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The D-And-f-Block Elements

Question

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Assign reasons for the following:
Transition metals and their many compounds act as good catalyst.

Solution

Transition metals acts as catalyst due to the following reasons:
(i) Their partially empty d-orbitals provide surface area for reactant molecules.
(ii) They combine with reactant molecules to form transition states and lowers their activation energy.
(iii) They show multiple oxidation states and by giving electrons to reactants they form complexes and lower their energies.0

V₂O₅ (in contact process for manufacture of H₂SO₄), finely divided iron (in Haeber’s process for NH₃ manufacture) and Ni (in catalytic hydrogenation) are examples of their good catalytic activities.

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

How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?

Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?

Which is a stronger reducing agent Cr²⁺ or Fe²⁺ and why?

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?

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