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One of manganese compounds is Mn3(PO4)2 : (1) Write the electron configuration of manganese ion in this compound. (2) is oxidizing manganese ion in this compound easy or difficult? Explain.
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Here's the breakdown:
(1) Electron Configuration of Manganese Ion:
Manganese's Atomic Number: Manganese (Mn) has an atomic number of 25, meaning it has 25 electrons in its neutral state.
Manganese Ion in Mn3(PO4)2: The manganese ion in this compound is Mn²⁺. To form a +2 charge, manganese loses two electrons.
Electron Configuration of Mn²⁺: The electron configuration of a neutral manganese atom is [Ar] 3d⁵ 4s². After losing two electrons, the electron configuration of Mn²⁺ becomes [Ar] 3d⁵.
(2) Oxidizing Mn²⁺:
Oxidation State: In Mn3(PO4)2, manganese is already in a +2 oxidation state.
Ease of Oxidation: Oxidizing Mn²⁺ to a higher oxidation state is relatively difficult because the d orbitals are half-filled in Mn²⁺. Half-filled d orbitals are relatively stable due to Hund's rule, which states that electrons prefer to occupy separate orbitals with the same spin before pairing up in the same orbital. To further oxidize Mn²⁺, you'd need to overcome this stability.
In summary: Mn²⁺ in Mn3(PO4)2 has a relatively stable half-filled d orbital configuration, making it less likely to be oxidized further.
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