Important Conditions for Hydrogen Bonding
Hydrogen Bonding is possible in cases when the molecule contains a highly electronegative atom linked to the hydrogen atom. The hydrogen bonding in water is a vigorous bond between the nearest water molecule containing one Hydrogen atom between two oxygen atoms. Hydrogen bonding is major of two types of intramolecular and intermolecular hydrogen bonding, on the basis of the atoms involved in it. Hydrogen bonding is maximum in solid-state compounds.
- The atom that is bonded to the hydrogen atom has a high electronegativity, making the bond suitably polar. A strongly electronegative atom connected to the hydrogen atom must be present in the molecule. The degree of polarisation of the molecule increases with increasing electronegativity.
- The electronegative atom attached to the Hydrogen atom should be smaller in size. Greater the electrostatic attraction, the smaller the size. So, the smaller size should attract the bonding electron pair effectively.
Hydrogen Bonding
In chemistry, a hydrogen bond is an electrostatic force of attraction between a hydrogen atom and another electronegative atom. It is a special type of dipole-dipole force. Hydrogen bonding is the phenomenon of the formation of Hydrogen Bonds.
H Bonds are stronger than any dipole-dipole bonds but weaker than covalent bonds. Hydrogen bonds can form between atoms within a molecule or between two different molecules.
Hydrogen bonds can form when:
- A hydrogen atom is covalently bonded to a more electronegative atom
- The other atom has a lone pair of electrons
Examples of hydrogen bonds Water, Ammonia, and Hydrogen Fluoride.
Table of Content
- What is Hydrogen Bond?
- What is Hydrogen Bonding?
- Important Conditions for Hydrogen Bonding
- Effects of Hydrogen Bonding on Elements
- Examples of Hydrogen Bonding
- Properties of Hydrogen Bonding
- Types of Hydrogen Bonding
- Difference between a Hydrogen Bond and Covalent Bond
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