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Ionic Covalent Hydrogen Bonds Comparison
Comparison of chemical bonds
Everything in the world is composed of particles, and there are chemical bonds between the particles, so that the material has a stable structure. Among the chemical bonds, ionic bonds, covalent bonds and hydrogen bonds are very important, and they are compared in detail today.
Ionic bonds are formed by strong electrostatic interaction between anions and cations. Active metals and active non-metals meet, and metal atoms are prone to lose electrons into cations. Non-metallic atoms are prone to electrons into anions. Anions and cations are combined by electrostatic attractive forces to form ionic bonds. For example, sodium chloride, a sodium atom loses an electron to form a sodium ion, and a chlorine atom gains an electron to form a chloride ion. The two are combined by ionic bonds. When ionic bonds are formed, electrons transfer to form ionic compounds. Such compounds usually have high melting and boiling points, and require more energy to destroy due to strong ionic bonds. They can conduct electricity in molten or aqueous solutions, because anions and cations can move freely.
Covalent bonds are different, which are the interactions between atoms formed by sharing electron pairs. Non-metallic atoms are mostly bound in this way, because they have similar electron gain and loss abilities, making it difficult to transfer electrons. Like hydrogen molecules, two hydrogen atoms each provide one electron to form a common electron pair, which is a covalent bond. Covalent bonds are divided into polar covalent bonds and non-polar covalent bonds. Covalent bonds formed by different kinds of atoms, due to the different atom attraction ability to electrons, the common electron pair is biased towards the atom with strong electron attraction ability. This is a polar covalent bond, such as hydrogen chloride; the covalent bond formed by the same kind of atom, the common electron pair is not offset, and it is a non-polar covalent bond, such as oxygen. Substances formed by covalent bonds have large differences in melting and boiling points. Like diamond, atoms are connected by covalent bonds to form a spatial network structure, and the melting point is extremely high; while some covalent compounds, such as carbon dioxide, are bound by weak intermolecular forces, and the melting point is low. Most covalent compounds do not conduct electricity in the molten state, and some can conduct electricity in aqueous solutions due to ionized ions.
Hydrogen bond is different from the above two. It is not a real chemical bond, but a strong intermolecular force. After the hydrogen atom is covalently bonded with atoms with large electronegativity and small radius (such as fluorine, oxygen, nitrogen), the hydrogen atom is partially positively charged and can generate electrostatic attraction with lone pairs of electrons in another electronegativity and small radius atom, which is called hydrogen bond. If there are hydrogen bonds between water molecules, the melting boiling point of water is higher than that of hydrides of the same family. Because hydrogen bonds enhance the intermolecular force, more energy is required to destroy. Hydrogen bonds have a significant impact on the properties of substances, not only affecting the melting boiling point, but also affecting the solubility of substances. For example, ammonia is highly soluble in water, which is related to the formation of hydrogen bonds between ammonia molecules and water molecules.
In summary, ionic bonds, covalent bonds and hydrogen bonds have their own characteristics. Ionic bonds are based on the electrostatic interaction of anions and cations to form ionic compounds; covalent bonds bind atoms with shared electron pairs; hydrogen bonds, as special intermolecular forces, have unique effects on the properties of substances. Only by discerning the three can we know the wonders of the structure and properties of substances.
Everything in the world is composed of particles, and there are chemical bonds between the particles, so that the material has a stable structure. Among the chemical bonds, ionic bonds, covalent bonds and hydrogen bonds are very important, and they are compared in detail today.
Ionic bonds are formed by strong electrostatic interaction between anions and cations. Active metals and active non-metals meet, and metal atoms are prone to lose electrons into cations. Non-metallic atoms are prone to electrons into anions. Anions and cations are combined by electrostatic attractive forces to form ionic bonds. For example, sodium chloride, a sodium atom loses an electron to form a sodium ion, and a chlorine atom gains an electron to form a chloride ion. The two are combined by ionic bonds. When ionic bonds are formed, electrons transfer to form ionic compounds. Such compounds usually have high melting and boiling points, and require more energy to destroy due to strong ionic bonds. They can conduct electricity in molten or aqueous solutions, because anions and cations can move freely.
Covalent bonds are different, which are the interactions between atoms formed by sharing electron pairs. Non-metallic atoms are mostly bound in this way, because they have similar electron gain and loss abilities, making it difficult to transfer electrons. Like hydrogen molecules, two hydrogen atoms each provide one electron to form a common electron pair, which is a covalent bond. Covalent bonds are divided into polar covalent bonds and non-polar covalent bonds. Covalent bonds formed by different kinds of atoms, due to the different atom attraction ability to electrons, the common electron pair is biased towards the atom with strong electron attraction ability. This is a polar covalent bond, such as hydrogen chloride; the covalent bond formed by the same kind of atom, the common electron pair is not offset, and it is a non-polar covalent bond, such as oxygen. Substances formed by covalent bonds have large differences in melting and boiling points. Like diamond, atoms are connected by covalent bonds to form a spatial network structure, and the melting point is extremely high; while some covalent compounds, such as carbon dioxide, are bound by weak intermolecular forces, and the melting point is low. Most covalent compounds do not conduct electricity in the molten state, and some can conduct electricity in aqueous solutions due to ionized ions.
Hydrogen bond is different from the above two. It is not a real chemical bond, but a strong intermolecular force. After the hydrogen atom is covalently bonded with atoms with large electronegativity and small radius (such as fluorine, oxygen, nitrogen), the hydrogen atom is partially positively charged and can generate electrostatic attraction with lone pairs of electrons in another electronegativity and small radius atom, which is called hydrogen bond. If there are hydrogen bonds between water molecules, the melting boiling point of water is higher than that of hydrides of the same family. Because hydrogen bonds enhance the intermolecular force, more energy is required to destroy. Hydrogen bonds have a significant impact on the properties of substances, not only affecting the melting boiling point, but also affecting the solubility of substances. For example, ammonia is highly soluble in water, which is related to the formation of hydrogen bonds between ammonia molecules and water molecules.
In summary, ionic bonds, covalent bonds and hydrogen bonds have their own characteristics. Ionic bonds are based on the electrostatic interaction of anions and cations to form ionic compounds; covalent bonds bind atoms with shared electron pairs; hydrogen bonds, as special intermolecular forces, have unique effects on the properties of substances. Only by discerning the three can we know the wonders of the structure and properties of substances.
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