JEE Main 2026 — Jan 21, Shift 2 — Chemistry solution

JEE Main2026Jan 21, Shift 2Chemistry

Given below are two statements :

Statement I : The correct order in terms of bond dissociation enthalpy is $C l_{2} > B r_{2} > F_{2} > I_{2}$

Statement II : The correct trend in the covalent character of the metal halides is $[S n C l_{4} > S n C l_{2}]$ , $[P b C l_{4} > P b C l_{2}]$ and $[U F_{4} > U F_{6}]$

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

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

Solution

Statement I: Bond dissociation enthalpy of halogens follows $C l_{2} > B r_{2} > F_{2} > I_{2}$ . $F_{2}$ is anomalously low because of lone-pair–lone-pair repulsion in the small $F_{2}$ molecule. True.

Statement II: By Fajan’s rules a higher cationic charge produces greater covalent character, so $S n C l_{4} > S n C l_{2}$ and $P b C l_{4} > P b C l_{2}$ are correct. However the U pair is given as $U F_{4} > U F_{6}$ , which contradicts Fajan’s rules — $U F_{6}$ (U in +6) is actually more covalent than $U F_{4}$ (U in +4). False.

So I true, II false.

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