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The D-And-f-Block Elements

Question
CBSEENCH12007170
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Account for the following facts:
The reduction of a metal oxide is easier if the metal formed is in liquid state at the temperature of reduction.

Solution

The entrophy is higher if the metal is in liquid state than when it is in solid state.In solid state, the entropy or randomness will be less due to high intermolecular force of attraction while in liquid state, the entropy will be more comparatively. Therefore value of entropy change (ΔS) of the reduction process is more +ve side when the metal formed is in liquid state and the metal oxide being reduced is in solid state. Thus the value of ΔG° becomes more on negative side and the reduction becomes easier.

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

Silver atom has a completely filled d orbitals (4d10) in its ground state. How can you say that it is a transition element?

In the series Sc (Z = 21) to Zn(Z = 30), the enthalpy of atomisation of zinc is the lowest i.e., 26, kJ mol. Why?

The E° (M2+/M) value for copper is positive (+ 0.34 V). What is possibility the reason for this? 

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?

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