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

Question 1426

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What is the significance of comparing calculated and observed E° values in Fig. 4.4?

It proves the thermochemical model is completely accurate.
It shows that calculations are always more accurate than experiments.
It indicates that thermochemical parameters are unreliable.
It highlights deviations from the simple thermochemical model, indicating additional stabilizing factors for certain elements.

Question 1427

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Why is the d3 configuration (t2g^3) particularly stable in an octahedral field?

Because it has paired electrons.
Because it is a high-spin configuration.
Because it occupies the eg orbitals.
Due to the symmetrical distribution of electrons in the lower energy t2g orbitals, minimizing repulsion.

Question 1428

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Which of the following best describes the relationship between ionization enthalpies and the E°(M2+/M) trend across the transition series?

Decreasing ionization enthalpies generally lead to E°(M2+/M) values becoming less negative.
Ionization enthalpies remain constant, so they do not affect the E°(M2+/M) trend.
Ionization enthalpies decrease sharply, causing E°(M2+/M) to become more negative.
Increasing ionization enthalpies generally lead to E°(M2+/M) values becoming less negative.

Question 1429

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What is the main thermodynamic reason why copper does not react with dilute H2SO4?

Copper is too dense.
Dilute H2SO4 is not a strong enough acid.
The negative E°(Cu2+/Cu) makes the cell potential for the reaction positive.
The positive E°(Cu2+/Cu) makes the cell potential for the reaction negative.

Question 1430

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If an element in the transition series has an E°(M2+/M) value significantly more negative than its neighbors, what could be a likely electronic reason?

Its M2+ ion has a very high charge density.
Its atomic radius is significantly smaller.
Its ionization enthalpies are significantly lower.
Its M2+ ion achieves a particularly stable electronic configuration (e.g., d5 or d10).

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