Given below are two statements: Statement I: The covalency of...

Statement I: The electronic configuration of oxygen is $1s^{2} 2s^{2} 2p^{4}$. Due to the absence of d-orbitals, its maximum covalency is limited to four (using one 2s and three 2p orbitals). Its covalency is generally two, but it can exceed two and go up to four in certain compounds. In $SO_2$, oxygen is more electronegative than sulphur, so its oxidation state is $-2$. In $OF_2$, fluorine is more electronegative than oxygen, so the oxidation state of oxygen is $+2$. Thus, Statement I is true.

Statement II: Oxygen differs from the rest of the group 16 elements due to its small atomic size, high electronegativity, and the absence of d-orbitals in its valence shell. This leads to its anomalous behaviour, such as the ability to form strong hydrogen bonds and $p\pi-p\pi$ multiple bonds. Thus, Statement II is true.

Both Statement I and Statement II are true.

Answer: Both Statement I and Statement II are true