially filled d electrons is must.
Copper Cu , has 29 electrons.
so electronic configuration will be 1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰
but in case of Cu+ ion, 28 electrons so:
electronic configuration will be 1s²2s²2p⁶3s²3p⁶3d¹⁰
Cu+ion will loose its 4s¹ electron, and as it has filled 3d¹⁰ orbital,therefore no transition and hence cu+ ion will not have any colour.
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