module 11 to 13 Flashcards
Describes the behavior of matter in terms of particles in motion.
Kinetic-molecular theory
A collision between gases in which no energy is lost
elastic collision
measure of the average kinetic energy of the particles in a sample of matter.
temperature
Movement of one material through another.
diffusion
states that the rate of effusion/diffusion for a gas is inversely proportional to the square root of its molar mass.
Graham’s law of effusion
Force per unit area
pressure
Used to measure atmospheric pressure.
barometer
SI unit of pressure; equal to one newton per square meter
pascal
Equal to 101.3 Kilopascal (kPa)
atmosphere
States that the total pressure of a mixture of gases is equal to the sum of pressures of all gases in the mixture.
Dalton’s law of partial pressures
Weak forces that result from temporary shifts in the density of the electrons in electron clouds.
dispersion force
Attractions between oppositely charged regions of polar molecules
dipole-dipole force
A dipole-dipole attraction that occurs between molecules containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone electron pair.
hydrogen bond
Measure of the resistance of a liquid to flow.
viscosity
The energy required to increase the surface area of a liquid by a given amount.
surface tension
Compounds that lower the surface tension of water
surfactant
solid whose atoms, ions, or molecules are arranged in an orderly, geometric structure
crystalline solid
The smallest arrangement of atoms in a crystal lattice
unit cell
Elements that exist in different forms at the same state.
allotrope
Solids not arranged in a regular, repeating pattern; the opposite of crystalline solids
amorphous solid
The temperature at which the forces that hold the crystal lattice of a solid together are broken and becomes a liquid.
melting point
Process by which a liquid changes to a gas or vapor.
vaporization
When vaporization only occurs only at the surface of a liquid.
evaporation
The pressure exerted by a vapor over a liquid is called
vapor pressure
The temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure
boiling point
The temperature at which a liquid is converted into a crystalline solid.
freezing point
The process by which a gas or a vapor becomes a liquid.
condensation
process by which a substance changes from a gas or vapor into a solid without becoming a liquid.
deposition
A graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure.
phase diagram
The point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist.
triple point
States that the volume of a fixed amount of a gas held at a constant temperature varies inversely with the pressure.
Boyle’s law
Zero on the Kelvin scale; represents the lowest possible theoretical temperature.
absolute zero
States that the volume of a given amount of gas is directly proportional to its Kelvin temperature at constant pressure.
Charles’s law
States that the pressure of a fixed amount of gas varies directly with the Kelvin temperature when the volume remains constant.
Gay-Lussac’s law
States that the relationships between pressure, temperature, and volume of a fixed amount of gas.
Combined Gas law
States that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.
Avogadro’s principle
The volume that 1 mol occupies at 0.00 degrees Celsius and 1.00 atm.
molar volume
I mole has 22.4L
The conditions of 0.00 degrees Celsius and 1.00 atm.
standard temperature and pressure (STP)
Experiments using known values of P, V, T, and n have determined the value of this constant
Ideal gas constant
Represented by R
Describes the physical behavior of an ideal gas in terms of the pressure, volume, temperature, and number of moles of gas present.
Ideal gas law
A mixture containing particles that are large enough that, if left undisturbed, will settle out over time due to gravity.
Suspension
Heterogenous mixture of intermediate size that cannot be separated by settling or filtration.
colloid
The erratic movement of colloid particles
Brownian motion
The scattered light by dispersed colloid particles.
Tyndall effect
A substance that can dissolve in a solvent is…
soluble
Two liquids that are soluble in each other in any proportion are…
miscible
A substance that does not dissolve in a solvent is…
insoluble
Two liquids that can be mixed but separate shortly after are…
immiscible
A measure of how much solute is dissolved in a specific amount of solvent or solution.
concentration
The number of moles of solute dissolved per liter of solution concentration
molarity (M)
Describes solutions in terms of how many moles of solute are dissolved in a specific mass(kg) of solvent
molality
m
The ratio of the number of moles of solute or solvent in solution to the total number of moles of solute and solvent
mole fraction
The process of surrounding solute particles with solvent particles to form a solution
solvation
The overall energy change that occurs during the solution formation process
heat of solution
Occur when no more solute can be dissolved.
saturated solution
Contain less dissolved solute for a given temperature and pressure than a saturated solution
unsaturated solution
Contains more dissolved solute than a saturated solution at the same temperature.
supersaturated solution
States that at a given temperature, the solubility of a gas in a liquid directly proportional to the pressure
Henry’s law
Physical properties of solutions that are affected by the number of particles but not by the identity of dissolved particles
colligative property
Due to the number of solute particles in solution and is colligative property of solutions
vapor pressure lowering
The temperature difference between a solution’s boiling point and a pure solvent’s boiling point
boiling point elevation
A solution’s difference in temperature between its freezing point and the freezing point of its pure solvent
freezing point depression
The diffusion of a solvent through a semipermeable membrane
osmosis
The amount of additional pressure cause by water molecules that moved into the concentrated solution
osmotic pressure
