Given below are two statements — Assertion A and Reason R:

Assertion A: $\mathrm{H_2Te}$ is more acidic than $\mathrm{H_2S}$ .

Reason R: Bond dissociation enthalpy of $\mathrm{H_2Te}$ is lower than $\mathrm{H_2S}$ .

Choose the most appropriate answer:

Question

Given below are two statements — Assertion A and Reason R:

Assertion A: $\mathrm{H_2Te}$ is more acidic than $\mathrm{H_2S}$ .

Reason R: Bond dissociation enthalpy of $\mathrm{H_2Te}$ is lower than $\mathrm{H_2S}$ .

Choose the most appropriate answer:

Paaras Thakur · Accepted Answer

Both A and R are true and R is the correct explanation of A. 🧠 Acidity of group 16 hydrides depends primarily on bond dissociation enthalpy (not electronegativity), since weaker bonds release H⁺ more easily. 🗺️ Evaluate Assertion A: Acidity order of group 16 hydrides (down the group): {H_2O < H_2S < H_2Se < H_2Te} H2Te is more acidic than H2S → A is TRUE ✓ Evaluate Reason R: Bond dissociation enthalpies: H–O H–S H–Se H–Te (bond strength decreases as the central atom gets larger and its orbital overlaps with H decreases). Weaker H–Te bond → H is released more easily → higher acidity of H2Te compared to H2S. R is TRUE ✓ and R correctly explains A ✓ ⚠️ Common trap: students think electronegativity (O S Se Te) should make H2O the most acidic. But in aqueous phase, bond strength dominates — the H–Te bond is so weak that H2Te ionizes far more readily. Answer: Both A and R are true and R is the correct explanation

Answer

Both A and R are true but R is NOT the correct explanation of A

Answer

Both A and R are true and R is the correct explanation of A

Answer

A is false but R is true

Answer

A is true but R is false

Given below are two statements — Assertion A and Reason R: Assertion A: H2Te is more acidic than H2S. Reason R: Bond…

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