IMF

Intermolecular Forces (IMFs)

The forces of attraction between molecules.

Types of IMFs

London Dispersion Forces, Dipole-Dipole Interactions, Hydrogen Bonding.

London Dispersion Forces

Caused by temporary shifts in electron density.

Dipole-Dipole Interactions

Occur between polar molecules due to permanent dipoles.

Hydrogen Bonding

Occurs when hydrogen bonds with N, O, or F atoms.

London Dispersion Forces in Nonpolar Molecules

Even nonpolar molecules experience London Dispersion Forces.

Molecular Size and London Dispersion

Larger molecules have stronger London Dispersion Forces.

Dipole-Dipole Strength

Increases with polarity of molecules.

Hydrogen Bonding Strength

Stronger than dipole-dipole interactions due to electronegativity.

Water Boiling Point

Water has a high boiling point due to hydrogen bonding.

IMF Strength Order

London Dispersion < Dipole-Dipole < Hydrogen Bonding.

IMFs and Boiling Points

Stronger IMFs result in higher boiling points.

IMFs and Melting Points

Stronger IMFs result in higher melting points.

IMFs and Vapor Pressure

Stronger IMFs result in lower vapor pressures.

IMFs and Viscosity

Stronger IMFs increase viscosity (resistance to flow).

IMFs and Surface Tension

Stronger IMFs increase surface tension.

Polarizability

Refers to how easily a molecule's electron cloud is distorted.

Molecular Shape and Dispersion Forces

Linear shapes lead to stronger London Dispersion Forces.

Nonpolar Molecules

Experience only London Dispersion Forces.

Example of Nonpolar Molecule

CO₂, which has only London Dispersion Forces.

Example of Polar Molecule with Dipole-Dipole Forces

HCl.

Example of Molecule with Hydrogen Bonding

H₂O, which exhibits hydrogen bonding.

Boiling Point and Molecular Mass

Nonpolar molecules with greater mass have higher boiling points.

Stronger IMFs and Vaporization

Stronger IMFs decrease the rate of vaporization.Intermolecular Forces (IMFs)

Types of IMFs

London Dispersion Forces, Dipole-Dipole Interactions, Hydrogen Bonding.

London Dispersion Forces

Caused by temporary shifts in electron density.

Dipole-Dipole Interactions

Occur between polar molecules due to permanent dipoles.

Hydrogen Bonding

Occurs when hydrogen bonds with N, O, or F atoms.

London Dispersion Forces in Nonpolar Molecules

Even nonpolar molecules experience London Dispersion Forces.

Molecular Size and London Dispersion

Larger molecules have stronger London Dispersion Forces.

Dipole-Dipole Strength

Increases with polarity of molecules.

Hydrogen Bonding Strength

Stronger than dipole-dipole interactions due to electronegativity.

Water Boiling Point

Water has a high boiling point due to hydrogen bonding.

IMF Strength Order

London Dispersion < Dipole-Dipole < Hydrogen Bonding.

IMFs and Boiling Points

Stronger IMFs result in higher boiling points.

IMFs and Melting Points

Stronger IMFs result in higher melting points.

IMFs and Vapor Pressure

Stronger IMFs result in lower vapor pressures.

IMFs and Viscosity

Stronger IMFs increase viscosity (resistance to flow).

IMFs and Surface Tension

Stronger IMFs increase surface tension.

Polarizability

Refers to how easily a molecule's electron cloud is distorted.

Molecular Shape and Dispersion Forces

Linear shapes lead to stronger London Dispersion Forces.

Nonpolar Molecules

Experience only London Dispersion Forces.

Example of Nonpolar Molecule

CO₂, which has only London Dispersion Forces.

Example of Polar Molecule with Dipole-Dipole Forces

HCl.

Example of Molecule with Hydrogen Bonding

H₂O, which exhibits hydrogen bonding.

Boiling Point and Molecular Mass

Nonpolar molecules with greater mass have higher boiling points.

Stronger IMFs and Vaporization

Stronger IMFs decrease the rate of vaporization.