Electrons revolve around their atoms in orbits. In valence bond theory, atomic orbitals of one atom can overlap with the orbitals of other atoms to form a molecule, creating brand new, hybrid orbitals. This phenomenon is known as hybridization. Determining the hybridization of a molecule can help identify its shape and structure. For example, many molecules settle in a shape that minimizes the amount of repulsion between atoms and electrons, creating a shape that requires as little energy as possible to maintain. Knowing the types of shapes a molecule will take when hybridized helps researchers better understand how that molecule may interact with others. Hybridization affects the types of bonds that a molecule can make.
Determine the types of bonds in the molecule by first drawing the chemical structure of the molecule. In particular, note the number of single, double and triple bonds each atom is making. For example, a molecule of carbon dioxide has two double bonds. The molecule can be represented as O=C=O, where each oxygen atom creates a double bond with the central carbon.
Hybridization is defined in terms of sp orbitals. The 's' and 'p' are a way to denote the shape of the orbital paths the electrons travel. For s orbitals, the path is roughly circular. For p orbitals, the shape of the path is more like a dumbbell, with the electron existing primarily in one of two regions rather than in a circular orbit.
Determine each atom's hybridization using the types of bonds present. The presence of no double bonds indicates a hybridization of sp3. An atom with a single double bond has a hybridization of sp2. An atom with two or more double bonds, or with a single triple bond, has a hybridization of sp.
The carbon atom in CO2 has two double bonds, one with each atom of oxygen. Therefore, the carbon's hybridization is sp.
Determine the hybridization for the other atoms in the molecule. Each oxygen atom in CO2 has a single double bond with the carbon. The hybridization of each oxygen is therefore sp2.
Find the overall hybridization of the molecule by determining that of the central atom. In the case of CO2, carbon is the central atom. Because carbon has a hybridization of sp, then the overall hybridization of the molecule is sp.
About the Author
An avid lover of science and health, Meg Michelle began writing professionally about science and fitness in 2007. She holds a bachelor’s degree in physics from Creighton University and master’s degree in science writing from Johns Hopkins. Her work has appeared in publications such as EARTH Magazine.