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In 1916, American scientist Lewis proposed that when atoms combine with each other, there is a tendency to form a rare gas electronic configuration.
When atoms of an element with poor electronegativity form a bond, they can share electron pairs to achieve the electronic configuration of a rare gas
.
The chemical bonds formed by sharing electron pairs are called covalent bonds, and the molecules formed are called covalent molecules
In the H 2 molecule, two H atoms share a pair of electrons, so that each H atom can reach the 2-electron stable structure of the He atom, and a covalent bond is formed between the two H atoms; in the H 2 O molecule, O atom and 2 H atoms each share a pair of electrons, H atom and O atom both reach the stable electronic configuration of noble gas, O atom and 2 H atoms each form a covalent bond
.
When drawing the Lewis structure, use small black dots to represent electrons, such as
For convenience, a short line is usually used to represent a shared pair of electrons, which means that a single bond is formed; two short lines are used to represent two pairs of electrons shared to form a double bond; and three short lines are used to represent three pairs of electrons to form a triple bond
.
[Example 6-2] Give the Lewis structural formulas of the following molecules or ions, and use short lines to indicate shared electron pairs
.
H 2 , O 2 , N 2 , OH - , NO + , H 2 O, NH2 .
3 , CH .
The solution results are as follows
The Lewis theory can explain that two elements with a small difference in electronegativity can bond to form a stable compound, but it cannot explain the essence of the bond, let alone the fact that the atoms in the molecules of some compounds do not satisfy the electronic configuration of rare gases, such as BCl 3 ( There are only 6 valence electrons around B), PCI 5 (10 valence electrons around P), SeF 6 (12 valence electrons around Se)
Related links: The properties of ionic crystals and the structure of AB-type cubic ionic crystals