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

Question 16

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Why do the actinoid elements generally have lower melting and boiling points than the corresponding lanthanoids?

Because actinoids are radioactive.
Because actinoids have higher atomic numbers.
Because actinoids are heavier.
Because the 5f electrons in actinoids are less likely to participate in strong metallic bonding compared to the more localized 4f electrons in lanthanoids, leading to weaker interatomic forces.

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Why do the complexes [Fe(CN)6]^4- and [Fe(CN)6]^3- exhibit different magnetic properties?

Because CN- is a ligand.
Because they have different charges.
Because Fe^2+ (d^6) and Fe^3+ (d^5) have different numbers of d-electrons, leading to different electron configurations and numbers of unpaired electrons in the strong field environment of CN- ligands.
Because they are both iron complexes.

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Why do the standard electrode potentials for M^2+/M couples in the first transition series not show a regular trend?

Because they are metals.
Because the concentration varies.
Because the temperature varies.
Because the electrode potential depends on multiple factors including sublimation enthalpy, ionization enthalpy, and hydration enthalpy, each of which varies irregularly due to electronic configuration effects.

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Why do the heats of formation for transition metal compounds vary significantly, even for compounds of the same metal in the same oxidation state?

Because transition metals are reactive.
Because they form complex ions.
Because the temperature varies.
Because the stability of a compound depends not only on the metal and its oxidation state but also critically on the specific ligands or anions involved and their interactions.

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Why do the electron affinities of transition metals generally have small or even positive values?

Because transition metals are metals.
Because they have high ionization enthalpies.
Because they form complex ions.
Because adding an electron to a metal atom generally requires energy due to the atom's tendency to lose, rather than gain, electrons, and the added electron often goes into a higher energy orbital.