JEE Main 2025 Apr 8 Shift 2, Chemistry Q20: Group 16 Elements: The Oxygen Family

JEE Main2025Apr 8, Shift 2Chemistry

Given below are two statements:

Statement I: H $_{2}$ Se is more acidic than H $_{2}$ Te.

Statement II: H $_{2}$ Se has higher bond enthalpy for dissociation than H $_{2}$ Te.

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

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

Solution

Acidic strength of the hydrogen chalcogenides increases down the group as the H-X bond becomes weaker and easier to ionise, so H $_{2}$ Te, with a weaker H-Te bond, is expected to be more acidic than H $_{2}$ Se.

Statement I, which claims H $_{2}$ Se is more acidic than H $_{2}$ Te, is therefore false.

Bond dissociation enthalpy data show H $_{2}$ Se (about 276 kJ/mol) has a higher bond enthalpy than H $_{2}$ Te (about 238 kJ/mol), consistent with H $_{2}$ Se possessing the stronger H-Se bond.

Statement II is therefore true.

Hence Statement I is false and Statement II is true, matching option (4).

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JEE Main 2025 Apr 8 Shift 2, Chemistry Q20: Group 16 Elements: The Oxygen Family

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