- Intermolecular Forces - Forces BETWEEN molecules (ie: London dispersion, dipole-dipole, hydrogen bonding). Controls physical properties (ie: boing, melting points).
- Intramolecular Forces- Forces WITHIN molecules (ie: covalent, ionic, metallic bonds) Stronger than IMFS
- van der Waals Forces- Total of intermolecular forces (LDFs, Dipole-Dipole, and Hydrogen bonding)
- London Dispersion Forces- Weakest of IMFS. Due to movement of electrons, they create a TEMPORARY dipole. ↑ # of electrons, ↑ the LDF. ALL molecules have LDFs.
- Dipole-Dipole Forces- Polar molecules. Attractive forces between positive side of one polar molecule and negative side of another polar molecule. The more polar, the higher the boiling point.
- Hydrogen Bonding- Strongest of IMFS. SUPER dipole-dipole, H only bond with F, O, N.
- Ion-Dipole Interactions- Not van der Waals forces. When cation or anion is attracted to dipole
- Heating Curve- chart of time vs temperature of a system
- Endothermic- absorbing energy, (+)
- Exothermic- releasing energy, (-)
- Heat of fusion (▲H of fus)- heat absorbed of a solid at its melting point to convert it to a liquid or heat released from a liquid at freezing point to convert it to a solid (temperature does NOT change)
- Heat of vaporization (▲H of vap)- heat absorbed of a liquid at its boiling point to convert it to a gas or heat released from a gas at condensing point to convert it to a liquid (temperature does NOT change)
- Phase Diagram- chart showing conditions of a substance at various pressures and temperatures
- Condensation- phase change of gas → liquid
- Sublimation- phase change of solid → gas
- Deposition- phase change of gas → solid
- Melting- phase change of solid → liquid
- Freezing- phase change of liquid → solid
- Critical Point- when liquid and vapor cannot be told apart from each other
- Triple Point- when all states (solid, liquid, gas) exist at the same time at equilibrium
- Covalent Network Solid- very hard, very high melting point (ie: Diamond, C; quartz, SiO2)
- solute- substance dissolved in a solution
- solvent- in what solute is dissolved, substance with greatest amount
- Solvation- interactions between solute and solvent
- Hydration- interactions of solutions when solvent is water
- Entropy- Amount of disorder in solution
- saturated- solution with solute not dissolved at equilibrium
- solubility- amount of solute needed for a given amount of solvent to form a saturated solution
- unsaturated- Solution that contains less solute than needed for saturated solution
- supersaturated- Solution that contains more solute than needed for saturated solution
- miscible- able to dissolve
- immiscible- not able to dissolve