Hydrogen shortcut is an electrostatic attraction between two polar groups that occurs as soon as a hydrogen atom (H), covalently bound to a extremely electronegative atom such as flourine (F), oxygen (O) and nitrogen (N) atoms.
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Because the hydrogen bonds, hydrogen peroxide has greater melting and boiling temperature than various other molecules.
Intermolecular forces exist in between the molecules or the surrounding particles. These can be attractive and repulsive forces.
Classification the intermolecular forces:
1. Dipole-dipole attraction
When a dipole interacts with one more dipole, these pressures come into play. The charged component of one molecule it s okay attracted to the oppositely charged part of another molecule and dipole-dipole attractions occur. Such types of attractions are shown by carbon dioxide and hydrogen fluoride.
2. Ion-dipole forces
Such forces result from the communication of ion and also a neutral molecule. This neutral molecule is composed of a dipole.
3. Ion-induced dipole forces
An ion induces a dipole once it philosophies a non-polar molecule. The electron arrangement and distribution in the non-polar molecule is disturbed by these forces.
4. Dispersion forces
Atoms and molecules exist because of the visibility of dispersion forces in in between them. Such forces are likewise called Vander Waals or London forces.
5. Hydrogen bonding
When the interaction in between a hydrogen atom and a highly electronegative aspect takes place, hydrogen bonding is said to occur. Hydrogen forms this type of shortcut with elements like nitrogen, oxygen and also fluorine.
There is the visibility of hydrogen bonds in between the electronegative oxygen atom and a hydrogen atom in the situation of hydrogen peroxide
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Grade: Senior School
Chapter: Ionic and covalent bonding
Keywords: hydrogen peroxide, H2O2, hydrogen bonds, melting, boiling, intermolecular forces, gases.