Explore the question in detail with explanation, related questions, and community discussions.
Copper is a transition metal with the atomic number 29. Its electronic configuration is [Ar] 3d¹⁰ 4s¹. Copper commonly exhibits two oxidation states: +1 (Cu⁺) and +2 (Cu²⁺). The magnetic properties of a copper ion depend on the presence of unpaired electrons in its d-orbitals.
A diamagnetic substance has all paired electrons and shows no attraction to an external magnetic field. For copper, the Cu⁺ ion has the configuration [Ar] 3d¹⁰, meaning all the d-orbital electrons are paired. Therefore, Cu⁺ is diamagnetic.
In contrast, Cu²⁺ has the configuration [Ar] 3d⁹, which contains one unpaired electron, making it paramagnetic. Oxidation states like Cu³⁺ and Cu⁴⁺ are rare and usually exist in specific complex compounds. Cu³⁺ has an incomplete d-orbital configuration with unpaired electrons, so it is paramagnetic as well. Cu⁴⁺ is extremely unstable and also contains unpaired electrons in the d-orbitals.
Understanding the relationship between oxidation state, electronic configuration, and magnetism is crucial in inorganic chemistry, especially when predicting the magnetic behavior of transition metal ions. Diamagnetic and paramagnetic properties affect the spectral behavior, chemical reactivity, and bonding characteristics of the metal.
The diamagnetic nature of Cu⁺ is also observed in complex formation, where copper(I) forms colorless and stable complexes because of the fully filled 3d shell. This makes Cu⁺ unique compared to Cu²⁺ in chemical behavior and magnetic properties.
In summary, the oxidation state of copper that is expected to be diamagnetic is Cu⁺, as it has a completely filled 3d¹⁰ configuration.
Discussion
Leave a Comment