explain way cu+ ion is not coloured
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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.
Answered by
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Cu+ ion loses its 4s electrons and gets filled up with 3d orbital which does not have any transition, this is the reason no color is shown. Color is always shown because of the transition between d-electrons.
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