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The D-And-f-Block Elements

Question
CBSEENCH12011418
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It is because of inability of ns2 electrons of the valence shell to participate in bonding that

  • Sn2+ is reducing while Pb4+ is oxidising

  • Sn2+ is oxidising while Pb4+ is reducing

  • Sn2+ and Pb2+ are both oxidising and reducing

  • Sn4+ is reducing while Pb4+ is oxidising

Solution

A.

Sn2+ is reducing while Pb4+ is oxidising

Inability of ns2 electrons of the valence shell to participate in bonding on moving down the group in heavier p-block elements is called inert pair effect
As a result, Pb(II) is more stable than Pb(IV)
Sn(IV) is more stable than Sn(II)
∴ Pb(IV) is easily reduced to Pb(II)
∴ Pb(IV) is oxidising agent
Sn(II) is easily oxidised to Sn(IV)
∴ Sn(II) is reducing agent

Some More Questions From The d-And-f-Block Elements Chapter

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?

Why Zn, Cd and Hg are not regarded as transition elements?

Name the first element of 3rd transition series.

Though copper, silver and gold have completely filled sets of d-orbitals yet they are considered as transition metals. Why?

Why are transition elements so named?

Why are transition elements known as d-block elements?

Write the general electronic configuration of d-block elements.

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