In first transition series, the melting point of Mn is low because

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due to d¹⁰configuration, metallic bonds are strong

due to d⁷configuration, metallic bonds are weak

due to d⁵ configuration, metallic bonds are weak

None of these

answer is C.

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Detailed Solution

Due to d⁵ configuration, Mn has exactly half filled d-orbitals. As a result the electronic configuration is stable means 3d electrons are more tightly held by the nucleus and this reduces the delocalization of electrons resulting in weaker metallic bonding.

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