Pb⁴⁺ is less stable than Sn⁴⁺. It is because of
(a) Higher value of IE₁ + IE₂ + IE₃ + IE₄ for Pb than Sn
(b) Lesser polarising power of Pb⁴⁺ than Sn⁴⁺
(c) Inert pair effect in Pb
(d) None of these
Answers
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Pb⁴⁺ is less stable than Sn⁴⁺ because of
(c) Inert pair effect in Pb
1. As we move down a group in the periodic table the inert part effect increases.
2. It gets more pronounced in the heavier elements at the bottom of the groups.
3. In group 14 of the periodic table, Pb comes after Sn and hence Pb has a stronger inert pair effect as compared to that of Sn.
4. Due to inert pair effect Pb2+ is very stable and hence Pb4+ is unstable and easily gets reduced to Pb2+.
Answered by
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Inert pair effect in Pb is the correct option.
Explanation:
- Inert pair effect is seen in heavier elements.
- In case of lead and tin, both are from group 14.
- Here, the outermost electronic configuration of the elements are ns2 np2.
- As we go down a group, newer shells are added to the elements.
- The energy levels of higher s orbitals and p orbitals get farther apart.
- So these elements tend not to loose or break the paired up s orbital.
- As lead is more down than tin, so lead has more inert pair effect.
- So it tends to form divalent cation whereas tin tends to form tetravalent cation.
For more information about inert pair effect,
https://brainly.in/question/3205962
inert pair effect definition - Brainly.in
https://brainly.in/question/5836177
What is Inert pair effect ? Explain in detail with examples... :] - Brainly.in
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