Hybridization, in summary and simple explanation, is the combination and transformation of the original orbitals of an atom forming special orbitals to have the ability to bond with others. When an atom undergoes and undergoes a hybridization process, the electronic model is modified to represent it using special orbitals to form new molecules. Since it is already known that only valence electrons are used in the bonding of atoms or molecules, the valence orbitals only change externally. Therefore, hybridization does not add or remove the original orbitals associated with an atom but simply refigures them. There are five types of atomic hybridization: sp, sp2, sp3, dsp3 and d2sp3. Each type has its own number of groups, also called electron pairs, bond angle, and geometry. The first type of atomic hybridization is sp. In sp hybridization, a pair of orbitals arranged in opposite directions from each other is required for two pairs of electrons in an atom. An example of where sp hybridization most often occurs is the carbon atom of carbon dioxide, which contains one carbon and two oxygens. The two transformed special orbitals are s and p. Rather than having the original three 2p and one 2s orbitals, the carbon atom in carbon dioxide now has two 2p and two sp orbitals. A hybridized carbon atom and a normal carbon atom have the same number of orbitals, except that they are modified to bind both oxygens more efficiently. The bond angle in sp hybridization is 180 degrees because the two newly formed sp orbitals are in a straight line and directly opposite each other. Geometry is linear for the same reason. Another example of sp orbital hybridization occurs in a magnesium hydride atom, where the 3s and one of the original 3p orbitals co...... middle of paper ...... effective orbitals and specially designed rather than leaving it with its original orbitals. In turn, this provides us with stronger molecules that we can use in everyday necessities like plastic and gas. If it weren't for the hybridization of atoms, we might not have some of the things we take for granted. We have atoms and hybridization to thank for working so hard to be better. Works Cited Steven S. Zumdahl and Susan A. Zumdahl (2010). Chemistry. Belmont, CA: Brooks Cole, Richard F. Daley, and Sally J. Daley (2005). Organic Chemistry. New York, NY: HarperCollinsFrancis, E. (2003) Types of Hybridization. Dl.clackamas.cc.or.us Retrieved November 17, 2013 from dl.clackamas.cc.or.us/ch106-02/typesof.htm Harpreet, C. Hybrid orbitals. Chemwiki.ucdavis.edu. Retrieved November 20, 2013, from chemwiki.ucdavis.edu/Organic_Chemistry/Fundamentals/Hybrid_Orbitals