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The D-And-f-Block Elements

Question
CBSEENCH12011392
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More the number of oxidation states are exhibited by the actinoids than by the lanthanoids. The main reason for this is:

  • more energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals

  • the lesser energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals

  • the greater metallic character of the lanthanoids than that of the corresponding actinoids

  • more active nature of the actinoids

Solution

B.

the lesser energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals

A number of oxidation states are exhibited by the actinoids than by the lanthanoids due to the lesser energy difference between 5f and 6d orbitals than between 4f and 5d orbitals.

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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