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The D-And-f-Block Elements

Question

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Why is the + 2 oxidation state of manganese quite stable while the same is not true for iron? |Mn = 25, Fe = 26]

Solution

Electronic configuration of Mn²⁺ is 4s⁰ 3d⁵ and electronic configuration for Fe²⁺ is 3d⁶. Mn²⁺ is more stable due to half filled d-orbitals but Fe²⁺ is not stable because it does not have half filled d-orbitals.

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

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?

The outer electronic configuration of copper is 3d¹⁰ 4s¹, yet it is considered transition element. Why?

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