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

Question 76

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Why do small, highly electronegative elements like oxygen and fluorine tend to stabilize the highest oxidation states of transition metals?

Because they are metals.
Because they have low ionization enthalpies.
Due to their high electronegativity and small size, they form strong bonds and effectively stabilize high positive charges on the metal.
Because they are inert gases.

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Which 3d series element is expected to have the highest third ionization enthalpy, and why?

Iron (Fe), due to its higher atomic number.
Manganese (Mn), because removing the third electron disrupts the stable half-filled 3d^5 configuration.
Chromium (Cr), because of its unique electronic configuration.
Vanadium (V), as it has fewer electrons.

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What is the main reason why zinc does not participate in metallic bonding using its 3d electrons, unlike other 3d series metals?

Zinc has no d-electrons.
In zinc, the 3d orbitals are completely filled and do not contribute to metallic bonding.
Zinc only uses s-electrons for metallic bonding.
Zinc forms ionic bonds instead of metallic bonds.

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Why is Silver (Z=47) considered a transition element despite having a filled 4d subshell in its ground state?

Because it has a completely filled 4d subshell in its ground state.
Because it can exhibit a +2 oxidation state with incompletely filled 4d orbitals.
Because it belongs to the d-block of the periodic table.
Because it forms colored compounds.

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Why are the highest oxidation states of transition metals often found in oxoanions rather than simple oxides?

Oxoanions are smaller molecules.
Oxoanions are always coloured.
Oxoanions allow for charge dispersal and additional stabilization through resonance.
Simple oxides are ionic.