Respuesta :
Electronic configuration of Cu is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d9 ([Ar] 4s2, 3d9), whereas for Cu2+ is [Ar],[tex]3d^{9}[/tex] and it has 1 unpaired electron.
For the Cu2+ ion we remove a total of two electrons (one from the 4s1 and one form the 3d10) leaving us with[tex]1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{9}[/tex].
How to write an electronic configuration?
1. Identify the given element and its atomic number from the periodic table.
2. Write the electron configuration by the energy level and the type of orbital first, then the number of electrons present in the orbital as superscript.
The easiest way to write the electronic configuration for any element is by using a diagonal rule for electron filling order in the different subshells according to the Aufbau principle.
The 3 rules for writing the electron configuration in the orbital box diagram are – the Aufbau rule, the Pauli-exclusion rule, and Hund's Rule.
To learn more about Cu2+ , refer
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