Question:
The relative basic strength of the compounds is correctly shown in the option:
The relative basic strength of the compounds is correctly shown in the option:
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Basicity depends on lone pair availability. Hydrogen bonding can reduce basic strength significantly.
Updated On: May 20, 2025
- \( \text{NH}_2\text{OH}>\text{NH}_3>\text{N}_2\text{H}_4 \)
- \( \text{N}_2\text{H}_4>\text{NH}_2\text{OH}>\text{NH}_3 \)
- \( \text{NH}_3>\text{N}_2\text{H}_4>\text{NH}_2\text{OH} \)
- \( \text{N}_2\text{H}_4>\text{NH}_3>\text{NH}_2\text{OH} \)
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The Correct Option is C
Solution and Explanation
Basic strength is related to the availability of lone pairs on nitrogen:
- Ammonia (NH\(_3\)) has a free lone pair on nitrogen, making it more basic.
- Hydrazine (N\(_2\)H\(_4\)) has two nitrogen atoms with lone pairs, but intramolecular hydrogen bonding and repulsion reduce basicity slightly compared to NH\(_3\).
- Hydroxylamine (NH\(_2\)OH) has a nitrogen lone pair involved in hydrogen bonding with OH, decreasing its availability for donation, hence the weakest base.
\[ \text{Basicity order: } \text{NH}_3>\text{N}_2\text{H}_4>\text{NH}_2\text{OH} \]
- Hydrazine (N\(_2\)H\(_4\)) has two nitrogen atoms with lone pairs, but intramolecular hydrogen bonding and repulsion reduce basicity slightly compared to NH\(_3\).
- Hydroxylamine (NH\(_2\)OH) has a nitrogen lone pair involved in hydrogen bonding with OH, decreasing its availability for donation, hence the weakest base.
\[ \text{Basicity order: } \text{NH}_3>\text{N}_2\text{H}_4>\text{NH}_2\text{OH} \]
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