d and f BLOCK ELEMENTS MCQ Quiz: GKFix - Bridge of Knowledge

Question 1401

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What is the primary reason Cr2+ (d4) is a better reducing agent than V2+ (d3), according to principles discussed in the text?

Cr2+ has a higher charge.
V2+ is more stable than Cr2+.
Cr2+ has a lower atomic number.
Cr2+ achieves greater stability by losing an electron to reach the d3 configuration with a half-filled t2g level, compared to V2+ which is already relatively stable.

Question 1402

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Why is the E°(M2+/M) value for Zn more negative than expected from the simple trend according to the text?

Its low atomic mass.
Its high ionization enthalpy.
Its low hydration enthalpy.
Because the formation of the stable, fully filled d10 electronic configuration in Zn2+ provides extra stability not fully captured by basic thermochemical calculations.

Question 1403

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If a metal's calculated E°(M2+/M) value is less negative than its observed value, what might this imply according to the context provided by the text?

The calculation is perfectly accurate.
The calculation overestimates the energy cost.
The calculation overestimates the energy gain.
The calculation might underestimate the stability gained by forming the M2+ ion due to specific electronic configurations.

Question 1404

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What is the main factor determining the general trend of E°(M2+/M) values becoming less negative across the first transition series, according to the text?

The general decrease in atomization enthalpy.
The general increase in hydration enthalpy.
The stability of half-filled d orbitals.
The general increase in the sum of the first and second ionization enthalpies.

Question 1405

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Why is the d5 electronic configuration significant in the context of Mn chemistry, according to the text?

It makes Mn2+ highly reactive and unstable.
It makes Mn3+ a strong reducing agent.
It has no significant impact on Mn's redox behavior.
It provides extra stability to the Mn2+ ion, making Mn3+ a strong oxidizing agent.

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