d and f BLOCK ELEMENTS

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.

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.

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.

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.

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.