Manganate and permanganate ions adopt tetrahedral geometry, with p-bonding occurring through the overlap of p orbitals of oxygen with d orbitals of manganese. The paramagnetism of green manganate arises from one unpaired electron, while permanganate is diamagnetic due to the absence of unpaired electrons.
Describe the molecular geometry of manganate and permanganate ions, and what orbital interactions contribute to their magnetic properties?
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The manganate ion (MnO₄²⁻) has a tetrahedral molecular geometry, where manganese (Mn) is surrounded by four oxygen (O) atoms. Permanganate ion (MnO₄⁻), on the other hand, has a tetrahedral geometry with a slightly distorted structure due to its negative charge. The magnetic properties of these ions result from the presence of unpaired electrons in the manganese 3d orbitals. The orbital interactions, particularly the incomplete occupation of the 3d orbitals, contribute to paramagnetism. Unpaired electrons align with an external magnetic field, enhancing magnetic susceptibility and highlighting the magnetic behavior of manganese compounds in different oxidation states.