KMT & States
Temperature is a direct measure of this average energy of the molecules.
This weakest intermolecular force is present in all atoms and molecules, both polar and nonpolar
London Dispersion Forces (LDFs)
This term describes the attraction between like molecules.
The direct phase transition from a solid to a gas without passing through a liquid phase
Sublimation
Brass is an example of this solid type of solution.
Alloy
This state of matter has an intermediate IMFA strength and particles that can slide or move past one another over short distances.
Liquid
Hydrogen bonding occurs when hydrogen is directly bonded to one of these three highly electronegative elements.
Flourine, Oxygen, and Nitrogen
This property is defined as a fluid's resistance to flow.
Viscosity
Phase changes where heat is released and molecular order increases are classified by this thermal term (Delta H < 0).
Exothermic process
This classic chemistry rule dictates that polar solutes dissolve in polar solvents, while nonpolar solutes dissolve in nonpolar solvents.
“Like dissolves like”
According to KMT, matter is composed of these three tiny types of particles.
atoms, molecules, or ions
This type of force exists between polar molecules possessing permanent dipole moments
Dipole-dipole interactions
Water forms a concave meniscus in a glass cylinder because this type of attraction exceeds cohesion.
Adhesion
The direct phase transition from a gas to a solid.
Deposition
A solution that contains more dissolved solute than its normal solubility limit at equilibrium.
Supersaturated solution
This state of matter has negligible or weak IMFA and continuous, random motion over large distances.
Responsible for dissolving ionic compounds like NaCl in water, this force occurs between a charged ion and a polar molecule.
Ion-dipole interaction
Liquids with stronger intermolecular forces will exhibit a lower value for this type of pressure exerted by gas in dynamic equilibrium.
Vapor pressure
On a phase diagram, this specific point represents the temperature and pressure where solid, liquid, and gas phases all coexist in dynamic equilibrium.
Triple point
This state is reached when a solution contains an amount of dissolved solute that is in dynamic equilibrium with undissolved solute at a given temperature.
Saturated solution
This property of solids describes their inability to be easily compressed compared to gases.
Virtually incompressible
London dispersion forces depend on this property, which measures the ease of distorting an electron distribution.
Polarizability
A liquid reaches this specific point when its vapor pressure equals atmospheric pressure.
Boiling point
Above this critical point on a phase diagram, liquid and gas boundaries vanish and merge into this single state.
Supercritical fluid
Solution formation is driven not only by enthalpy changes but also by this thermodynamic driving force toward increased disorder or chaos.
Entropy