Copper is the first element of Group IB of the periodic table and displays four oxidation states: Cu(O), 2025

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But copper has a more stable +2 oxidation state called cupric. This is because the d orbital will be half filled in +2 oxidation state that results in high negative enthalpy of hydration that makes it more stable in forming aqueous solutions. So, oxidation states of copper are +1 and +2.
Explanation: Its an energy balance. Donating additional valence electrons to make higher oxidation states costs energy. This has to be made up with the electron affinity of the nonnetal and greater electrostatic attraction to negative ions and dipoles.
The oxidation number of metallic copper is zero. In its compounds, the most common oxidation number of Cu is +2. Less common is +1.
Potassium (K) is an alkali metal, underneath sodium and above rubidium, and the first element of period 4.
Copper, nickel, and zinc do not generally show oxidation states greater than +2 due to their high third ionization energies and the stability associated with their electronic configurations. The increased effective nuclear charge after losing two electrons makes it energetically unfavorable to lose a third electron.
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Copper is also known to exist in the +3 oxidation state, which is believed to be involved in some biological electron-transfer reactions. (a) Would you expect this oxidation state of copper to be stable? Explain. (b) Name the compound K 3 CuF 6 and predict the geometry of the complex ion and its magnetic properties.

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