d and f BLOCK ELEMENTS

What would be the expected impact on the E°(M2+/M) value if an element's M2+ ion achieved a d10 configuration, based on the text's explanation for Zn?

• The E°(M2+/M) value would be less negative than expected.
• The E°(M2+/M) value would be unaffected.
• The E°(M2+/M) value would become positive.
• The E°(M2+/M) value would likely be more negative than expected from the simple thermochemical trend.

Why is the statement 'copper's positive E° is solely due to its high ionization enthalpies' incomplete according to the text?

• Because copper has low ionization enthalpies.
• Because ionization enthalpies are not important.
• Because the text only mentions hydration enthalpy.
• Because the text emphasizes the high atomization enthalpy and insufficient hydration enthalpy as the primary reasons.

How does the concept of half-filled subshell stability explain the redox behavior of Mn according to the text?

• Mn2+ loses an electron to achieve the stable d4 configuration of Mn3+.
• Mn atoms prefer the d5 configuration in their ground state.
• Half-filled subshells make elements less reactive.
• Mn3+ gains an electron to achieve the stable d5 half-filled configuration of Mn2+, making Mn3+ an oxidizing agent.

What is the primary difference in the redox behavior of Cr2+ and Mn3+ despite both having d4 configurations, according to the text?

• Cr2+ is more stable than Mn3+.
• Mn3+ is more stable than Cr2+.
• They behave identically.
• Cr2+ acts as a reducing agent by losing an electron to gain stability, while Mn3+ acts as an oxidizing agent by gaining an electron to gain stability.

Why is the E°(M2+/M) value for Mn more negative than expected from the simple trend according to the text?

• Its low atomic mass.
• Its high ionization enthalpy.
• Its low hydration enthalpy.
• Because the formation of the stable, half-filled d5 electronic configuration in Mn2+ provides extra stability not fully captured by basic thermochemical calculations.