Why do the transition element exhibit higher enthalpies of atomisation
Hello Riya,
Transition elements exhibit higher enthalpies of atomisation due to the following reasons:
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Strong Metallic Bonding:
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Transition metals have more unpaired d-electrons, leading to stronger interatomic interactions.
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This results in a higher amount of energy required to break the metallic bonds.
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Transition metals have more unpaired d-electrons, leading to stronger interatomic interactions.
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Partially Filled d-Orbitals: The (n-1)d and ns electrons participate in bonding, increasing metallic bond strength.
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High Number of Unpaired Electrons: Elements in the middle of the series (like Fe, Co, Ni) have maximum unpaired d-electrons, leading to strong bonding and higher enthalpy of atomisation.
Thus, transition metals need more energy to separate atoms, leading to high enthalpies of atomisation compared to s- and p-block elements.
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