MHT CET Chemistry Question (2026) — Solution

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The melting point of transition metals depends on the strength of metallic bonding, which is directly proportional to the number of unpaired electrons available for bonding. The electronic configurations of the given elements are: V : [ Ar ] 3d^3 4s^2 (3 unpaired electrons) Cr : [ Ar ] 3d^5 4s^1 (6 unpaired electrons) Mn : [ Ar ] 3d^5 4s^2 (5 unpaired electrons) Fe : [ Ar ] 3d^6 4s^2 (4 unpaired electrons) Chromium (Cr) has the maximum number of unpaired electrons (6), which leads to the strongest metallic bonding among the given elements. Manganese (Mn) has an anomalously low melting point because its stable half-filled 3d^5 configuration restricts the participation of electrons in metallic bonding. Therefore, Cr has the highest melting point. Answer: Cr