Shanxian Chemical
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Dipole Dipole Dispersion Hydrogen Bonding
The theory of physical properties
The physical properties of the world are complex, among which the dipole-dipole interaction (Dipole-Dipole), the dispersion force (Dispersion) and the hydrogen bond (Hydrogen Bonding) are particularly critical.
The dipole-dipole interaction originates from the polarity of the molecule. Polar molecules have positive and negative charge centers, and opposite charges attract each other. This effect is quite significant in polar substances. Such as halogenated hydrogen gas, hydrogen chloride (HCl) molecules have uneven charge distribution due to the stronger electronegativity of chlorine than hydrogen. Many hydrogen chloride molecules attract each other due to dipole-dipole interaction, which affects their melting and boiling points.
Dispersion force exists in all molecules. The constant movement of electrons in the molecule will instantaneously cause the uneven distribution of electron clouds, resulting in instantaneous dipoles. Neighboring molecules are affected by this, and dipoles are also induced, and mutual attraction is the dispersion force. Although its force is relatively weak, for non-polar molecules, such as rare gases, this force dominates their intermolecular interactions, which is related to their condensed properties. Such as argon, which is composed of non-polar argon atoms, condenses into liquids at low temperatures by dispersion force.
Hydrogen bonds are special intermolecular forces. When hydrogen atoms are covalently bonded with atoms with large electronegativity and small radius (such as fluorine, oxygen, and nitrogen), the hydrogen nucleus is exposed, and it will attract the lone pair of electrons of such electronegative large atoms in another molecule, forming a hydrogen bond. In water (H _ 2O), hydrogen binds to oxygen and forms hydrogen bonds between water molecules. Hydrogen bonds make the melting and boiling point of water abnormally high, and have a profound impact on the properties of water such as density and solubility.
These three, dipole-dipole interaction, dispersion force, and hydrogen bond, are the key to the relationship between the microstructure of matter and macroscopic properties, such as intertwined veins, left and right physical properties, which are the keys to the exploration of microscopic physical properties. Scholars must study the reasons.
The physical properties of the world are complex, among which the dipole-dipole interaction (Dipole-Dipole), the dispersion force (Dispersion) and the hydrogen bond (Hydrogen Bonding) are particularly critical.
The dipole-dipole interaction originates from the polarity of the molecule. Polar molecules have positive and negative charge centers, and opposite charges attract each other. This effect is quite significant in polar substances. Such as halogenated hydrogen gas, hydrogen chloride (HCl) molecules have uneven charge distribution due to the stronger electronegativity of chlorine than hydrogen. Many hydrogen chloride molecules attract each other due to dipole-dipole interaction, which affects their melting and boiling points.
Dispersion force exists in all molecules. The constant movement of electrons in the molecule will instantaneously cause the uneven distribution of electron clouds, resulting in instantaneous dipoles. Neighboring molecules are affected by this, and dipoles are also induced, and mutual attraction is the dispersion force. Although its force is relatively weak, for non-polar molecules, such as rare gases, this force dominates their intermolecular interactions, which is related to their condensed properties. Such as argon, which is composed of non-polar argon atoms, condenses into liquids at low temperatures by dispersion force.
Hydrogen bonds are special intermolecular forces. When hydrogen atoms are covalently bonded with atoms with large electronegativity and small radius (such as fluorine, oxygen, and nitrogen), the hydrogen nucleus is exposed, and it will attract the lone pair of electrons of such electronegative large atoms in another molecule, forming a hydrogen bond. In water (H _ 2O), hydrogen binds to oxygen and forms hydrogen bonds between water molecules. Hydrogen bonds make the melting and boiling point of water abnormally high, and have a profound impact on the properties of water such as density and solubility.
These three, dipole-dipole interaction, dispersion force, and hydrogen bond, are the key to the relationship between the microstructure of matter and macroscopic properties, such as intertwined veins, left and right physical properties, which are the keys to the exploration of microscopic physical properties. Scholars must study the reasons.
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