Mixing of pure orbitals having nearly equal energy to form equal number of completely new orbitals is said to be hybridization.
For the compound, [tex]CH_3CH_2CH_3[/tex] the electronic configuration of the atoms, carbon and hydrogen are:
Carbon (atomic number=6): In ground state= [tex]1s^{2}2s^{2}2p^{2}[/tex]
In excited state: [tex]1s^{2}2s^{1}2p^{3}[/tex]
Hydrogen (atomic number=1): [tex]1s^{1}[/tex]
All the bonds in the compound is single bond([tex]\sigma[/tex]-bond) that is they are formed by head on collision of the orbitals.
The structure of the compound is shown in the image.
The Carbon-Hydrogen bond is formed by overlapping of s-orbital of hydrogen to p-orbital of carbon.
In order to complete the octet the required number of electrons for carbon is 4 and for hydrogen is 1. So, the electron in [tex]1s^{1}[/tex] of hydrogen will overlap to the 2p^{3}-orbital of carbon.
Thus, the hybridization of Hydrogen is [tex]s[/tex]-hybridization and the hybridization of Carbon is [tex]sp^{3}[/tex]-hybridization.
The hybridization of each atom is shown in the image.
