More number of oxidation states are exhibited by the actinides than by the lanthanides. The main reason for this is:
- more energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals
- lesser energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals
- greater metallic character of the lanthanides than that of the corresponding actinides
- more active nature of the actinides
The Correct Option is B
Solution and Explanation
Actinoids display more oxidation states because of very small energy gap between 5f, 6d and 7s sub shells. Thus, the outermost electrons get easily excited to the higher energy level giving variable oxidation state.
Hence, the correct option is (B): lesser energy difference between 5f and 6d orbitals than that between 4f and 5d orbitals
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Concepts Used:
D and F Block Elements
The d-block elements are placed in groups 3-12 and F-block elements with 4f and 5f orbital filled progressively. The general electronic configuration of d block elements and f- block elements are (n-1) d 1-10 ns 1-2 and (n-2) f 1-14 (n-1) d1 ns2 respectively. They are commonly known as transition elements because they exhibit multiple oxidation states because of the d-d transition which is possible by the availability of vacant d orbitals in these elements.
They have variable Oxidation States as well as are good catalysts because they provide a large surface area for the absorption of reaction. They show variable oxidation states to form intermediate with reactants easily. They are mostly lanthanoids and show lanthanoid contraction. Since differentiating electrons enter in an anti-penultimate f subshell. Therefore, these elements are also called inner transition elements.
Read More: The d and f block elements