chem

• Intermolecular forces (IMF)


  Attractive forces between neighboring particles of one or more substances
• Intramolecular forces


  Forces within a molecule or ionic compound
• Kinetic energy (KE)


  Keeps the particles at a distance and/or moving around
• Solid to gas


  Low kinetic energy to high kinetic energy
• Intramolecular bonds are stronger than intermolecular forces
• Van der Waals forces

  Intermolecular forces of attraction between neutral molecules
• Electronegativity


  Ability of an atom to attract electrons toward itself in a chemical bond
• Intermolecular forces


  • Dipole-dipole forces
  • Ion-dipole forces
  • London dispersion forces
  • Hydrogen bonding
• Dipole-dipole forces


  Attractive forces between polar molecules with dipole moments
• Hydrogen bonds


  Strong type of dipole-dipole interaction
• Ion-dipole forces


  Attraction between an ion and a polar molecule
• London dispersion forces


  Exist between all atoms and molecules, present in nonpolar molecules due to continuous movement of electrons, stronger for larger molecules
• The bigger the molecule, the stronger the London dispersion force between two molecules
• Cohesive forces


  Intermolecular forces that bind like molecules to one another
• Adhesive forces


  Intermolecular forces that bind a substance to a surface
• Water


  Adhesive forces are greater than cohesive forces
• Mercury


  Cohesive forces are greater than adhesive forces
• Surface tension


  Property of a liquid to resist an external force, due to strong attractive and cohesive forces
• Viscosity


  Resistance of a liquid to flow, greater for substances with stronger intermolecular forces
• Vapor pressure


  Pressure of a substance's vapor in thermodynamic equilibrium, increases with temperature as molecule energy increases
• Boiling point


  Temperature at which vapor pressure equals surrounding atmospheric pressure
• Heat of vaporization


  Molar heat required to vaporize one mole of a substance at its boiling point
• Capillary action


  Manifestation of surface tension
• Solid


  • Closely packed together, least amount of kinetic energy
• Crystalline solid


  • Crystals, particles arranged in order and symmetry
• Amorphous solid


  • Solids without form, no repeating lattice pattern
• Pseudo-solid


  • Doesn't have a melting point
• Types of solids


  • Ionic solid
  • Covalent solid
  • Molecular solid
  • Metallic solid
• Ionic solid


  • Formed by cation and anion, typical metals and nonmetals
• Molecular solid


  • Neutral molecules forming molecular lattice structures, low melting and boiling points, non-conductors
• Covalent network solid


  • Distinct atoms all bound covalently, high melting and boiling points
• Metallic solid


  • Metallic bonding, great conductors of heat and electricity, melting and boiling points vary
• Phase diagram


  Graphical representation of pressure-temperature relationships for phase equilibria of a substance
• Solution


  Homogeneous mixture of two or more substances
• Solute


  Substance(s) present in the smaller amount(s)
• Solvent


  Substance present in the larger amount
• Types of solutions


  • Saturated
  • Unsaturated
  • Supersaturated
• Molality


  Number of moles of solute per kilogram of solvent
• Molarity


  Number of moles of solute per liter of solution
• Mole fraction


  Ratio of moles of a component to total moles in a solution