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The melting points of transition metals rise to a maximum at d⁵ configuration. This is because:
AHalf-filled orbitals are unstable
BThe metals have low density
CMaximum number of unpaired electrons (d⁵, all 5 unpaired) maximises interatomic metallic bonding via overlap
Dd-orbitals do not participate in bonding
Answer & Solution
Correct answer: C. Maximum number of unpaired electrons (d⁵, all 5 unpaired) maximises interatomic metallic bonding via overlap
Atomisation enthalpy and m.p. peak near d⁵ because **5 unpaired electrons per atom give maximum interatomic bonding** (besides ns electrons). Cr and Mo show high m.p. while Mn dips due to its half-filled stability (electrons unavailable for bonding).
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