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How Hydrogen Bond Is Formed
"On the Formation of Hydrogen Bonds"
The hydrogen bond is a wonderful structure of chemistry. Its formation is not achieved overnight, but is based on the combination of various elements.
Hydrogen atoms are reactive and often combine with atoms with strong electronegativity, such as fluorine, oxygen, and nitrogen. When hydrogen bonds with atoms such as Si, due to their unique electronegativity, the distribution of charges is uneven. One end of hydrogen is slightly positively charged, and the positively charged hydrogen then attracts electrons to the electron-rich regions in adjacent molecules, especially the lone pair of electronegativity atoms.
This attraction force is extraordinary, so it forms a hydrogen bond. Although its force is weaker than covalent bonds, it has a huge impact on the properties of matter. Looking at the characteristics of water, its boiling point is different from common sense, and the work of real hydrogen bonds is also. The molecules of water are connected by hydrogen bonds, and in order to gasify them, it is necessary to break this hydrogen bond, so the energy needs to be quite large, and the boiling point is high.
In biological systems, the importance of hydrogen bonds is also recognized. The structure of proteins depends on hydrogen bonds to maintain their folded state; the base pairing of nucleic acids is also based on hydrogen bonds, so as to obtain accurate transmission of genetic information.
From this perspective, the formation of hydrogen bonds is related to the difference in atomic electronegativity, the distribution of electric charges, and the interaction between molecules. This subtle combination is responsible for the wonders of the chemical and biological worlds.
The hydrogen bond is a wonderful structure of chemistry. Its formation is not achieved overnight, but is based on the combination of various elements.
Hydrogen atoms are reactive and often combine with atoms with strong electronegativity, such as fluorine, oxygen, and nitrogen. When hydrogen bonds with atoms such as Si, due to their unique electronegativity, the distribution of charges is uneven. One end of hydrogen is slightly positively charged, and the positively charged hydrogen then attracts electrons to the electron-rich regions in adjacent molecules, especially the lone pair of electronegativity atoms.
This attraction force is extraordinary, so it forms a hydrogen bond. Although its force is weaker than covalent bonds, it has a huge impact on the properties of matter. Looking at the characteristics of water, its boiling point is different from common sense, and the work of real hydrogen bonds is also. The molecules of water are connected by hydrogen bonds, and in order to gasify them, it is necessary to break this hydrogen bond, so the energy needs to be quite large, and the boiling point is high.
In biological systems, the importance of hydrogen bonds is also recognized. The structure of proteins depends on hydrogen bonds to maintain their folded state; the base pairing of nucleic acids is also based on hydrogen bonds, so as to obtain accurate transmission of genetic information.
From this perspective, the formation of hydrogen bonds is related to the difference in atomic electronegativity, the distribution of electric charges, and the interaction between molecules. This subtle combination is responsible for the wonders of the chemical and biological worlds.
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