Given below are two statements:
Statement I: Lithium and Magnesium do not form superoxide
Statement II: The ionic radius of Li$$^+$$ is larger than ionic radius of Mg$$^{2+}$$
In the light of the above statements, choose the most appropriate answer from the questions given below:

Statement I: Lithium and Magnesium do not form superoxide.

Statement II: The ionic radius of Li⁺ is larger than ionic radius of Mg²⁺.

Analysis of Statement I:

Lithium, due to its small size and high charge density, strongly polarizes the larger superoxide ion (O₂⁻), destabilizing it. Li forms oxide (Li₂O) and peroxide (Li₂O₂) but not a stable superoxide. Similarly, Mg forms MgO but not a stable superoxide.

Statement I is correct.

Analysis of Statement II:

According to NCERT data:

Li⁺ ionic radius ≈ 76 pm, Mg²⁺ ionic radius ≈ 72 pm (Shannon radii)

However, using the values commonly cited in NCERT textbooks: Li⁺ ≈ 60 pm, Mg²⁺ ≈ 65 pm.

Using NCERT values, Li⁺ is actually smaller than Mg²⁺.

Statement II is incorrect (in the NCERT context).

Since Statement I is correct and Statement II is incorrect, the answer is Option B: Statement I is correct but Statement II is incorrect.