Hybridization chemistry (Sp3, Sp2, and sp)

is equalization between the energy level through the incorporation of a covalent or covalent compounds orbital hybridization koordination. Hybridization theoretical promoted by chemist Linus Pauling in explaining the structure of molecules such as methane (CH4). Historically, the concept was developed for chemical systems that are simple, but this approach was then applied more widely, and today it is considered as an effective heuristic for rationalizing the structure of organic compounds.

Hybridization theory is not as practical as the molecular orbital theory in terms of quantitative calculations. The problems in hybridization is evident in the bond involving d orbitals, as well as on coordination chemistry and organometallic chemistry. Although hybridisation schemes in transition metal can be used, it is generally inaccurate.

It is important to note that orbitals are a model representation of the behavior of electrons in molecules. In the case of simple hybridisation, this approach is based on the atomic orbitals of hydrogen. Hybridised orbitals is assumed as a combination of atomic orbitals that overlap one another with varying proportions. Orbitals of hydrogen is used as the basis for hybridization schemes because he is one of the few orbital equation Schrödingernya have known analytic solution. Orbitals are then assumed to be distorted a little to atoms heavier such as carbon, nitrogen, and oxygen. With these assumptions, the theory of hybridisation most applicable. It should be noted that we do not need hybridisation to describe molecules, but for molecules composed of carbon, nitrogen, and oxygen, the hybridization theory makes the description easier.

Hybridization theory is often used in organic chemistry, is usually used to describe molecules consisting of atoms C, N, and O (sometimes also P and S). The explanation starts from how an organized bond in methane

a. Sp3 hybridization

Hybridisation describes the bonding atoms from the viewpoint of an atom. For a tetrahedral coordinated carbon (such as methane, CH4), carbon should have orbitals has the right symmetry with four hydrogen atoms.

Carbon ground state configuration is 1s2 2s2 2px1 2py1 or more easily seen:

b. Hybridization sp2

Carbon compounds or other molecules can be explained as described in methane. For example, ethylene (C2H4), which has a double bond between carbon-carbon.

Carbon will perform as orbtial-hybridization sp2 hybrid orbitals will form only sigma bond and one pi bond as required for the double bond between carbon-carbon. Hydrogen-carbon bond has a long and strong connective same. This is consistent with experimental data.

In sp2 hybridization, orbital 2s just joined two 2p orbitals:

c. Hybrid sp

Chemical bonds in compounds such as alkynes with triple bonds is explained by hybridization sp.

In this model, only the 2s orbital joining the p-orbital, resulting in two sp orbitals and leaving two p orbitals. Chemical bonds in acetylene (ethyne) consists of sp-sp overlap between the two carbon atoms form sigma bonds, pi bonds and two additional formed by overlapping pp. Each carbon is also bonded to hydrogen with s-sp overlap angle of 180 °.