SOLIDS, LIQUIDS, AND GAS Flashcards
Condensed phase
Refers to solid and liquid states
IMF strength based on physical state
Gasses have weaker IMF due to larger distances, solids and liquids have stronger IMF from closer molecules
Intermolecular force
Bonds between different molecules
Intramolecular force
Bonds between atoms
London dispersion
Temporary attractive force due to temporary formation of dipoles in non polar molecules and present in all molecules
Dipole-dipole
Attractive forces between one end of a positive molecule and one end of negative molecule
Hydrogen bond
When hydrogen atoms bind to an electronegative F, O, N
Why is water more dense in liquid than solid
The water molecules are pushed farther apart when it is ice. Whereas when its liquid, each H2O molecule only bonds to some H bond so molecule stays closer together = more dense
What’s so special about ionic bonds
They do not have IMF so they exhibit high melting and boiling points
Order of strength of IMF
London dispersion –> Dipole –> Hydrogen –> Ionic
Surface tension
Resistance of a liquid to increase its surface area caused by an uneven pull toward center of liquid
Capillary action
Phenomenon that liquids simultaneously enter and rise up on narrow glass tube
Adhesive force
IMF that form meniscus between glass and liquid
Cohesive force
IMF that form bump between liquid molecules
Viscosity
Resistance of a liquid to flow impacted by strong IMF and temperature
High viscosity
= Strong IMF = molecules are attracted strongly and dont move as much
Low viscosity
= Weak IMF = molecules are not as attracted strong and move easily
Phase transitions (6)
- Freezing/fusion: Liquid –> solid
- Melting: Solid –> Liquid
- Condensation: Gas –> liquid
- Vaporization: Liquid –> gas
- Sublimation: Solid –> gas
- Deposition: Gas –> solid
Vapor pressure
When rates of evaporation and condensation are equal and the pressure above liquid is constant
Normal boiling point
The temperature at which its vapour pressure is equal to 1atm (Pvap1 in Clausius)
What do the delta Vap H circle mean
Energy required to vaporize 1 mol
Clausius-Clapeyron equation
ln(pvap2/pvap1) =-deltavapH/R(1/T2-1/T1)
- T should be in Kelvin
Trends of phase transition
Some phase transitions in opposite directions have some energy with opposite signs
Heating curve
Temperature response of substance when heat is added at a constant rate
