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The D-And-f-Block Elements

Question
CBSEENCH12007167
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Why are Ni2+ compounds thermodynamically more stable than Pt2+ compounds while Pt4+ compounds are relatively more stable than Ni4+ compounds?

Solution

A compound has more thermodynamic stability if the ionization energy of the metal is low. Since the ionization energy of Ni2+ is less than that for Pt2+, therefore Ni2+, compounds are thermodynamically more stable than Pt2+ compounds.
Ni → Ni2+ + 2e– ΔH = 2490 kJ mol–1
(low energy more stable)
Pt → Pt2+ + 2e–  ΔH = 2660 kJ mol–1
(high energy less stable)
Pt4+ compounds are stable than Ni4+ compounds because the energy needed to remove 4 electrons in Pt is less than that in Ni.
Pt → pt4+ + 4e–    ΔH = 6770 kJ mol–1
(low energy more stable)
Ni → Ni4+ + 4e–  ΔH = 8800 kJ mol–1
(high energy, less stable)

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

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?

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?

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