Given below are two statements :
Statement I : C < 0 < N < F is the correct order in terms of first ionization enthalpy values.
Statement II: S > Se > Te > Po > 0 is the correct order in terms of the magnitude of electron gain enthalpy values.
ln the light of the above statements, choose the correct answer from the options given below:

We need to evaluate two statements about ionization enthalpy and electron gain enthalpy.

Analysis of Statement I: C < O < N < F is the correct order of first ionization enthalpy.

The first ionization enthalpies (in kJ/mol) are approximately: C (1086), O (1314), N (1402), F (1681). The correct increasing order is: C < O < N < F.

Nitrogen has a higher ionization enthalpy than oxygen because nitrogen has a half-filled $$2p^3$$ configuration, which provides extra stability. Removing an electron from this stable configuration requires more energy than removing one from oxygen's $$2p^4$$ configuration (where one orbital has a paired electron, causing electron-electron repulsion).

The order C < O < N < F given in Statement I is correct. Statement I is TRUE.

Analysis of Statement II: S > Se > Te > Po > O is the correct order of magnitude of electron gain enthalpy.

Electron gain enthalpy (magnitude, in kJ/mol): O (141), S (200), Se (195), Te (190), Po (174). Oxygen has an anomalously low electron gain enthalpy due to its small atomic size, causing significant electron-electron repulsion in the compact $$2p$$ orbital.

The correct order is: S > Se > Te > Po > O. This matches Statement II. Statement II is TRUE.

The correct answer is Option 4: Both Statement I and Statement II are true.