IMF

• • The Kinetic Molecular Theory explains the  properties of solids and liquids in terms of  intermolecular forces of attraction and the  kinetic energy of the individual particles.
• All matter is made up of tiny particles.
• These particles are in constant motion.
• The speed of a particle is proportional to temperature. Increased temperature means greater speed. 
• Solids, liquids, and gasses differ in distances  between particles, in the freedom of motion of  particles, and in the extent to which the  particles interact.
• Solid has Fixed volume; fixed shape (regardless of size and shape of container)
• These two matters has high density: Liquid and Solid
• The molecules of Solid vibrates in place.
• INTERMOLECULAR FORCES

  • Are attractive forces between molecules or particles in the solid or liquid states.
• Intramolecular forces are forces within the molecules forming bonds
• Intramolecular forces hold atoms together in a molecule.
• The intermolecular forces of attraction in a  pure substance are collectively known as van der Waals forces.
• Types of Intermolecular forces (strongest to weakest)

  1. Dipole-dipole
  2. Hydrogen bonding 
  3. Ion-dipole
  4. London dispersion
  5. Dipole-induced dipole force
• an IMF that exists between polar molecules: Dipole-dipole
• Hydrogen Bonding is a special and very strong type of dipole –  dipole force that exists between a hydrogen  atom
• Hydrogen  bond  occurs  in  polar  molecules containing H and any of highly electronegative elements, in particular Nitrogen, Fluorine, and Oxygen.
• The  ions  and  the  oppositely  charged  ends  of the polar water molecules overcome the  attraction  between  ions  themselves: Ion-dipole
• London Dispersion Force is the weakest type of intermolecular force.
• London Dispersion force is sometimes called an induced  dipole-induced dipole attraction.
• Dipole-induced Dipole Force is the interaction between Polar and nonpolar molecules.
• • Liquids do not have a simple or regular structure.
• Surface Tension is the measure of the elastic force on the surface of a liquid.
• it is the amount of energy required to stretch or increase the surface of a liquid by a unity area: Surface Tension
• The liquids that have STRONG IMF also have HIGH SURFACE TENSION.
• Capillary action is the tendency of a liquid to rise in narrow tubes or be drawn into small openings
• CAPILLARITY is an intermolecular attraction between the solid and liquid materials.
• Two types of forces that is involved in capillary action: Cohesion and Adhesion
• Cohesion is the intermolecular attraction between LIKE molecules (the liquid molecules)
• Adhesion is an attraction between UNLIKE molecules
• Cohesive force > adhesive forces = convex
• Cohesive force < adhesive forces = concave
• Viscosity is defined as the resistance of a liquid to flow.
• It is loosely referred to as the  thickness or thinness of a  liquid: Viscosity
• The stronger the IMF the higher the viscosity.
• Vapor Pressure is the pressure exerted by its vapor when in equilibrium with liquid or solid.
• The higher the temperature of the water, the higher the vapor pressure is.
• The substances with relatively strong intermolecular forces will have low vapor pressure because the particles will have difficulty escaping as a gas.
• Boiling point of is the temperature at which its vapor pressure is equal to the external or atmospheric pressure.
• INCREASE TEMP = HIGHER KINETIC ENERGY
• The greater intermolecular force, the higher the energy needed to increase the kinetic energy of the molecules to break these forces.