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The hybridisations of the atomic orbitals of nitrogen in NO3-, NO2+ and NH4+ respectively are
 
  • a)
    sp2, sp and sp3
  • b)
    sp2, sp2 and sp3
  • c)
    sp3, sp and sp2
  • d)
    sp3, sp2 and sp
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
The hybridisations of the atomic orbitals of nitrogen in NO3-, NO2+ an...

In NO2+ it has only 2 bond pair and no lone pair so it is sp hybridised.
In NO3 it has only 3 bond pair and no lone pair so it is sp2 hybridised.
In NH4+ it has only 4 bond pair and no lone pair so it is sp3 hybridised.
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Community Answer
The hybridisations of the atomic orbitals of nitrogen in NO3-, NO2+ an...

Explanation:

NO3-
- Nitrogen in NO3- has a trigonal planar molecular geometry.
- In NO3-, nitrogen forms 3 sigma bonds with oxygen atoms.
- The hybridization of nitrogen in NO3- is sp2. This is because nitrogen forms 3 sigma bonds and has one lone pair of electrons, leading to the sp2 hybridization.

NO2+
- Nitrogen in NO2+ has a linear molecular geometry.
- In NO2+, nitrogen forms 2 sigma bonds with oxygen atoms and has one lone pair of electrons.
- The hybridization of nitrogen in NO2+ is sp. This is because nitrogen forms 2 sigma bonds and has two lone pairs of electrons, leading to the sp hybridization.

NH4+
- Nitrogen in NH4+ has a tetrahedral molecular geometry.
- In NH4+, nitrogen forms 4 sigma bonds with hydrogen atoms.
- The hybridization of nitrogen in NH4+ is sp3. This is because nitrogen forms 4 sigma bonds, leading to the sp3 hybridization.
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