Properties of Hydrogen Bonding
- Volatility – The boiling point of compounds incorporating hydrogen bonding between distinct molecules is greater, hence they are less volatile.
- Solubility – Because of the hydrogen bonding that can occur between water and the alcohol molecule, lower alcohols are soluble in water.
- Lower density of ice than water – In the case of solid ice, hydrogen bonding causes water molecules to form a cage-like structure. In fact, each water molecule is tetrahedrally connected to four other water molecules. In the solid state, the molecules are not as tightly packed as they are in the liquid state. This case-like structure collapses as ice melts, bringing the molecules closer together. As a result, the volume of water reduces while the density increases for the same quantity of water. As a result, at 273 K, ice has a lower density than water. Ice floats because of this.
- Viscosity and Surface Tension – Hydrogen bonding is found in compounds that have an associated molecule. As a result, their flow becomes more complicated. They have high surface tension and higher viscosity.
Why do hydrogen-bonded compounds have high melting and boiling points?
The melting and boiling temperatures of hydrogen-bonded compounds are unusually high. The elevated melting and boiling points of hydrogen-bonded compounds are attributable to the additional energy required to break these bonds.
- At room temperature, H2O is a liquid, whereas H2S, H2Se, and H2Te are all gases. Hydrogen bonding produces links in the water molecules, resulting in water having a higher boiling point than the other chemicals.
- Because there is hydrogen bonding in NH3, but not in PH3, ammonia has a higher boiling point than PH3.
- The presence of hydrogen bonding accounts for hydrogen fluoride’s particularly high boiling point among the halogen acids.
- Because ethanol contains hydrogen bonds, it has a higher boiling point than diethyl ether.
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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