why the Second ionisation enthalpy for Cr chromium and Cu copper is usually high ? explain

Let’s see the detail behind this

1. In case of Chromium

In case of Chromium, its configuration is d⁶ , after loosing an electron it attains the d⁵ configuration. Now this configuration has half filled d orbital which makes it stable thus we will need more energy.

2. In case of copper

Now in this case we get d¹⁰ configuration on loosing one electron , thus it is hard to remove one more electron from d-subshell. Thus it increases the second ionisation enthalpy.

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