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Difference Between Ionic Covalent and Hydrogen Bonds
On the differences between ionic bonds, covalent bonds and hydrogen bonds
The formation of all things in the world depends on the force of chemical bonds. Chemical bonds maintain the force between atoms and molecules, while ionic bonds, covalent bonds and hydrogen bonds have different properties and different uses.
Ionic bonds are often born between metals and non-metallic elements. Those with strong metallic properties are prone to lose electrons into cations; those with strong non-metallic properties are prone to obtain electrons into anions. Anions and cations attract electrostatically and form ionic bonds. The force of their bonds comes from the phase of charge, so ionic compounds have high melting points and high boiling points, and can conduct electricity in molten states or aqueous solutions because their ions can move freely. Such as sodium chloride, the sodium atom loses an electron, and the chlorine atom gains an electron. The two are combined by ionic bonds to form a stable crystal structure.
Covalent bonds are not the case, and are mostly found between non-metallic elements. Non-metallic atoms, in order to achieve a stable structure, often share electron pairs, which is the formation of covalent bonds. The electron pairs of covalent bonds, or equally shared by two atoms, are non-polar covalent bonds, such as oxygen molecules, and the two oxygen atoms are connected by non-polar covalent bonds; or they are unevenly shared, and the electron pairs are biased towards atoms with strong electronegativity, which are polar covalent bonds, such as hydrogen chloride molecules. Hydrogen and chlorine are bound by polar covalent bonds. The properties of covalent compounds vary depending on the molecular structure. Most of them have low melting points, and some of them can be ionized and electrically conductive in aqueous solutions.
Hydrogen bonds are different from the previous two. Hydrogen bonds are not strictly chemical bonds, but are a weak interaction between or within molecules. When a hydrogen atom is connected to an atom with a large electronegativity and a small radius (such as fluorine, oxygen, nitrogen), the hydrogen atom is partially positively charged and can attract another atom with a large electronegativity, which is called a hydrogen bond. Although the force of hydrogen bonds is weaker than ionic bonds and covalent bonds, it has a great impact on the properties of substances. For example, water, due to hydrogen bonds, has a higher melting boiling point than hydrides of the same family, and has special physical and chemical properties, such as higher surface tension and specific heat capacity.
Although ionic bonds, covalent bonds, and hydrogen bonds are all elements of matter composition, their essence, formation conditions, and effects on material properties are different. Understanding this, we can know the mystery of the structure and properties of all things, which is of great benefit to chemical research and applications.
The formation of all things in the world depends on the force of chemical bonds. Chemical bonds maintain the force between atoms and molecules, while ionic bonds, covalent bonds and hydrogen bonds have different properties and different uses.
Ionic bonds are often born between metals and non-metallic elements. Those with strong metallic properties are prone to lose electrons into cations; those with strong non-metallic properties are prone to obtain electrons into anions. Anions and cations attract electrostatically and form ionic bonds. The force of their bonds comes from the phase of charge, so ionic compounds have high melting points and high boiling points, and can conduct electricity in molten states or aqueous solutions because their ions can move freely. Such as sodium chloride, the sodium atom loses an electron, and the chlorine atom gains an electron. The two are combined by ionic bonds to form a stable crystal structure.
Covalent bonds are not the case, and are mostly found between non-metallic elements. Non-metallic atoms, in order to achieve a stable structure, often share electron pairs, which is the formation of covalent bonds. The electron pairs of covalent bonds, or equally shared by two atoms, are non-polar covalent bonds, such as oxygen molecules, and the two oxygen atoms are connected by non-polar covalent bonds; or they are unevenly shared, and the electron pairs are biased towards atoms with strong electronegativity, which are polar covalent bonds, such as hydrogen chloride molecules. Hydrogen and chlorine are bound by polar covalent bonds. The properties of covalent compounds vary depending on the molecular structure. Most of them have low melting points, and some of them can be ionized and electrically conductive in aqueous solutions.
Hydrogen bonds are different from the previous two. Hydrogen bonds are not strictly chemical bonds, but are a weak interaction between or within molecules. When a hydrogen atom is connected to an atom with a large electronegativity and a small radius (such as fluorine, oxygen, nitrogen), the hydrogen atom is partially positively charged and can attract another atom with a large electronegativity, which is called a hydrogen bond. Although the force of hydrogen bonds is weaker than ionic bonds and covalent bonds, it has a great impact on the properties of substances. For example, water, due to hydrogen bonds, has a higher melting boiling point than hydrides of the same family, and has special physical and chemical properties, such as higher surface tension and specific heat capacity.
Although ionic bonds, covalent bonds, and hydrogen bonds are all elements of matter composition, their essence, formation conditions, and effects on material properties are different. Understanding this, we can know the mystery of the structure and properties of all things, which is of great benefit to chemical research and applications.
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