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The d-And-f-Block Elements

Short Answer Type

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

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2. 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 extent of metallic bonding an element undergoes deideds the enthalpy of atomization the more extensive the metallic bonding of an element the more will be its enthalpy of atomization.

Sc & Zn belongs to 3^rd group of periodic table. In all transition metals (except Zn, electronic configuration: 3d¹⁰ 4s²), there are some unpaired electrons that account for their stronger metallic bonding. Due to the absence of these unpaired electrons, the inter-atomic electronic bonding is the weakest in Zn and as a result, it has the least enthalpy of atomization.

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

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

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

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

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7. Calculate the 'spin only' magnetic moment of M²⁺_(aq) ion (Z = 27).

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8. Explain why Cu⁺ ion is not stable in aqueous solutions?

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9. Actinoid contraction is greater from element to element than lanthanoid contraction. Why?

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10. On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?

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