Intermolecular Forces Definition Intermolecular forces are the forces of attraction that exist between molecules. These forces play a crucial role in determining the physical and chemical properties of substances, such as boiling points, melting points, solubility, and viscosity. Intermolecular Forces The three main types of intermolecular forces are: London dispersion forces (also known as Van der Waals forces): These forces are present in all molecules, whether they are polar or nonpolar. They arise due to temporary fluctuations in electron distribution, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces. London dispersion forces increase with increasing molecular size and shape. Substances with stronger London dispersion forces tend to have higher boiling points and melting points. London Dispersion force London dispersion forces are the weakest intermolecular forces. They occur due to temporary fluctuations in electron distribution within molecules, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces. London dispersion forces increase with increasing molecular size and shape. Substances with stronger London dispersion forces tend to have higher boiling points and melting points. Examples of substances with predominant London dispersion forces include noble gases like helium and nonpolar molecules like hydrocarbons. 2 .Dipole-dipole interactions: These forces occur between polar molecules. They arise due to the attraction between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole interactions are stronger than London dispersion forces and contribute significantly to the physical properties of polar substances . Dipole dipole interaction Polar molecules have an uneven distribution of electron density, resulting in a permanent dipole moment. The positive end of one polar molecule is attracted to the negative end of another polar molecule. Dipole-dipole interactions are stronger than London dispersion forces. These forces contribute significantly to the physical properties of polar substances. Examples of substances with predominant dipole-dipole interactions include hydrogen chloride (HCl) and water (H2O). 3.Hydrogen bonding: This is a special type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is also attracted to another electronegative atom in a different molecule. Hydrogen bonding is exceptionally strong compared to other intermolecular forces and has a significant impact on the properties of substances. It is responsible for many unique properties of water, such as its high boiling point, surface tension, and the ability to form ice with a lower density than liquid water.

1. Intermolecular Forces
Definition
Intermolecular forces are the forces of attraction that exist between molecules. These
forces play a crucial role in determining the physical and chemical properties of
substances, such as boiling points, melting points, solubility, and viscosity.
Intermolecular Forces
The three main types of intermolecular forces are:
1. London dispersion forces (also known as Van der Waals forces): These forces
are present in all molecules, whether they are polar or nonpolar. They arise due to
temporary fluctuations in electron distribution, creating temporary dipoles. These
temporary dipoles induce dipoles in neighboring molecules, resulting in attractive
forces. London dispersion forces increase with increasing molecular size and
shape. Substances with stronger London dispersion forces tend to have higher
boiling points and melting points.

2. London Dispersion force
● London dispersion forces are the weakest intermolecular forces.
● They occur due to temporary fluctuations in electron distribution within
molecules, creating temporary dipoles.
● These temporary dipoles induce dipoles in neighboring molecules, resulting in
attractive forces.
● London dispersion forces increase with increasing molecular size and shape.
● Substances with stronger London dispersion forces tend to have higher boiling
points and melting points.
● Examples of substances with predominant London dispersion forces include
noble gases like helium and nonpolar molecules like hydrocarbons.
2 .Dipole-dipole interactions: These forces occur between polar molecules. They
arise due to the attraction between the positive end of one polar molecule and the
negative end of another polar molecule. Dipole-dipole interactions are stronger than
London dispersion forces and contribute significantly to the physical properties of polar
substances
.

3. Dipole dipole interaction
● Polar molecules have an uneven distribution of electron density, resulting in a
permanent dipole moment.
● The positive end of one polar molecule is attracted to the negative end of another
polar molecule.
● Dipole-dipole interactions are stronger than London dispersion forces.
● These forces contribute significantly to the physical properties of polar
substances.
● Examples of substances with predominant dipole-dipole interactions include
hydrogen chloride (HCl) and water (H2O).
3.Hydrogen bonding: This is a special type of dipole-dipole interaction that occurs when
a hydrogen atom is bonded to a highly
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