Step 1: Explanation of Ionization Energies.
Ionization energy is the energy required to remove an electron from an atom in its gaseous state. The configuration plays a key role in determining the ionization energy. For atoms with the same principal quantum number, the order of ionization energy can be explained by electron shielding and the effective nuclear charge.
Step 2: Understanding configurations and IE.
- (A) ns²np¹: The element with this configuration has an electron in an unfilled p-orbital, which results in a lower ionization energy compared to a fully filled p-orbital (ns²np⁶). Therefore, its IE is lower. This corresponds to value (Q) 801 kJ/mol.
- (B) ns²np⁶: This configuration is highly stable because the p-orbital is fully filled. It has a higher ionization energy, as it requires more energy to remove an electron from a stable, filled orbital. Therefore, its IE corresponds to value (P) 2080 kJ/mol.
- (C) ns²: This configuration represents a noble gas, which is highly stable with a completely filled s-orbital. The ionization energy here is relatively low compared to other configurations, corresponding to (S) 899 kJ/mol.
- (D) ns²np³: This configuration corresponds to an atom with half-filled p-orbitals, which is relatively stable. Its ionization energy is moderate, and it corresponds to value (R) 1402 kJ/mol.
Step 3: Conclusion.
The correct matching based on the ionization energies is:
- A → Q (801 kJ/mol),
- B → P (2080 kJ/mol),
- C → S (899 kJ/mol),
- D → R (1402 kJ/mol). Final Answer: (C) A → Q; B → P; C → S; D → R
