Chemistry

• Intermolecular forces


  Dipole-dipole (between polar molecules)<|>Ion-dipole (between an ion and a polar molecule, strongest)<|>London dispersion (between all atoms and molecules, weakest)
• Hydrogen bonds are a type of dipole-dipole arrangement of atoms
• Hydrogen bonds can only exist when atoms are bonded with N, O, F
• Types of Solids


  • Amorphous (disordered structure)
  • Crystalline (highly regular)
• Hydrogen bonds


  DATE
• Cations are + ions
• Molecular


  Discrete molecules
• Ionic


  Composed of metal atoms
• Network


  Composed of nonmetal atoms
• Group 8A


  Noble gases
• Crystallattice


  Geometric arrangement of atoms
• Concentrationof solution


  Percent by mass, percent by volume, percent by mass-volume
• Molality


  Moles of solute / mass of solvent (kg)
• Molarity


  Moles of solute / volume of solution (L)
• Mole fraction


  Moles of solute / total moles of solution
• Parts per million (PPM)


  Grams of solute / 1×10^6 grams of solution
• S

  1. Convert moles of given substance to moles of desired substance using balanced chemical equation. Convert moles of given substance to moles of desired substance using balanced chemical equation

  2. Convert moles of desired substance to desired units
• Colligative properties


  Vapor pressure lowering, freezing point depression, boiling point elevation, osmotic pressure
• Osmotic pressure


  Π = MRT
• Thermochemistry is the study of energy flow or heat
• The change in energy of a system is equal to the heat absorbed by the system and the work done on it
• Vapor pressure lowering


  AP = X solvent * Psolvent
• Freezing point


  Tf = (-molality) (Kf)
• Boiling point

  Tb = (molality) (Kb) + 100 °C
• First law of thermodynamics

  The change in energy of a system is equal to the absorbed (q) by the system and the work (w) done on it
• Surface tension


  • Energy/work required to increase the surface area of a liquid due to intermolecular forces
• Viscosity


  • Resistance of a liquid to flow
• Vapor pressure


  • Pressure exerted by a liquid's vapor when in equilibrium with its gas/solid
• Boiling point

  • Temperature at which a liquid's vapor pressure is equal to the external/atmospheric pressure
• Heat of vaporization


  • Amount of heat required to vaporize 1 mole of a substance at its boiling point
• Capillary action


  • Ascension of liquids through slim tubes
• Cohesive forces


  • Attraction between like molecules
• Adhesive forces


  • Attraction between unlike molecules
• Vapor pressure lowering


  AP = X solvent. Proivent
• X solvent


  Mole fraction of the solvent
• Pooivent


  Vapor pressure of the solvent
• Freezing point


  1. T₁ = (-molality) (k+)

  2. (P) mol solute to nom

  3. -morality

  4. mol solvent

  5. K = freezing point constant
• Boiling point

  1. Tb = (molality) (kb) + 100 °C

  2. molality = mol solute / mol solvent

  3. Kb = Boiling point constant
• First law of thermodynamics: The change in energy of a system is equal to the absorbed (q) by the system and the work (w) done on it.
• When the work is done on the system (+w), when the system does the work (-w), when the system absorbs heat (+q), system releases heat (-q)