Is hybrid orbital theory important in organic chemistry?

Hybrid orbital theory is very important in organic chemistry, and understanding hybrid orbital theory can be a good help to understand the configuration of molecules in organic chemistry. The hybrid orbital theory (proposed by Pauling L et al. in 1931 on the basis of valence bond theory, it is still essentially a modern valence bond theory, but it enriches and develops the modern valence bond theory in terms of bonding ability and spatial configuration of molecules.

Hybrid Orbital Essentials:

1.In the process of bonding, due to the interaction between atoms, several different types of atomic orbitals with similar energy (i.e., wave function) in the same atom can be linearly combined, redistribute energy and determine the spatial direction, and form a new atomic orbital with an equal number of equals.

2.The angular function of the hybrid orbital in a certain direction is much larger than that before hybridization, which is more conducive to the maximum overlap between atomic orbitals, so the hybrid orbital has a stronger bonding ability than the original orbital (the orbital is bonded after hybridization).

The shape of the electron cloud.

3.The hybrid orbitals try to take the maximum angle distribution in space, so that the repulsion energy between them is minimized, so the bond formed is relatively stable. Different types of hybrid orbitals have different angles between them, and the molecules formed after bonding have different spatial configurations.

Hybrid orbitals: a modern valence bond theory.

It is very important, and it will be used in the literature or research in the future, and if you look at it carefully, you will find that it is not very difficult. Take a good look at the chapter on atomic structure first (if you forgot it) and then look at the valence bond theory, which will have the effect of doing more with less.

The undergraduate level is not important. If it is a graduate professional course, it will not exceed 8 points.

Organic or mainly depends on the properties of organic compounds in the previous chapters.

Of course, the spectrum in organic is much more important than hybridization.

The latter sugars, proteins, steroids, etc., are slightly more important than hybridization.

The concept of hybridization is one of the two core concepts of valence bond theory (the other is resonance theory), and valence bond theory is the earliest chemical bond theory developed in history. Personally, I think that the later developed molecular orbital theory has a better interpretation of the bonding of organic molecules, but in fact, the two are in the same way. The organic keys are structure, bonding, and reactivity.

Therefore, molecular orbital theory and valence bond theory (including the concepts of hybridization and resonance) are very important for learning organic. You don't have to look at inorganic hybridization, just look for an organic textbook, and the better organic textbooks must start with bonding.

important, the basis of microchemistry.

1) Hybrid orbitals.

The basic points of the theory:

Atomic orbitals with similar energies.

in order to participate in hybridization.

The hybrid orbit is large at one end and small at the other, with an electron cloud.

The dense end overlaps with the atomic orbital of the bonding atom in the direction of the bond axis, forming a bond.

Due to the greater overlap of atomic orbitals after hybridization, covalent bonds are formed.

It is more stable than the covalent bond formed by the original atomic orbitals.

The hybrid orbital has the same energy and the same composition, for example, each sp3 hybrid orbital occupies 1 s orbital and 3 p orbitals.

The total number of hybrid orbitals is equal to the sum of the number of atomic orbitals involved in hybridization.

2) the relationship between the hybrid orbitals of s and p and the geometry of simple molecules.

3) Application range of hybrid orbitals: Hybrid orbitals should only be used to form bonds or to accommodate lone pairs of electrons that do not participate in bond formation.

4) The method of judging the hybridization mode of the central atom: see whether the central atom has formed a double bond or a triple bond, if there is one triple bond, then there are two bonds.

Two p orbitals are used, and sp hybridization is formed; If there is 1 double bond, then there is 1 bond in it, forming sp2 hybridization; If all the socks are single-bonded, sp 3 hybridization is formed.

The hybrid orbital theory is a scientific theory. In the process of forming a polyatomic molecule, several atomic orbitals of the central atom with similar energy are recombined to form a new set of orbitals, and this process is called the hybridization of orbitals, and the resulting new orbitals are called hybrid orbitals.

Take, for example, the formation of the CH4 molecule. The outer electron configuration of the ground state c atom is 2s22px12py1. On binding to the H atom, one electron on 2S is excited into the 2pz orbital, and the C atom participates in the chemical binding in the excited state 2S12Px12py12PZ1.

Of course, it takes energy for an electron to be excited from 2s to 2p, but it is compensated by the fact that two more covalent bonds can be generated, releasing more energy. Before bonding, the four single-electron orbitals 2S, 2px, 2py, 2pz of the excited C atom will be with each other"Miscellaneous", linearly combined into four new fully equivalent hybrid orbitals. This hybrid orbital is formed by the hybridization of one s orbital and three p orbitals, so it is called sp3 hybrid orbital.

The hybrid orbitals are large at one end and small at the other, and their direction is directed towards the four vertex angles of the regular tetrahedron, and the energy is different from the original atomic orbitals. The four sp3 hybrid orbitals formed overlap with the 1s atomic orbitals of the four h atoms to form (sp3-s) bonds, resulting in the formation of ch4 molecules. Because the electron cloud distribution of the hybrid orbital is more concentrated, the bonding ability of the hybrid orbital is stronger than that of the unhybridized atomic orbitals, so the energy of the system decreases and the stability of the molecule is enhanced after the formation of the CH4 molecule.

I'm asking about the pros and cons.

In general, the hybrid orbital theory only considers the hybridization and bonding of the central atom, but does not consider the influence of the spatial position of the ligand. However, in the case of a large number of ligands and complex spatial structure, there are many alternative orbitals for hybrid orbitals, and various combinations need to be considered, and the explanatory ability is weak. Valence electrons are mutual.