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The d-And-f-Block Elements
Question
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The ionisation enthalpies of Cr and Cu are larger than their neighbours. Why?

Answer

Electronic configuration of Cr is 4s1 3d5 and the electronic configuration of Cu is 3d10 4s1. Since both are stable due to having half filled or fully filled orbital thus Cr and Cu show higher ionisation enthalpies than their neighbours.

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Some More Questions From The d-And-f-Block Elements Chapter

The E° (M2+/M) value for copper is positive (+ 0.34 V). What is possibility the reason for this? 

How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?

Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?

Which is a stronger reducing agent Cr2+ or Fe2+ and why?

Explain why Cu+ ion is not stable in aqueous solutions?

Actinoid contraction is greater from element to element than lanthanoid contraction. Why?

On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?

The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?

Why the melting points of transition elements are high?