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abi.ayan
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Though there are other atoms with less electronegativity which can form effective attraction forces,why hydrogen is taken as a speacial case?
Hydrogen bonding is considered a special type of intermolecular force because it is significantly stronger than other types of intermolecular forces, such as London dispersion and dipole-dipole interactions. This is due to the large electronegativity difference between hydrogen and other highly electronegative atoms, such as oxygen and nitrogen, which allows for a strong dipole-dipole attraction.
The small size of hydrogen atoms allows them to be highly polarizable, meaning they can easily form temporary dipoles with neighboring atoms. This makes them more likely to participate in intermolecular interactions, particularly hydrogen bonding, which contributes to the overall strength of intermolecular forces.
Hydrogen bonding is only possible with specific atoms, such as oxygen and nitrogen, because these atoms have high electronegativity values, meaning they strongly attract electrons. This creates a large electronegativity difference between hydrogen and these atoms, allowing for the formation of strong dipole-dipole interactions.
Hydrogen bonding plays a significant role in determining the physical properties of substances. It can contribute to higher melting and boiling points, increased surface tension, and greater viscosity. This is due to the strength of hydrogen bonds, which requires more energy to break and results in stronger intermolecular forces between molecules.
Yes, hydrogen bonding can occur between molecules of the same substance. This is known as intramolecular hydrogen bonding and can be seen in molecules such as ethanol and acetic acid. In these cases, the hydrogen bond forms between different functional groups within the same molecule, rather than between separate molecules.