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

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 Question:

Given below are two statements:

Statement I: H₂Se is more acidic than H₂Te
Statement II: H₂Se has higher bond enthalpy for dissociation than H₂Te

📷 Question Image:

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

Short Text Solution:

Concept Used: Acidity of hydrides of Group 16 elements depends mainly on bond strength and atomic size.

  • H₂Se vs H₂Te:

    • Bond Enthalpy: H₂Se > H₂Te → H₂Se bond stronger

    • Acidity Trend: H₂Te > H₂Se > H₂S > H₂O

Explanation:

  • Even though H₂Se has higher bond enthalpy than H₂Te, acidity depends on ease of H⁺ release.

  • Larger atoms (like Te) hold H less tightly → easier H⁺ release.

  • So H₂Te is more acidic than H₂Se, not the other way.

✅ Conclusion:

  • Statement I is false

  • Statement II is true

📷 Solution Image:

Conclusion – Video Solution:

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