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Correct Statements About Hydrogen Bonding
The following is an ancient essay with "Which Of The Following Statements About Hydrogen Bonding Is Correct" as the core and "Correct Statements About Hydrogen Bonding" as the direction:
On Hydrogen Bonding It is said that
Between heaven and earth, everything has its own reason, and the beauty of chemistry, hydrogen bonding is one of them. Now on the theory of hydrogen bonding, which is correct?
The hydrogen bond is not a chemical bond, but its force cannot be underestimated. Its formation also depends on the interaction of hydrogen atoms with atoms with large electronegativity and small radius, such as fluorine, oxygen, and nitrogen. This effect makes the relationship between molecules or within molecules different, and has a profound impact on the properties of substances.
Or: "Hydrogen bonds only exist between molecules." This is not true. In fact, there are also hydrogen bonds in molecules. Looking at o-nitrophenol, its hydroxyl group is similar to the nitro group, and it can form an intramolecular hydrogen bond, resulting in a lower melting boiling point and a lower p-nitrophenol. The effect of this intramolecular hydrogen bond is also known. Therefore, it is known that hydrogen bonds exist between molecules and within molecules, and both are present. This is one of the true theories.
There is another cloud: "The force of hydrogen bonds is always in van der Waals forces." It is true that the force of hydrogen bonds is between chemical bonds and van der Waals forces. The van der Waals force is a weak interaction that generally exists between molecules, and the hydrogen bond is connected to the strongly electronegative atom due to the special position of the hydrogen atom, resulting in a stronger force than the van der Waals force. The boiling point of common water is different from common sense, and the hydrogen bond between the water-capping molecules is strong. To vaporize it, you need to break the hydrogen bond, so you need more energy and a high boiling point. This obvious hydrogen bond force is greater than the van der Waals force. This is another positive statement.
Furthermore, it is wrong to say that "there is no tropism and saturation of hydrogen bonds". Hydrogen bonds are tropism, and hydrogen atoms form a specific angle with donor and receptor atoms to achieve the lowest energy. And with saturation, a hydrogen atom can only form a hydrogen bond with a receptor atom. Like the structure of ice, water molecules are connected by hydrogen bonds, and they are arranged in an orderly manner, all due to the directivity and saturation of hydrogen bonds, which is also the correct theory about hydrogen bonds.
In summary, it is clear that hydrogen bonds exist between and within molecules, and the force is greater than van der Waals force, with directivity and saturation. Only then can we correctly discuss the way of hydrogen bonds. The theory of chemistry is subtle, and only by understanding its correct theory can we explore the wonders of material changes and the mystery of natural laws.
On Hydrogen Bonding It is said that
Between heaven and earth, everything has its own reason, and the beauty of chemistry, hydrogen bonding is one of them. Now on the theory of hydrogen bonding, which is correct?
The hydrogen bond is not a chemical bond, but its force cannot be underestimated. Its formation also depends on the interaction of hydrogen atoms with atoms with large electronegativity and small radius, such as fluorine, oxygen, and nitrogen. This effect makes the relationship between molecules or within molecules different, and has a profound impact on the properties of substances.
Or: "Hydrogen bonds only exist between molecules." This is not true. In fact, there are also hydrogen bonds in molecules. Looking at o-nitrophenol, its hydroxyl group is similar to the nitro group, and it can form an intramolecular hydrogen bond, resulting in a lower melting boiling point and a lower p-nitrophenol. The effect of this intramolecular hydrogen bond is also known. Therefore, it is known that hydrogen bonds exist between molecules and within molecules, and both are present. This is one of the true theories.
There is another cloud: "The force of hydrogen bonds is always in van der Waals forces." It is true that the force of hydrogen bonds is between chemical bonds and van der Waals forces. The van der Waals force is a weak interaction that generally exists between molecules, and the hydrogen bond is connected to the strongly electronegative atom due to the special position of the hydrogen atom, resulting in a stronger force than the van der Waals force. The boiling point of common water is different from common sense, and the hydrogen bond between the water-capping molecules is strong. To vaporize it, you need to break the hydrogen bond, so you need more energy and a high boiling point. This obvious hydrogen bond force is greater than the van der Waals force. This is another positive statement.
Furthermore, it is wrong to say that "there is no tropism and saturation of hydrogen bonds". Hydrogen bonds are tropism, and hydrogen atoms form a specific angle with donor and receptor atoms to achieve the lowest energy. And with saturation, a hydrogen atom can only form a hydrogen bond with a receptor atom. Like the structure of ice, water molecules are connected by hydrogen bonds, and they are arranged in an orderly manner, all due to the directivity and saturation of hydrogen bonds, which is also the correct theory about hydrogen bonds.
In summary, it is clear that hydrogen bonds exist between and within molecules, and the force is greater than van der Waals force, with directivity and saturation. Only then can we correctly discuss the way of hydrogen bonds. The theory of chemistry is subtle, and only by understanding its correct theory can we explore the wonders of material changes and the mystery of natural laws.
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