Hydrogen Bonds in DNA (Deoxyribonucleic Acid).Intramolecular hydrogen bonding is responsible for different types of proteins such as secondary proteins, tertiary proteins, and quaternary proteins and as well as for the structure of the nucleic acids. The high surface tension of water is explained by this property.

When water droplets fall on a leaf, the hydrogen bonds present between the molecules of water are more substantial than the intermolecular forces of adhesion between the water molecules and the leaf. Water has the property to stick to itself (cohesion) and also with other molecules (adhesion). Some of the applications and effects of hydrogen bonds are given below. In different types of chemical and biological processes, hydrogen bonding is necessary. The hydrogen bonding in carboxylic acid doubles the size of the molecule. Hydrogen bonding can occur in a pure carboxylic acid in between two molecules of acid in order to produce a dimer. When any molecule containing the hydrogen atom is connected to either oxygen or nitrogen directly, it usually has the tendency to form hydrogen bonding. Nitrogen is a highly electronegative atom that is linked to hydrogen atoms in order to make hydrogen bonds.įluorine is an element that has the highest value of electronegativity, and it forms the strongest hydrogen bond.Īlcohols are organic compounds. The hydrogen bonds in ammonia (NH 3 ) are formed between nitrogen and hydrogen atoms. The electrons of the shared pair are attracted more by the oxygen atom, and this end of the molecule becomes negative, and the hydrogen atoms become positive. WaterĪ water molecule is composed of a highly electronegative oxygen atom linked to the hydrogen atom. Some examples of hydrogen bonding are as follows. Hydrogen bonds are comparatively weaker than covalent and ionic bonds. It is stronger than the weak Van der Waals bonds. As a result of this, it makes it less volatile. For example, if hydrogen bonding is present, it increases the melting and boiling point of a substance. It is a weak force of attraction between molecules.Īny compound or molecule having hydrogen bonding shows different physical properties. Some of the properties of hydrogen bonding are given below. The donor atoms and acceptor atoms that took part in hydrogen are present in suitable positions where they can interact.Įxamples of Intermolecular Hydrogen Bond - Some Examples of Intermolecular Bonds of Hydrogen Bonds are given below. One more example of a molecule that shows this type of hydrogen bonding is salicylaldehyde(C₇H₆O₂).Īn intermolecular hydrogen bond is formed between two or more separate molecules in a substance. Here hydrogen bonding is present between the two groups due to molecular geometry. They must be present within each other’s proximity.Įxamples Intramolecular Hydrogen Bonding -Įthylene glycol (C₂H₄(OH)₂) has two hydroxyls groups.

In order to form intramolecular hydrogen bonding, the hydrogen donor and hydrogen acceptor must be present within one molecule.

It is formed when two functional groups of a molecule form hydrogen bonds with each other. Within a single molecule, an intramolecular hydrogen bond is formed. Now understand each type of hydrogen bonding in detail. There are two types of hydrogen bondings which are given below. To form a bond the donor atom effectively shares its hydrogen with the acceptor atom mainly through electrostatic attraction. F, N, or O, contain an electron pair that is not shared, which provides it with a slight negative charge. Its high electron affinity makes the hydrogen atom take on a slight positive charge. One is that it can occur between atoms of different molecules or in the atoms of the same molecule.Īnd another one in which atom of the pair, which is also known as donor as it donated electrons ( mostly fluorine (F), nitrogen (N), or oxygen (O) atom), is covalently bonded to a hydrogen atom (-FH, -NH, -OH). Hydrogen-bonding used to be competitively weaker than ionic bonding or covalent bonding, but it is stronger than van der Waals forces. A hydrogen bond is a kind of bonding that is present between an atom of hydrogen and a pair of other atoms having a high electronegativity.