Chemistry · p-Block Elements (Group 15-18)

JEE Main 2025 — 8 April, Evening Shift — Question 10

Given below are two statements:

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

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

In the light of the above statement, choose the correct answer from the options given

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

Answer: C

Step-by-step solution

$\therefore \quad \mathrm{H}_{2} \mathrm{Te}$ is more acidic than $\mathrm{H}_{2} \mathrm{Se}$ because of lesser bond dissociation energy of $\mathrm{H}_{2} \mathrm{Te}$ It can release

$\mathrm{H}^{+}$ more easily

$\mathrm{pK}_{\mathrm{a}_{1}}: \mathrm{H}_{2} \mathrm{Se}(3.89)>\mathrm{H}_{2} \mathrm{Te}(2.6)$

Answer key and solution verified before publishing.

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Exam: JEE Main 2025
Paper: 8 April, Evening Shift
Subject: Chemistry
Chapter: p-Block Elements (Group 15-18)
Topic: Comparisons between the different compounds formed by Group 16 elements