Determine the hybridization and the approximate bond angle of the labeled atom in the following molecule:
During hybridization, atomic orbitals of nearly equal energy combine to form an equal number of hybridized orbitals.
While finding hybridization, we only consider sigma bonds and lone pairs of the central atom.
Hence each single, double, triple bond, and lone pair is considered as a single electron density.
For 2 electron densities taken together, hybridization = sp.
For 3 electron densities taken together, hybridization = sp2.
For 4 electron densities taken together, hybridization = sp3.
For 5 electron densities taken together, hybridization = sp3d.
When there is no lone pair, bond angle is 180 for sp, 120 for sp2, and 109.28 for sp3.
Bond angle decrease from the above normal bond angles, where there is lone pair(s).
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