Dianfeng Chemical
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Intermolecular Forces in Hydrogen Sulfide
The intermolecular force in hydrogen sulfide
There must be a reason for the accumulation and dispersion of the material. For hydrogen sulfide ($H_2S $), the intermolecular force is very important.
There is a van der Waals force between the molecules of hydrogen sulfide. This force covers the dispersion force, the induction force and the orientation force. The dispersion force is caused by the instantaneous displacement of electrons in the molecule, resulting in the generation of the instantaneous dipole of the molecule, and the interaction between adjacent molecules. Although hydrogen sulfide molecules are polar, the dispersion force still accounts for a large proportion of the intermolecular force. Because of the relatively large electron cloud of sulfur atoms, the movement of electrons is prone to instantaneous dipoles, which in turn produces dispersion force.
Inductive force, when the polar molecule is adjacent to the non-polar molecule, the inherent dipole of the polar molecule deforms the electron cloud of the non-polar molecule, generating an induced dipole, and the interaction between the two is the inductive force. In the hydrogen sulfide system, if there are non-polar molecules coexisting with it, there will be this force.
Orientation force exists between polar molecules. Hydrogen sulfide is a polar molecule, and its molecular inherent dipole interaction makes the molecules tend to be aligned. This interaction force is the orientation force.
In addition, there is no hydrogen bond between hydrogen sulfide molecules compared with water molecules. The formation of hydrogen bonds requires hydrogen atoms to be connected to atoms with large electronegativity and small radius (such as fluorine, oxygen, and nitrogen). The electronegativity of sulfur atoms is smaller than that of oxygen and other atoms, so it is difficult to form hydrogen bonds between hydrogen sulfide molecules. This difference makes the physical properties of hydrogen sulfide, such as boiling point and melting point, different from those of substances containing hydrogen bonds.
In summary, the intermolecular forces of hydrogen sulfide are mainly van der Waals forces, and there is no hydrogen bond. This property profoundly affects many of its physical and chemical properties.
There must be a reason for the accumulation and dispersion of the material. For hydrogen sulfide ($H_2S $), the intermolecular force is very important.
There is a van der Waals force between the molecules of hydrogen sulfide. This force covers the dispersion force, the induction force and the orientation force. The dispersion force is caused by the instantaneous displacement of electrons in the molecule, resulting in the generation of the instantaneous dipole of the molecule, and the interaction between adjacent molecules. Although hydrogen sulfide molecules are polar, the dispersion force still accounts for a large proportion of the intermolecular force. Because of the relatively large electron cloud of sulfur atoms, the movement of electrons is prone to instantaneous dipoles, which in turn produces dispersion force.
Inductive force, when the polar molecule is adjacent to the non-polar molecule, the inherent dipole of the polar molecule deforms the electron cloud of the non-polar molecule, generating an induced dipole, and the interaction between the two is the inductive force. In the hydrogen sulfide system, if there are non-polar molecules coexisting with it, there will be this force.
Orientation force exists between polar molecules. Hydrogen sulfide is a polar molecule, and its molecular inherent dipole interaction makes the molecules tend to be aligned. This interaction force is the orientation force.
In addition, there is no hydrogen bond between hydrogen sulfide molecules compared with water molecules. The formation of hydrogen bonds requires hydrogen atoms to be connected to atoms with large electronegativity and small radius (such as fluorine, oxygen, and nitrogen). The electronegativity of sulfur atoms is smaller than that of oxygen and other atoms, so it is difficult to form hydrogen bonds between hydrogen sulfide molecules. This difference makes the physical properties of hydrogen sulfide, such as boiling point and melting point, different from those of substances containing hydrogen bonds.
In summary, the intermolecular forces of hydrogen sulfide are mainly van der Waals forces, and there is no hydrogen bond. This property profoundly affects many of its physical and chemical properties.
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