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  • Why first ionisation enthalpy of {Cr} is lower than that of {Zn}?

Why first ionisation enthalpy of \text {Cr} is lower than that of \text {Zn}?

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Given below is the electronic configuration of chromium and zinc
\text {Cr (24)}=\text {[Ar]}\; \text {3d}^{5}\text {4s}^{2}                  \text {Zn (30)}=\text {[Ar]}\; \text {3d}^{10}\text {4s}^{2}
\text {Cr} has half-filled d orbital which is very stable and results in lower Ionization enthalpy. Similarly, the value for \text {Zn} is higher because its electron comes out from completely filled 4s orbital.

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