The species in which nitrogen atom is in a state of sp hybridisation is
- NO3-
- NO2
- NO2+
- NO2-
The Correct Option is C
Solution and Explanation
To find the hybridisation of nitrogen in different species, we use this rule:
- Count the regions of electron density (i.e., number of sigma bonds + lone pairs).
- Use the following chart:
| Number of regions | Hybridisation | Geometry |
|---|---|---|
| 2 | sp | Linear |
| 3 | sp2 | Trigonal planar |
| 4 | sp3 | Tetrahedral |
1) NO3− (Nitrate ion):
- N is bonded to 3 O atoms.
- It has no lone pair.
- Total regions = 3 → sp2 hybridisation.
2) NO2 (Nitrogen dioxide):
- N is bonded to 2 O atoms.
- It has 1 lone pair.
- Total regions = 3 → sp2 hybridisation.
3) NO2− (Nitrite ion):
- N is bonded to 2 O atoms.
- It has 1 lone pair.
- Total regions = 3 → sp2 hybridisation.
4) NO2+ (Nitronium ion):
- N is bonded to 2 O atoms.
- It has no lone pair.
- Total regions = 2 → sp hybridisation.
Conclusion: Only NO2+ has nitrogen in sp hybridisation.
Correct answer: (C) NO2+
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