Why is the first ionization enthalpy of zn high?
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It is because the shell is complete. Zinc's electronic configuration is [Ar]3d10 4s2 which is a complete configuration for a transition metal. The next element in the same period is Ga, which starts filling 4p orbitals ([Ar]3d10 4s2 4p1). The Zinc's electronic configuration causes a sort of special stability because of the filled electronic states. Also the effective nuclear charge is greater than Cu's, so it's more difficult to ionize Zn.
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