IMF
Properties of Solids, Liquids, and Gases
Phase Diagrams
Phase Changes
Crystalline Solids
100
The type of force that increases as the size of the molecules increase
What is london dispersion forces
100
The property of a liquid that is a measure of resistance to flow.
What is viscosity
100
Points on a line on a phase diagram represent this
What is two phases in dynamic equilibrium
100
This phase change is a surface phenomenon
What is evaporation
100
This solid is classified as being soft and non-conductive
What is molecular solid
200
The type of force present in mixtures of ionic compounds and polar solutions
What is ion-dipole
200
The property related to the distribution of the kinetic energies of the molecules
What is vapor pressure
200
This point on the diagram is where the three phases coexist simultaneously in dynamic equilibrium.
What is the triple point
200
This phase change is the opposite of vaporization.
What is condensation
200
In this solid, particles are held in place by anion-cation attractive forces.
What is an ionic solid.
300
The force present in all polar molecules
What is dipole-dipole
300
This occurs when surface molecules experience an unequal attraction to bulk molecules.
What is surface tension
300
Normal substances' fusion curves have this slope
What is positive
300
If one were to reeduce the atmospheric pressure, this decreases.
What is boiling point
300
In this solid, there is no discrete molecules
What is covalent network solid
400
The strongest force for pure substances.
What is Hydrogen bonding
400
Vapor pressure occurs when the vapor and this are in dynamic equilibrium.
What is the liquid
400
This compound is specified as having molecules with sufficient energy to overcome the IMF (as in a gas) but pushed closed together (as in a liquid)
What is a supercritical fluid
400
The three endothermic phase changes are: vaporization, fusion, and this.
What is sublimation
400
This solid is generally ductile and malleable
What is metallic solid
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