Let's talk about how to determine the type of hybridization

Let's talk about how to determine the type of hybridization, and also consider the geometric structure of the molecule.

History of appearance

At the beginning of the twentieth century, L. Pauling proposed a theory of the geometry of molecules with a covalent bond. As a basis for the formation of communication, the overlapping of electron clouds was taken. The method was called valence bonds. How to determine the type of hybridization of atoms in compounds? The author of the theory proposed to take into account the mixing of hybrid orbitals.

Definition

In order to understand how to determine the type of hybridization in compounds, let us examine what this term means.

Hybridization is the mixing of electronic orbitals. This process is accompanied by the distribution of energy in them, a change in their form. Depending on how much s- and p-orbitals are mixed, the type of hybridization can be different. In organic compounds, the carbon atom can exist in the state sp, sp2, sp3. There are more complex forms in which, besides sp, d-orbitals participate.

Rules for the detection of inorganic substances in molecules

Identify the hybridization option is possible for compounds with a covalent chemical bond, having the type ABp. A is a basic atom, B is a ligand, n is a number from two or more. In such a situation, only the valence orbitals of the main atom will be involved in the hybridization.

The methods for determining

Let's talk in more detail about how to determine the type of hybridization. In the chemical sense, this term implies a change in the energy and shape of the orbitals. A similar process is observed in those cases where electrons are used to form the bond, which belong to different types.

To understand how to determine the type of hybridization, consider the methane molecule. This substance is the first representative of the homologous series of saturated (limiting) hydrocarbons. In space, the CH4 molecule is a tetrahedron. The single carbon atom forms bonds with hydrogen, similar in energy and length. In order to form such hybrid clouds, three p-and one es-electron are used.

Four clouds are mixed, and there are four identical (hybrid) species, having the form of an irregular figure-eight. This type of hybridization is called sp3. All hydrocarbons, which contain only simple (single) bonds, are characterized by this type of hybridization of a carbon atom. The valentine angle is 109 degrees 28 minutes.

We will continue our discussion on how to determine the type of hybridization. Examples of unsaturated hydrocarbons of the ethylene series give an idea of sp2-hybridization. For example, in an ethylene molecule of four valence electrons in the formation of a chemical bond, only three are used. The remaining non-hybrid p-electron goes to the formation of a double bond.

Acetylene is the simplest representative of the class CnH2n-2. A feature of this class of hydrocarbons is the presence of a triple bond. Of the four valence electrons of the carbon atom, only two change their form and energy, becoming hybrid. The two remaining electrons participate in the formation of two double bonds, determining the unsaturated nature of this class of organic compounds.

Conclusion

Considering the question of the covalent chemical bond for organic and inorganic substances, allow for the hybridization of atomic orbitals. This aligns their energy and shape. An electron located near the nucleus of a bound atom is characterized by a set of orbitals that have the same quantum number. Information on the type of hybridization makes it possible to evaluate the chemical properties of a substance.