A basic introduction to chemical bonds, as well as precautions. Be as detailed as possible!!

Ahhh

This data is ** on the map, and the final result is subject to the latest data on the map.

Chemical bond refers to the strong interaction force between two or more adjacent atoms (or ions) within a molecule or crystal. High definition: The force that binds ions or atoms together is commonly known as chemical bonds.

There are 3 limit types of chemical bonds, namely ionic bonds, covalent bonds, and metallic bonds. Ionic bonds are the mutual attraction of oppositely charged ions, such as chlorine and sodium bonded together to form sodium chloride. A covalent bond is an attraction created by two or more atoms by sharing a pair of electrons, and a typical covalent bond is formed by two atoms by attracting a pair of bonding electrons.

For example, two hydrogen nuclei attract a pair of electrons at the same time, forming a stable hydrogen molecule. Metallic bonds, on the other hand, are interactions that bind metal atoms together and can be seen as highly delocalized covalent bonds. A chemical bond that is positioned between two atoms is called a localized bond.

A polycentric bond formed by the common electrons of multiple atoms is called a delocalized bond. The metal ions are fixed to the lattice junction and are in the "ocean" of delocalized electrons. In addition to this, there are also transition types of chemical bonds:

Due to the difference in the magnitude of the attraction of particles to electrons, the covalent bond that skews the bond electrons to one side is called a polar bond, and the chemical bond that provides the bonding electrons by one side is called a coordination bond. The limits of both ends of a polar bond are ionic and non-polar bonds, and the limits of both ends of a delocalized bond are a localized bond and a metallic bond.

1 Pinyin 2 Annotations.

huà xué jiàn

The strong interaction between two or more adjacent atoms (ions) in a molecule or crystal is called a chemical bond. Chemical bonding should first emphasize intramolecular. Molecular interactions, van der Waals forces, or hydrogen bonds are not considered chemical bonds.

Interactions mainly refer to neighboring atoms. Non-neighboring atoms also interact with each other, but weakly, only a few percent of the former. In addition to the strong interaction between the two adjacent tremor chain atoms, some polyatomic molecules also form chemical bonds through conjugation, such as delocalized bonds in conjugated molecules such as benzene, butadiene [1, 3], and NO2.

In NaCl crystals, an infinite number of ions interact with each other to form ionic bond slag suspicions. Strong interactions predict the strength of the chemical bonds, which can be quantitatively estimated using bond energies. The bond energy of a general chemical bond is 100 to several hundred kj mol.

The bond energy of hydrogen bonding is about 40kJ mol or less. The formation of chemical bonds holds atoms firmly together into molecules in a certain way, so it is the fundamental reason for the stable existence of molecules or crystals. The main types of chemical bonds are ionic bonds, covalent bonds (including coordination bonds), and metallic bonds.

The essence of chemical bonds mainly revolves around the study of the genesis of covalent bonds, and the chemical bond theory with valence bond theories such as hole hands, molecular orbital theory and coordination field theory as the main body has been formed.

Chemical bond is a general term for the strong interaction force between two or more adjacent atoms (or ions) within a pure molecule or crystal. The force that binds ions or atoms together is known as chemical bonding.

Ionic bonds, covalent bonds, and metallic bonds have different causes, and ionic bonds are formed by electrostatic action through the transfer of electrons between atoms to form positive and negative ions. The causes of covalent bonds are complex and <>

Lewis theory believes that covalent bonds are formed by the sharing of one or more pairs of electrons between atoms, and other explanations include valence bond theory, valence shell electron repulsion theory, molecular orbital theory and hybrid orbital theory. A metallic bond is a modified covalent bond that is formed by multiple atoms sharing some free-flowing electrons.

Explanation of chemical bonds.

The interaction between adjacent atoms in a molecule is produced by the interaction of electrons. The chemical structure is denoted by ** ( ).

Word decomposition Interpretation à nature or morphological change : change. Split apart.

Rigidity. Teaching. Melt.

Melt. Exert a subtle influence on. Turn dry into jade silk.

Buddhists and Taoists raise money: turn into a book of Bu Lingyuan. Fasting.

Used after a noun or adjective, it indicates a transformation into a certain nature or state: ugliness. Greening.

Customs, wind.

SO4 )2-, NH3 is a base-bent imitation ion group or molecular head formed by covalent bonding.

The bonds that bind between the ions and the ions (or ion clusters) are (Cu(NH3)4)2+ and (SO4)2- in this question

The most important thing is that Cu 2+ and (NH3)4 (4 ammonia molecules) in the complex are bound by coordination bonds, so they are complexes.

The strong interaction that exists between two or more adjacent atoms in a molecule and crystal.

For example, two covalent bonds are formed between two hydrogen atoms and one oxygen atom in a water molecule, which are strongly bonded together to become a stable H2O molecule. Another example is that in table salt crystals, sodium ions and chloride ions are strongly combined through electrostatic action to form stable NaCl crystals.

Chemical bonds mainly include covalent bonds, ionic bonds, and metallic bonds. Intermolecular forces as well as hydrogen bonds are not chemical bonds. Compared with chemical bonds, the intermolecular force is very weak, and the intermolecular force can be destroyed by providing less energy, so that the substance of the molecular crystal melts, for example, ice is easy to melt into water, and it is the intermolecular force that is destroyed; If water is to be decomposed, high temperatures are required to break the covalent bonds of hydrogen and oxygen.

In the case of ionic bonds, the adjacent atom is the ion, the charged atom.

Ionic bonds: chemical bonds formed between positive and negative charged groups at different parts of the same molecule or on different molecules.

The attraction of anisotropic charges of anions and anions is balanced by the repulsion between the nuclei and the formation of stable ionic bonds.

Take the combination of sodium and chloride to form sodium chloride as an example (as shown in the figure): from the perspective of atomic structure, there is one electron in the outermost electron shell of the sodium atom, which is easy to lose; The chlorine atom has 7 electrons in the outer electron shell and easily gets one electron. When the sodium atom and the chlorine atom meet, the sodium atom loses one of the outermost electrons and becomes a sodium ion, which is positively charged, and the chlorine atom gets the electrons lost by sodium and becomes a negatively charged chloride ion.

Covalent bonds: Chemical bonds formed between atoms by sharing electron pairs.

After reading this, you will understand very well.

You're stupid, you can't ask the teacher.