Given below are two statements: Statement I : The second ionisation enthalpy of Na is larger than the corresponding ionisation enthalpy of Mg. Statement II : The ionic radius of O ²⁻ is larger than that of F ⁻ . In the light of the above statements, choose the correct answer from the options given below

Step-by-step solution

Statement I examines second ionization enthalpy: Na (1s ^2 2s ^2 2p ^6 3s ^1 ) loses its first electron to achieve a stable noble gas configuration. The second ionization would break into the 2p core, requiring enormous energy. Mg (1s ^2 2s ^2 2p ^6 3s ^2 ) loses its second electron from the 3s orbital, which is less stable. Thus, IE₂ of Na is much larger than IE₂ of Mg. Statement I is TRUE. Statement II compares O ²⁻ and F ^- : both are isoelectronic with 10 electrons. O ²⁻ has 8 protons while F ^- has 9 protons.