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Chloroform Hydrogen Bonding
On the Hydrogen Bonds of Chloroform
Chloroform is also a chemical quality. To determine whether it has hydrogen bonds, the structure and characteristics of its molecules should be investigated in detail.
Chloroform, the molecular formula is $CHCl_ {3} $. The hydrogen atom is attached to the carbon atom, not the highly electronegative atoms such as nitrogen, oxygen, and fluorine. The hydrogen bond is the weak interaction between the hydrogen atom and the electronegative atom with a large and small radius (such as nitrogen, oxygen, and fluorine) after being covalently bonded, and then with another electronegative atom.
In chloroform molecules, although the electronegativity of chlorine is larger than that of carbon, the molecule is polar, but the electronegativity difference between hydrogen and chlorine is not enough to make hydrogen show strong positive electricity, and the atomic radius of chlorine is large, which is difficult to achieve the conditions required for the formation of hydrogen bonds. Therefore, there is no typical hydrogen bond between chloroform molecules.
Or if there is a doubt, in a special environment, chloroform may have a hydrogen-like bond with others. However, strictly speaking, this is not a hydrogen bond in the traditional sense. Therefore, based on conventional cognition and theoretical analysis, chloroform has no true hydrogen bond.
From this perspective, to explore the hydrogen bond of chloroform, it is necessary to analyze the molecular structure and properties in detail according to chemical principles in order to obtain an accurate conclusion.
Chloroform is also a chemical quality. To determine whether it has hydrogen bonds, the structure and characteristics of its molecules should be investigated in detail.
Chloroform, the molecular formula is $CHCl_ {3} $. The hydrogen atom is attached to the carbon atom, not the highly electronegative atoms such as nitrogen, oxygen, and fluorine. The hydrogen bond is the weak interaction between the hydrogen atom and the electronegative atom with a large and small radius (such as nitrogen, oxygen, and fluorine) after being covalently bonded, and then with another electronegative atom.
In chloroform molecules, although the electronegativity of chlorine is larger than that of carbon, the molecule is polar, but the electronegativity difference between hydrogen and chlorine is not enough to make hydrogen show strong positive electricity, and the atomic radius of chlorine is large, which is difficult to achieve the conditions required for the formation of hydrogen bonds. Therefore, there is no typical hydrogen bond between chloroform molecules.
Or if there is a doubt, in a special environment, chloroform may have a hydrogen-like bond with others. However, strictly speaking, this is not a hydrogen bond in the traditional sense. Therefore, based on conventional cognition and theoretical analysis, chloroform has no true hydrogen bond.
From this perspective, to explore the hydrogen bond of chloroform, it is necessary to analyze the molecular structure and properties in detail according to chemical principles in order to obtain an accurate conclusion.
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