Let's talk about how to determine the type of hybridization, and also consider the geometric structure of the molecule.
History of the term
At the beginning of the twentieth century, L. Pauling proposed a theory of the geometry of molecules with covalent bonds. The basis for the formation of communication was taken to overlap electronic clouds. The method began to be called valence bonds. How to determine the type of hybridization of atoms in compounds? The author of the theory suggested taking 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 a mixing of electronic orbitals. This process is accompanied by the distribution of energy in them, a change in their shape. Depending on how much s- and p-orbitals will be mixed, the type of hybridization may be different. In organic compounds, a carbon atom can exist in the state of sp, sp2, sp3. There are more complex forms in which, in addition to sp, d-orbitals, are involved.
Rules for the identification of inorganic substances in molecules
A hybridization variant can be revealed for compounds with a covalent chemical bond having the ABP type. A is the main atom, B is the ligand, and n is a number from two or more. In such a situation, only the valence orbitals of the main atom will enter into hybridization.
Determination methods
Let's talk in more detail about how to determine the type of hybridization. In chemical terms, this term implies a change in the energy and shape of the orbitals. A similar process is observed in those cases when electrons that belong to different types are used to form bonds.
To understand how to determine the type of hybridization, consider a methane molecule. This substance is the first representative of the homologous series of saturated (saturated) hydrocarbons. In space, the CH4 molecule is a tetrahedron. A single carbon atom forms bonds with hydrogens that are similar in energy and length. In order to form such hybrid clouds, three p and one ES electrons are used.
Four clouds mix, and four identical (hybrid) species appear, having the shape of an irregular figure eight. This type of sp3 hybridization is called. All hydrocarbons, which contain only simple (single) bonds, are characterized by this type of hybridization of the carbon atom. The valence angle is 109 degrees 28 minutes.
We continue the discussion on how to determine the type of hybridization. Examples of unsaturated hydrocarbons of a number of ethylene give an idea of sp2 hybridization. For example, in an ethylene molecule of four valence electrons , only three are used in the formation of a chemical bond. The remaining non-hybrid p-electron is spent on the formation of a double bond.
Acetylene is the simplest representative of the class SpN2p-2. A feature of this class of hydrocarbons is the presence of a triple bond. Of the four valence electrons of a carbon atom, only two change their shape and energy, becoming hybrid. The two remaining electrons take part in the formation of two double bonds, determining the unsaturated nature of this class of organic compounds.
Conclusion
When considering the issue of covalent chemical bonds for organic and inorganic substances, the hybridization of atomic orbitals is taken into account . In this case, their energy and shape are aligned. 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.