Question

The group 14 elements A and B have the first ionisation enthalpy values of 708 and 715 kJ mol$^{-1}$ respectively. The above values are lowest among their group members. The nature of their ions A$^{2+}$ and B$^{4+}$ respectively is:

• A. both reducing
• B. both oxidising
• C. reducing and oxidising
• D. oxidising and reducing

Hint:

In general, elements with low ionization enthalpies are reducing agents because they can easily lose electrons, while elements with high ionization enthalpies tend to attract electrons and thus act as oxidizing agents.

Answer 1

The Correct Option is C

Step 1: Ionization Enthalpy Defined
Ionization enthalpy is the energy needed to remove an electron from a gaseous, neutral atom. A lower value signifies easier electron loss. Elements A and B exhibit the lowest ionization enthalpies within their respective groups, indicating they ionize more readily than other group members.
Step 2: Ion Characteristics Analysis
Element A: Possessing low ionization enthalpy, A readily loses electrons. Consequently, the A\(^{2+}\) ion readily accepts electrons, undergoing reduction. Therefore, element A functions as a 
reducing agent.
Element B: Element B's ionization enthalpy is marginally higher than A's. The B\(^{4+}\) ion exhibits a tendency to attract electrons, classifying it as a potent 
oxidizing agent.
In summary, A\(^{2+}\) ions are reducing in nature, while B\(^{4+}\) ions are oxidizing.