Given below are two statements: Statement I: H2Se is more acidic than H2Te. Statement II: H2Se has higher bond enthalpy…

🧠 Acidity of group 16 hydrides increases down the group because bond dissociation enthalpy decreases (weaker bond → easier H⁺ release). Electronegativity of S and Se are both relatively low so that's not the driving factor.

🗺️ Statement I — $\ce{H2Se}$ is more acidic than $\ce{H2Te}$:

Acidity order (group 16): $\ce{H2O} < \ce{H2S} < \ce{H2Se} < \ce{H2Te}$

$\ce{H2Te}$ is MORE acidic than $\ce{H2Se}$ (not the other way around).

Statement I is FALSE ✗

Statement II — $\ce{H2Se}$ has higher bond enthalpy than $\ce{H2Te}$:

Bond dissociation enthalpy decreases down the group (larger atom, poorer orbital overlap):

$\text{H–O} > \text{H–S} > \text{H–Se} > \text{H–Te}$

So $\ce{H2Se}$ has higher Se–H bond enthalpy than Te–H bond enthalpy in $\ce{H2Te}$.

Statement II is TRUE ✓

$\boxed{\text{Answer: Statement I is false but Statement II is true}}$