* Copper's electronic configuration: Copper has an atomic number of 29, meaning it has 29 electrons. Its electronic configuration is [Ar] 3d¹⁰ 4s¹. This means it has one electron in its outermost shell (4s).
* Losing electrons: When copper loses two electrons, it loses the one electron from its 4s orbital and one electron from its 3d orbital.
* Formation of Cu²⁺: The loss of two electrons leaves copper with a +2 charge, resulting in the copper(II) ion (Cu²⁺). This ion is now stable with a full 3d subshell.
Note: Copper can also lose one electron to form the copper(I) ion (Cu⁺), but this is less common.
