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

Question 46

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Why is the density of transition metals generally higher than that of s-block elements?

Because they are harder.
Due to their smaller atomic sizes combined with relatively high atomic masses, leading to more mass packed into a smaller volume.
Because they have more electrons.
Because they form stronger metallic bonds.

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What is the typical trend in atomic radii across the first transition series (Sc to Zn), and what causes this trend?

Atomic radii increase significantly.
Atomic radii remain constant.
Atomic radii generally decrease slightly, though not as smoothly as in main group elements, due to the imperfect shielding of 3d electrons.
Atomic radii decrease sharply like in main group elements.

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Why is Zinc (Zn) not typically considered a transition element despite being located in the d-block of the periodic table?

Because it is a metal.
Because its common oxidation state (Zn^2+) has a completely filled d-subshell (d^10), lacking the characteristic incomplete d-orbitals.
Because it is located at the end of the series.
Because it has a high melting point.

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What is the primary reason for the variable oxidation states commonly observed in transition elements?

Because they are reactive.
Because they have unpaired electrons.
The involvement of both ns and (n-1)d electrons in bonding, allowing for multiple electron loss configurations.
Because they form complex ions.

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Why do transition metal ions often form colored compounds, unlike many main group metal ions?

Because they are metals.
Because they have more electrons.
Due to d-d electronic transitions within the partially filled d-orbitals, which absorb specific wavelengths of visible light.
Because they form ionic bonds.