Explanation:Hybridization is the concept of combining ATOMIC orbitals to make new hybrid orbitals appropriate to represent their properties of bonding. Hybridized orbitals are helpful in describing the shape of molecular orbitals apart from being a major part of valence bond theory. The name hybrid applies to the atomic orbitals that contribute to the hybridization. For example, in methane whose CHEMICAL formula is CH4, a set of sp3 orbitals develops by combining one s-orbital and three p-orbitals on the carbon atom. These orbitals direct towards the four hydrogen atoms placed at the vertices of a regular tetrahedron. Ethene(C2H4) consists of a double bond between the carbon atoms. Here, the carbon hybridizes by sp2. In sp2 hybridization, the 2s orbital mingles with two among the three 2p orbitals available, making total 3sp2 orbitals with one remaining p-orbital. In ethane, two atoms of carbon develop a sigma bond by OVERLAYING two sp2 orbitals, where every carbon atom makes two covalent bonds with hydrogen by overlapping all s-sp2 with 120o angles. The pi bond among the carbon atoms develops by a 2p-2p overlap. The hydrogen-carbon bonds have equal length and strength that satisfies with experimental proof. MANY bonds also exist between non-similar atoms. When two atoms of oxygen are brought near opposite sides of the carbon atom in CO2, one among the p orbitals on every oxygen makes a pi bond with anyone among the p-orbitals of carbon. Here, the sp hybridization forms two double bonds.