Nitrogen trifluoride (NF3) Molecule Shape, Geometry, Hybridization
Nitrogen trifluoride (NF3) lewis structure contains three sigma bonds and one lone pair around nitrogen atom. Therefore, there are total of four electrons regions around nitrogen atom. So, hybridization of center atom, nitrogen is sp3. Because there are four electrons regions, geometry is tetrahedral and shape is trigonal pyramidal.
Nitrogen trifluoride (NF3) lewis structure
To decide the geometry, shape and hybridization of a molecule, drawing the correct lewis structure is very important as the initial step.
Number of electron regions in nitrogen trifluoride
Total electron region is taken by the summation of sigma bonds and lone pairs around relevant atom from drawn lewis structure.
Number of electron regions around nitrogen atom in NF3
According to the lewis structure given above, there are three sigma bonds and one lone pair around the nitrogen atom. Therefore, total number of electron regions around nitrogen atom is four.
Geometry and shapes of molecules according to the number of electron regions
You can decide geometry and shapes of molecules from following table according to the number of electron regions.
- Geometry is decided by the total number of electron regions.
- Shape of molecule is decided by how many lone pairs and how many sigma bonds are located around the center atom under specific total number of electron regions.
Geometry around nitrogen atom in NF3
Because, number of electron regions around nitrogen atom is four, geometry should be tetrahedral.
Molecular shape of NF3
Because, there are three sigma bonds and one lone pair around nitrogen atom, molecular shape of NF3 molecule is trigonal pyramidal.
Hybridization of NF3 molecule
Hybridization is also decided by the number of electron regions around an atom. A table is given below for identifying hybridization.
Because number of electron regions around nitrogen atom is four, hybridization of nitrogen atom is sp3
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