Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in `CH_(4)` molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the numbe of atomic orbitals involved is equal to the number of hybrid orbitals formed of equal energy.
According to hybridization theory, the `%s` character in `sp^(3)` hybrid orbitals is :

Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in CH_(4) molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the numbe of atomic orbitals involved is equal to the number of hybrid orbitals formed of equal energy. Increasing order of the energy of hybrid orbitals is :

Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in CH_(4) molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the numbe of atomic orbitals involved is equal to the number of hybrid orbitals formed of equal energy. The number of axial and equatorial positions in trigonal bipyramidal geometry having sp^(3)d hybridizaton are respectively :

The number of hybrid orbitals formed in sp^3 hybridization

The number of hybrid orbitals in a molecule of decane are

Hybridisation is the mixing of atomic orbital of comparable energy and the number of hybrid orbitals formed is equal to the number of pure atomic orbitals mixed up and hybrid are occupied by sigma -bond pair and lone pair. Which of the following geometry is most likely to not form from sp^(3)d hybridisation of the central atom.

Hybridisation is the mixing of atomic orbital of comparable energy and the number of hybrid orbitals formed is equal to the number of pure atomic orbitals mixed up and hybrid are occupied by sigma -bond pair and lone pair. Which of the following geometry is most likely to not form from sp^(3)d hybridisation of the central atom.

As the s-character of a hybrid orbital increases the bond angle

sp^(3) hybrid orbitals have equal s and p characters .