Given below are two statements : Statement I : Oxygen exists as a diatomic gas because it can form strong p - p multiple bonds with itself, whereas heavier members of Group 16 prefer to form single bonds and exist as polyatomic solid molecules. Statement II : Oxygen can expand its covalency to six and form compounds like OF ₆ due to its exceptionally high electronegativity. In the light of the given statements, choos

Step-by-step solution

Statement I is true: Due to its small size and high electronegativity, oxygen forms strong p - p double bonds ( O = O ), allowing it to exist as a diatomic gas. Heavier Group 16 elements like sulphur are larger and do not form strong p - p bonds, so they satisfy their valency by forming single bonds in polyatomic molecules (e.g., S ₈ ). Statement II is false: Although oxygen is highly electronegative, it belongs to the second period and completely lacks d-orbitals in its valence shell. Therefore, it cannot expand i