JEE Main 2026 — Apr 4, Shift 1 — Chemistry solution

JEE Main2026Apr 4, Shift 1Chemistry

Given below are two statements :

Statement I : The covalency of oxygen is generally two but it can exceed upto four. The oxidation state of oxygen in $S O_{2}$ is $- 2$ and in $O F_{2}$ it is $+ 2$ .

Statement II : The anomalous behaviour of oxygen when compared to the other elements of group $16$ is due to its small size and high electronegativity.

In the light of the above statements, choose the correct answer from the options given below :

A
Both Statement I and Statement II are true
B
Both Statement I and Statement II are false
C
Statement I is true but Statement II is false
D
Statement I is false but Statement II is true

Solution

Oxygen most commonly shows covalency $2$ , but in species such as $H_{3} O^{+}$ or coordination through lone pairs it can extend up to $4$ . In $S O_{2}$ , oxygen is more electronegative than sulphur, so O carries $- 2$ ; in $O F_{2}$ , fluorine is more electronegative than oxygen, so O takes $+ 2$ . Statement I is correct.

Oxygen's anomalous behaviour within group $16$ (high tendency to form double bonds, restricted to covalency $2$ in most molecules, etc.) stems from its small atomic radius, high electronegativity, and absence of accessible $d$ -orbitals. Statement II is correct and is the standard explanation given in textbooks.

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