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# What is the bond angle of the molecule undergoing ${\mathrm{sp}}^{2}$hybridization?

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## Bond angle:It is defined as the angle between the orbitals containing bonding electron pairs around the central atom in a molecule or complex ion.The bond angle is measured in degrees.It can be obtained experimentally using spectroscopic methods.Hybridization:When an atom undergoes mixing and recasting of two atomic orbitals with almost the same energy levels to form new orbitals of equal number with equivalent energy, maximum symmetry, and a fixed orientation in space is known as hybridization.${\mathrm{sp}}^{2}$ hybridization:When an atom undergoes mixing and recasting of one s and two p orbitals with similar energies to form three new ${\mathrm{sp}}^{2}$hybrid orbitals with equivalent energies, maximum symmetry, and fixed orientation in space is called ${\mathrm{sp}}^{2}$ hybridization.The bond angle of ${\mathrm{sp}}^{2}$ hybridization:The molecules forming ${\mathrm{sp}}^{2}$hybridization have a bond angle of ${120}^{°}$and the geometry is trigonal planar.The repulsion between the bond pair and lone pair of electrons causes the atoms to be at the maximum distance apart causing the bond angle of ${120}^{°}$.A mixture of $\mathrm{s}&\mathrm{p}$ orbitals formed in trigonal symmetry maintains the angle at ${120}^{°}$All the three hybrid orbitals remain in one plane and make an angle of ${120}^{°}$ with one another. Each of the hybrid orbitals formed has a $33.33%\mathrm{s}$ character and $66.66%\mathrm{p}$ character.Example: In boron trichloride ${\mathrm{BCl}}_{3}$ undergoes ${\mathrm{sp}}^{2}$hybridization where there are three sigma bonds with ${120}^{°}$bond angle and trigonal planar geometry.   Suggest Corrections  0      Similar questions
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