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(A) The melting points of transition metals depend on the number of unpaired electrons and the strength of metallic bonding. Generally,the melting poi

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$Zn < Cu < Ni < Fe$

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(A) The melting points of transition metals depend on the number of unpaired electrons and the strength of metallic bonding. Generally,the melting point increases as the number of unpaired electrons increases,reaching a maximum in the middle of the series. For the $3d$ series elements: $Zn$ $([Ar] 3d^{10} 4s^2)$ has no unpaired electrons,resulting in weak metallic bonding and a low melting point $(419 \ ^\circ C)$. $Cu$ $([Ar] 3d^{10} 4s^1)$ has one unpaired electron,resulting in a relatively low melting point $(1083 \ ^\circ C)$. $Ni$ $([Ar] 3d^8 4s^2)$ has two unpaired electrons $(1455 \ ^\circ C)$. $Fe$ $([Ar] 3d^6 4s^2)$ has four unpaired electrons,leading to stronger metallic bonding and a higher melting point $(1538 \ ^\circ C)$. Therefore,the correct order of increasing melting point is $Zn < Cu < Ni < Fe$.

Which of the following is arranged in order of increasing melting point?

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