What is a hydrogen link?

Hydrogen bond is a relatively weak binding that hydrogen atoms form with electrongative atoms with nitrogen, oxygen or fluorine. Hydrogen bonds are weaker than ionic, covalent and metal bonds, but still slightly strong, with energy usually between 5 and 30 kJ/mol. On the other hand, weak covalent bonds have an energy of about 155 kJ/mol. Hydrogen binding can be either intermolecular (between molecules) or intramolecular (between different parts of molecules) bonds. This type of binding can occur in both organic molecules such as DNA, and inorganic molecules such as water. The hydrogen bond is partially responsible for the complex secondary and tertiary protein structure. The oxygen atom in each water molecule has two lonely electrons, which are immediately connected to the hydrogen atoms in other water molecules. In addition, two hydrogen atoms were connected to each oxygen binding to the oxygen molecules in the neighboring water molecules. This intermolecular connection is responsible for a relatively high boiling point of water. WaterIt has an extremely high boiling point due to materials consisting of molecules of similar size. If these bonds did not exist, the water would boil at a temperature of similar carbon dioxide (which is boiled at -78 ° C or -108.4 ° F) and life, as we know it would be impossible.

The hydrogen bond consists of an acceptor of a hydrogen bond, target atom and a hydrogen bond donor, the hydrogen atom itself. Sometimes in molecules, such as chloroform (want _{3 ), the carbon can be connected to a hydrogen bond, especially if it is surrounded by electrongative atoms such as chlorine. Hydrogen bond is unusual and is often called electrostatic dipole-lower interaction (weak intermolecular interaction), accumulating it with more transient bonds caused by current quantum fluctuations in electric charge, but also has many characteristics of much stronger covalent bonds where electron clouds actuallyeckey. These properties include the directional, strength, production of interactomic distances shorter than those that are typical of transient van der waals, and a limited number of interaction partners, which is the diagnosis of stronger links.}

The length of hydrogen bonds varies depending on the strength of the binding, temperature and pressure. The strength of the binding is also dependent on a number of factors, including temperature, binding angles, pressure and environment. The water is typical of the hydrogen bond of 1.97 á (197 pm).