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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?

Solution

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.

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?

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