Given below are two statements :
Statement (I) : The oxidation state of an element in a particular compound is the charge acquired by its atom on the basis of electron gain enthalpy consideration from other atoms in the molecule.
Statement (II) : p π-p π bond formation is more prevalent in second period elements over other periods.
In the light of the above statements, choose the most appropriate answer from the options given below :

Solution

Chemistry ma’am · 3 steps

Oxidation state comes from electronegativity, not electron gain enthalpy. That one word sinks Statement I.

1. Statement I. Oxidation state is the charge an atom would carry if the more electronegative atom took all the shared electrons in each bond. The definition uses electronegativity, which describes an atom pulling a shared pair within a molecule. Electron gain enthalpy describes an isolated gaseous atom taking an extra electron, so Statement I is incorrect.
2. Statement II. Second period atoms such as C, N and O are small, so their 2p orbitals come close enough to overlap sideways well. That is why they form strong pπ–pπ bonds, as in O₂, N₂ and C=C. Larger atoms from period 3 onwards overlap poorly and rarely form such bonds, so Statement II is correct.
3. So. Statement I is incorrect and Statement II is correct, which is option (c).

The idea to keep. Oxidation number means giving the bonding electrons to the more electronegative atom. Small second period atoms are the ones that make strong pπ–pπ multiple bonds.

Answer from the NTA final answer key. Solution by PrepWiser.