Given below are two statements:
Statement I: $ H_2Se $ is more acidic than $ H_2Te $
Statement II: $ H_2Se $ has higher bond enthalpy for dissociation than $ H_2Te $
In the light of the above statements, choose the correct answer from the options given below.
Given below are two statements:
Statement I: $ H_2Se $ is more acidic than $ H_2Te $
Statement II: $ H_2Se $ has higher bond enthalpy for dissociation than $ H_2Te $
In the light of the above statements, choose the correct answer from the options given below.
Show Hint
- Statement I is false but Statement II is true
- Statement I is true but Statement II is false
- Both Statement I and Statement II are false
- Both Statement I and Statement II are true
The Correct Option is A
Approach Solution - 1
To answer the question, we first need to analyze each statement separately in the context of chemistry, specifically the properties of hydrides within the chalcogen group.
- Statement I: \( H_2Se \) is more acidic than \( H_2Te \)
The acidity of hydrides in the group 16 elements (chalcogen group) increases as we move down the group. Therefore, the correct trend in acidity for \( H_2\text{X} \) hydrides (where \( \text{X} \) is a chalcogen) is: \( H_2O < H_2S < H_2Se < H_2Te \). Hence, \( H_2Te \) is more acidic than \( H_2Se \) due to an increase in atomic size and decrease in bond strength, which facilitates the release of protons.
Therefore, Statement I is false.
- Statement II: \( H_2Se \) has a higher bond enthalpy for dissociation than \( H_2Te \)
Bond enthalpy typically decreases as we move down the group due to the increasing size of the atoms, which results in weaker bonds. Therefore, \( H_2Se \), which is higher in the group than \( H_2Te \), will indeed have a higher bond enthalpy (i.e., stronger bonds) than \( H_2Te \).
Thus, Statement II is true.
Considering the above analysis, the correct option is that Statement I is false but Statement II is true.
Approach Solution -2
Analysis of Statement I:
- Acidic character increases down the group for hydrides (H2O < H2S < H2Se < H2Te) - H2Te is more acidic than H2Se because:
- Te is larger than Se, making Te-H bond weaker
- H+ ion is more easily released from H2Te
- Therefore, Statement I is false
Analysis of Statement II:
- Bond enthalpy decreases down the group (H-Se > H-Te)
- H2Se has higher bond dissociation enthalpy because:
- Se is smaller than Te, forming stronger bonds
- Bond strength decreases with increasing atomic size
- Therefore, Statement II is true
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