Profile
Settings
Refer your friends
Sign out
In simple terms, hydrogen bonding is the formation of hydrogen bonds. It mainly occurs between an electronegative and a hydrogen atom. Some of the common electronegative atoms are fluorine, chlorine, and oxygen. Compared to the covalent or ionic bond, the hydrogen bond is generally weaker. However, it is stronger than the van der Waals forces. Experts classified hydrogen bonds as a type of weak chemical bond.
On the topic of the conditions for hydrogen bonding, learn about hydrogen bonding and various conditions to form hydrogen bonding, along with related topics in detail.
Explain Hydrogen Bonding
Hydrogen bonding can be described as the process of forming hydrogen bonds that are an attractive intermolecular force’s special class which arises because of the interaction between the hydrogen atom and a highly electronegative atom. For example, in the case of water molecules, chemically denoted as H2O, hydrogen is bonded covalently to the electronegative oxygen atom.
As a result, hydrogen bonding rises in the water molecules because of the dipole-dipole interactions among oxygen atoms and hydrogen atoms. According to the experts, the hydrogen bonding is mostly strong when compared to the normal dispersion and dipole-dipole forces; however, it appears to be weak if compared to ionic bonds or true covalent bonds. Further, hydrogen bonding is divided into two major parts. These include-
Intermolecular Hydrogen Bonding is a type of hydrogen bonding where it takes place between different molecules that have either the same or different compounds.
Intramolecular Hydrogen Bonding is another type of hydrogen bonding that mainly occurs within the molecule only. This type of hydrogen bonding takes place in compounds that have two groups.
Conditions of Hydrogen Bonding
In the molecule where the atom is closely connected to the electronegative atom, the shared piece of an electron is attracted. As a result, the molecule’s end appears slightly negative, whereas the other part becomes positive. Both the ends attract one another, which leads to the formation of a weak bond between them. The bond explained is referred to as the hydrogen bond.
Because of the hydrogen bonding, a single hydrogen atom is closely linked to two electronegative atoms at the same time. Out of the two, one is connected to the covalent bond, whereas; another is by the hydrogen bond. Here are two major conditions of hydrogen bonding –
Electronegative atom’s size should be small. The lesser the size of electronegative atoms will be, the more the electrostatic attraction will be.
Each molecule should have a highly electronegative atom connected to the hydrogen atom. The more the electronegativity will be, the higher the molecule’s polarisation.
Because of the hydrogen bonding, the Carboxylic acid molecules appear dimmer. The cell groups of all such compounds are twice in size.
Hydrogen Bonding Examples
Here is the list of some most common examples of hydrogen bonding –
Hydrogen bonding in the water
A water molecule has an electronegative oxygen atom connected to hydrogen atoms. Since the oxygen atom tends to attract the electron’s shared pair, its end becomes negative. However, the hydrogen atom becomes positive.
Hydrogen bonding in carboxylic acid and alcohols
Alcohol is referred to as an organic molecule with an -OH group. Generally, in case any molecule that has a hydrogen atom is either linked to nitrogen or oxygen directly. Later, hydrogen bonding becomes easier.
Hydrogen bonding in the hydrogen fluoride
Since fluorine has the highest value of electronegativity, it leads to the formation of the strongest hydrogen bond.
H−F···H−F···H−F
Hydrogen bonding in the ammonia
It has electronegative atom nitrogen connected to hydrogen atoms.
Hydrogen bonding in the polymer
In order to determine properties and 3D structures acquired by natural and synthetic proteins, hydrogen bonding is a crucial factor. It also plays a significant role in defining the cellulose structure along with derived polymers, including flax or cotton.
Do the compounds with hydrogen bonding have a high boiling and melting point?
Hydrogen bonding compounds generally show extremely high melting and boiling points. This is because of the fact that a larger amount of energy is required to break bonds. Since hydrogen bonding is present, the boiling point between halogen acids is generally high.
Conclusion
Hydrogen bonding is the process of forming hydrogen bonds, which are an attractive intermolecular force’s special class that arises because of the dipole-dipole interaction between the hydrogen atom and a highly electronegative atom. Experts classified hydrogen bonds as a type of weak chemical bond. It mainly occurs between an electronegative and a hydrogen atom.
Some of the common examples of hydrogen bonding are Hydrogen bonding in hydrogen fluoride, Hydrogen bonding in the water, Hydrogen bonding in ammonia, Hydrogen bonding in the polymer, and so on. There are mainly three conditions for the formation of hydrogen bonding, which we discussed in detail. In the latter part, we also discussed how compounds with hydrogen bonding have a high boiling and melting point. We hope this has helped us attain a better understanding of conditions for hydrogen bonding.
