Question:

Among the following pairs of ions, the lower oxidation state in aqueous solution is more stable than the other, in

Updated On: Jul 2, 2022
  • $Ti ^{+}, Ti ^{3+}$
  • $Cu ^{+}, Cu ^{2+}$
  • $Cr ^{2+}, Cr ^{3+}$
  • $V ^{2+}, VO ^{2+}$
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The Correct Option is A

Solution and Explanation

As we move down in $13,14$ and $15$ groups the inertness of $s^{2}$ electrons of valence shell increases and therefore, metals in the lower portion of the group show lower oxidation state e.g., lead show $+2$ inspite of $+4$. Similarly $+3$ oxidation state of bismuth is more stable than $+5$ oxidation state. Thus, due to inert pair effect, titanium shows $+1$ oxidation state rather than $+3$.
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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.

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